JAMB 2024 CHEMISTRY LIKELY QUESTIONS AND ANSWERS

JAMB 2024 CHEMISTRY LIKELY QUESTIONS AND ANSWERS

Questions

Chemistry 1983 

1. X is crystalline salt of sodium. Solution of X in water  turns litmus red produces a gas which turns lime water  milky when added to sodium carbonate. With barium  chloride solution, X gives a white precipitate which is  insoluble in dilute hydrochloric acid. X is 
2. Na2,CO3 B. NaHCO3

C NaHSO4 D Na2SO3 

1. Na2SO4
2. The alkanol obtained from the production of soap is 

sweet taste and melts on heating. In the presence of  yeast and in the absence of air X is converted to  compound Y in the absence of air, X is converted to  compound Y and colourless gas. 

Compound Y reacts with sodium metal to produce a  gas Z which gives a ‘pop’ sound with a glowing splint.  Y also reacts with ethanoic acid to give a sweetsmelling  compound W. 

8. Compound W is 
   
9. ethanol B. glycerol A. a soap B. an oil C. methanol D. propanol C. an alkane D. an ester E. glycol E. sucrose 
10. The flame used by welders in cotton metals is 9. The molecular formula of X is A. butane gas flame A. C H O B. C H O 12 22 11 6 12 6 B. acetylene flame C. C H O D. C H O 3 6 3 7 14 7 C. kerosene flame E. C H3O 
    
11. oxy-acetylene flame 
12. oxygen flame 
13. Consecutive members of an alkane homologous series  differ by 
14. CH B. CH2
15. CH3 D. CnHn
16. CnH2n+2
17. If an element has the lectronic configuration 1s22s2 2p  

4 4 

10. reaction of X with yeast forms the basic of the A. plastic industry 
11. textile industry 
12. brewing industry 
13. soap industry 
14. dyeing industry. 
15. A mixture of common salt, ammonium chloride and  barium sulphate can best be separated by 

6

3s2 3p2, itis 

1. a metal 
2. an alkaline earth metal 
3. an s-block element 
4. a p-block element 
5. a transition element 
6. addition of water followed by filtration then  sublimation 
7. addition of water followed by sublimation then  filtration 
8. sublimation followed byaddition of water then  filtration 
9. fractional distillation 
10. fractional crystallization. 
11. Some copper (11) sulphate pentahydrate (CuSO45H2O),  was heated at 120oC with the following results: Wt of  crucible= 10.00 g; Wt of crucible + CuSO45H2O=14.98g;  Wt of crucible + residue = 13.54g. How manymolecules  of water of crystallization were lost? [H=1, Cu =63.5,  O=16, S=32] 
12. 1 B. 2 
13. 3 D. 4 
14. 5 
15. The three-dimensional shape of methane is A. hexagonal B. tigonal 
16. linear D. tertrahedral 
17. cubical 

Question 8-10 are based on the following 

An unknown organic compound X has a relative  molecular mass of 180. It is a colourless crystalline solid,  readily soluble in water. X contains the element C, H,  and O in the atomic ratio 1:2:1. The compound has a 

12. Which of the following relationships between the  pressure P, the volume V and the temperature T,  represents and ideal gas behaviors? 
13. P&VT B. P& T/V 
14. PT& V D. PV&VT 
15. P & V/T 

In the above experiment (fig1) the litmus paper will  initially 

1. be bleached B. turn green 
2. turn red D. turn blue 
3. turn black 
4. The colour imparted to a flame by calcium ion  is 
5. How many isomeric forms are there for themolecular  formula C3H6Br2? 
   
6. green B. blue A. 1 B. 2 C. brick-red D. yellow C. 3 D. 4 E. lilac E. 5
   
7. In the reaction M+ N P; H = + Q kJ.  Which of the following would increase the  concentration of the product? 
8. Decreasing the concentration of N 
9. Increasing the concentration of P 
10. Adding a suitable catalyst. 
11. Decreasing the temperature 
12. In which of the following processes is iron being  oxidized? 
13. Fe + H2SO4 H2 + FeSO4
14. FeSO4+ H2S FeS + H2SO4

3 FeCl + CI22FeCL3 

4 FeCl3+ SnCI22FeCL2 +SnCI4 

1. 1 only B. 2 only 
2. 3 only D. 1 and3 
3. 2 and4. 

Fig.2 

In the above experiment (fig.2), a current was passed  for 10 minutes and 0.63 g of copper was found to be  deposited on the cathode of CuSO4 cells. The weight  of AgNO3 cell during the same period would be [Cu =  63, Ag –108] 

1. 0.54g B. 1.08 g 
2. 1.62g D. 2.16 g 
3. 3.24g 
4. In the reaction Fe + Cu2+ Fe2+ + Cu, iron displaces  copper ions to form copper. This is due to the fact that A. iron isin themetallic formwhile dthe copper is  in the ionic form 
5. the atomic weight of copper is greater than  that of ion 
6. copper metal has more electronsthan ion metal D. iron is an inertmetal 
7. iron is higher in the electrochemicalseriesthan  copper. 
8. C2H5 C =CH2

CH3 

The correct name of the compound with the above structural formula is 

1. 2-methylbut-1-ene 
2. 2-methylbut-2-ene 
3. 2-methylbut-1-ene 
4. 2-ethyprop-1-ene 
5. 2-ethylprop-2-ene 
6. A piece of burning sulphur will continue to burn in a  gas jar of oxygen to give misty fumes which readily  dissolve in water. The resulting liquid is 
7. sulphur (1V)trioxide 
8. Tetraoxosulphate acid (V1) 
9. Trioxosulphate (1V) acid 
10. Dioxosulphate (11) acid 
11. Hydrogen sulphide 
12. Sodium decahydrate (Na2SO4 10H2O) an exposure to air  loses all its water of crystallization. The process of loss  is known as 
13. Efflorescence B. Hygroscopy C. Deliquescence D. Effervescence E. Dehydration 
14. Which of the following happens during theelectrolysis  of molten sodiumchloride? 
15. Sodium ion loses an electron 
16. Chlorine atom gains anelectron 
17. Chloride ion gains an electron 
18. Sodium ion isoxidized 
19. Chloride ion isoxidized. 
20. Crude petroleum pollutant usuallyseen on some Nigeria  creeks and waterways can be dispersed or removed by. A. heating the affected parts order to boil off the  petroleum 
21. mechanically stirring to dissolve the petroleum  in water 
22. pouring organic solvents to dissolve the  petroleum 
23. spraying the water with detergents 
24. cooling to freeze out thepetroleum. 
25. An element is electronegativeif 
26. it has a tendency to exist in the gaseousform B. its ions dissolve readily in water 
27. it has a tendency to lose electrons 
28. it has a tendency to gain electrons 
29. it readily forms covalent bonds 
30. Solution X,Y, and Z have pH values 3.0, 5.0 and 9.0  respectively. Which of the following statements is  correct? 
31. All the solution are acidic 
32. All solution are basic 
33. Y and Z are more acidic than water 
34. Y ismore acidic than X. 
35. Z is the leastacidic 
36. In the reactions  

(1) H2 (g) + 1 

2 O2(g) H 2O(1); H =-2.86kJ 

(11) C(s)+ O2(g) CO2(g); H= -406 kJ 

the equations imply that 

1. more heat is absorbed heat is evolved in (1) B. more heat is absorbed in (11) 
2. less heat is evolved in (1) 
3. reaction (11) proceeds faster than(1) 
4. reaction (1) proceeds faster than (11) 
5. Which of these metals, Mg, Fe, Pb, and Cu will dissolve  in diluteHCI? 
6. All themetals 
7. Mgm Fe, andCu 
8. Mg, Fem and Pb 
9. Mg and Fe only 
10. Mg only 
11. Stainless steel is an alloy of 
12. Carbon, iron and lead 
13. Carbon, ion andchromium 
14. Carbon iron and copper 
15. Carbon, iron and silver 
16. Carbon and iron only 
17. What volume of 0.50 MH2SO4 will exactly neutralize  20cm3 of0.1 M NaOH solution? 
18. 2.0 cm3 B. 5.0 cm3
19. 6.8 cm3 D. 8.3 cm3
20. 10.4 cm3
21. Which of the following pair of gases will NOT react  further with oxygen at a temperature between 30oC and  400oC? 
22. SO2 and NH3B. CO2 and H2
23. NO2 and SO3 D. SO3 and NO E. CO and H2
24. Some metals are extracted from their ores after some  preliminary treatments by electrolysis (L) some by  thermal reaction(T) and some by a combination of both  processes(TL). Which set-up in the following for the  extraction of iron copper and aluminum is correct? 
25. Iron (L), copper(L) m aluminum (T) 
26. Iron (T), copper (L), aluminum(T) 
27. Ion (TL), copper (TL), aluminium (TL) 
28. Iron (L), copper (T), aluminium (T). 
29. Ion (T), copper (L), aluminium (TL). 
30. Column chromatography 
31. Evaporation 
32. Increasing the pressure of a gas 
33. lowers the average kinetic energy of the  molecules 
34. decreases the density of the gas 
35. decreases the temperature of the gas 
36. increases the density of the gas 
37. increases the volume of the gas. 
38. 2.5 g of a hydrated barium salt gave on heating, 2.13 g  ofthe anhydrous salt. Given that the relative molecular  mass of the anhydrous salt is 208, the number of  molecules of water of crystallization of the barium salt  is 
39. 10 B. 7 
40. 5 D. 2 
41. 1 
42. 3.06 g of a sample of potassium trioxochlorate (v) (KCIO3) was required to make a saturated solution  with 10cm3 of water at 25oC. The solubility of the salt at  25oCis[K=39,CI =35.5,O=16] 
43. 5.0 moles dm3 B. 3.0 moles dm3 C. 2,5 moles dm3 D. 1.0 moles dm3 E. 0.5 moles dm3
44. The cracking processis veryimportant in the petroleum  industry because it 
45. gives purer products 
46. Yields morelubricants 
47. Yieldsmore engine fuels 
48. Yields more asphalt 
49. Yieldmore candlewax 
50. A gas that can behave as reducing agent towards  chlorine and as an oxidizing agent toward hydrogen  sulphide is 
51. O2 B. NO 
52. SO2 D. NH3
53. CO2
54. Which if the following solution will give a white precipitate with barium chloride solution and a green  flame test? 
    
56. In the preparation of some pure crystals of Cu (NO3)2 C. 

starting with CuO, a student gave the following  

Na2SO4 CaSO4 

1. D. 

CuSO4 CaCI2 

statements as steps he employed. Which of these shows  a flaw in hisreport? 

1. Some CuO was reacted with excess dilute  H2SO4
2. The solution was concentrated 
3. When the concentrate was cooled, crystals  formed were removed by filtration. 
4. The crystals were washed with very cold water E. The crystals were then allowed to dry. 
5. Which of the following seperation processes is most  likely to yield high qualityethanol (>95%) from palm  wine? 
6. Fractional disllation without a dehydrant B. Simple distillation without adehydrant 
7. Fractional distillation with a dehydrant 
8. (NH4)2 SO4
9. The mass of an atomis determined by 
10. its ionization potential 
11. its electrochemical potential 
12. the number of protons 
13. the number of neutrons and protons 
14. the number of neutrons and electrons 
15. Which ofthe following is neutralization  reaction? 
16. Addition of chloride solution 
17. Addition of trioxonirate (V) acid (nitricacid)  to distilledwater. 
18. Addition of trioxonirate (V) acid (nitricacid)  to tetraoxosulphate (V1) acid (sulphuric acid).
19. Addition of trioxonirate (V) (potassium nitrate)  solution 
20. More CuCI is formed at 10oC 2 
21. Less CuCI2is formed at 10oC 
    
22. Addition of trioxonirate (V) acid (nitricacid)  potassium hydroxide solution. 

D there is no change CuCI2 10oC 

formed at 40oC and 

43. A jet plane carrying 3,000 kg of ethane burns off all the 
44. More CuCI is consumed at 40oC 2 
    

gas forming water and carbondioxide. If all the 48. Zn + H2SO ZnCI + H 4 2 2 

carbondioxide is expelled and the water formed is  condensed and kept on board the plane, then the gain  in weight is 

1. 1,800kg B. 900kg 
2. 600kg D. 2,400 kg  
3. 1,200kg 
4. Liquid X, reacts with sodium trioxocarbonate (IV)  (Na2CO3) to give a gas which turns calcium chloride  solution milky. Xis 
5. Na2SO4 (aq) B. KI(ag) C. An alkali D. An acid E. A hydrocarbon. 
6. Which of the following statements isFALSE? A. copper (11) ion can be reduced to copper (1)  ion by hydrochloric acid and zinc. 
7. Sodium metal dissolves in water givingoxygen C. Nitrogen is insoluble inwater 
8. Carbondioxide issoluble in water 
9. Lead has a higher atomic weight than copper 
10. When sodium dioxonitrate (111) (HaNO2 \) dissolvesis A. Exothermic B. Endothermic C. Isothermic D. Isomeric 
11. Hydroscopic 
12. The equilibrium reaction between copper (1) chloride  and chloride at 25oC and 1 atmosphere is represented  by the equation: 

2CuCI2+ CI 2CuCI2 H = -166kJ . Which ofthe 

2 

following statement is TRUE for the reaction, pressure  remaining constant. 

1. More CuCI is formed at 40oC 

2 

The rate of the above reaction will be greatly increased  if. 

1. the zinc isin the powered form 
2. a greater volume of the acid is used 
3. a smaller volume ofthe acid is used 
4. the reaction vessel isimmersed in an ice-bath E. the zinc isin the form of pellets. 
5. Zn + H2SO4 ZnSO4 + H4

In the above reaction how much zinc will be left undissolve if 2.00 g of zinc treated with 10cm3of 1.0 M  of H2SO4? [Zn =65, S=32, O = 16, H = 1] 

1. 1.35g B. 1.00 g 
2. 0.70g D. 0.65 g 
3. 0.06g 
4. 30cm3 of 0.1 M AI(NO3)3 solution is reacted with  100cm3 of 0.15M of NaOH solution. Which is in excess  and by how much? 
5. NaOH solution, by70cm3 
6. NaOH solution, by60cm3 
7. NaOH solution by40cm3 
8. AI (NO3)3, solution by 20cm3 
9. AI (NO3)3solution, by 10cm3
   

Chemistry 1984 

1. Sodium chloride may be obtained from brineby A. titration B. decantation 
2. distillation D. evaporation E. sublimation 
3. 20cm3 of hydrogen gas are sparked with 20cm3 of  oxygen gas in an eudiometer at 373K (100oC) and 1 at  atmosphere. The resulting mixture is cooled to 298 K  (25oC) and passed over calcium chloride. The volume  of the residual gas is 
4. 40cm3 B. 20cm3
5. 30cm3 D. 10cm3
6. 5 cm3
7. For the reaction NH4NO 2 N2 + 2H2O calculatethe  volume of nitrogen that would be produced at S.T.P  from 3.20 g ofthe trioxonirate (111)salt. 
8. 2.24dm3 B. 2.24cm3
9. 1.12cm3 D. 1.12dm3
10. 4.48dm3

(Relative atomic masses: N = 14m O =16, H=1). 

4. Manganese (1V) oxide reacts with concentrated  hydrochloric acid according to the equation 

MnO2+ xHCI MnCI2+ CI +yH2O. x and y are A. 2 and 5 respectively 

1. 2 and 4 respectively
2. and 2 respectively 
3. 4 and s2 respectively 
4. 4 and 1 respectively 
5. A molar solution of caustic soda is prepared by  dissolving 
6. 40 g NaOH in 100 g of water 
7. 40 g NaOH in 1000 g of water 
8. 20 g NaOH in 500 g ofsolution 
9. 20 g NaOH in 1000 g ofsolution 
10. 20 g NaOH in 80 g ofsolution. 
11. Which among the element 1. Carbon 2. Oxygen 3.  Copper 4. Bromine 5. Zinc will NOT react with either  water ofstream? 
12. 1 and 2 B. 2 and 3 
13. 3 and 4 D. 1, 2, and 3 
14. 2, 3 and 5 

Fig 1 

Which of the curves shown in fig 1 represents the  relationships between the volume (v) and pressure (p)  of an ideal gas at constant temperature? 

1. 1 B. 2 
2. powdering the reactant ifsolid 
3. 1,2 and 3 B. 1,3 and 5 C. 2, 3 and 5 D. 3 and4 E. 3 and5 

11 The balance equation for the reaction of  tetraoxosulphate (V1) acid with aluminium hydroxide  to give water and aluminium tetraoxosulphate (V1) is A. H2SO4 +AISO42H2O +AISO4 

1. HSO4+ AIOH H2O +AISO4 
2. 3H2SO4 +2AIH36H2OH + AI(SO4)3
3. 3H2SO4 + 2AI(OH)3 6H2O + AI(SO4)3 E. H2SO4+AI (OH)3 H2O +AI2(SO4)3

Fig. 2. 

The solubility curves of four substances are shown in  Fig.2. Which of the four substances would crystallize  from a saturated solution cooled from 353 K (80oC)to  323 K(50oC) 

1. P and Q B. P and R 
2. P and S D. R and S 
3. Q andR. 
4. which of the following mixtures would result in a  solution of pH greater than 7? 
   
5. 3 D. 4 
6. 25.00 cm3 of 0.05 M H SO 

and 25.00 cm3 of  

1. 1 and3 

2 

4 

0.50 m Na2CO3 

25. 25.00 cm3 of 0.50 M H SO 

and 25;00 cm3 of  

8. Naphthalene when heated melts at 354K (81oC). At this  

2 

4 

0.10 M NaHCO3 

temperature the molecules of naphthalene . 

25. 25.00 cm3 of 0.11 M H SO 

and 25.00 cm3 of 

1. decompose into smallermolecules 

2 

4 

0.10M NaOH 

1. change their shape 
2. 25.00 cm3 of 0.11 M H SO 

and 50.00 cm3 of 

1. are oxidized by atmospheric oxygen 

2 

4

0.50 M NaOH 

1. contract 
2. 25.00 cm3 of0.25MH SO and 50.00cm3 of).20  
   
3. become mobile as the inter molecular forces  are broken. 

M NaOH 

2 4 

9. The ration ofthe number of moleculesin 2g of hydrogen  to that in 16 g of oxygen is 
10. 2:1 B. 1:1 
11. 1:2 D. 1:4 
12. 1:8 
13. Which combination of the following statements is  correct? 
14. lowering the activation energy 

2 conducting the reaction in a gaseous state 3. increasing the temperature 

4. removing the products as soon as they are  formed 
5. In which of the following reactions does hydrogen  peroxide acts as a reducing agent? 
6. H2S + H2O S +2H2O 
7. PbSO3+ H2O2PbSO4 +H2O 
8. 2‘! + 2H + H2O I2 +2H2O 
9. PbO2 + 2HNO3 +H2O2Pb (NO3)2 +2H2O + O2
10. SO + H2O2 H2SO4
11. For the reaction 2Fe +2e- 2Fe2+ +I , which of the 2 

following statements is TRUE? 

1. Fe is oxidized to Fe3
2. Fe3+ is oxidized to Fe2+
   
3. I–is oxidized to I 21. An element that can exist in two or more different 
   

2 

1. I- is reduced to I2
2. I–is displacing an electron fromFe3+

The diagram above (Fig.3) shows the energy profile for  the reaction A+B = C+ D. form this diagram, its clear  that the reaction is 

1. spontaneous B. isothermal 
2. adiabatic D. exothermic 
3. endothermic 

structure forms which possess the desame chemical  properties is said to exhibit 

1. polymerism B. isotropy C. isomorphism D. isomerism E. allotropy. 
2. Sulphur…. 
3. Forms two alkalineoxides 
4. Is spontaneously flammable 
5. Burns with a blue flame 
6. Conducts electricity in the molten state E. Is usually stored in the form ofsticks in water. 
7. Which off the following statements is NOT true of  carbon monoxide? 
8. CO is poisonous 
9. CO isreadily oxidized at room temperature by  air to form Co2
10. CO may be prepared by reducing CO2, mixed coke heated to about 1000oC 
11. CO may be prepared by heating charcoal with  a limited amount ofO2
12. CO is a good reducing agent. 
13. In dilute solute the heat of the following NaOH + HCI =  NaCI + H2O+ H2SO4 Na2SO4 + 2H2Ois 
14. +28.65 kJ B. –28.65kJ 
15. +57.3 kJ D. –114.6 kJ 
16. –229.2 kJ 
17. From the reactions: 

ZnO + Na2O Na2ZnO and 

ZnO+ CO2 ZnCO3it may be concluded that zinc oxide is 

3. For the reactions: (1 Melon oil + NaOH ! Soap +  E. 

Glycerol (11) 3Fe + 4H2O Fe3O4 + 4H2 (111) N2O4 

neutral  acidic 

a mixture 

1. D. 

basic  

amphoteric 

2NO2. Which of the following statements istrue? 25. 

1. Each of the three reactionsrequires a catalyst B. All the reactions demonstrate Le Chatelier’s  

An example of a neutral oxide is A. AL2O3B. NO2 

principle 

2. The presence of a catalyst will increase the  

yield of products 

CO2 SO2 

1. CO 
   
2. Increase in pressure will result in higher yields  of the products in 1 and 11 only 
3. Increase in pressure willresult in higher ofthe  products in 111 only. 
4. Which ofthe following methods may be used to prepare  trioxonirate (V) acid (nitric acid) in the laboratory? A. Heating ammonia gas with tetraoxosulphate  (1V) acid 
5. Heating ammonium trioxosulphate (V) with  tetraoxonitrate (V)acid 
6. Heating sodium trioxonirate (v) with  tetraoxosulphate (V1) acid 
7. Heating potassiumtrioxonirate (V) with calcium  hydroxide. 
8. Heating a mixture of ammonia gas and oxygen\ 
9. Lime –water, which is used in the laboratory for the  detection of carbon (1V) oxide, is an aqueous solution  of: 
10. Ca (OH)2B. CaCO3
11. CaHCO3D. CaSO4
12. N2CO3
13. 3CI2+ 2NH3 N2 + 6HCI. In the above reaction,  ammonia acts as. 
14. a reducing agent 
15. an oxidizing agent 
16. an acid 
17. a catalyst 
18. a drying agent 
19. In the Haber processfor the manufacturer of ammonia,  finely divided iron is used as 
20. an ionizing agent 
21. a reducing agent 
22. a catalyst 
23. a dehydrating agent 
24. an oxidizing agent. 
25. An organic compound with a vapour density 56.5 has  the following percentage composition: C = 53.1%, N =  12.4%, O = 28.3%, H = 6.2%. The molecular formula of  the compound is 
26. C3H6O2N B. C5H6O2N 
27. (C5H7O2N)½ D. C5H7O2N 
28. (C5H7ON)2.

Relative atomic masses: N = 12.4%, O = 28.3%, H = 1) 

29. The hybridization of the carbon atom in ethyne is 
30. Sp^ B. sp335. which ofthe following statement is NOT correct about  
    
31. sp2 D. sp 
32. s 
33. When the kerosene fraction form petrol is heated at  high temperature, a lower boiling liquid is obtained.  This process is known as 
34. polymerization B. refining 
35. hydrogenation D. cracking 
36. fractional distillation  

O 

31. CH3- CH2-C 

OH 

Is 

1. acetic acid B. propanal 
2. propanol D. ethanoic acid E. propanoic acid 
3. Alkaline hydrolysis of naturally occurring fats and oils  yields. 
4. fats and acids 
5. soaps and glycerol 
6. margarine and butter 

all four ofthe acids: HBr, HNO H CO and H SO ?They 3 2 3 2 4 A. dissolve marble to liberate litmusred 

1. have a pH less than 7 
2. turn blue litmusred 
3. neutralize alkalisto form salt 
4. react with magnesium to liberate hydrogen. 
5. If the cost of electricity required to deposit 1 g old  magnesium is N5.00. How much salt would it cost to  deposit 10 g of aluminium? 
6. N10.00 B. N27.00 
7. N44.44 D. N66.67  
8. N33.33. 

(Relative atomic masses: AI = 27, Mg = 24). 

37, In an experiment, copper tetraoxosulphate (V1) solution  was electolysed using copper electrodes, The mass of copper  deposited at the cathode by the passage of 16000 coulombs of electricity is 

16. 16.70g B. 17. 60g 
17. 67.10g D. 10. 67g 
18. 60.17g 

(Relatively atomic masses: Cu = 63.5m O = 16, 

H = 1, S = 32). 

38. esters 38. 3 R 19 U 24 S20 T19 . Which of the following 
    
39. detergents. 
40. Which of the following represents a carboxylic acid? OH 
41. R C

O 

OR 

1. R C 

O 

1. H2SO4, 
2. R – COOCOR 

H 

1. R C 

O 

34. which ofthe statement isINCORRECT? A. fractional distillation of crude petroleum will give  following hydrocarbon fuelsin order ofincreasing  boiling point: Butane < petrol < kerosene 
35. H2C = CH2 will serve as a monomer in the  preparation of polythene 
36. Both but – 1- ene and but –1-1yne willdecolorize  bromine readily. 
37. But –2 – ene will react with chlorine to form 2, 3 – dichlorobutane. 
38. Calcium carbide will react with water to form any  alkayne 

1 9 12 10 7 

statements is NOT true of the elements R, U, S, T, Y? A. R is an isotope of hydrogen 

1. U and Y are isotopes 
2. R,U,S and T are metals 
3. T is a noble gas 
4. S will react with oxygen to form SO 
5. Nitrogen can best be obtained from a mixture of oxygen  and nitrogen by passing the mixture over 
6. potassium hydroxide 
7. heated gold 
8. heated magnesium 
9. heated phosphorus 
10. calciumchloride. 
11. Water issaid to be ‘hard’if it 
12. easily formsice 
13. has to be warmed before sodium chloride  dissolves in it 
14. forms an insoluble scum with soar 
15. contains nitrates 
16. contains sodium ions. 
17. Sodium hydroxide (NaOH) pellets are 
18. deliquescent B. hygroscopic C. efflorescent D. hydrated 
19. fluorescent. 
20. Which of the following structure formulae is NOT  numeric with others? 
21. H H H H 

| | | |  

H–C- C – C – OH 

| | | |  

H H H H

1. H H H H 

| | | | H– 

C- O- C – C – C- H 

| | | | 

H H H H 

1. H H H H 

| | | | H– 

C- C – C – C-H 

| | | |  

H OH H H 

1. H O H 

| | 

H–C- C – C – C- H 

| | | |  

H H H H 

1. H H O H 

| | 

H–C – C – C – C-H 

| | | | 

H H H H 

43. Alkalines 
44. are all gases 
45. have the general formula CnH2n +2O 
46. contains only carbon and hydrogen 
47. are usually soluble inwater 
48. are usually active compounds. 
49. If an excess of a liquid hydrocarbon is poured into a jar  of chlorine, and the sealed jar isthen exposed forseveral hours to bright sunlight, all the chlorine gas is  
50. A piece ofsea shell, when dropped into a dilute solution  of hydrochloric acid produces a colourless odorless  gas, which turns clear limewater milky. The shell  contains 
51. sodium chloride 
52. ammonium nitrate 
53. calcium carbonate 
54. calcium chloride 
55. magnesium chloride 
56. An aqueous solution of a metal salt, Mm gives a white  precipate with NaOH, which dissolvesin excess NaOH.  With aqueous ammonium the solution of M also gives  a white precipate which dissolves in excess ammonia.  Therefore the caution in Mis 
57. Zn++
58. Ca++
59. AI+++
60. Pb++
61. Cu++
62. The I.U.P.A. C name for the compound 

H 

| 

CH- C – CH2 – CH3 

| 

CH3 is 

1. isopropylethene 
2. acetylene 
3. 3-methylbutane 
4. 2-methybutane 
5. 5-methypentane. 
6. At S.T.P how many litres of hydrogen can be obtained from the reaction of 500cm3 of0.5 M H SO  
   

consumed. The hydrocarbon is said to have undergone A. a polymerizationreaction 

1. an isomerixation reaction 
2. an addition reaction 
3. a substitution reaction 
4. a reduction reaction 
5. The function of conc. H2SOH4 in the etherification of  

2 

metal. 

22. 22.4 dm3
23. 11.2 dm3
24. 6.5 dm3
25. 5.6 dm3
26. 0.00dm3

excess zinc 4

ethanoic acid with ethanol isto A. serves as a dehydrating agent B. serves as solvent 

1. act as a catalyst 
2. prevent any side reaction E. serve as an oxidizingreaction 

(Gram molecular volume of H2 = 22.4 dm3) 

Fig. 1 

Chemistry 1985 

25. 25.0 moles B. 12.5 moles 
26. 6.25 moles D. 3.125 moles 
27. 0.625 moles 
28. 3.0 g of a mixture of potassium carbonate and potassium  chloride were dissolved in a 250cm3standard flask. 25 cm of  

3 

this solution required 40.00cm3 of 0.1 M HCI for  

neutralization. What is the percentage by weight of K2CO3 

in themixture? 

1. 60 B. 72 
2. 82 D. 89 
   
3. Figure shows part of the periodic Table. Which of the  elements belongs to the p-block? 
4. S,T and U. 
5. V, W andX 
6. S and T only 
7. P, Q and R 
8. V,W, X andS. 
9. Which of the following conducts electricity? A. Sulphur B. Graphite 
10. Diamond D. Red phosphorus E. Yellow phosphorus. 
11. An organic compound contains 72% carbon 12%  hydrogen and 16% oxygen by mass. The empirical  formula of the compound is 
12. C6H22O3 B. C6H10O3
13. C12H12O D. C6H12O 
14. C3CH10( H= 1, C = 12, O= 16). 4. 0.499 of CuSO .xH O when heated to constantweight 
15. 92 (K= 39, O = 16, C= 12). 

Figure 2 below represents the solubility curb\ves of two salts, X  and Y, in water. Use this diagram to answer question9 to 11 

9. At room temperature (300K) 
   
10. Y is twice as soluble as X 4 2
    

gave a residue of 0.346 g. The value of x is  

1. 0.5 B. 2.0 
2. 3.0 D. 4.0 
3. 5.0. 

(Cu= 63.5, S = 32.0 O = 16, H = 1). 

5. In an experiment which of the following observation  would suggest that a solid sample is a mixture? The A. solid can be ground to a fine powder 
6. density of the solid 2.25 g dm-3 
7. solid begins to melt until 648 K 
8. solid absorbs moisture from the atmosphere  and turns into aliquid 
9. solid melts at 300 K. 
10. Hydrogen diffuses through a porous plug A. at the same rate as oxygen 
11. at a slower rare than oxygen 
12. twice as fast as oxygen 
13. three times as fast as oxygen 
14. four times as fast as oxygen. 
15. Given the molecular mss of iron is 56 and that of oxygen  is 16, how many moles of Iron (111) oxide will be  contained in 1 kg of the compound? 
16. X is twice as soluble as Y 
17. X and Y soluble to the same extent 
18. X is three times as soluble asY 
19. Y is three times as soluble asX 
20. If 80 g each of X and Y are taken up in 100g of water at  353 K we shall have. 
21. only 10 g of X and Yundissolve 
22. only 16 g of Y undissolve 
23. 10 g of X and 16 g of Y undissolved 
24. all X and Y dissolved 
25. all X and Yundissolved 
26. Ifthe molar mass of X is 36 g, the number ofmoles of X  dissolved at 343 is 
27. 0.2 moles B. 0.7 moles 
28. 1.5 moles D. 2.0 moles 
29. 3.0 moles 
30. Some properties of chemical substances are mentioned  below (i) solar taste (ii)slippery to touch (iii)yields  alkaline gas with ammonium salts (iv) has pH less than  7 (v) turns phenolphthalein pink. Which of the above  are NOT typical properties of alkaline? 
31. (i), (iv) and(v) 
32. (iv) and (v)
33. (i) and (iv) 
34. (ii) and (v) 
35. (ii),(iii) and (v) 
36. A certain volume of a gas at 298K is heated such that  its volume and pressure are now four times the original  values. What is the newtemperature? 
37. 18.6K B. 100.0K 
38. 298.0K D. 1192.0K 
39. 47689.0K 
40. Hydrogen is not liberated when trioxonirate (v) acid  reacts with zinc because 
41. Zinc is rendered passive by the acid 
42. Hydrogen produced is oxidized towater C. Oxides of nitrogen areproduced 
43. All nitrates are soluble in water 
44. trioxonitrate v acid is a strong acid. 
45. The boiling points of water, ethanol, toluene and  button-2-ol are 373.OK, 351.3K, 383.6 K and 372.5 K  respectively. Which liquid has the highest vapour  pressure at 323.0K? 
46. water B. Toluene 
47. Ethanol D. Butan-2-ol 
48. None 
49. In what respect will two dry samples of nitrogen gas  differ from each other if samples 1 is prepared by  completely removing CO2and O2from air and sample 2  is prepared by passing purified nitrogen (i) oxide over 

heated copper? Sample 1 is 

1. purer than sample2 
2. slightly denser than sample2 
3. in all respects the same as sample 2 
4. colourless but sample 2 has a light brown. 

carbon monoxide and high level of methane, the  probable source(s) of the pollution must be 

1. automobile exhaust and biological  decomposition 
2. combustion of coal and automobile exhaust C. biological decomposition only 
3. combustion of coal, automobile exhaust and  biological decomposition 
4. combustion of coal and biological  decomposition. 
5. A correct electrochemical series can be obtained from  K, Na, Ca, Al, Mg, Zn, Fe, Pb, H, Cu, Hg, Ag, Au by  interchanging 
6. Al and Mg B. Zn and Fe 
7. Zn and Pb D. Pb and H 
8. Au and Hg. 
9. A certain industrial process is represented by the  chemical equation 2A(g) + B(g) ’!C(g) + 3D(g) H = XkJ  mol–. Which of the following conditions will favour the  yield of the product? 
10. Increases in the temperature, decrease in  pressure. 
11. Increase in temperature increase in pressure C. Decrease in temperature, increasein pressure D. Decrease in temperature, increase in pressure. E. Constant temperature, increase in pressure. 
12. 2MnO – + 10Cl– + 16H+ ’! 2Mn2++ 5Cl + 8H O.which of 4 2 2 

the substances serves as an oxidizing agent? 

1. Mn2+ B. Cl
2. H2O D. MnO4
3. Cl2
   
4. slightly less reactive than sample 2 24. In the reaction HO ’! H2 + ½O2 H=-2436000kJ2, 2 (g) (g) (g) 

which of the following has no effect on the equilibrium  

17. Copper sulphate solution is electrolyzed using platinum  electrodes. A current of 0.193 amperes is passed for  2hrs. How many grams of copper are deposited? A. 0.457g B. 0.500 g 
18. 0.882g D. 0.914 g 
19. 1.00 g (Cu = 63.5m F = 96500 coulombs) 
20. X + Y Z is an equilibrium reaction. The addition of  a catalyst 
21. increases the amount of W produced in a given  time 
22. increase the rate of change in concentrations of X,  Y andZ 
23. increases the rate of disappearance of X and Y D. increases the rate of the forwardreaction 
24. decreases the amounts of X and Y left after the  attainment ofequilibrium. 
25. What is the formula of sodium gallate if gallium (Ga)  showsan oxidation number of +3. 
26. NaGaO3 B. Na2G(OH)2
27. NaGa(OH)3 D. NaGa (OH)4
28. NaGaO 
29. If the ONLY pollutants found in the atmosphere over a  city are oxides of nitrogen suspended lead compounds, 

position? 

1. Adding argon to the system 
2. Lowering the temperature 
3. Adding hydrogen to the system 
4. Decreasing the pressure 
5. Increasing the temperature. 
6. which ofthe following metals will displace iron from a  solution of iron(11)tetraoxosulphate(1V)? 
7. copper B. mercury 
8. silver D. Zinc 
9. Gold 
10. Complete hydrogenation of ethyne yields A. benzene B. methane 
11. ethene D. propane 
12. Ethane 
13. Which of the following is used in the manufacture of  bleaching powder? 
14. sulphur dioxide B. chlorine C. hydrogen tetraoxosulphate 
15. hydrogen sulphide 
16. nitrogen dioxide 
17. A man suspected to being drunk is made to pass his  breath into acidified potassium dichromate solution. If

has breath carries a significant level of ethanol, the  final colour of the solution is. 

1. Pink B. Purple 
2. Orange D. Blue-black 
3. Green. 
4. When pollen grains are suspended in water and viewed  through a microscope, they appear to be in a state of  constant but erratic motion. This is due to 
5. convection currents 
6. small changes in pressure 
7. small changes intemperature 
8. a chemical reaction between the pollengrains  and water 
9. the bombardment of the pollen grains by  molecules ofwater. 
10. The energy change (H) for the reaction  CO(g) +½O2(g) CO2(g) is 
11. -503.7kJ B. +503.7 kJ 
12. –282.9 kJ D. +282.9 kJ 
13. +393.3kJ 

( Hi(CO) = -110.4 kJ mol-1( Hi(CO ) = -393 kJ mol-1 2 

31. The product formed on hydrolysis of 
32. The neutralization reaction between NaOH solution and  nitrogen (1V) oxide (NO2) produces water and 
33. NaNO2 andNaNO3
34. NaNO3 andHNO3
35. NaNO2
36. NaNO3
37. NaN2O3

CH3. 

33. The oxidation of CH- CH- C- O gives 

H H 

1. 2-butanone B. 2-butanal 
2. butane D. butanoic acid E. 3-butanal. 
3. Tetraoxosulphate (V1) ions are finally tested using A. acidified silver nitrate 
4. acidified bariumchloride 
5. lime –water 
6. dilute hydrochloric acid 
7. acidified lead nitrate 
8. The I.U.P.A.C name for the compound 

CH3 

CH3– CH- CH –CH = CH – CH3 is 

1. 2-methl-3-patene 
2. 4-methy-2-pentane 
3. 2-methl-2-penten 
4. 4-methyl-3-pentene 
5. 2-methyl-3-pentane 
6. Mixing of aqueous solution of barium hydroxide and  sodium tetraoxocarbonate(1V) yields a white precipitate  of 
7. barium oxide 
8. sodium tetraoxocarbonate(1V) 
9. sodium, oxide 
10. sodium hydroxide 
11. barium tetraoxocarbonate. 
12. An organic compound decolorized acidified KMnC4 solution but failed to react with ammoniacal silver nitrate  solution. Theorganic compound is likely to be. 
13. a carbonxyllic acicd 
14. an alkane 
15. an alkene 
16. an alkyne 
17. an alkanone 
18. Solid sodium hydroxide on exposure to air absorbs a  gas and ultimately gives another alkaline substance  with the molecularformula. 
19. NaOH.H2O B. NaOH.N2
20. Na2CO3D. NaHCO3
21. NaNO3
22. Which of the following is the functional group of  carboxylic acids? 
23. -OH 
24. >C= O 
25. >C-OH  

O 

1. -C 

OH 

1. -C= N
2. Which of the following substances is the most  abundant in the universe? 
3. Carbon B. Air 
4. Water D. Oxygen 
5. Hydrogen 

Question 41 and 42 are based on the following. A colourless organic compound X was burnt in exces  air to give two colourless and odourless grass, Y and Z , as products. X does not decolorize bomine vapour; Y  turnslime milkywhileZ gives a blue colour with copper (11) tetraoxosulphate (V1). 

41. Compound X is 
42. an alkene 
43. an alkane 
44. an alkyne 
45. tetra chloromethane 
46. Dichloromethane 
47. Y and Z arerespectively. 
48. CO2and NH3 B. CO andNH3 C. SO2and H2O D. CO2 and H2O E. SO2 andNH3
49. Which of the following compounds is NOT the correct  product formed when the parent metal is heated in air? A. Calcium oxide(CaO) 
50. Sodium oxide(Na2O) 
51. Copper (11) oxide (CuO) 
52. Tri-iron tetroxide (Fe3O4) 
53. Aluminium oxide (Al2O3) 
54. The atomic number of an element whose caution, X2+, has the ground state electronic configuration is  Is22s22P63s22p6is 
55. 16 B. 18 
56. 20 D. 22 
57. 24 
58. When marble is heated to 1473 K, another whiter solid  is obtained which reacts vigorously with water to give  an alkaline solution. The solution contains 
59. NaOH B. KOH 
60. Addition of dilute hydrochloric acid to an aqueous  solution of a crystalline salt yielded a yellow precipitate  and a gas which turned dichromate paper green. The  crystalline salt was probably 
61. Na2SO4 B. Na2S 
62. NaS2O3.5H2O D. NaCO3
63. NaHCO3
64. The process involved in the conversion of an oil into  margarine is known as 
65. hydrogenation B. condensation C. hydrolysis D. dehydration E. cracking 
66. An aqueous solution of an inorganic salt gave white  precipate (i) soluble in excess aqueous NaOH (ii)  insoluble in excess aqueous NH3 (III) with dilute HCI.  The caution present in the inorganic salt is 
67. NH3 + B. Ca++

4 

1. N++ D. Al+++
2. Pb++
3. Which ofthe following roles doessodium chloride play  in soap preparation? It 
4. reacts with glycerol 
5. purifies the soap 
6. accelerates the decomposition of the fat and  oil 
7. separates the soap form the glycerol 
8. converts the fat acid to its sodium salt. 
9. The function of sulphur during the vulcanization of  rubber is to . 
10. act as catalyst for the polymerization ofrubber  molecules 
11. convert rubber from thermosetting tio thermo  plastic polymer 
12. from chains which bind rubber molecules  together 
13. break down rubber polymermolecule 
14. shorten the chain length of rubber polymer. 
    
15. E. 

Mg(OH)2 Ca(OH)2 

1. Zn(OH)2

Chemistry 1986 

1. The movement of liquid molecules from the surface of  

the liquid gaseous phase above it is known as3. 10cm3 of hydrogen fluoride gas reacts with 5cm3 of  A. Brownianmovement 2 2 of a 

dinitrogen difllouride gas (N F ) to form 10cm3 

1. Condensation 
2. Evaporation 
3. Liquefaction 
4. What mass of a divalent metal M (atomic mass= 40)  would react with excess hydrochloric acid to liberate  22 cm3 of dry hydrogen gas measured as S.T.P? 
5. 8.0 g B. 4.0 g 
6. 0.8 g D. 0.4 g 

[ G. M. V = 22.4 dm3] 

single gas. Which of the following is the most likely  equation to the reaction? 

1. HF + N2F2 N2HF3
2. 2HF + N2F22NHF2
3. 2HF + N2F2 N2H2F4
4. HF +2N2F2 N4HF4
5. The number of atom chlorine present in 5.85 g of NaCI  is 
6. 6.02 x 1022
7. 5.85 x1023 C. 6.02 x 1023
8. 5.85 x1024

[Na = 23, Cl = 35.5] 

Avogadro’s Number = 6.02 x 1023] 

5. How much of magnesium is required to react with  250cm3 of0.5 M HCl? 
6. 0.3 g B. 1.5 g 
7. 2.4 g D. 3.0 g 

[Mg = 24] 

6. 200cm3 of oxygen diffuse through a porous plug in 50  seconds. Hoe long will 80 cm3 ofmethane (CH4) take to  diffuse through the same porous plug under the same  conditions? 
7. 20 sec B. 20 sec 
8. 14 sec D. 7 sec  

[C= 12, O= 16, H= 1] 

7. The relationship between the velocity (U) of gas  molecules and their relative molecule mass(M) is shown  by the equation 

A Û = (kM) ½ 

1. Û =(kM)2
2. Û =k

m

D Û = (k/ ) ½ 

m 

8. An element with atomic number twelve is likely to be A. electrovalent with a valency of 1 
9. electrovalent with a valency of 2 
10. covalent with a valency of 2 
11. covalent with a valency of 4 
12. Which of the following group of physical properties  increases form left to right of the periodic table? 1  lonization energy 2Atomic radius 3Electronegativity 4  Electron affinity 
13. 1 and 2 B. 1, 2 and 3 
14. 3 and 4 D. 1, 2, 3 and 4 

In the solubility curve above, water at 98oC is saturated  with KCl impurity in the crystals formed when the  solution is cooled to 30oC? 

1. NaHSO4,Ph<5 
2. Na CO , Ph>8 

2 3 

1. Na2Cl, Ph=7 
2. NaHCO3, Ph<6 
3. Which of the following is an acid salt? 
4. NaHSO4 B. Na2SO4
5. CH3CO2Na D. Na2S 
6. Which of the following solution will conduct the least  amount of electricity? 
7. 2.00 M aqueous solution of NaOH 
8. 0.01 M aqueous solution of NaOH 
9. 0.01 m aqueoussolution of hexaonic acid D. 0.01 M aqueous solution of sugar. 

10. When 50 cm3 of a saturated solution of sugar (molar  mass 342.0 g) at 40oC was evaporated to dryness, 34.2 g  dry of solid was obtained. The solubility of sugar of  40oCis 
11. 10.0 moles dm-3 B. 7.0 molesdm-3

In the electrolysis of aqueous solution of K2SO4  above cell, which species migrate to the anode? A. SO 2-and OH- B. K+and SO2- 4 

1. OH and H O D. H O and K+ 3 3 

in the 

3. 3.5 moles dm-3 D. 2.0 moles dm-3 16. How many coulombs of electricity are passedthrough  a solution in which 6.5 amperes are allowed to runfor 

1.0 hour? 

12. 3.90 x 102coulombs 
13. 5.50 x 103coulombs 
14. 6.54 x 103coulombs 
15. 2.34 x104coulombs 
16. Which of these represents a redox reaction? 
17. AgNO3+ NaCl AgCl + NNO3
18. H2s + Pb(NO3)2PbS + 2HNO3
19. CaCO3 CaO +CO2
20. Zn + 2HCl ZnCI2 + H2
    
21. How many electrons are transferred in reducing one  atom of Mn in the reaction 

MnO2+ 4HCl MnCl2+ 2H2O + Cl2 

1. 2 B. 3 
2. 4 D. 5 
3. 20 cm3 of 0.1 molar NH4OH solution whenneutralized  with 20.05 cm3 of 0.1 molar HCl liberated 102 Joules of  heat. Calculate the heat of neutralization of NH4OH  A. -51.0 kJ mol-1 B. +57.3 kJmol-1 C. +57.0kJmol-1 D. +51.0kJ mol-1
4. What is the consequence of increasing pressure on  the equilibrium reaction ZnO(s) + H2(g Zn(s) + H2O(i) A. The equilibrium is driven to the left 
5. The equilibrium is driven to the right 
6. There is no effect 
7. More ZnO(s) is produced 
8. The approximate volume of air containing 10cm of  oxygen is 
9. 20cm3 B. 25cm3
10. 50cm3 D. 100cm3
11. The reaction Mg+ H2O MgO + H2 takes placeonly  in the presence of 
12. excess Mg ribbon 
13. excess cold water 

C very hot water 

1. steam 
2. When steam is passed through red hot carbon, which  of the following are produced? 
3. Hydrogen and oxygen and carbon(1V)  

oxide 

1. Hydrogen and carbon (1V) oxide 
2. Hydrogen and carbon (11) oxixde 
3. Hydrogen and trioxocarbonate(1V) acid 
4. Which of the following contains an efflorescent, a  deliquescent and a hydroscopic substance  respectively? 
5. Na2SO4, concentrated H2SO2CaCl2
6. Na2CO3.H2O, FeSO2.7H2O, concentrated  H2SO4 
7. Na2CO3. 10H2O, FeCl3 concentratedH2SO4 D. Concentrated H2SO4, FeSO4.7H2O,MgCl2
8. The tabulated results below were obtained bytitrating 10.0 cm3 ofwater with soap. The titration wasrepeated  with the same sample of water after boiling. 

Before boiling After boiling 

Final (cm3) 25.0 20.0 

26. The exhaust fumes from a garage in a place that uses  petrol of high sulphur content are bound to contain A. CO and SO3
27. CO and SO2
28. CO, SO2 and SO3
29. CO and H2S 
30. Oxygen-demanding wastes are considered to be a water  pollutant because they. 
31. deplete oxygen which is necessary for the  survival of aquatic organisms 
32. increase oxygen which is necessary for the  survival of aquatic organisms 
33. increase other gaseous species which are  necessary for survival of aquatic organisms 
34. deplete other gaseous species which are  necessary for the survival of aquatic  

organisms. 

28. Which of the following will react further with oxygen  to form a higher oxide? 
29. NO and H2O 
30. CO andCO2
31. SO2 and NO 
32. CO2 andH2O 
33. In the course of an experiment, two gases X and Y  were produced. X turned wet lead ethanoate to black  and Y bleached moist litmus paper. What are the  elements(s) in each ofthe gases X and Y respectively? 
34. H and S;Cl 
35. H and O; Cl 
36. H and S;C and O 
37. H and Cl;S and O 
38. Which of the following sulphides is insoluble in dilute  HCl? 
39. Na2S B. ZnS 
40. CuS D. FeS 
41. When chlorine is passes into water and subsequently  exposed to sunlight, the gas evolved is 
42. HCl B. HOCl 
43. O2 D. Cl2O2
44. Which of the following metals does NOT form a stable  trioxocarbonate(1V) 
45. Fe B. Al 
46. Zn D. Pb 
47. Which of the following metals with NaOH to give salt  and water only. When Z is treated with dilute HCl, a  gas is evolved which gives a yellow suspension on  passing into concentrated H SO . Substance Z is. 
    

Initial(cm3) 10.00 15.0 A. C. 

The ratio of permanent to temporary hardness is 

NaHS NaS 

2 4 B. 

Na2SO3 NaHSO3 

34. 1:5 B. 1:4 34. Ammonia gas is normally dried with C. 4:1 D. 5:1 A. concentrated sulphuric acid B. quicklime 
35. anhydrous calcium chloride 
36. magnesium sulphate,
    
37. What are the values of x, y and z respectively in the  equation xCu +yHNO3xCu(NO3)2+ 4H2O + zNO?s  A. 4;1;2 
38. 3;8;2 
39. 2;8;3 
40. 8;3;2 
41. The iron (111) oxide impurity in bauxite can be removed  by 
42. fractional crystallization in acidsolution B. dissolution in sodium hydroxide and filtration C. extraction with concentrated ammonia and  reprecipitation 
43. electrolysis of moltenmixture. 
44. A white solid suspected to be lead trioxonirate (V), zinc  trioxocarbonate(1V) of calcium trioxocarbonate (1V) was  heated strongly. Its residue, which was yellow when  hot and white when cold, is 
45. lead (11) oxide B. calcium oxide C. zinc oxide D. lead nitrite 
46. Which of the following compounds would give lilac  fame coloration and a white precipitate with acidified  barium chloride solution? 
47. KCl B. NaNO3
48. K2SO D. CaSO4
49. How will a metal X, which reacts explosively with air  and with dilute acids be best extracted from its ores? A. Electrolysis of the solution of its salt 
50. Decomposition of its oxide 
51. Displacement from solution byan alkali metal D. Electrolysis of fused salt 
52. Which of the following is NOT correct for the named  organic compound in each case? 
53. Butanoic acid solution gives effervescence  with Na2CO3solution 
54. Glucose when reacted with Na CrO at 0oC will 2 4 

show immediate discharge of colour 

1. When but-2-ene is reacted with dilute solution  of KmnO4 the purple colour of KMnO is  

discharge readily even at roomtemperature 

1. When butan-2-ol is boiled with Butanoic acid  with a drop of concentrated H2SO4 a sweet  

smelling liquids isproduced. 

42. Which of the following is used as an‘anti-knock’ in  automobile engines? 
43. Tetramethylsilane 
44. Lead tetra-ethyl 
45. Glycerol 
46. N-heptanes 
47. What reaction takes place when palm-oil is added to  potash and foams are observed? 
48. Neutralization 
49. Saponification 
50. Etherification 
51. Salting-out 
52. How many isomers can be formed from organic  compounds with the formulaC3H8O? 
53. 2 B. 3 
54. 4 D. 5 
55. Which of the structural formula for pent-2-enoic acid?
56. When ethanol is heated with excess concentrated  sulphuric acid, theethanol is 
57. oxidized to ethene 
58. polymerized to polyethene 
59. dehydrated to ethene 
60. dehydrated to ethyne. 
61. Which of the following compounds is NOT formed by the action of chlorine on methane? 
62. CH3Cl B. C2H5Cl 
63. CH2Cl2 D. CHCl3
64. The general formula of an alkyl halide (where X  represent the halide)is 
65. CnH2n 2X B. –CnH2n +1X 
66. CnH2n +2X D. CnH2nX 
67. Which of the following are made by the process of  polymerization? 
68. Nylon and soap B. Nylon and rubber C. Soap and butane D. Margarine and Nylon 
69. Starch can converted to ethyl alcohol by A. distillation B. fermentation C. isomerization D. cracking. 

.

Chemistry 1987 

1. A brand of link containing cobalt (11), copper (11) and  irons can best be separated into its various components  by. 
2. fractional crystallization 
3. fractional distillation 
4. sublimation 
5. The atomic numbers of two elements X and Y are 12  and 9 respectively. The bond in the compound formed  between the atoms of these two elements is. 
6. ionic B. convalent 
7. neutral D. co-ordinate. 10. An element Z, contained 90% of 16 Z and 10% of 18 Z.  
   
8. chromatography. 

Its relative atomic massis 

8 8 

2. Which of the following substances is a mixture? A. Granulated sugar 
3. Sea-water 
4. Sodium chloride 
5. Iron fillings 
6. The number of molecules of carbon (1V) oxideproduced  when 10.0 g CaCO istreated with 0.2 dm3 of1 M HCl in  3 

the equation CaCO3+ 2HCI CaCl2 + H2O + CO2 is  A. 1.00 x1023 

6. 6.02 x 1023
7. 6.02 x 1022
8. 6.02 x 10 23

[Ca= 40,O= 16,C= 12,NA=6.02 x 10 ,H= 1,Cl=35.5] 23 

16. 16.0 B. 16.2 
17. 17.0 D. 17.8 
18. The greater the difference in electronegativity between  bonded atoms, the 
19. lower the polarity of the bond 
20. higher the polarity of the bond  

C weaker the bond 

1. higher the possibility of the substance formed  being amolecule. 
2. A stream of air was successively passed through three  tubes X, Y, and Z containing a concentrated aqueous  solution of KOH, red hot copper powder and fused  calcium chloride respectively. What was the  composition of gas emanating from tube Z? 
3. CO2 and the inert gases 
   
4. In the reaction CaC + 2H O Ca (OH + C H B. N2, CO2 and the inert gases 2(s) 2 (1) 2(s) 2 2(g) C. N and the inert gases 
   

what is the mass of solid acetylene gas at S.T.P?  A. 3.8 g B. 2.9 g 

2. 2.0 g D 1.0 g 

[C= 12, Ca –40,G.M.V= 22400 cm3] 

5. If the quality of oxygen occupying a 2.76 liter container  at a pressure of 0.825 atmosphere and 300 K isreduced  by one-half, what is the pressure exerted by the  remaining gas? 
6. 1.650 atm B. 0.825 atm 
7. 0.413 atm D. 0.275 atm 
8. Which of the following substances has the lowest  vapour density? 
9. Ethanoic acid B. Propanol 
10. Dichlomethane D. Ethanal 

[O = 16, Cl = 35.5, H =1, C = 12] 

7. If d representsthe density of a gas and K is a constant,  the rate of gaseous diffusion is related to the equation A. r =k  

d 

1. r =kd 
2. r =k 

d 

1. r = k d
2. An isotope has an atomic number of 17 and a mass  number of 36. Which of the following gives the correct  number of neutrons and protons in an atom of the  isotope? 

Neutrons Protons 

1. 53 17 
2. 17 36 
3. 19 17 
4. 36 17 

2 

1. Water vapour, N2 and the inert gases. 
2. In the purification of town water supply, alum is used  principally to. 
3. kill bacteria 
4. control the pH ofwater 
5. improve the taste of the water 
6. coagulate small particles of mud. 
7. Which of the following water samples will have the  highest titer value wagestitrated for the Ca2+ ions using  soap solution? 
8. Permanently hard water after boiling 
9. Temporarily hard water after boiling 
10. Rain water stored in a glass jar for two years D. Permanently hard water passed through  permutit 
11. Oil spillage in ponds and creeks can be cleaned up by A. burning off the oil layer 
12. spraying with detergent 
13. dispersal with compressed air 
14. spraying with hot water. 
15. The solubility of Na3AsO4(H2O)12 is 38.9 g per 100 g  H2O. What is the percentage of Na3AsO4 in the  saturated solution? 
16. 87.2% B. 38.9% 
17. 19.1% D. 13.7%

[As = 75, Na = 23, O = 12, H= 1] 

17. Which is the correct set results for tests conducted  respectively on fresh lime and ethanol? 

Test Fresh lime juice Ethanol
A. Add crystals of NaHCO3 B. Test with methyl orange C. Taste  D. Add a piece of sodium	Gas evolve  Turns colourless Bitter  No gas evolved	No gas evolved  No change Sour  H2 evolved

 

 

18. In which of the following are the aqueous solutions  of each of the substances correctly arranged in order  of decreasing acidity? 
19. Ethanoic acid, milk ofmagnesia, sodium  chloride, hydrochloric acid and sodium  

hydroxide. 

1. Ethanoic acid hydrochloric acid, milk of  magnesiam sodium chloride and sodium,  

hydroxide. 

1. Hydrochloric acid, ethanoid acid solution  chloride, milk of magnesia and sodium  

hydroxide 

1. Hydrochloric acid sodium hydroxidesodium  chloride ethanoic acid and milk ofmagnesia 
2. The basicity of tetraoxophosphate (v) acid is A. 7 B. 5 
3. 4 D. 3 
4. If 24.83 cm3 of 0.15 M NaOH is tritrated to its end  point with 39.45 cm3 ofHCl, what isthe molarity of  the HCl ? 
5. 0.094 M B. 0.150M 
6. 0.940M D. 1.500M 
7. A quantity of electricity liberates 3.6 g of silver from  its salt. What mass of aluminium will be liberated  from its salt by the same quantity of electricity? 

A 2.7 g B. 1.2 g 

1. 0.9 g D. 0.3 g 
2. Which ofthe following statements is CORRECT if 1  Faraday of electricity is passed through 1 M CuSO4 solution for 1 minute? 
3. The pH of the solution at the cathode  

decreases 

1. The pH of the solution at the anode  

decreases 

1. 1 mole of Cu will be liberated at the cathode D. 60 moles of Cu will be liberated at the anode. 
2. What mass of magnesium would be obtained by  passing a current of 2 amperes for 2 hrs. 30mins  through molten magnesium chloride? 
3. 1.12g B. 2.00 g 
4. 2.24g D. 4.48 g 

[1 faraday = 96500 coulombs, Mg = 24] 

24. In the reaction of 3CuO+ 2NH33Cu + 3H2O +N2 how many electrons are transferred for each mole to  copper produced? 
25. 4.0 x 10-23 B. 3.0 x10–23
26. 1.2x 1024 D. 6.0x 1024
27. Z is a solid substance, which liberates carbon (1V) oxide  on treatment with concentrated H2SO4, KnnO4. The solid  substance, Z is 

.A. sodium hydrogen trioxocarbonate(1V) 

1. ethanoic acid 
2. iron (11) trioxocarbonate(1V) 
3. ethanedioc acid (oxalicacid) 
4. 5 g of ammonium trioxonirate (V) on dissolution in water  cooled its surrounding water and container by 1.6kJ.  What is the heat of solution of NH4NO3? 
5. +51.4 kJ mol-1 B. +25.6 kJ mol-1 C. +12.9 kJ mol-1 D. –6.4 kJ mol-1 [N = 14, O = 16, H = 1] 
6. Tetraoxosulphate (1V) acid is prepared using the  chemical reaction SO3(g) + H2O(1) H2SO4(1). Given the  heat of formation for SO3(g), H2O(1) and H2SO4(1) as –395  kJ mol-1 –286 kJ mol-1 and – 811 kJ mol-1 respectively  is 
7. -1032kJ B. – 130kJ 
8. +130kJ D. +1032kJ 
9. The times taken for iodine to be liberated in the reaction  between sodium thisosulphate and hydrochloric acid  at various temperatures are asfollows: 

TempoC  Time (seconds)

25  72

35  36

45  18

 

These results suggest that. 

1. for a 10orise in temperature rate of reaction is  doubled 
2. for a 10orise in temperature rate of reaction is  halved 
3. time taken for iodine to appear does not depend  on temperature 
4. for a 10orise in temperature, rate ofreaction is  tripled. 
5. The reaction between sulphur (1V) oxide and oxygen is  represented by the equilibrium reaction 

2SO2(g H + O2(g) 2SO3(g), H = – 196 kJ. What factor  would influence increased production SO3(g)? 

1. Addition of a suitable catalyst 
2. Increase in thetemperature of the reaction C. Decrease in the temperature of SO2(g)
3. Decrease in the concentration of SO2(g)
4. Which of the following equations correctly represents  the action of hot concentrated alkaline solution on  chlorine? 
5. Cl2(g) + 2OH(g) OCl(q) + Cl(q) + H2O(1)
6. 3Cl2(g) + 6OH ClO3(aq)+ 5Cl (aq) + 3H2O(1) C. 3CI + 6OH(aq) ClO + 5Cl– + 3H O 2(g) 3(s) (aq) 2 (1) 
7. 3Cl2(g) + 6OH(aq) 5ClO3(aq) + Cl (aq) +3H2O(1)
8. Magnesium ribbon was allowed to burn inside a given  gas P leaving a white solid residue Q. Addition of water  to Q liberated a gas which produced dense white fumes  with a drop of hydrochloric acid. The gas Pwas 
9. nitrogen B. chlorine 
10. oxygen D. sulphur (1V) oxide
11. The best treatment for a student who accidentally  poured concentrated tetraoxosulphate(V1) acid on his  skin in the laboratory is to wash he skinwith 
12. cold water 
13. sodium trioxocarbondioxide solution 
14. Iodine solution 
15. Sodium triocarbonate (1V)solution. 
16. In which of the following pairs of elementsis allotropy  exhibited by each element? 
17. Phosphorus and hydrogen 
18. Oxygen and chlorine 
19. Sulphur and nitrogen 
20. Oxygen and sulphur. 
21. Which of the following gases can best be used for  demonstrating the fountain experiment? (i) Nitrogen 
22. Which of the following compounds will give a  precipitate with an aqueous ammoniacal solution of  copper (1) chloride? 
23. CH3CH =CHCH3
24. CH3C——CCH3
25. CH =C—CH2CH3
26. CH2=CH-CH-=CH2
27. The efficiency of petrol as a fuel in high compression inetrnal combustion engines improves with an increase  in the amount of 
28. Branched chain alkanes B Straight 

chain alkanes C. Cycloalkanes D. Halogenated  hydrocarbons 

43. A palm wine seller stoppered a bottle of his palm wine  in his stall and after a few hours the bottle represents  the reaction that occurred? 
    

(ii) Ammonia (iii) Nitrogen (l)oxide (iv) Hydrogen A. C H Oenzymes 2 C H OH + 2CO 

chloride 

1. (ii) and (iii) B. (i) and(iii) 
2. (ii) and (iv) D. (ii) only. 
3. When calcium hydroxide us heated with ammonium  tetraoxosulphate (V1), the gas given off may be  collected by 
4. bubbling it through concentrated H2SO4.
5. Bubbling it through water and then passing it through calcium oxide 
6. Passing it directly through calcium oxide 
7. Passing it directly through calcium chloride. 
8. Which ofthe following elements will form oxide which  will dissolve both dilute HNO3 and NaOH solution to  form salts? 
9. Cl B. Mg 
10. Ag D. Mn 
11. Stainless steel is an alloy of 
12. iron, carbon and silver 
13. ironm carbon and lead 
14. iron, carbon andchromium 
15. iron and carbon only. 
16. Alloys are best prepared by. 
17. high temperature are welding of the metals B. electrolysis using the major metallic  component as cathode 
18. reducing a mixture ofthe oxides ofthe elements D. cooling a molten, mixture of the necessary  elements. 
19. Corrosion is exhibited by. 
20. iron only 
21. electropositive metals 
22. metals belowhydrogen in the electrochemical  series 
23. all metals 
24. Inspite of the electronic configuration, 1s22s p22,carbon  

6 12 6 2 5 2(g) 

1. C2H5OH CH2 = CH2(G)) + H2O 
2. C2H5OH + dil H2SO4 C2H5OSO2OH 
3. 2C6H12O6 C12H12O13 +H2O 
4. ethanol reacts with aqueoussodium mono-oxoio date(1)  to gives a bright yellowsolid with a characteristic smell.  The products is 
5. trichlomethane 
6. ftriiodomethane 
7. iodoethane 
8. ethanal 
9. The most volatile fraction obtained from fractional  distillation of crude petroleumcontains 
10. butane propane and kerosene 
11. butane propane and petrol 
12. ethane, methane and benzene 
13. ethane methane and propane 
14. Local black soap is made by boiling palm with liquid  extract of ash. The function of the ash is to provide the A. acid B. ester of alkanoic acid C. alkali D. alkanol 
15. Synthetic rubber is made by polymerization of A. 2 methylbuta-1,3-diene 
16. 2 methl buta-1, 2 – diene 
17. 2 methyl buta – 1-ene 
18. 2 methy buta –2-ene 
19. Complete oxidation of propan – 1 – of gives A. propanal 
20. propan-2-L 
21. propan-1-one 
22. propanoic acid 
23. When water drops are added to calcium carbide in a  container and the gas produced is passed called and A. oxyethylene flame 
24. oxyhydrocarbon flame 
25. oxyacetylene flame 
    

2 

is tetravalent because 

1. oxymethane flame. 
2. the electrons in both 2s and 2p orbital have equal  energy 
3. the electrons in both 2s and 2p orbital are  equivalent 
4. both the 2s and2p orbital hybridize 
5. the six orbital hybridize to four. 
6. The structure of benzoic acid is.
   

Chemistry 1988 

1. Boyle B. Charles 
2. Graham D. Gay-lussac 

7, An increase in temperature causes an increase in the  

pressure in the 

1. average velocity of the molecules 
2. number of collisions between the molecules 
3. density of the molecules 
4. free mean path between each molecules and  

other. 

2. The forces holding naphthalene crystal together can  
   

In the experiment above, ammonium chloride crystals deposit  on the walls of the tube is as a result of 

1. Evaporation 
2. Recrystallization 
3. Sublimation 
4. Fractional precipitation. 
5. The formula of the compound formed in a reaction  between a trivalent metal M and a tetravalent non-metal X  is.A. MX B. M X 

3 4 

1. M4X3 D. M3X2
2. 2.25 g ofsample of an oxide of a copper. 2.50 g of another  oxide of Copper on reduction also gave2.0 g of copper.  These results are in accordance with the law of 
3. constant composition 
4. conversation of matter 
5. multiple proportions 
6. definite proportions. 
7. One role of propane is mixed with fivemoles of oxygen.  The mixture is ignited and the propane burns completely.  What is the volume of the products at soap? 
8. 112.0 dm3 B. 67.2 dm3
9. 56.0 dm3 D. 44.8 dm3

[G.M.V = 22.4 dm3mol-1] 

5. 0.9 dm3 of a gas at s. t. p was subjected by means of a  movable piston to two times the original pressure with  the temperature being now kept at 364 K. What is the  volume of the gas in dm3at this pressure? 
6. 2.0 B. 4.5 
7. 6.0 D. 8.3 
8. Which of the gas laws does the above graph illustrate? 

be overcome when naphthalene is heated to a  temperature of 354 K resulting in the crystals melting.  These forces are known as. 

1. coulombic B. ionic 
2. covalent D. van der waals 
3. A metallic ion X2+with an inert gasstructure contain 18  electrons. How many protons are there in this ion?  A. 20 B. 18 
4. 16 D. 2 
5. Which of the following physically properties decreases  across the periodic table. 
6. Ionization potential 
7. Electron affinity 
8. Electronegativity 
9. Atomic radius 
10. What are the possible oxidation numbersfor an element  if its atomic is 17? 
11. -1 and 7 B. – 1 and 6 
12. – 3 and 5 D. – 2 and 6 
13. The energy change accompanying the addition of an  electron to a gaseous atom is called 
14. first ionization energy 
15. second ionization energy 
16. electron affinity 
17. electronegativity 
18. The molar ratio of oxygen to nitrogen in dissolved air is  2:1 whereasthe ratio is 4:1 in atmospherics air because A. nitrogen is less soluble than oxygen 
19. oxygen is heavier than nitrogen 
20. nitrogen has a higher partial than pressure in  air 
21. gases are hydrated in water. 
22. An eruption polluted an environment with a gas  suspected to H2S, a poisonous gas. A rescue team  should spray the environment with 
23. water 
24. moist SO2
25. acidified KmnO4 andwater 
26. water, acidified KnnO4 and oxygen.
27. 1.34 g of hydrated sodium tetraoxosulphate (V1) was  heated to give an anhydrous salt weighing 0.71g. The  formula of thehydrated salt. 
28. Na2SO4.7H2O 
29. Na2SO4.3H2O 
30. Na2SO4.2H2O 
31. Na2SO4.H2O. 

[Na = 23, S =32, O = 16, H=1]. 

16. The ion that may be assumed to have negligible  concentration in a sample of water that lathers readily  with soap is 
17. Mg2+ B. K+

electricity. G passing through the electrolyte. This is  represented graphically by. 

325. CO2- D. HCO325. A mixture of starch solution and potassium iodide was 3
     
326. A substance S is isomorphous with another substance R. When a tiny crystal of R, 
327. S dissolves in the solution 
328. Crystals of R areprecipitated 
329. There is no observable change 
330. R and S react to the generate heat. 
331. Which of the following dilute solutions has thelowest  pH value? 
332. Calcium trioxocarbonate(1V)  

B Sodium trioxocarbonate(1V) 

1. hydrochloric acid 
2. ethanoic acid 
3. Which of the following in aqueous solution neutralize  litmus? 
4. NH4Cl B. Na2CO3
5. FeCl3 D. NaCl. 
6. What volume of a 0.1 M H3PO will be required to  neutralize 45.0cm3of a 0.2 M NaOH? 
7. 10.0cm3 B. 20.0cm3
8. 27.0cm3 D. 30.0cm3
9. Which of the following substances is a basic salt? A. Na2CO3 B. Mg(OH)Cl 
10. NaCHO3

placed in a test tube. On adding dilute tetraoxosulphate  (V1) acid and then K2Cr2O7solutions, a blue-black colour  was produced. In this reaction, the 

1. iodine ion isoxidized 
2. tetraoxosulphate(V1) acid acts as an oxidizing  agent 
3. starch has been oxidized 
4. K2Cr2O7 is oxidized. 

Which of the following statements isTRUE? A. The dissolution of NaOH(s) in water is  endothermic 

1. The heat of solution of NaOH(s) is positive C. The NaOH(s) gains heat from the  surroundings. 
2. The heat of solution of NaOH(s) is negative. 
3. K2SO4.Al2(SO4)3.24H2O. 
4. Which of the following acts both as reducing and an  oxidizing agent? 
5. H2 B. SO2
6. H2S D. C 
7. Which of the following reactions takes place in the  cathode compartment during the electrolysis of copper (11) chloride solution? 
8. Which of the following will produced the greatest  increase in the rate ofthe chemical reaction represented  by the equation 

Na2S2O3(aq)+2HCl(a q2NaCl(aq)+ H2O(1) + SO2(g) +S(s)? A. decrease in temperature and an in increase in the concentration of the reactants 

1. An increase in the temperature and a decrease  in the concentration of the reactants 
2. An increase in the temperature and an increase  in the concentrations of the reactants 
   
3. Cu2+(aq) + 2e Cu(s) D. A decrease in the temperature and a decrease 
   
4. 2Cl – 2e Cl2 C. Cu(s) – 2e Cu2+(aq) 

in the concentration of the reactants. 

29. Cu2+(aq) + 2Cl CuCl2(aq) 29. Which property of reversible reaction is affected by a  
    

(aq 

24. The mass of a substance, M liberated at an electrode  during electrolysis is proportional to the quantity of 

catalyst? 

1. heat content(enthalpy) B. energy of activation C. free energy change D. equilibrium position. 
   
2. Which of the following is used in fire extinguishers? A. Carbon (11) oxide 
3. Carbon (1V) oxide 
4. Sulphur (1V)oxide 
5. Ammonia 
6. When H2S gas is passed into a solution of iron (111)  chloride, the colour changes from yellow to green. This  is because. 
7. H2S is reduced to S 
8. Fe3+ ions are oxidized by H S 

2 

1. H S ions are oxidized by Fe3+

2 

1. Fe3+ ions are reduced to Fe3+ ions 

Carbon (11) oxide may be collected as shown above  because it 

1. is heavier than air 
2. is less dense than air 
3. is insoluble inwater 
4. burnsin oxygen to form carbon(1V)oxide. 
5. In the reaction C5H10O5(s) 6C(s) + 5H2O concentrated  H2SO4 is acting as 
6. a reducing agent 
7. an oxidizing agent 
8. a dehydrating agent 
9. a catalyst 
10. Suitable regents for the laboratory preparation of  nitrogen are 
11. sodium trioxonirate (lll) and ammonium  chloride 
12. sodiumtrioxonirate(V) and ammoniumchloride C. sodium chloride and ammonium trioxonirate  (V) 
13. sodium chloride andammonium trioxonirate(lll) 
14. The thermal decomposition of copper (ll) trioxonirate (V) yields copper (ll) oxide, oxygen and 
15. nitrogen (ll) oxide 
16. nitrogen(ll) oxide 
17. nitrogen (lV) oxide 
18. nitrogen 
19. Chlorine is produced commercially by 
20. electrolysis of dilute hydrochloric acid 
21. electrolysis of brine 
22. neutralization of hydrogen chlorine 
23. heating potassiumtrioxochlorate(V) 
24. Which of the following is used in the manufacture of  glass? 
25. Sodium chlorine 
26. Sodium trioxocarbonate(lV) 
27. Sodium tetraoxosulphate (Vl) 
28. Sodium trioxonirate(V) 
29. Aluminium is extracted commercially from its ore by A. heating aluminium oxidewith cokein a furnace B. the electrolysis of fused aluminium oxide in  cryolite 
30. treating cryolite with sodium hydroxide  solution under pressure 
31. heating sodium aluminium silicate to a high  temperature. 
32. Given the reactions 

(i) Fe(s)+ (NO3)2(aq) Fe(NO3)2(aq) +X(s) 

(ii) H2(g) + XO(s) X(s) + H2O(g), X islikely to be. A. copper B. zinc 

1. calcium D. lead. 
2. Crude copper can be purified by the electrolysis of  CuSO4(aq) if 
3. platinum electrodes are used 
4. the crude copper is made the anode ofthe cell C. the crude copper is made the cathode of the  cell 
5. crude copper electrodes areused. 

O 

41. The IUPACname for CH3CH2CHC 

CH3 OH 

1. 2 – methylbutanoic acid 
2. 2 – methyl – -hydrosyketone 
3. 2 – methyl – – hydroxyl baldheaded 
4. 2 – methylpentanoicacid 
5. Alkanoates are formed by the reaction of alkanoic acids  with 
6. alkyl halides B. alkanols C. ethers D. sodium 
7. The acidic hydrogen in the compound 

1 2 3 4 5 

H—C= C—CH=CH—CH3 is the hydrogen  

attached to carbon number 

1. 5 B. 4 
2. 3 D. 2 
3. The four classes of hydrocarbons are 
4. ethane, ethene ethyne and benzene 
5. alkanes, alkenesm alkynes and aromatics C. alkanes, alkenes, alkynes and benzene 
6. methane, ethane, propane and butane 
7. Alkanes 400-700oC smaller + alkanes +hydrogen. The catalyst alkanes 

above reaction is known as 

1. Photolysis B. Cracking 
2. Isomerization D. Reforming.

diastase 

47. In the reaction 2(C6H10O5) n + nH2O nC12H22O11 diastase is functioning as 
48. a dehydrating agent 
49. a reducing agent 
50. an oxidizing agent 
51. a catalyst. 
52. 48. which of the following compounds has the  highest boiling point? 
53. CH3 CH2 CH2 CH2OH 
54. CH3 CH2 CH2CHO 
55. CH3 CH2 CH2CH3
56. CH3 CH2 OCH2CH2
57. Detergents have the general formula 
58. R(CH2)NOH 
59. RSO3 Na+ 
60. RCO2 Na+ 
61. RCO2H 
62. What process would coal undergo to give coal gas,  coal tar, ammoniac liquor and coke? 
63. steam distillation 
64. Destructive distillation 
65. Liquefaction, 
66. Hydrolysis. 
    

Chemistry 1989 

1. Which of the following would support the  conclusion that a solid sample ismixture? 
2. The solid can be ground to a fine powder B. The density of the solid is 2.25 g dm3
3. The solid has a melting range of 300oC to  375oC. 
4. The solid of the moisture fromthe  

atmosphere. 

2. The molar of carbon to hydrogen of volatile liquid  compound is 1:2. 0.12 g of the liquid evaporation at s.t.p gave 32 cm3 of vapour. The molecular formula of  the liquids is 
3. The minimum volume of oxygen required for the  complete combustion of mixture of 10cm3 of CO and  15 cm3 ofH2 is 
4. 25.0 cm3

B 12.5 cm3 

C 10.0 cm3 

D 5.0 cm3 

6. What is the partial pressure of hydrogen gas  collected over water at standard atmospheric  

pressure and 25oC if the saturation vapour pressure  of water is 23 mm Hg at that temperature?. 

1. C H B. C H A. 737mmHg B. 763 mmHg 3 6 4 8 

C C H D. C H C. 777mmHg D. 737 mmHg 5 10 6 12 

[ G.M.V = 22.4 DM3, C=12, H=1] 

7. The atomic radius Li, Na and K are 1:33 Am 1.54Aand  

1.96A respectively. Which of the following explain this  

gradation in atomic radius? 

1. Electropositivity decreasesfrom Li to Na to K 
2. Electronegativity decreases from Li to Na to  
4. The number of electron shells increase from  

Li to Ma toK 

1. The elements are in the same period. 

It can be deduced from the vapour of pressure curves  

above that. 

1. liquid has the highest boiling point 
2. liquid has the highest boiling point 
3. liquid lll has the highest boiling point 
4. liquid lll has the lowest boiling point. 
   
5. 20.00 cm3 of a solution containing 0.53 g of  anhydrous Na2CO3 in 100 cm3 requires 25.00 cm3 of  H SO for complete neutralization. The concentration 

2 4 

of the acid solution in moles per dm3 is 

1. 0.02 B 0.04 

C 0.06 D. 0.08 

[ H= 1, C = 12, 0 = 16, Na = 23 , S =32] 

Which of the curves in the above graph illustrates the behaviors of an ideal gas? 

1. W B. X 
2. Y D. Z
3. Elements X and Y have electronic configurations  1s22s22p4and 1s22s22p63s23p1respectively. When they  combine, the formula of the compound formed is 
4. A hydrated salt of formula MSO4.XH2O contains 45.3%  by mass of thewater of crystallization. 

Calculate the value of X. 

1. XY B. YX A. 3 B. 5 C. X2Y3D. Y2X3C. 7 D. 10[M= 56, S= 32, O =16, H= 1] 
2. The atomic number of cesium is 55 and its atomic mass 

is 133. The nucleus of cesium atom therefore contains 17 

1. 78 protons and 55 electrons 
2. 55 protons and 78 neutrons 
3. 55 neutrons and 78 electrons 
4. 78 neutron and 55 neutrons 
5. Four elements P,Q,R and S have atomic numbers of 4,  

10, 12, and 14 respectively. Which of these elements is  

a noble gas? 

1. P B. Q 
2. R D. S 
   
3. How many valence electrons are contained in the  element represented by 31 P? 

15 

If the graph above 1 dm3 of a saturated solution of HCI  is cooled from 80oC, the mass of crystals deposited will 

1. 3 B. 5 be. 
2. 15 D. 31 A. 7.45 g B. 14.90 g C. 74.50 g D. 149.00 g 
3. [K= 39,Cl= 35.5] 
4. Using 50cm3 of 1 M potassium hydroxide and 100cm3  

of 1M tetraoxosulphate(Vl) acid, calculate the respective  

volumes in cm3 of bade and acid 100 cm3 of base and  

acid that would be required to produce the maximum  

amount of potassium tetraoxosulphate(Vl) 

1. 50,50 B. 25,50 
2. 50,25 D. 25,25 

[K = 39, S= 32, O = 16, H = 1] 

19. A solution of calcium bromide contains 20 g dm3

What is the molarity of the solution with respect to  

calcium bromide and bromide ions? 

In the above set up, substances X and Y are  

respectively. 

1. Lime water and copper (ll)tetraoxosulphate  (Vl) 
2. Potassium trioxocarbonate(lV) and alkaline  prygallol 
3. Potassium hydroxide and alkaline pyrogallo D. Potassium trioxocarbonate (lV) and  concerntrate tetraoxosulphate (Vl)aid 
4. The gaseous pollutant sulphur (lV) oxide is most likely  to be detected in fairly reasonable quantities in the  area around a plant for the 
5. extraction of aluminium from bauxite 
6. production ofmargarine 
7. smelting of copper 
8. production of chlorine from brine 
9. Calcium hydroxide is added in the treatment of town  water supply to 
10. kill bacteria in the water 
11. facilitate coagulation of organicparticles C. facilitate sedimentation 
12. improve the tase of thewater. 
13. 0.1,0.1 B. 0.1,0.2 
14. 0.1,0.05 D. 0.05,0.1 

[Ca = 40, Br = 80] 

20. The substance of ZnO dissolves in sodium hydroxide  solution and mineral acid solution to gives soluble  products in each case. ZnO is therefore referred to as. A. an allotropic acid 
21. an atmophericoxide 
22. a peroxide 
23. a dioxide. 
24. An acid its conjugate base . 
25. can neutralize each other toform a salt 
26. differ only by a proton 
27. differ only by the opposite charges they carry D. are always neutral substances 
28. The same current is passed for the same time through  solutions of AgNO3 and CuSO4 connected in series.  How much silver will be deposited if 1.0 g of copper is  produced? 
29. 1.7 g B. 3.4 g 
30. 6.8 g D. 13. 6 g  

[Cu = 63.5, S = 32, O = 16MAg = 108, N = 14] 

23. What is discharged at the cathode during the  electrolysis of copper (ll) tetraoxosulphate (Vl)solution? A. Cu2+ only B. H+ only 
24. Cu and H+ D. Cu2+ and SO2- 2+ 
25. An element, Z forms an anion whose formula is  [Z(CN) ]y. If has an oxidation number of +2, what isthe  6 

value of y? 

1. -2 B. 3 

and –396 kJ respectively. Calculate the molar heat of  formation of ethane in kJ. 

1. -2792 B. +2792 
2. –64 D. +64 
3. CO(g) + H2O CO2(g) + H2(g) H = -41000 J.Which of the following factors favour the formation of hydrogen in the above reaction? I high pressure II low  pressure III high temperature IV use of excess steam 
   
4. –4 D. –5 A. I, III, and IV B. III only C. II, III and I D. Iv only. 
5. Which of the reaction is NOT an example of a redox  
   

reaction? 

I Fe + 2Ag+ Fe2+ + 2Ag+  

II 2H2S + SO22H2O + 3S  

III N2+ O22NO 

IV CaCO3 CaO +CO2 

1. I, II, III B. II and III C. III and IV D. IV only.

The above graph shows a typical heating curve from  the solid phase through the liquid phase to the gaseous  phase of a substance . What part of the curve shows  solid and liquid in equilibrium? 

1. T B. U 
2. X D. Y 
3. Which of the following represents the balanced  equation for the reaction of copper with concentrated  trioxonirate (V)acid? 
   
5. B. 
6. D. 

2NHO3(aq) Cu(NO3)2(aq) + H2(g) 

Cu(s) + 4HNO3 Cu(NO3)2(aq) + 2H2O(l) +  2NO2(g) 

3Cu(s) + 8HNO3(aq) 3Cu(NO3)2(aq) + 4H2O(l) + 2NO(g) 

3Cu(s) + 4 HNO3(aq 3Cu(NO3)2(aq) + 2H2O(l)+ 2NO(g). 

31. The catalyst used in the contact process for the 

manufacture of tetraoxosulphate(Vl) acid is 

1. Manganese (lV) oxide 

The above diagram gives the potential energy profile B. Manganese (ll) tetraoxosulphate (lV) of the catalyzed uncatalysed reactions of C. Vanadium (V)oxide 

X(g) + Y(g) XY(g) . Deduce the respective D. Iron metal 

activation energies in kJ of the catalyzed and 

uncatalysed reverse reactions. 32. Some products of destructive distillation of coal are XY(g) + X(g) X(g) + Y(g) A. carbon (iV) oxide and ethanoic acid A. 300,500 B. 500,300 B. trioxocarbonate (lV) acid and methanoic acid C. –300,-500 D. –5000. C. producer gas and water gas D. coke and ammonialiquor 

27. The combustion of ethene, C2H2, is given by the equation 
    

C2H42CO2+ 2H2O; H = -1428 kJ. Ifthe molar heats of formation of water and carbon (l) oxide are –286kJ 

33. Gunpowder is made from charcoal, sulphur and potassium trioxonirate (V). The salt in the mixture performs the function of 
34. an oxidant B. a reductant C. a solvent D. a catalyst 
35. Which of the followingreaction is (are) feasible?  l Br (2l) + 2Cl(aq 2Br(aq) + Cl2(aq

) ll 21(aq) + Br2(1) 2Br(aq) + l2(s) 

lll 2F(aq) + Cl2(aq 2Cl(aq) + F2(g)  

lV 2F(ag) + Br2(1) 2Br(aq) + F2(g) 

A l B. ll 

C I and lll D. lll andlV 

35. Bleaching powder, CaOCl2.H2O, deteriorates on exposure to air because 
36. it loses its water ofcrystallization 
37. atmospheric nitrogen displaces chlorine from it 
38. carbon (lV) oxide ofthe atmosphere displaces  chlorine fromit 
39. bleaching agents should be stored insolution 
40. The product ofthe thermal decomposition of ammonium  trioxonirate (V)are. 
41. NO2 and oxygen 
42. NH3 and oxygen 
43. nitrogen and water 
44. N2O andwater. 
45. The scale of a chemical balance is made of iron plate  and coated with copper electrolytically because. A. iron is less susceptible to corrosion than  copper 
46. copper is less susceptible corrosion as ion C. copper is less susceptible to corrosion than  ion 
47. copper and ion are equally susceptible to  corrosion. 
48. Ametal is extracted for, its ore by the electrolysis oftits  molten chlorine and it displace lead from lead (ll) 
49. When excess chlorine is mixed with ethene at room  temperature, the product is 
50. 1,2 – dichloroethane 
51. 1,2 – dichloroethene 
52. 1, 1- dichloroethane 
53. 1, 1-dichloroethene. 
54. Vulcanization of rubber is a process by which A. Isoprene units are joined to produce rubber B. Rubber latex is coagulated 
55. Sulphur is chemically combined in the rubber D. Water is removed from therubber. 
56. The reaction between ethanoic acid and sodium  hydroxide is an example of 
57. esterification B. neutralization C. hydrosylation D. hydrolysis 
58. The bond which joins two ethanoic acid molecules in  the liquid state is 
59. a covalent bond 
60. an ionic bond 
61. a dative covalent bond 
62. a hydrogen bond 
63. The alkaline hydrolysis of fats and oils produces soap  and 
64. propane 1, 1, 3-triol 
65. propane – 1, 3, 3-triol 
66. propane-1-2-2-triol 
67. propane-1-2-3-triol 
68. which of the following is NOT amonomer?  A.
    

trioxonirate(V) solution. The metal is B. CH2 = CH2 A. copper B. aluminium 

1. zinc D. sodiumD. CH2 = CHCl 
2. Mortar is NOT used for under-water construction  

because. 

1. It hardens by loss of water 
   
2. Its hardening does not depent upon  evaporation 
3. It requires concrete to harden 
4. It will be washed away by the flow of water. 40. Which of the following is NOT involved in the  extraction ofmetals from their ores? 
5. reduction with carbon 
6. reduction with other metals 
7. reduction by electrolysis 
8. oxidation with oxidizingagent. 

41 Which ofthe following compounds is an isomer of the  compound. 

1. CH-CH2-CH-CH2-CH3 B. CH-CH2-CH-CH2-CH3 CH3 C2H5
2. CH-CH2-CH-CH3 D. CH3-CH-CH2-CH3 C2H5 CH3
3. What is the IUPAC name for the compound CH3

CH2 = C 

CH2CI 

1. 1-chloro-2-methylprop-2, 3-ene 
2. 1-chloro-2-methlprop-2-ene 
3. 3-chloro-2-methylprop-1-ene 
4. 3-chloro-2-methyprop-1,2-ene 
5. The gas responsible for most of the fatal explosion in  coal minesis 
6. butane B. ethene C. ethane D. methane
   
7. Three liquids X,Y and Z containing only hydrogen and  

carbon were burnt on a spoon, X and Y burnt with sooty flames  

while Z did not. Y is able to discharge the colour of bromine  

water whereas X and Z cannot. Which of the liquids would be  

aromatic in nature? 

1. X and Z B. Y 
2. X D. Z 

Chemistry 1990 

[G.M.V at s.t.p = 22.40 dm3] 

1. Which of the following is a physical change? 
2. The bubbling of chlorine into water 
3. The bubbling of chlorine into jar containing  hydrogen 
4. The dissolution of sodium chlorine inwater D. The passing of steam over heated iron. 
5. Changes in the physical states of chemical substances  T are shown in the schemebelow. 

Liquid T 

7. Equal volumes of CO, SO2 NO2 and H2S, were released  into a room at the same point and time. Which of the  following gives the order of the room? 
8. CO2, SO2,NO, H2S, 
9. SO2,NO2,H2S,CO 
10. CO, H2S, SO2,NO2
11. CO, H2S, NO2,SO2

[S = 32, C=12, 0=16, N = 14, H =1] 

8. A basic postulate of the kinetic theory of gases is that  the molecules of a gas move in straight lines between  collisions. This impliesthat. 

Z 

Y 

1. collisions are perfectlyelastics 

Solid T X Gaseous T  

The letters X, Y and Z respectivelyrepresent 

1. sublimation, condensation and freezing 
2. sublimation, vaporization andsolidification 
3. freezing, condensation and sublimation 
5. evaporation, liquefaction and sublimation. 
6. In the reaction: SnO2 + 2C Sn + 2CO the mass of coke containing 80% carbon required to reduce 0.032 kg of  pure tin oxideis 
7. 0.40kg B. 0.20kg 
8. 0.06kg D. 0.40g 

[Sn = 119, O = 16, C = 12] 

4. TheAvogadro’s number of 24 of magnesium issame as  
5. forces of repulsion exist 
6. forces of repulsion and attraction are in  equilibrium 
7. collisions are inelastic. 

	P	Q	R	S
Proton  Electron  Neutron	13  13  14	16  16  16	17  17  35	19  19  20

 

Which of the four atoms P,Q,R and S in the above data  can be described by the following properties: relative  atomic mass is greater than 30 but less than 40 ; it has  an odd atomic number and forms a unipositive ion in  solution? 

1. P B. Q 
2. R D. S 

that of 

1. 1 g of hydrogen molecules 
2. 16 g of oxygenmolecules 
3. 32 g of oxygenmolecules 
4. 35.5 of chlorinemolecules. 
5. If a gas occupies a container of volume 146 cm3 at 18oC  and 0.971 atm, its volume on cm3 at s.t.p is 
6. 133 B. 146 
7. 266 D. 292 
8. The volume occupied by 1.58 g of gas s.t.p is 500 cm3.  What is the relative molecule mass of thegas? 
9. 28 B. 32 
10. 344 D. 71
11. Which of the following terms indicates the number of  bonds that can be formed by atom? 
12. Oxidation number 
13. Valence 
14. Atomic number 
15. Electronegativity. 
16. X(g) X(g). The type of energy involved in the above transformation is 
17. ionization energy 
18. sublimation energy 
19. lattice energy 
20. electron affinity 
21. Chlorine, consisting of two isotope of mass numbers  35 and 37, has an atomic of 35.5. The relative abundance  of the isotope of mass number 37 is. 
22. What is concentration of H+ions in moles per dm3 of a  solution of pH4.398? 
23. 4.0x 10-5 B. 0.4 x10-5
    
24. 20 B. 25 C. 4.0 x 10-3 D. 0.4x 10-3 C. 50 D. 75 
    
25. 10.0 dm3 of air containing H S as an Impuritywas passed  2 

through a solution of Pb(NO3)2 until all the H2S had  reacted. The precipitate of PbS was found weight 5.02 g. According to the equation: Pb(NO3)2 + H2O ’! PbS  “!+2HNO3 the percentage by volume of hydrogen  sulphides in the air is. 

50. 50.2 B. 47.0 
51. 4.70 D. 0.47 

[Pb = 207, S = 23, GMV ats.t.p = 22.4 dm3] 

14. A blue solid, T, which weighted 5.0 g was placed on a  table. After 8 hours, theresulting pink sold was found  to weight 5.5 g. It can be inferred that substance T A. is deliquescent 
15. is hydroscopic 
16. hassome molecules ofwater of crystallization D. is efflorescent 
17. The effluent of an industrial plant used ins the  electrolysis of concentrated brine, with a flowing  mercury cathode may contain impuritieslike. 
18. oxygen 
19. hydrogen 
20. mercury (ll)chloride 
21. hydrogen chloride 
22. What volumeof 11.0 M hydrochloric acid must be dilute  to obtain 1 dm3 of 0.05 M acid? 
23. 0.05dm3 B. 0.10 dm3 C. 0.55dm3 D. 11.0 dm3
24. If 10.8 g of silver is deposited in a silver coulometer  connected in series with a copper coulometer, the  volume of oxygen liberated is 
25. 0.56dm3 B. 5.50 dm3 C. 11.20dm3 D. 2 2 . 4 0 dm3

[Ag = 108, Cu = 64, GMV at s.t.p = 22.40 dm3]. 

23. 0.1 faraday of electricity deposited 2.95 g of nickel  during electrolysis is an aqueous solution. Calculate  the number of moles of nickel that will Be deposited by 0.4 faraday 
24. 0.20 B. 0.30 
25. 0.034 D. 5.87 

[Ni = 58.7] 

24. Cr2O 2- + 6Fe2+ + 14H+ 2Cr3+ + 6Fe3+ + 7H O.In the 7 2 

above chromium change from. 

1. +7 to +3 B. +6 to +3 C. +5 to +3 D. –2 to+3 
   
2. In the reaction 10– + 51– + 6H+ 31 

+ 3H2O, the 

16. The solubility in moles per dm3 of 20 g of CuSO  

3 

2 

oxidizing agent is 

4 

dissolved in 100 g of water at 180oC is 

1. 0.13 B. 0.25 
2. H+ B. 1–
   
3. 1.25 D. 2.00C. 10– D. 12

3

[Cu = 63.5, S = 32, O = 16] 26. Fe O + 2Al Al O +2Fe are –1670 kJ mol-1 and 2 3(s) 2 3 (s) 

17. Smoke consists of 
18. solid particles dispersed inliquid 
19. solid or liquid particles dispersed in gas C. gas or liquid particles dispersed in liquid D. liquid particles dispersed inliquid. 
20. NaC2O4 + CaCl CaC2O4 + 2NaCl. Given a solution  of 1.9 g of sodium oxalate in 50 g of water at room  temperature, calculate the minimum volume of 0.1 M  calcium oxalate required to produce maximum calcium  oxalate using the above equation. 
21. 1.40x 102 dm3
22. 1.40x 102cm3
23. 1.40x 10-2 dm3
24. 1.40x 10-2cm3

–822kJ mol-1 respectively, the enthalpy change in kJ  for the reason is 

1. +2492 B. +848 C. –848 D. 2492 
2. Iron galvanized with zinc catholically protected from  corrosion. This is because 
3. zinc has a more positive oxidation potential than  iron 
4. zinc has a less positive oxidation potential than  iron 
5. both have the sameoxidation potential 
6. zinc is harder than iron. 
7. Which of the following samples will react faster with  dilute dtrioxonitrate (V) acid? 
   
8. 5 g of lumps of CaCO at25oC 19. 2.0 g of monobasic acid was made up to 250 cm3 with B. o

3 

distilled water. 25.00 cm3 ofthissolution required 20.005 g of powered CaCO3 at 25C C. 5 g of lumps of CaCO at 50oC cm3 of 0.1 M NaOH solution for completeneutralization. D. o 3 

The molar mass of the acid is 

1. 200 g B. 160 g 

5 g of powered CaCO3 at 50C 

29. In the reaction , 
    
30. 100 g D. 50 g 2Hl(g)H2(g)+ I2(g), H = 10 kJ; the concentration of iodine in the equilibrium mixture  

can be increased by 

1. raising the pressure 
   
2. raising the temperature 
3. adding the temperature 
4. lowering the pressure 
5. Which of the following gases can be collected by  upward displacement of air? 
6. NO B. H2
7. NH3 D. Cl2
8. The brown fumes given off when trioxonirate(V) acid  consist of 
9. NO2and O2 B. H2O and NO2 C. NO2, O2 andH2O D. NO2 and H2O 
10. Which of the following tests will completely identify  any one of sulphur (lV) oxide, hydrogen, carbon (lV)  oxide and nitrogen (ll) oxixde? 
11. pass each gas into water and test with blue  litmus pare 
12. pass each gas into limewater 
13. expose each gas to atmospheric air 
14. passs each gas to concentrated  tetraoxosulphate(Vl) acid. 
15. In the Haber process for the manufacture of ammonia,  the catalyst commonly used is finely divided. 
16. vanadium B. platinum C. iron D. copper 
17. A metallic oxide which reacts with both HCl and NaOH  to give salt and water only can be classified as 
18. an acidic oxide 
19. an atmospheric oxide 
20. a neutral oxide 
21. an atmospheric oxide 
22. Which of the following metals will liberate hydrogen  form steam or diluteacid? 
23. copper B. iron 
24. lead D. mercury 
25. Coal fire should not be used in poorly ventilated rooms  because 
26. of theaccumulation of CO2 which cause deep  sleep 
27. it is usually too hot 
28. of the accumulation of CO which causes  suffocation 
29. it removes most of the gases in the room 
30. The major component of the slag from the production  of iron is 
31. an alloy of calcium and iron 
32. coke 
33. impure ion 
34. calcium trioxosilicate(V) 
35. Sodium hydroxide should be stored in properlyclosed  containers because it 
36. readily absorbs water vapour from the air B. is easily oxidized by atmospheric oxygen C. turns golden yellow when exposed to light. D. Melts at a low temperature. 
37. To make coloured glasses, small quantities of oxides of  metals which form coloured silicates are often added to  the reaction mixture consisting of Na2CO3and SO2. Such  a metal is 
38. potassium B. barium C. zinc D. copper 
39. Which of the following compounds gives a yellow  residue when heated and also reacts with aqueous  sodium hydroxide to give a white gelatinous precipitate  soluble in excess sodium hydroxide solution. 
40. (NH4)2CO3 B. ZnCO3 C. Al2(SO4)3 D. PbCO3
41. A cycloalkane with molecular formula C5H10 has A. one isomer B. two isomers C. three isomers D. four isomers 
42. The structure of cis-2butene is 
43. CH3-CH=CH-CH3

– 

43. What is the IUPAC name for the hydrocarbon CH3

CH3—C = CH— CH—CH3 

CH2 

CH3 

1. 2-ethyl-4-methylpent-2-ene 
2. 3,5-dimenthylhex-3-ene 
3. 2,4-dimenthylhex-3-ene 
4. 2-methyl-4-ethylpent-3-ene 
5. CH3= CH P. Compound P, in the above reaction,is. A. CH— C = CH NH2

NH2 

1. CH3 — C CHNa 
2. CH3 — C C — Na 
3. CH3 — CC — NH2
4. The label on a reagent bottle containing a clear organic  liquid dropped off. The liquid was neutral to litmus and  gave a colourless gas with metallic sodium. The liquid  must be an 
5. alkanoate B. alkene C. alkanol D. alkane
6. COOH COOH + H2O + NaOH

COOH COO-Na+ 

The above reaction is an example of 

1. displacement reaction 
2. a neutralization reaction 
3. an elimination reaction 
4. Saponification 
5. Alkanoic acids have low volatility compared with Alkanoic because they 
6. are morepolar than alkanols 

B have two oxygen atoms while alkanols have one 

50. Which of the following compounds represents the polymerization product of ethyne? 

A.. 

1. form two hydrogen bonds while alkanols B. 

donot 

1. form two hydrogen bondswhile alkanolsform 

one.

48. The octane number of a fuel whose performance is the 

same as that of a mixture of 55 g of 2, 2, 4-trimethyl C.  

pentane and 45 g of n-heptanes is 

1. 45 B. 55 
2. 80 D. 100 
3. Which of the following isformed when maltose reacts  with concentrated tetraoxosulphate (Vl)acid. 
4. Carbon (lV) oxixde D. 
5. Coaltar 
6. Charcoal 
7. Toxic fumes 

Chemistry 1991 

1. Which of the following can be obtained by fraction of  distillation? 
2. Nitrogen from liquidair 
3. Sodium chloride for seawater 
4. Iodine from a solution of iodine in carbon  tetrachloride 
5. Sulphur from a solution of sulphur in carbon  disulphide. 
6. Which ofthe following aremixture? I Petroleumii Rubber  latex. Iii Vulcanizes’solution. Iv Carbon (ll)sulphides A. I, ii and iii 
7. I, ii and iv 
8. I and iionly 
9. I and iv 
10. Anironoreisknowntocontain70.0%FeO . The mass 
11. In two separate experiments 0.36 g and 0.71 g of chlorine  combine with a metal X to give Y and Z respectively.  An analysis showed that Y and Z contain 0.20 g and 0.40 g of X respectively. The data above represents the  law of. 
12. multiple proportion 
13. conversation ofmass 
14. constant composition 
15. reciprocal proportion. 
16. 30cm3 of oxygen at 10 atmosphere pressure is placed in  a 20 dm3container. Calculate the new pressure it  temperature is kept constant. 
17. 6.7 atm B. 15.0atm 
18. 6.0atm D. 66.0atm 

3 

2 3 6. A given quantity of gas occupies a volume of 228cm 

of iron metal which can theorically be obtained from  80kg of the ore is. 

35. 35.0kg B. 39.2 kg C. 70.0kg D. 78.4 kg [Fe = 356, O = 16] 

at a pressure of 750 mm Hg. What will be its volume at  atmospheric pressure? 

1. 200cm3 B. 225 cm3 C. 230 cm3 D. 235 cm3
2. Calculate the volume of carbon (lv) oxide measure at s.t.p,  produced when 1 kg of potassium hydrogen  trioxocarbonate (iV) istotally decomposed by heat. A. 28dm3 B. 56dm3
3. 112dm3 D. 196dm3

[G.M.Vats.t.p = 22.4 dm3, K = 39, O = 16, C= 12, H= 1] 

8. A sample of a gas exerts a pressure of 8.2 atm when  confined in a 2.93dm3container at 20oC. The number of  moles of gas in the sampleis 
9. 1.00 B. 2.00 
10. 3.00 D. 4.00 

[ R= 0.082 litre atm/deg mole] 

9. Atoms of element X (with 2 electronsin the outer shell)  combine with atoms of Y( with 7 electrons in the outer  shell). Which of the following is FALSE?The compound  formed 
10. has formulaXY 
11. is likely to be ionic 
12. contains X2+ ions 
13. contains Y ions 
14. The ions X and Y+are isoelectronic, each containing a  total of 10 electrons. How many proteins are in the  nuclei of the neutral atoms of X and Y respectively? A. 10 and 10 B. 9 and 9 C. 11 and 9 D. 9 and11 
15. The electronic configuration of an element is 1s2 2s22p6 3s2 3p3. How many unpaired electron are there in the  element. 
16. 5 B. 4 
17. 3 D. 2 
18. Which of the following represents thetype of bonding  present in ammonium chloride molecule? 
19. Ionic only 
20. Covalent only 
21. Ionic and dative covalent 
22. Dative covalent only. 
23. Which ofthe following is arranged in order ofincreasing  electronegativity? 
24. Chlorine, aluminium, magnesium, phosphorus,  sodium. 
25. Sodium, magnesium, aluminium phosphorus,  chlorine 
26. Chlorine, phosphorus, aluminium, magnesium,  sodium. 
27. Sodium, chlorine, phosphorus, magnesium,  aluminium. 
28. A quantity of air was passed through a weighed mount  of alkaline pyrogallol. An increase in the weight of the  pyrogallol would result from the absorption of. 
29. nitrogen B. neon 
30. argon D. oxygen. 

The electrons of two atoms of Y and Z are arranged in  shells as shown above. The bond formed between the  atoms of Y and Z is 

1. ionic 
2. covalent 
3. dative 
4. metallic. 
5. Which of the following ionsis a pollutant in drinking  water even in trace amount? 
6. Ca2+
7. Hg2+
8. Mg2+
9. Fe2+
10. The solubility of copper (ll) tetraoxosulphate (Vl) is 75  g in 100 g ofwater at 100oC and 25 g in 100 g ofwater at  30oC.What mass ofthe salt would crystallize, if 50 g of  copper (ll) tetraoxosulphate (Vl) solution saturated at  100oC were cooled to 30oC? 
11. 57.5g B. 42.9 g 
12. 28.6g D. 14.3 g 
13. A sample of temporary hard water can be prepared in  the laboratory by. 
14. dissolving calcium chloride in distilled water B. saturating lime water with carbon(lV) oxide C. saturating distilled water with calcium  hydroxide 
15. dissolving sodium hydrogen trioxocarbonate  (lV)in some distilled water. 
16. A property of a colloidal dispersion which a solution  does not have is . 
17. the Tyndall effect 
18. homogeneity 
19. osmotic pressure 
20. surface polarity. 
21. 50 cm3 ofsulphur (lV) oxide, 800cm3 of ammonia, 450  cm3 of hydrogen chloride, 1.0 cm3 of water at 15oC.  Which of the following is suitable for demonstrating  the fountain experiment? 
22. Sulphur (lV) oxide and hydrogen chloride B. Carbon (lV) oxide and ammonia 
23. Ammonia and hydrogen chloride 
24. Carbon (lV) oxide and sulphur (1V) oxide
    
25. C. lower the activation energy for the reaction D. lower the heat of reaction, H, for the reaction, 
26. 1.1 g of CaCl dissolved in 50 cm3 of water caused a rise  

2 

in temperature of 34oC. The heat reaction, H for CaCl 2 

in kJ per moles is 

71. -71.1 B. –4.18 
72. +17.1 D. +111.0 

[Ca = 40, Cl = 35.5, specific heat of water is 4.18 KJ-1 

29. NO + CO 1/2 N2 + CO2 H = -89.3kJ 

.What conditions would favour maximum conversion  

Which of the following substances could be  

satisfactorily used as X in the above figure? 

1. Ammonia and Potassiumhydroxide 
2. Potassium hydroxide and sodiumchloride C. Ammonia and ethanoicacid 
3. Ethanoic and sodiumchloride 
4. What volume of CO2 at s.t.p would be obtained by  reacting 10cm3 of 0.1 M solution of anhydrous sodium  trioxocarbonate (lV) with excess acid? 
5. 2.240cm3 B. 22.40cm3 C. 224.0cm3 D. 2240 cm3 [G.M.V at s.t.p = 22.4 dm3
6. If a current of 1.5 A is passed for 4.00 hours through a  

of nitrogen (ll) oxide and carbon(ll) oxide in the reaction  above? 

1. low temperature and high pressure 
2. high temperature and low pressure 
3. high temperature and high pressure 
4. low temperature and lowpressure. 
5. Which of the following equilibria is unaffected by a  pressure change? 
6. 2NaCl 2Na + Cl2
7. H2+ I22HI 
8. 2O33O2
9. 2NO2 N2O4

molten tin salt and 13.3 g of tins is deposited, What is  the oxidation state of the metal in thesalt? A. 1 B. 2 

Initial concentration of no in molesInitial Rate (moles / sec)
0.001  0.002	3.0 x 10-5  1.2 x 10 -4

 

 

1. 3 D. 4 

[Sn = 118.7, F = 96500 C mol-1] 

24. Which of the following equivocal solutions, Na2CO3,  Na2SO4, FeCl3, NH4Cl and CH3 COONa, have pH greater  than? 
25. FeCl3 and NH4Cl 
26. Na2CO3 CH3 COONa andNa2SO4, 
27. Na2CO3 and CH3COONa 
28. FeCl3 , CH3, COONa.NH4Cl 
29. MnO– + 8H+ + ne M++ + 4H O. Which is the value  4 2 

of n the reaction above? 

1. 2 B. 3 
2. 4 D. 5 
3. 2H2(g) + SO2(g) 3S(s) + 2H2O(1). The above reaction is A. a redox reaction in which H2S is the oxidant and  SO2 is the reductant. 
4. a redox reaction in which SO2is the oxidant and H2S is the reductant. 
5. Not a redox reaction because there is no oxidant in the reaction equation 
6. Not a redox reaction because there is no reductant  in the reaction equation. 
7. Manganese(lV) oxide is known to hasten the  decomposition of hydrogen peroxide. Its main actions  is to. 
8. increase the surface area of the reactants B. increase the concentration of the reactants 

The data in the table above shows the rate of reaction of nitrogen  (ll) oxide with chlorine at 25oC. It can be concluded that doubling  the intial concentration of NO increase the rate of reaction by  factor of 

1. two B. three 
2. four D. five 
3. Which of the following gases will rekindle a brightly  glowing splint? 
4. NO2 B. NO 
5. N2O D. Cl2
6. Which of the following salts can be melted without  decomposition? 
7. Na2CO3 B. CaCO3
8. MgCO3 D. ZnCO3
9. Oxygen gas can be prepared by heating A. ammonium trioxonirate (V) 
10. ammonium trioxonirate (lll) 
11. potassium trioxonirate (V) 
12. manganese (lV)oxide.

The appropriate test paper to use in the above 

42. The final products of the presence of ultraviolet light  are hydrogen chloride and 
43. chloromethane 
44. tetrachloromethane 
45. trichloromethane 
46. dichloromethane 
47. How many grams of bromine will be required to  completely react with 10 g of propyne? 
48. 20 g B. 40 g 
49. 60 g D. 80 g 

[C = 12, H = 1, Br = 80]. 

44. Ethene when passed into concentrated H SO israpidly experimentismoist. 24 
    
45. litmus paper 
46. potassium heptaoxodichromate (1V)  

paper 

1. lead (11)trioxonirate (V) paper. 
2. Universal indicator paper. 
3. Addition of aqueous ammonia to a solution of Zn++ gives a white precipitate which dissolves in an excess  of ammonia because. 
4. zinc isamphoteric 
5. zinc hydroxide is readily soluble 
6. zinc forms a complex which is readily  soluble in excessammonia 
7. ammonia solution is a strong base. 
8. Which ofthe following, in clear solution, forms a white  precipitate when carbon(1V) oxide is bubbled into it for  a short time? 
9. KOH B. NaOH 
10. Ca(OH)2D. Al(OH)3
11. Copper (11) tetraoxosulphate (V1) is widely used as a A. Fertilizer B. Fungicide 
12. Disinfectant D. Purifier 
13. Which of the following metals can be prepared in  samples by the thermal decomposition to their  trioxonirate (V)salt? 
14. Copper and mercury 
15. Silver and copper 
16. Mercury and silver 
17. Magnesium and mercury 
18. Which of the following compounds can exist as  geometric isomers? 
19. 2-methylbut2-ene 
20. But-2-ene 
21. But-1-ene 
22. H 

Cl — C—Br  

H 

41. How many structural isomers can be written for the  alkyl bromideC2H9Br? 
42. 3 B. 4 
43. 6 D. 8

absorbed. The product is diluted with water and then  warmed to produce. 

1. ethanol B. diethyl ether C. ethanal D. diethyl sulphate. 
2. One of the advantages of detergents over soap is that  detergents. 
3. are easier tomanufacture 
4. foam more than soap 
5. form soluble salts with hard water 
6. are able to deter germ more than soap. 
7. CH3CH2CHCH3alc.KOH CH3CH = CHCH3 X CHCH + CH CH CH =CH 

3 3 2 2 

The above reaction is an example of 

1. dehydration 
2. dehydrohalogenation 
3. neutralization 
4. a fission reaction 
5. A certain liquid has a high boiling point. It is viscous,  non-toxic, miscible with water to be hygroscopic. This  liquid is most likely to be. 
6. CH3CH2CH2CH2OH 
7. CH3CH2OHCH3
8. CH3CH2CHOHCH3
9. CH3OHCHOCH2 OH 
10. The compound. 

CH3¯CH¯CH3 

sCH2Cl  

Is known as 

1. 1-chloro-2-methylbutane 
2. 1-chloro-2-methylpronane 
3. 2-chloromethylethane 
4. 1-chloro-2,2-dimethylethane 
5. Which of the following statements is TRUE of the  complete hydrolysis of a glyceride by sodium  hydroxide? 
6. 3 moles of NaOH are required for each mole of  glyceride 
7. 3 moles of glycerol areproduced 
8. onlyone mole of soap is formed. 
9. Concentrated H2SO4 is essential for the completion of the reaction. 
   
10. Which of the following are the products of the reaction  

between CH3COOH and Cl2 in sunlight? 

1. ClCH2COOH+ HCl 
2. CH3COCl + HOCl 
3. CH3COOCl + HCl 
4. CH3COCl +H2O 

Chemistry 1992 

1. Which of the following substances is not a  homogeneous mixture? 
2. Filtered sea water 
3. Soft drink 
4. Flood water 
5. Writing ink 
6. There is a large temperature interval between themelting  point and the boiling point of a metalbecause. 
7. metals have very high melting points 
8. metals conduct heat very rapidly 
9. melting does not break the metallic bond but  boiling does. 
10. The nucleus of the isotope tritium, contains A. two neutrons with no protons 
11. one neutron and one proton 
12. two neutron and one electron 
13. two neutron, one proton, and one electron. 
14. Howmany lone pairs of electron are there on the central  atom of the H2Omolecules? 

A.1 

1. 2 
2. 3 
3. 4 
4. 14 N + X 17 O + 1 H . In the above reaction ,  
   
5. the crystal lattice of metals is easily broken. 

X is a 

8 1 

3. Howmanymoles of[H+] are there in 1 dm3 of 0.5 solution  of H SO 

2 4 

2. 2.0 moles B. 1.0mole C. 0.5mole D. 0.25mole 
3. wH2SO4 + xA(OH)3yH2O + zAl2(SO4)3. The  respective values of w, x, y and z in the equation above  are 
4. 2,2,5 and 1 B. 3,2,5and 2 
5. 3,2,6 and 1 D. 2,2,6 and 2 
6. A given mass of gas occupies 2 dm3at 300 K. At what 

temperature will its volume be doubled keeping the  pressure constant? 

1. 400K B. 480K 
2. 550K D. 600K 
3. If 100 cm3 of oxygen pass through a porous plug is 50  seconds, the time taken for the same volume of  hydrogen to pass through the same porous plug is  A. 10.0 s B. 12.5 s 
4. 17.7 s D. 32.0 s  

[ O = 16, H = 1] 

7. Which of the following is a measure of the average  kinetic energy of the molecules of a substance. 
8. Volume B. Mass 
9. Pressure D. Temperature 

8 An increase in temperature causes an increase in the  pressure of a gasin a fixed volume due to an increase in  the 

1. number of molecules of the gas 
2. density of the gas molecules 

C number of collisions between the gas 

1. number of collision between the gasmolecules  and the walls of thecontainer. 
2. neutron, B. Heliumatom 
3. Lithium atom D. Deutriumatom 
4. Four elements P,Q,R and S have 1,2,3 and 7 electrons  in their outermost shells respectively. The element which is  unlikely to be a metal is 
5. P B. Q 
6. R D. S 
7. The pollutants that are likely to be present in an  industrial environment are 
8. H S, SO and oxides of nitrogen 

2 2 

1. NH3, HCl and CO 
2. CO2 NH3 andH2S 
3. Dust, No and Cl2
4. Which of the following gases dissolves in water  vapour to produce acid rain during rainfall? 
5. Oxygen 
6. Carbon (11) oxide 
7. Nitrogen 
8. Sulphur (lV)oxide 
9. Water for town supply is chlorinate to make itfree  from 
10. bad odour 
11. bacteria 
12. temporary hardness 
13. permanent hardness. 
14. On which of the following is the solubility of a  gaseous substance dependant? 1. Nature of solvent. 11. Nature of solute 11. Temperature. 1V.Pressure. A. l, ll,lll and lV B. l and ll only C. ll only D. l, lll and iV only
15. An emulsion paint consist of A. gas or liquid particles dispersed in liquid B. liquid particles dispersed inliquid 
16. In which of the following is the entropy change  positive? 
17. H2O(l) H2O(g) 
    
18. solid particles dispersed in liquid B. Cu2+(aq) + Fe(s) Fe2+(aq)+Cu(s)
    
19. solid particles dispersed in solid 
20. A sample of orange juice is found to have a pHof 3.80. What is the concentration of the hydroxide ion  in the juice? 
21. 1.6x 10-4 B. 6.3 x10-11
22. 6.3x 10-4 D. 1.6x 10-11
23. Arrange HCl, CH3 COOH, C6H5CH3 in order of  increasing conductivity. 
24. HCl,CH3COOH,C6H5CH3
25. C6H5CH3 HCl, CH3,COOH 
26. C6H5CH3 COOH,HCl, 
27. CH3, COOH,C6H5CH3,HCl 
28. Which of these is an acid salt? 
29. K2SO4Al2(SO4)3.24H2O 
30. CuCO3.Cu(OH)2
31. NaHS 
32. CaOCl2
33. How many grams of H2SO4 are necessary for the  preparation of 0.175 dm3 of 6.00 M H SO ? 
34. N2(g) + 3H2(g 2NH3(g)
35. 2HCl(s) N2(g) + Cl2(g)
36. In what way is equilibrium constant for the forward  reaction related to that that of the reverse reaction? A. The addition of the two is expected to be  one 
37. The product of the two is expected to be  one 
38. The two equilibrium constants are identical D. The product of the two is always greater  than one. 
39. Which of the following equilibra shows little orno  net reaction when the volume of the volume of the  system is decreased? 
40. H2(g)+ l2(g 2Hl(g)
41. 2NO2(g N2O4(g)
42. PCl5( PCl3(g) +Cl2(g)
43. ZnO(s) + CO2(g ZnCO3(s)
44. For a general equation of the nature xP+ yQ mR + nS, the expression for the equilibrium constant is 
    
45. 206.0 g B. 103.0 g C. 98.1 g D. 51.5 g 

2 4 

[S = 32.06, O = 16.00, H = 1.00]. 

1. k [P]x[Q]y B. [P]x[Q]y

[R]m [S]n 

22. Copper (ll) tetraoxosulphate (lV) solution is  electrolyzed using carbon electrodes. Which of the  following are produced at the anode and cathode  respectively. 
23. Copper and oxygen 
24. Oxygen and copper 
25. Hydrogen and copper 
26. Copper and hydrogen 
27. Calculate the mass, in kilograms, of magnesium  produced by the electrolysis of magnesium(ll)  

chloride in a cell operating for 24 hours at 500 amperes.  A. 2.7 B. 5.4 

10. 10.8 D. 21.7 

[Faraday = 96,500 C mmol-1, Mg = 24] 

24. MnO + 2Cl–+ 4H Mn2+ +Cl + 2H O. The change 2 2 2 

is oxidation numbers when the manganese, chlorine  and hydrogen ions react according to the above  equation are respectively. 

1. 2, 2, 4 B. –1,-2 4 
2. –2, 1, 0 D. 2, 4, 0 
3. S O32- + l S O62- + 21. In the reactionabove, 2 4 

2 

the oxidizing agents is 

1. S O32-
2. [R]m [S]n

[P]x[Q]y 

1. m [R] n [S]  

X [P] y [Q]. 

30. Which of these statements is TRUE about  carbon(1V)oxide? 
31. It supports combustion 
32. It is strong acidic inwater 
33. It is very soluble in water 
34. It supports the burning of magnesium to  produce magnesiumoxide. 
35.  
36. l2

2 

In the experiment above, Z can be 

1. S O62-
2. a solution of sodium dioxonitrate(lll)and  
3. l–

4 

ammoniumchloride 

1. a solution of lead trioxonitrate(V)
2. a solution of sodium trioxonitrate(V)and  ammoniumchloride 
3. concentrated tetraoxosulphate (Vl) acid and  sodiumtrioxonitrate(V). 
4. Which of the following combination of gases is used  for metal welding? 1. Oxygen and ethyne. ll Hydrogen  and ethyne. 1ll. Hydrogen and oxygen. 1V Ethyne,  hydrogen and oxygen. 
5. 1 and 11 B. 111 and1V 
6. 1 and 111 D. 11 and1V 
7. Which of the following oxides of nitrogen is unstable  in air? 
8. NO2 B. NO 
9. N2O4 D. N2O5
10. The gasformed when ammonium trioxonitrate (V)is  heated with sodium hydroxide is 
11. hydrogen 
12. nitrogen(1V) oxide 
13. oxygen 
14. ammonia 
15. Safety matches contain sulphur and 
16. Potassiumtrioxochlorate(V) 
17. CH3

CH3¯C = CH¯CH2¯CH¯CH3  

CH2 

CH3 

The IUPAC name for the hydrocarbon above is A. 2-ethyl-5-methylhex-2-ene 

1. 2, 5-dimethylhex-2-ene 
2. 3,5-dimethylhept-3-ene 
3. 3,6-dimethylhexpt –3-ene 
4. Which of the following compounds is a secondary  alkanol? 
5. CH3¯ CH2¯CH¯CH3

OH 

1. CH3 CH2 CH2 CH2OH 
2. CH3 CH2 OCH2 CH3

CH3 

CH3¯ C¯OH 

CH 

44. Potassium trioxonitrate (V) 44.3 Which of the following compounds reacts with sodium 
    
45. Charcoal 
46. Phosphorus sulpide 
47. Addition of an aqueous solution of barium chloride  to the aqueous solution of a salt gives a white  precipate. 
48. nitrate B. carbonate C. chloride D. sulphide 
49. Sodium hydroxide solution can be conveniently  stored in a container made of 
50. lead B. zinc 
51. aluminum D. copper 
52. Which of the following is NOT used asraw material  in the solvary process? 
53. Ammonia 
54. Sodium chloride 
55. Calcium trioxocarbonate 
56. Sodium trioxocarbonate(V1) 
57. Duralumin consists of aluminum, copper, A. zinc and gold 
58. lead and manganese 
59. nickel and silver 

metals as well as silver and copper salt. 

1. CH3 Ca = C ¯CH3

B CH3 CH2 CH2 CH2CH3 

1. CH3 Ca CH3
2. CH3 CH CHCH3
3. Which of the following are isomers? 
4. Ethanol and dimethyl ether 
5. Benzene and methylbenzene 
6. Ethanol and propanone 
7. Trichloromethane and tetrachloromehane 
8. The function group present in an treatment with a  saturated solution of NaHCO3 is. 
9. hydroxyl group 
10. carbonalkoxyl group 
11. carbonyl group 
12. carboxy group. 
13. Thecharacteristic reaction of carbonyl compounds is. A. Substitution B. Elimination C. Addition D. Saponificatioon 
14. An organic compound containing 40.1% carbon and  6.667% hydrogen has an empirical formula of. 
15. manganese and magnesium. A. C2H4O2
16. C2H3O2
    

CH2O D. CH3O 

40. CaO(s) + H2O(l ) Ca(OH)2(s) H = -65kJ. The  process represented by the above equation is known as. A. dissolution B. slackin 
41. liming D. mortaring 
42. The carbon atoms in ethane are 
43. sp3 hybridized 
44. sp hybridized 
45. sp2 hybridized 
46. not hybridized. 
47. Alkanals can be differentiated from alkanones by  reaction with. 
48. 2,4-dinitrophenlhydrazine 
49. hydrogen cyanide 
50. sodium hydrogen sulphite 
51. tollen’s reagent. 
52. An example of a polysaccharide is 
53. dextrose B. mannose  

C.glucose D. starch.

Chemistry 1993 

1. The dissolution of common salt in water is physical  
   

change because 

1. the salt can be obtained by  

crystallization 

1. the salt can be recovered by the evaporation  of water. 
2. Heat is not generated during mixing 
3. greater than the forces of attraction in both  solid and the liquid phases 
4. An element, E, has the electronic configuration  1s22s22p63s23p3. The reaction of E with a halogen X can give. 
   
5. The solution willnot boil at 100oC A. EX and EX B. EX only 3 5 3 
   
6. Which of the following substances is mixture? A. Sulphur powder B. Bronze C. Distilled water D. Ethanol 
7. How many moles of oxygen molecules would be  produced dfrom the decompostition of 2.5 moles of  potassium trioxochlorate (V)? 
8. 2.50 B. 3.50 
9. 3.75 D. 7.50 
10. A balanced chemical equation obeys the law of A. Conservation of mass 
11. Definite proportions 
12. Multiple proportions 
13. Conservation of energy 
14. At 25oC and 1 atm, a gas occupies a volume of 1.50  dm3. What volume will it occupy at 100oC at 1 atm?  A. 1.88dm3 B………………….6.00dm3
15. 18.80dm3 D. 60.00dm3
16. A gaseous mixture of 80.0 g of oxygen and 56.0 g of  nitrogen has a total pressure of 1.8 atm. The partial  pressure of oxygen in the mixture is 
17. 0.8atm B. 1.0atm 
18. 1.2atm D. 1.4 atm  

[O= 16, N= 14] 

Which of the curves above represents the behavior  of 1 mole of an ideal gas? 

1. 1 B. 11 
2. 111 D. 1V 
3. For iodine crystals to sublime on heating, the  molecules must acquire energythat is 
4. less than the forces of attraction in the solid B. equal to the forces of attraction in the solid C. necessary to melt the solid 
5. EX5only D. EX2 andEX3
6. Two atoms represented as 235 Uand 238 U are 92 92 
7. isomers B. allotropes 
8. isotopes D. anomers 
9. As the difference in electronegativity between  bonded atoms increase, polarity of the bond 
10. decreases B. increases 
11. remains unchanged 
12. reduces to zero. 
13. Which group of elements forms hydrides that are  pyramidal in structure? 
14. 111 B. 1V 
15. V D. V1 
16. Water has a rather high boiling point despite its low  molecular mass because of the presence of 
17. hydrogen bonding 
18. covalent bonding 
19. ionic bonding 
20. metallic bonding 
21. Argon is used in gas-filled electric lamps because it  helps to 
22. prevent the reduction ofthe lamp filament 
23. prevent oxidation oflamp filament 
24. make lamp filaments glowbrightly 
25. keep the atmosphere in the lamp inert. 
26. The air around a petroleum refinery is most likely to  contain 
27. CO2 SO3 and N2O 
28. CO2 CO and N2O 
29. SO3 CO and NO2
30. PH3 H2O andCO2
31. Water can be identified by the use of 
32. an hydrogen copper(11) tetraoxosulphate(1V) B. an hydrogen sodium trioxocarbonate(1V) C. potassium heptaoxochromate(vii) 
33. copper (11) trioxocarbonate(iv) 
34. The phenomenon whereby sodium trioxocarbonate (1) decahydrate loses some of its water crystallization  on exposure to the atmosphere is known as 
35. deliquescence B. hygroscopy C. effervescence D. efflorescence
36. A student prepares 0.5 M solution each of hydrochloric  and ethanoic acids and then measured their pH. The  result would show that the 
37. pH values are equal 
38. HCl solution has higher pH 
39. Sum of the pH values is 14 
40. Ethanoic acid solution has a higher pH. 

For which salt in the graph above does the solubility  increase most rapidly with rise in temperature 

1. CaSO4 B. KNO3
2. NaCl D. KCl 
3. NH3+ H3O NH4 + H2O. it may be deduced from  the reaction above that 
4. a redox reaction has occurred 
5. H O+acts as an oxidizingagent 

3 

1. H O+acts as an acid 

3 

1. Water acts as an acid 
2. 4.0 g of sodium hydroxide in 250 cm3 ofsolution  contains 
3. 0.40 moles perdm3
4. 0.10 moles perdm3
5. 0.04 moles perdm3
6. 0.02 moles perdm3
7. During the electrolysis of a salt of metal M, a current  of 0.05 A flow for 32 minutes 10 second and deposit 0.325 g of M. What is the charges of the metal ion? A.1 

B.2 

C.3 

D.4 

[M = 65,l = 96,500 C per mole of electron] 

23. Which of the following reactions occurs at the anode  during the electrolysis of a very dilute aqueous  solution of sodium chloride? 
24. OH –CH OH 
25. Cl–– e– Cl 
26. OH + Cl– HCl 
27. Na+ + e– Hg Na/Hg amalgam 
28. Half – cell reaction E0

From the data above, it can be deduced that the most  powerful reducing agent of the four metals is 

1. Cu B. Fe 
2. Ba D. Zn 
3. The oxidation states of chlorine in HOCl, HClO3and  HClO4 are respectively 
4. -1, +5 and +7 
5. –1 ,-5 and7 
6. +1, +3 and +4 
7. +1, +5 and +7 
8. A reaction takes place spontaneously if A. ÄG =O 
9. ÄS < O and ÄH > O 
10. ÄH <TÄS 
11. ÄG>O 
12. The standard enthalpies of formation of CO2(g),  H2O(g) and CO(g)in kJmol-1 are –394, -242 and –110  respectively. What is the standard enthalpy change  for the reaction CO(g) + H2O CO2(g) + H2(g)? A. -42kJ mol-1 
13. +42 kJmol-1 
14. –262 kJmol-1 
15. +262 kJmol-1 
16. 10 g of a solid is in equilibrium with its own vapour.  When 1 g of a small amount of solid is added, the  vapour pressure 
17. remain the same 
18. drops 
19. increase by 1% 
20. increase by 99% 

In the diagram above, curve X represents the energy  profile for a homogeneous gaseous reaction. Which  of the following conditions would produce curve Y  for the same reaction? 

1. increase in temperature 
2. increase in the concentration of a rectant C. addition of a catalyst 
3. increase in pressure. 
4. NaCl(s) + H2SO4(1) HCl(g) + NaHSO4(s). In the  reaction above. H2SO4 behaves as 
   

Cu2+(aq) + 2e Cu(s) +0.34V A. a stron acid Fe2+(aq) + 2e Fe -0.44V B. an oxiding agent Ba2+(aq) + 2e Ba(s) -2.90V C. a good solvent Zn2+(aq) + 2e Zn(s) -0.76V D. a dehydrating agent.

32. Which of these salts will produce its metal, oxygen and  nitrogen(1V) oxide onheating? 
33. Silvertrioxonitrate(V) 
34. Sodium trioxonitrate (V) 
35. Calcium trioxonitrate (V) 
36. Lithium trioxonitrate (V) 
37. An experiment produces a gaseous mixture of carbon  (1V) oxide and carbon(11) Oxide. In order to obtain  pure carbon (11) oxide, the gas mixture should be A. passed over heated copper(11) oxide 
38. bubbled through concentrated  

tetraoxosulphate(V1) acid 

1. bubbled through sodium hydroxide solution D. bubbled through water. 
2. Which of the following is property of ionic chlorides? A. They can be decomposed heat. 
3. They react with aqueous AgNO3 to give q  white precipitate which is soluble in excess  

ammonia 

1. They explode when in contact with dry  ammonia gas 
2. They react with concentrated  

tetraoxosulphate (V1) acid togive white  

fumes of chlorides gas 

35. When dilute aqueous solutions of (11) nitrate and  potassium bromide are mixed, a precipitate is  

observed. The products of this reaction are. 

1. PbO(s) + Br- (aq) + KNO3
2. Br2+ NO2(g) + PbBr2(s) 
3. PbO(s) PbO(s) + K+(aq) + Br(aq) +NO2(g) D. PbBr2(s) + K+(aq) + NO3(aq) 
4. Bronze is an alloy will react to 
5. Silver and copper 
6. Silver and gold 
7. Copper and nickel 
8. Copper and zinc 
9. Copper metal will react with concentrated  trioxonitrate (V) acid to give 
10. Cu(NO3)3 + NO + N2O4 +H2O 
11. Cu(NO3)2 + NO +H2O 
12. CuO +NO2 + H2O 
13. Cu(NO3)2 + NO2 + H2O 
14. The active reducing agent in the blast furnace for the  extraction of iron is 
15. carbon B. limestone 
16. carbon (11) oxide D. calcium oxide 
17. Al2O3(s) + 3H2SO4(aq)=Al2(SO4)3(aq) + 3H2O(1)  Al2O3(s) + 2NaOH(aq) + 3H2O(1) ’! 2NaAl(OH)4(aq). We can conclude from the equations above that  Al2O3(s) is 
18. an acidic oxide 
19. an amphotericoxide 
20. a basic oxide 
21. a neutral oxide 

H 

H2N CH C OH 

The two functional groups in the above compound are. 

A alcohol and amine 

1. acid and amine 
2. aldehyde and acid 
3. ketone andmine 
4. The fraction of crude oil used as jet fule is A. refinery gas 
5. diesel oil 
6. kerosene 
7. gasoline 
8. CH3CHCH2CHCH2CH3

CH3 CH3. 

The IUPAC nomenclature for the compound above is. A. dimethylhexane 

1. 3,5 dimethlpentane 
2. 1,1 dimethyl , 3 methylpentane 
3. 2,4 dimethylhexane. 
4. It is not desirable to use lead tetraethyl as an anti knock agent because 
5. it is expensive 
6. of pollution effects from the exhaust fumes C. it lowers the octane rating of petrol 
7. it is explosive. 
8. The carbon atoms on ethane are 
9. sp2 hybridized 
10. sp3 hybridized 
11. sp2d hybridized 
12. sp hybridized. 
13. Catalytic hydrogenation of benzene produces A. an aromatic hydrocarbon 
14. margarine 
15. cyclohexane 
16. D.D.T 
17. O O 

CH3 C-OCH2CH2 and CH3CH2CH2 C-OH are 

1. isomers 
2. esters 
3. carboxylic acids 
4. polymers. 
5. Palm wine turnssour with time because. A. the sugar content is converted into alcohol B. the carbon(1V) oxide formed during the  fermentation process has a sour taste 
6. it is commonly adulterated by the tappers  and sellers 
7. microbial activity results in the production  of organic acids within it.
   

48 49. Which of the represents Saponification? A. reaction of carboxylic acids withsodium 

hydroxide 

1. reaction of Alkanoates with acids 
2. reaction of carboxylic acids withsodium 

alcohols 

1. reaction of Alkanoates with sodium 

hydroxide. 

50. The confirmatory test for Alkanoic acids inorganic  

qualitative analysis is the 

1. turning of wet blue litmus paper red 
2. reaction with alkanols to form esters 
3. reaction with sodium hydroxide to foemsalt  
   

The function of the copper (11) tetraoxosulphate (V1)  in dilute H2SO4 in the figure above is to 

1. Dry the gas 
2. Absorb phosphine impurity] 
3. Absorb ethene impurity 
4. Form an acetylide withethyne. 

and water 

1. reaction with aqueous Na2CO3 to liberatea  gas which turnslime water milky. 
   

Chemistry 1994 

1. A mixture ofsand, ammonium chloride and sodium  
   

chloride is best separated by 

1. sublimation followed by addition ofwater  and filtration 
2. sublimation followed by addtion of water  and evaporation 
3. addition of water followed by filtration and  sublimation 
4. addition odf water followed by  

crystallization and sublimation. 

2. A pure solid usually melts 
3. over a wide rangeof temperature 
4. over a narrow range oftemperature 
5. at a lower temperature than the impureone D. at the same temperature as the impureone. 

3 At the same temperature and pressure, 50 cm3 of  nitrogen gas contains the same number of molecules  as 

1. 25 cm3of methane 
2. 40 cm3 ofhydrogen 
3. 50 cm 3 of ammonia 
4. 100 cm3of chlorine 
5. 8 g CH occupies 11.2dm3at s.t.p. What volume would  4 

22 g of CH3CH2CH occupy under the sme condition? A. 3.7 dm3 B. 11.2 dm3 

22. 22.4 dm3 D. 33.6 dm3

[C= 12, H=1] 

5. To what temperature must a gas 273 K be heated in  order to double both its volume and pressure? 
6. 298 K B. 546 K 
7. 819K D. 1092 K 
8. For a gas, the relative molecular mass is equal to 2Y.  What is Y? 
9. The mass of the gas 
10. The vapour density of the gas 
11. The volume of the gas 
12. The temperature of the gas 
13. The densities of two gases, X and Y are 0.5 g dm-3and 2.0 g dm-3respectively. What is the rate of diffusion of  X relative to Y? 
14. 0.1 B. 0.5 
15. 2.0 D. 4.0 
16. An increase in temperature curves causes an increase  in the pressure of a gas because 
17. it decreases the number of Collision between  the molecules 
18. the molecules of the gas bombard the walls of  the container more frequently 
19. it increase the number of Collision between  the molecules 
20. it causes the molecules to combine 
21. The shape of ammonia moleculesis 
22. trigonal planar 
23. octahedral 
24. square planar 
25. tetrahedral. 
26. The number of electrons in the valence shell of an  element of atomic number 14 is 
27. 1 B. 2 
28. 3 D. 4
29. Which of the following physical properties decreases  down a group ion the periodic table? 
30. Atomic radius 
31. Ionic radius 
32. Electropositivity 
33. Electronegativity. 

12 

Nucleus 

An Electron 

The diagram above represents atom of 

1. Mangnesium 
2. Helium 
3. Chlorine 
4. Neon 
5. Elements X, Y and Z belongs to groups 1,V and V11  respectively. Which of the following is TRUE about  the bond types of XZ and YZ 
6. Both are electrovalent 
7. Both are covalent 
8. XY is electrovalent and YZ3 is covalent D. XZ is covalent and YZ3 is electrovalent. 
9. Which of the following atoms represents deuterium?  ‘ No of No of No of protons neutrons electrons 
10. 1 0 0 
11. 1 0 1 
12. 1 1 1 
13. 1 2 1 

The set-up above would be useful for determining the  amount of 

1. Oxygen in air 
2. Water vapour in air 
3. CO2 in air 
4. Argon in air. 
5. A solid that absorbs water from the atmosphere and  forms an aqueous solution is 
6. hydrophilic 
7. efflorescent 
8. deliquescent 
9. hygroscopic 
10. A major effect of oil pollution in coastal water is the A. destruction of marinelife 
11. desalination of water 
12. increase in the acidity of the water 
13. detoxification of thewater. 
14. Sodium chloride has no solubility product value  because of its. 
15. saline nature 
16. high solubility 
17. low solubility 
18. insolubility 
19. The solubility in moles per dm3 of 20.2g of potassium  trioxonitrate (V) dissolved in 100g of water at room  temperature is 
20. 0.10 
21. 0.20 
22. 1.00 
23. 2.00 

[K = 39, O = 16, N = 14] 

20. A few drops of concentrated PCl are added to about  10cm3 of a solution of pH 3.4. The pH of the resulting  mixtureis 
21. less than 3.4 
22. greater than 3.4 
23. unaltered 
24. the same as that of pure water 
25. Which of the following compounds is a base? A. CO2
26. CaO 
27. H3PO3
28. CH3COOH 
29. 20cm3 of a 2.0 M solution of ethanoic acid was added to  excess of 0.05 M sodium hydroxide. The mass of the  salt produced is 
30. 2.50 g 
31. 2.73 g 
32. 3.28 g 
33. 4. 54g 

[Na = 23, C =12, O = 16, H = 1] 

23. What volume of oxygen measured at s.t.p would be  liberated on electrolysis by 9650 coulombs of  electricity? 

A………..22.4 dm3 

B…………………..11.2 dm3 

C…………………..1.12 dm3 

D…………….0.560dm3 

[Molar Volume of gas = 22.4 dm3, F = 96,500 C mol-1] 

24. Crude copper could be purified by the electrolysis of  concentrated copper911) chloride if the crude copper  is 
25. made both the anode and the cathode 
26. made the cathode 
27. made the anode 
28. dissolved in the solution.
    
29. H–(s) + H O(1) H (g) + OH–(aq). From the equation 31. Which of the following are produced when ammonium 2 2
    

above, it can be inferred that the 

1. reaction is a double decomposition 
2. hydride ion is reducing agent 
3. hydride ion is an oxidizing agent 
4. reaction is neutralization. 

26

The H for the reaction represented by the energy  profile above is 

1. -100kJ mol-1
2. +100 kJmmol-1
3. +50kJmol-1

trioxonirate(V) crystals are cautiously heated in a hard  glass round bottomed flask? 

1. N2O and steam 
2. NO2 and ammonia 
3. N2O4 and NO2
4. NO andNO2
5. 2HCl(aq) + CaCO3(s) CaCl2(aq) + H2O(10 + CO2g).  From the reaction above, which of the following curves  represents the consumption of calcium  trioxocarbonate(lV) as dilute HCl is added to it? 

1. –50 kJmol-1 A. L B. M C. N D. P 
2. An anhydride is an oxide of a non-metal. 
3. Which will not dissolve in water 33. 
4. whose solution water has pH greater than7 
5. whose solution in water has a pH less than 7 
6. whose solution in ware has a pH of 7 
7. MnO (aq) + 8H+(aq) + Fe2+(aq) Mn2+(aq) +5Fe3+ + 

4 

4H2O(1). The oxidation number of manganese in the  

above reaction change from 

1. +7 to +2 B. +6 to+2 
2. +5 to +2 D. +4 to+2 

In the diagram above, R is a mixture of 

1. potassium tetraoxochlorate(Vii) and  

concentrated H2SO4 

1. potassium tetraoxomanganate (vii) and 

concentrated HCl 

1. manganese(1V) oxide and concentrated HCl 
2. manganese (1V) oxide and concentrated HCl 
   

In the diagram above, the activation energy is  

represented by 

1. y-x B. x 
2. x-z D. y 
3. Which of the following is TRUE of Le Chatelier ’s  principle for an exothermic reaction? 
4. Increase in temperature will cause an increase  in equilibriumconstant 
5. Increase in temperature will cause adecrease  in the equilibriumconstant 
6. Addition of catalyst will cause an increase in  the equilibrium constant. 
7. Addition of catalyst will cause a decrease in  the equilibrium constant. 
8. Which of these metals CANNOT replace hydrogen  from alkaline solutions? 
9. Aluminium 
10. Zinc 
11. Tin 
12. Iron 
13. Clothes should be properly rinsed with water after  bleaching because 
14. the bleach decolourizes the clothes 
15. chlorine reacts with fabrics during bleaching C. the clothes are sterilized during bleaching D. hydrogen chloride solution is produced  during bleaching.
16. Which of these solutions will give a white precipate  with a solution of barium chloride acidified with  hydrochloride acid? 
17. Sodium trioxocarbonate(1V) 
18. Sodium tetraoxosulphate 
19. Sodium trioxosulphate (1V) 
20. Sodium sulphides 
21. SO3 is NOT directly dissolved in water in the  preparation of H2SO4 by the contact process  because. 
22. the reaction between SO3 and water is  violently exotheremic 
23. acid is usually added to water and never  water to acid 
24. SO3 is an acid not dissolve in water readily D. SO3 is an acidgas. 
25. In an electrolytic set-up to protect iron from  corrosion, the iron is 
26. made the cathode 
27. made the anode 
28. used with a metal of lower electropositive  potential 
29. initially coated withtin 
30. Which of the following is NOT true of metals? A. They are good conductors of electricity B. They ionize by electron loss 
31. Their oxides are acidic 
32. They have highmelting points. 
33. Which of the following is the correct order of  decreasing activity of the metal Fe, Ca, Al and Na? A. Fe > Ca > Al > Na 
34. Na > Ca > Al > Fe 
35. Al > Fe > Na > Ca 
36. Ca > Na > Fe >Al. 
37. H CH3 H H  

H¯C ¯ C¯ C P-C 

H CH3 

H 

The IUPAC name of the compound above is 

1. 2,2-dimethyl but-1-yne 
2. 2,2-dimethyl but-1-ene 
3. 3,3-dimethyl but-1-ene 
4. 3,3-dimethyl but-1-yne 
5. When sodium is added to ethanol, the products are A. sodium hydroxide andwater 
6. sodium hydroxide and hydrogen 
7. sodium ethnocide and water 
8. sodium ethnocide and hydrogen. 
9. The general formula of alkanones is 
10. RCHO 
11. R2CO 
12. RCOOH 
13. RCOOR 
14. When sodium ethanoate is treated with a few drops of  concentrated tetraoxosulphate(V1) acid one of the  products is 
15. CH3COOH 
16. CH3COOH3
17. CH3COOC2H5
18. C2H4COOCH 
19. One mole of a hydrocarbon contains 48 g of carbon.  If its vapour density is 28, the hydrocarbon is 
20. an alkane 
21. an alkene 
22. an alkyne 
23. aromatic 

[C= 12, H = 1] 

Use the diagram below to answer questions 47 and 48.

The reaction taking place in flask G is known as A. hydrolysis 

1. double decomposition 
2. dehydration 
3. pyrolysis 
4. The caustic soda solution in the conical flask serves to A. dry ethene 
5. remove carbon (1V) oxide fromethene C. remove carbon (11) oxide from ethene 
6. remove sulphur (1V0 oxide from ethene. 
7. Which ofthe following orbital of carbon are mixed  with hydrogen in methane? 
8. 1s and 2p 
9. 1s and 2s 
10. 2s and 2p 
11. 2s and 3p 
12. Which of the following reagents will confirm the  presence of instaurations in a compound? 
13. Fehling’ssolution 
14. Brominewater 
15. Tollen’sreagent 
16. Benedict’s solution
    

Chemistry 1995 

1. Chromatography is used to separate components of  mixtures which differ in their rates of 
2. diffusion B. migration 

C reaction D. sedimentation. 

2. Which of the following is an example of chemical  change? 
3. Dissolution of salt in water. 
4. Rusting ofiron 
5. Melting ofice. 
6. Separating a mixture by distillation. 
7. The number of hydrogen ions in 4.9 g of  tetraoxosulphate (VI) acidsis 
8. 3.01 x 1022 B. 6.02 x 1022

C.3.01 x1023 D. 6.02 x 1022. 

(S= 32, O=16,H=1,N = 6.02 x 1023). 

A 

4. What volume ofoxygen will remain afterreacting 8 cm3 of hydrogen with 20 cm3 of oxygen? 
5. 10 cm3 B. 12 cm3
6. 14 cm3 D. 16 cm3. 
7. A gas sample with initial volume of 3.25 dm3 is heated  and allowed to expand to 9.75 dm3 is heated and  allowed to expand to 9.75 dm3at constant pressure.  What is the ratio of the final absolute temperature to  the initial absolutetemperature? 
8. 3:1 B. 5:2 C.5:4 D. 8:3 
9. Two cylinders A and B each contains 30 cm3 of oxygen  and nitrogen respectively at the same temperature and  pressure. If there are 5.0 moles of nitrogen, then the  mass of oxygen is 
10. 3.2 g B. 6.4g 
11. 80.0g D. 160.0g. 
12. A liquid begins toboil when 
13. its vapour pressure is equal to vapour pressure of  its solid at the given temperature 
14. molecules start escaping from itssurface 
15. its vapour pressure equals the atmosheric pressure D. its volume isslightly increased. 
16. A particle that contains 8 protons, 9 neutrons and 7  electrons could be written as 
17. 16 O B. 17 O+

8 8 

1. 17 O+ D. 17 O. 
2. Which letter represents a non-metal that is a solid at  room temperature? 
3. T B. R. 
4. J. D. X. 
5. In the oil drop experiment, Milikan determined the A. charge to mass ratio of the electron 
6. mass of the electron 
7. charge of the electron 
8. mass of the proton. 
9. The stability of ionic solids is generally due to the A. negative electron affinity of most atoms 
10. crystal lattice forces 
11. electron pair sharing 
12. positive ionization potentials. 
13. Which of the following statements is FALSE about  isotopes of the same element? 

A.They have the same number of electrons in their  outermost shells. 

1. they have different atomicmasses. 
2. They have the same atomic number and the same  number of electrons. 
3. they have the same atomic number but different  number of electrons. 
4. Helium is often used in observation balloons because  it is 
5. light and combustible 
6. light and non-combustible 
7. heavy and combustible 
8. heavy and non-combustible. 
9. When plastic and packaging materials made from  chloromethane are burnt in the open, the mixture of  gases released into the atmosphere is most likely to  contain 
10. ethane B. chlorine 
11. hydrogen chlorine D. ethane. 
12. Deliquescent substances are also 
13. efflorescent B. anhydrous 
14. hydroscopic D. insoluble. 
    

9 8 17. The difference between colloids and suspensions is 

Use the section of the periodic table  

below to answer questions 9 and 10. 

1							2L
3G	X	5	6	7	8J	9E	10
11	12 M	13 R	14	15	16 T	17	18

 

9. Which of the lettersindicate an alkali metal and a noble  gas respectively? 
10. M and E. B. G and E. C. R and L. D. G and L.

brought out clearly by the fact that while colloids A. do not scatter light, suspensions cannot be  so separated 

1. can be separated by filteration, suspension  cannot be separated 
2. can be separated by a membrane, suspensions  cannot 
3. do not settle out on standing, suspensions  do. 
4. In general, an increase in temperatue increases the  solubility of a solute in water because 
5. more solute molecules collide with each other B. most solutes 

dissolve with the evolution of heat 

1. more solute molecules dissociate at higher  temperature 
2. most solutes dissolve with absorption of  heat. 
3. Neutralization involves a reaction between H O+and 
4. Condensation of water vapour. 
5. Boiling a sampled of water 
6. Cooling a saturated solution. 
7. Which of the following equibrai is shifted to the  right as a result of an increase in pressure? 
   

3 

1. CI– B. OH– C. NO – D. CO 2-. 
2. H2(g) + I2(g)

2H(g) 

N2O 3 3 2 2(g) 4(g) B.2N O 

20. Which of the following solutions will have a pH < 7? A. Na2SO4(aq) B. NaCI(aq)
21. Na2CO3(aq) D. NH4CI(aq).
22. What is the pH of a 2.50 x 10-5 M solution of sodium hydroxide? 
23. 3.6 B. 5.0 C. 9.4 D. 12.0. 

14 

12 

10 

8 

6 

25VOL OF BASE 

22. The graph above showsthe pHchanges for the titration  of a 
23. strong acid versus strong base 
24. weak acid versus strong base 
25. strong acid versus weak base. 
26. weak acid versus weak base. 
27. In the process ofsilver-plating a metal M, the metal M  is the 
28. anode and a direct current is used 
29. cathode and an alternating current is used C. anode and an alternating current is used. D. cathode and a direct current is used. 
30. How many moles of copper would be deposited by  passing 3F of electricity through a solution of copper (II) tetraoxosulphate (VI)? 
31. 0.5 B. 1.0 
32. 1.5 D. 3.0 

(F = 96 500 C mol-1). 

C.PCl5(g) PCl3(g) + Cl2(g) 

1. 2O3(g) 3O2(g) . 
2. The arrangement above can be used for the collection of A. sulphur (IV) oxide 
3. ammonia 
4. nitrogen 
5. hydrogen chloride. 

The activation energy of the uncatalysed reaction is A.x 

1. x +y 
2. x-y 
3. y 
4. It can be deduced that the rate of the reaction A. for path I is higher than path II 
5. for path II is higher than path I 
6. is the same for both paths at all  

temperatures 

1. depends on the values of both x and y at all  pressures. 
2. In the industrial production of hydrogen from natural  gas, carbon (IV) oxide produced along with the 
   
3. 2Cl-(aq) ’!CI 2(g)= 2e–(aq). The above half-cell reaction hydrogen is removed by 
   

occurring at the anode during the electrolysis  

of dilute ZnCI2 solution is 

1. ionization B. oxidation 
2. reduction. D. recombination. 26. Which of the following is a redox reaction? A. KCI(ag) + H2SO4(aq) KHSO4(aq) + HCI(aq)
3. 2FeBr2(ag) + Br2( !2FeBr3(aq)
4. AgNO3(ag) + FeCI3 !3AgCl(aq) + CO Fe(NO3)3(aq) D. H2CO3(aq) H2O(l) + CO2(g).
5. Cr O 2- + 14H+ + 6I– 2Cr3

++ 3I + 7H O(1)+. 

2 7 (aq) (ag) (aq) ’! (ag) 2(g) 2 

The change in the oxidation number of oxygen in the  equation above is 

7. O. B. 1 C. 2 D. 7. 
8. If an equilibrium reaction has “H < O, the reaction will  proceed favourably in the forward reaction at 
9. lowtemperature 
10. high temperatures 
11. all temperatures 
12. all pressures. 
13. Which of the following processes lead to increase in  entrophy? 
14. mixing a sample of NaCl andsand 
15. washing under pressure 
16. passing the mixture into the lime water 
17. using ammoniacal copper (I)chloride 
18. drying over phosphorus (V) oxide. 
19. Sulpur existsin six formsin the solid state. This property  is known as 
20. isomerism B. allotrophy 
21. isotopy D. isomorphism. 
22. A gas that will turn orange potassium  

heptaoxodichromate (VI) solution to clear green is A. sulpur (VI) oxide 

1. hydrogen sulphide 
2. sulpur (IV) oxide 
3. hydrogen Chloride. 
4. Which ofthe following ions will give a white precipitate  with aqueous NaOH and soluble in excess of the base? A. Ca2+ B. Mg2
5. Zn2+ D. Cu2+.
6. In the extraction ofiron in the blast furnace, limestone  is used to 
7. release CO2 for the reaction 
8. reduce the iron 
9. Increase in the strenght of Iron 
10. remove impurities. 
11. Which of the following compound will impart abrick red colour to a non-luminous Busenflame? 
12. NaCl B. LiCl 
13. CaCl2 D. MgCl . 

40.. Group 1 A metals are not found free in nature because  they 

1. are of low melting andboiling points 
2. have weak metallic bonding 
3. conduct electricity and heat 
4. are veryreactive. 
5. CH COOH+ CH CH OH Conc H SO X + Y.X andYin the 3 3 2 2 

reaction of above are respectively 

1. CH3 COCH3 andH2O 
2. CH3 CH2 COCH2 andH2O2
3. CH3 COOCH2 CH3 and H2O3
4. CH3CH2 CHO andCH4. 

42 CHCl3+ Cl2 HCl + CCl4. The reaction above is an  example of 

1. an addition reaction 
2. a substitution reaction 
3. chlorination reaction 
4. a condensation reaction. 
5. CH3 – CH –CH = CH –CH3 CH3. The IUPAC  nomenclature for the compound above is 
6. 1.1-dimenthyilbut –ene 
7. 2-methlypnet 3 –ene 
8. 4,4 –dimethy –1but –2–ene 
9. 4 –methylpent –2 –ene. 
10. Which of the following pairs has compounds that are  isomers? 
11. propanal and propanone 
12. ethanoic acid and ethylmethanoate 
13. ethanoic acid and thane –1 ,2 –diol 
14. 2 –methylbutnae and 2,2 –dimethylbutane 
15. Aromatic and aliphatic hydrocarbons can be  distinguished from each other by the 
16. action of bromine 
17. use of polymerizationreaction. 
18. Action of heat 
19. Use of oxidation reaction 
20. The role of sodium chloride in the preparation of soap  is to 
21. purify the soap 
22. separate the soap from glycerol 
23. accelerate the decomposition of the fat oroil D. react with glycerol.  

O 

CH3CH2=CH2– C – H 

47. The functional group represented in the compound  above is 
48. alkanol B. alkanal 
49. alkanone D. alkanoate 
50. CxHy+ 4O23CO2 + 2H2O. The hydrocarbon,  Cx Hy in the reaction above is 
51. propane B. propene 
52. propyne D. propanone. 
53. An example of a secondary amine is 
54. propylene B. di-butylamine  C . methylamine D. trimethylamine. 
55. The relatively high boiling points of alkanol are due to A. ionic bonding 
56. aromatic character 
57. covalent bonding 
58. hydrogen bonding. 
    

Chemistry 1997 

1. 35 cm3 of hydrogen was sparked with 12cm3 of  oxygen at 110o C and 760 mm Hg to produce steam.  What percentage of the total volume gas left after the  reaction is hydrogen 
2. 11% B. 31% 
3. 35% D. 69% 
4. 2.85 g of an oxide of copper gave 2.52g of copper on  reduction and 1.90 g of another oxide gave 1.52 g of  copper on reduction. The data above illustrates the  lawof 
5. constant composition 
6. conservation ofmass 
7. reciprocal proportions 
8. multiple proportions.
   

Use the graph below to answer question 3 and 4 10. In the periodic table, what is the property that decrease  along the period and increases down the group 

1. Atomic number 
2. Electron affinity. 
3. Ionization potential 
4. Atomic radius. 
5. Two elements, P and Q with atomic numbers 11 and8  

respectively, combine chemically values of x and y are 

1. 1 and 1 B. 1 and 2 
2. 2 and 1 D. 3 and 1 
3. Oxygen is a mixture oftwo isotopes 16 O and 188 O with 

8

relative abundance of 90% and 10% respectively. The  

A sample, X, solid at room temperature, was melted,  heated to a temprature of 358 K and allowed to cool as  shown in OPQR. 

3. The section PQ indicate thatX is 
4. a mixture ofsalt 
5. a hydrated salt 
6. an ionic salt 
7. a pure compound. 

4.. The section OP suggests that X is in the 

1. Liquid state 
2. Solid/liquid state 
3. Solid state 
4. Gaseous state. 
5. An element, X, format a volatile hydride XH3 with a  vapour density of 17.o. The relation mass of X is A. 34.0 B. 31.0 
6. 20.0 D. 14.0 
7. A mixture of 0.20 mole ofAr, 0.20 mole of N2and 0.30  mole of He exerts a total pressure of2.1 atm. The partial  pressure of He in the mixture is 
8. 0.90atm B. 0.80atm 
9. 0.70atm D. 0.60atm 
10. If 30cm3 of oxygen diffuses through a porous plug in  7s, how long will it take 60 cm3 of chlorine to diffuse  through the same plug 
11. 12 s B. 14 s 
12. 21 s D. 30 s 
13. The temperature of a body decreases when drops of liquid  placed on it evaporates because 
14. the atmospheric vapour pressure has a cooling effect  on the body 
15. a temperature gradient exists between the drops of  liquid and the body 
16. the heat of vapourization is drawn from the  bodycausing it to cool 
17. the random motion of the liquid molecules causes a  cooling effect on the body. 
18. The electron configuration oftwo elements with similar  chemical properties arerepresented by 
19. Is22s2 2p5and Is22s22p4 
20. Is22s2 2p4and Is22s22p63s1

C Is22s22p63s1and Is22sI 

1. Is22s2 2p4and Is22sI 

relative atomic mass of oxygen 

16. 16.0 B. 16.2 
17. 17.0 D. 18.0 
18. 200cm3 of air was passed over heated copper in a syringe  several times to produce copper (11) oxide. When  cooled the final volume of air recorded was 158cm3.  Estimate the percentage of oxygen in the air. 
19. 31% B. 27% 
20. 21% D. 19% 
21. Which of the following gases is the most dangerous  pollutant 
22. Hydrogen sulphide 
23. Carbon (1V)oxide 
24. Sulphur (1V)oxide 
25. Carbon (11) oxide 
26. A major process involve in the softening of hard water  is the 
27. conversion of a soluble calcium salt to its  trioxocarbonate (1V) 
28. decomposition of calcium trioxocarbonate  (1V) 
29. conversion of an insoluble calcium salt to its  trioxocrbonate (1V) 
30. oxidation of calcium atom to itsions. 
31. On recrystallization, 20g of magnesiumtetraoxosulphate  (V1) forms 41 g of magnesium tetraoxosulphate (1V)  crystals, MgSO4.yH2O. The value of y is 
32. 1 B. 3 
33. 5 D. 7 

(Mg = 24, S=32, O=16, H= 1) 

17 A satyrated solution of AgCI was found to have a  concentration of 1.30 x 100-5 mol dm-3. The solution  product of AgCI. thereforeis. 

1. 1.30×10-5mol 2 dm-6 
2. 1.30x 10-7mol2dm-6 
3. 1.69x 10-10mol2dm-6 
4. 2.60×10-12mol2dm–6 
5. The hydroxyl ion concentration, (OH-), in a solutionof  sodium hydroxide of pH 10.0 is 
6. 10-10 moldm-3
7. 10-6 moldm-3
8. 10-4 moldm-3
9. 10-2 moldm-3
10. Which of the aqueous solution with the pH values below  will liberate hydrogen when it reacts with magnesium  metal? 
11. 13.0 B. 7.0 
12. 6.5 D. 3.0 
13. Given that 15.00cm3 of H2SO4 was required to  completelyneutralize25.00 cm3 of0.125mol dm-3 NaOH,  calculate the molar concentration of the acid solution.  A. 0.925 moldm-3 B. 0.156 moldm-3 
14. 0.104 mol dm-3 D. 0.023 mol dm –3 
15. When platinum electrodes are used during the  electrolysis of copper (11) tetraoxosulphate (1V)  solution, the solution gets progressively 
16. acidic B. basic 
17. neutral D. amphoteric 
18. Howmany faradays of electricity are required to deposit 0.20 mole of nickel, if 0.10 faraday of electricity  deposited 2.98 g of nickel during electrolysis of its  aqueous solution? 
19. 0.20 B. 0.30 
20. 0.40 D. 0.50 

( Ni =058.7, IF=96 500C mol-1) 

23. What is the oxidation unmber of Z in K ZCI6? 
24. One method of driving the positon of equilibrium of an  endothermic reaction forward isto 
25. increase temperature at constant pressure B. decrease pressure at constant temperature C. cool down the apparatus with water 
26. decrease temperature at constant pressure. 
27. Oxidation of concentrated hydrochloric acid with  manganese(1V) oxide liberates a gas used in the 
28. manufacture of tooth pastes 
29. treatment ofsimple goiter 
30. valcanization ofrubber 
31. sterilization ofwater. 
32. mE+ nF pG + qH 

In the equation above, the equlibrium constant is given  by  

1. (E)m(F)n  

(G)p(H)q 

1. (E)(F) 

(G) (H) 

1. (G)p(H)q  
   

3 

1. -3 B. +3 C. –6 D. +6 

(E)m(F)n 

24. 2H2S(g) +SO2(g) +H2O(1) 3S (s) +3H2O(1)….(I) 3CuO(s) +2NH3(g) 3Cu(s)+3H2)(1)+N2(g)… (ii) In the equation above, the oxidizing agent in (I) and the reducing agent in (ii) respectivelyare  

A H2S and NH3 

B SO2 and CuO 

1. SO2 and NH3
2. H2S and CuO 
3. 2SO2(g)+O2(g) 2 SO3(g) 

In the reaction above, the standard heats of formation ofSO (g) and SO (g) are –297 kJmol-1 and –396 kJmol-1 2 3 

respectively. 

The heat change of the reaction is 

1. -99kJmol-1 B. –198 kJmol-1 C. +198kJmol-1 D. +683 kJmol-1 
2. ½ N2(g) +1/2 O2(g); H- = 89 kJ mol-1 

If the entropy change for the reaction above at 25oC is 11.8 J, calculate the change in free energy, G , for the  reaction at 250C 

88. 88.71KJ 
89. 85.48kJ 
90. –204.00 kJ 
91. –3427.40kJ 
92. If the rate law obtained for a given reaction is  rate=k(X)n(Y)m, what is the overall order of the  reaction? 
93. nm 
94. n 
95. (G)(H) 

(E) (F) 

31. A compound that willNOTproduceoxygen on heating is A. potassium dioxonitrate (111) 
32. lead (1V)oxide 
33. potassiumtrioxochlorate (V) 
34. potassiumtrioxochlorate (V) 
35. Coal gasismade up to carbon (11) oxide, hydrogen and A. nitrogen B. air 
36. argon D. methane 

In the diagram above, the gas Y could be 

1. hydrogen chloride 
2. oxygen 
3. carbon (1V) oxide 
4. chlorine. 

(aq) + MnO2(s)+(aq) 2(g) + Mn2+(aq) + 2H2O(1)

m 34. 2X C. n+m 

1. n-m 

+ 4H X 

The reaction above can be used for the laboratory  preparation of all halogens except fluorine because it is A. a poisonous gas 

1. an oxidizing agent 
2. electronegative in nature 
3. highly reactive. 
4. The reaction that occurs during the laboratory test for  the presence of tetraoxosulphate (V1) 
5. 3-ethyl-1, 1, 4-trimethypentane 
6. 3-ethyl-2,5,5-trimethypentane 
7. The reaction of an alkanol with an alkanoic acid in the  presence of concentrated H2SO4 will produce an 
8. Alkanal 
9. Alkanonate 
10. Alkanone 
11. Alkayne. 
    
12. SO2-4(aq) + Ba2+(aq)dilHNO3 BaSO443. The final product of the reaction of ethyne with  hydrogen iodide is 
13. Cu +4H ++ 2SO2- CuSO (s) + 2H O A. CH CHI (s) (aq) 4(aq) 4 2 (1) 3 2 
    
14. 4H+(aq)+2SO2-4(aq)+2e– SO2-4(aq) + SO2(g)

+SO2(g) 

+2H2 O 

(1)

1. CH2I CH21 C. CH3 CI3 D CH2=CHI 
   
2. CuO + 2H+ + SO2- CuSO +H OCH3 (s) (aq) 4(aq) 4(aq) 2 (1)44. CH3CH2 C CH3 36. The removal of rust from iron by treatment with  
   

tetraoxosulphate (V1) acid is based on the 

1. hydrolysis of the iron 
2. reaction of acid with base 
3. oxidation of the rust 
4. dehydration of the iron. 
5. Which of the following additives could improve the  quality of steel? 
6. Silicon B. Sulphur and phosphorus C. Carbon. D. Chromium andnickel. 
7. Sodium hydroxide is prepared commercially from  sodium chloride solution by. 
8. electrolysis using mercury as cathode 
9. hydrolysis in steam using a catal.yst 
10. electrolysis using iron as anode 
11. treating sodium chloride with ammonia and  carbon (1V) oxide. 

39 A sample of a substance containing onlyCand H burns  in excess O to yield 4.4 g of CO and 2.7 g of H O.The 2 2 2 

empirical formular of the substance is 

1. CH3 B. CH2
2. CH4 D. C2H5

(C= 12, O=16, H= 1) 

40. An undesirable paraffin in the petroleum industry which  is particularly prone to knocking is 
41. iso-octane 
42. n-heptane 
43. iso-heptane 
44. n-octane 

CH3 

41. CH3 CH CH CH2 CH 

CH3 CH2 CH3  

CH3 

The IUPAC nomenclature ofthe organic compund with  the above structural formularis 

1. 3-ethyl-2, 5-dimethylhexane 

CH3 

How many more isomers of the compound above can be obtained? 

1. 5 B. 4 
2. 3 D. 2 
3. Synthesis detergents are preferred to soap for laundry  using hard water because 
4. detergent are water soluble while soap not B. the calcium salts ofdetergent are watersoluble C. the magnesium salt of soap is soluble in hard  water 
5. soap does not have a hydrocarbon terminal  chain. 
6. The synthetic rubber obtained by the polymerization  of chlorobutadiene in the presence of sodium is called A. Teflon B. Isoprene 
7. Polythene D. Neoprene 
8. 25cm3 of 0.02 M KOHneutralized 0.03 g of a monobasic B. 4-ethyl-2, 5-dimethylexane 
   

organic acid having the general formula CnH2n+1COOH. The  molecular formula of the acid is 

1. C. 

HCOOH CH3COOH 

1. D. 

C2H5COOH 

C3H7COOH 

(C= 12, H=1, 0=16) 

48 When Fehling’s solution is added to two isomeric  carbonyl compounds X and Y with the molecular formula  C5H10O, compound X gives a red precipitate while Y  does not react. It can be inferred that X is 

O 

A .CH3 C CH2 CH2 CH3 

1. CH3 CH2 CH2 CH2 C H

O A. sp3 hybridized carbon atoms only B. sp3 hybridized carbon atoms only 

1. CH CH C CH C H C. sp3and sp hybridized carbon atoms 
   

3 2 2 

O 

1. CH3 CH C CH2CH3 CH3

CH3 

The compound above contains 

1. sp3and sp2 hybridized carbon atoms. 

H H H O 

50. H C C C C H 

H H H CH3 

The compound above is the product of the oxidation of 

1. 2 – methylbutan – 2 – o1 
2. 2 – methylbutan –1 – o1 
3. 2,3 – dimenthylpropan – 1 – o1 
4. Pentan –2 – o1 

Chemistry 1998 

6. A given amount of gas occupies 10.0 dm3 at 4 atm.  
   
7. The addition of water to calcium oxide leads to A. a physical change 
8. a chemical change 
9. the formation ofmixture 
10. an endothermic change. 
11. A mixture of iron and sulphur can be separated by  dissolving the mixturein 
12. steam 
13. dilute hydrochloric acid 

and 2730C. The number of moles of the gas present is 

1. 0.089mol 
2. 1.90mol 
3. 3.80mol 
4. 5.70mol 

[Molar volume of gas at s.t.p.= 22.4 dm3] 

7. If sulphur oxide and methane are released  simultaneously at the opposite ends of narrow tube,  the rates of diffusion R and R will be in the ratio 
   
8. dilute sodiumhydroxide A. 4:1 so2 B. CH4 2:1 
   
9. benzene 
10. 8.0 g of an element X reacted with an excess of copper (11) tetraoxosulphate (1V) solution to deposit 21.3 g of  copper. The correct equation for the reaction is 
11. X(s)+CuSO4(aq) Cu(s) +XSO4(aq)
12. X(s) +2CuSO4(aq) 2 Cu(s) + X(SO4)(aq)
13. 2X(s)+2CuSO4(aq) Cu(s)+ X2(SO4)(aq) D. 2X(s) +3CuSO4(aq) 3Cu(s) + X2(SO)3(aq)
14. C3H8(g) + 5O2(g) 4H2O(g) +3CO2(G) 
15. 1:2 D. 1:4 

[S=32, O= 16, C=12, H=1] 

8. A solid begins to melt when 
9. constituent particles acquire a greater kinetic  energy 
10. energy of vibration of particles of the solid is  less than the intermolecularforces 
11. Constituent particles acquire energy of the  above the average kinetic energy 
12. energy of vibration of particles of the solid 

From the equation abovem the volume of oxygen at 9. s.t.p. required to burn 50cm3 of propane is A. 250cm3 B. 150cm3 

1. 100cm3 D. 50cm3
2. 30cm3 of hydrogen was collected over water at 27oC  and 780 mm Hg. If the vapour pressure of water at the  temperature of the experiement was 10mm Hgm calcuale  the volume of the gas at 760mm Hg and 70C. 
3. 40.0cm3 B. 35.7cm3
4. 28.4cm3 D. 25.2cm3

equals the intermolecular forces. 

The diagram above represents an atom that can combine 

with chlorine to form 

1. a convalent bond 
2. an electrovalent bond 
3. a hydrogen bond 
4. a co-ordinate bond 
5. Which of the following electron configurations  indicates an atom with the highest ionization energy?  A. 2,8, 7 B. 2, 8, 8, 1 
6. 2, 8,8, 2 D. 2, 8, 8, 7 
7. The lines observe in the simple hydrogen spectrum are  due to emission of 
8. electron from the atom 
9. energy by proton transition 
10. energy by electron transition 
11. neutrons from the atom 

12 If an element X of atomic number Z and mass number Y  is irradiated by an intense concentration of neutrons  the relevant nuclear equation is 

17. 90.0 g of MgCI was placed in 50.0cm3 of water to give a  2 

saturated solution at 298 K. If the solubility of the salt  is 8.0-mol dm-3at the same temperature, what is the  mass of the salt felt undissolve at the given  temperature? 

52. 52.0g B. 58.5 g 
53. 85.5g D. 88.5 g  

[Mg = 24,CI=35.5] 

18. Soap leather is an example of a colloid in which a A. Liquid is dispersed in gas 
19. Solid isdispersed in liquid 
20. Gas is dispersed inliquid 
21. Liquid isdispersed in liquid. 
22. The pH of a solution obtained by mixing 100cm3 of a 0.1  M HCI solution with 100cm3 of a 0.2 M solution of  NaOHis 
23. 1.3 B. 7.0 
24. 9.7 D. 12.7 
25. In the conductance of aqueous potassium 
    

A.xy X +1 nY – 1 X tetraoxosulphate (1V) solution, the current carriers are 

o 

Z+1 

the 

1. ions B. electrons 
   
2. Y X +1 nY + 1 X Z o Z 
3. hydrated ions D. hydrated electrons 
4. y X + 1 nY

Z+1 XZ+121. What volume of 0.1 mol dm-3solution of  

Z 

tetraoxosulphate (1V) acid would be needed to dissolve 

o 

o Z-1 X2.86 g of sodium trioxocarbonate (1V) decahydrate  n 

1. Z X + 1Y + 1

Y 

13. The property used in obtaining oxygen and nitrogen  industrially from air isthe 
14. boiling point 
15. density 
16. rate of diffusion 
17. solubility 
18. Excess phosphorus was burnt in gasjar and the residual  gas passed successively over concentrated KOH  solution and concentrated H2SO4 before being collected  in a flask. The gases collectedare 
19. carbon (1V) oxide nitrogen and the rare gases B. nitrogen (1V) oxide and the rare gases 
20. nitrogen and the rare gases 
21. carbon (1V) oxide nitrogen (1V) oxide and the  rare gases. 
22. Potassium tetraoxomanganate (v11) is often added to  impure waterto 
23. reduce organic impurities 
24. reduce inorganic impurities 
25. destroy bacteria and algae 

crystals? 

1. 20cm3 B. 40cm 

3 

1. 80cm3 D. 100cm3

[H=1, C=12, 0= 16, 

S= 32, Na =23] 

22. 1.2 of electricity are passed through electrolytic cells  containing Na+, Cu2+ and AI3+ in series. How many  moles of each metal would be formed at the cathode of  each cell? 
23. 0.6 mole of Na, 1.2 moles ofCu and 1.2 moles  ofAI 
24. 1.2 moles ofNa, 0.6 mole ofCu and 0.4 mole of  AI 
25. 1.3mmoles ofNa, 2.4moles ofCu and 2.4moles  ofAI 
26. 1.2 moles ofNa, 2.4 moles ofCu and 3.6 moles  ofAI 
27. What mass of gold is deposited during the electrolysis  of gold (111) tetraoxosulphate (V1)when a current of 15  A is passed for 193 seconds? 
28. 1.97g B. 3.94g 
29. 5.91g D. 19.70g  

[Au = 97, F=96 5000Cmol-1] 

24. remove permanent hardness. 24. Fe(s) + Cu 2+(aq) Fe2+(aq) +Cu(s) From the reaction above it can be inferred that 
    
25. The soil around a batterymanufacturing factory islikely  to contain a high concentration of 
26. Ca2+ salts B. Pb2+ salts 
27. Mg2+ salts D. AI3+ salts. 
28. Fe isthe oxidizing agent B. Fe is reduced 
29. Cu2+ loses electrons D. Cu2+ isthe oxidizing agent.
30. 2FeCI2(s) + CI2(g) 2FeCI3(s)

The reducing agent in the reaction above is 

1. FeCI2 B. CI2
2. FeCI3 D. Fe 
3. The reaction that is accompanied by a decrease in  entropy when carried out constant temperature is A. N2O4(g) NO2
4. N2 + 3H22NH3
5. CaCO3 CaO + CO2
6. 2N2H43N2+ 4H2O 
7. 32g of anhydrous copper 11 tetraoxosulphate (1V)  dissolved in 1 dm3 of water generated 13.0kJ of heat.  The heat of solution is 
8. 26.0 kJmol-1 B. 65.0kJ mol-1 C. 130.0kJmol-1 D. 260.0 kJ mol-1
9. 3CuO(s) +2NH3(g) 3Cu(s) + 3H2O(1) + N2(g) (i) 2NH3(s) + 3CI2(g) 6HCI(s) + N(1) + H2O 

(ii) 4NH3(s) + 3CI2(g) 6H2O(I) + 2N2(g) + HCl 

The reactions represented by the equations above demonstrate the 

1. basic properties ofammonia 
2. acidicproperties of ammonia 
3. reducing properties of ammonia 
4. oxidizingproperties of ammonia. 
5. A gas that trun a filter paper previously soaked in  lead ethanoate solution black is 
6. hydrogen chloride 
7. hydrogen sulphide 
8. sulphur (1V) oxide 
9. sulphur (VI) oxide. 
10. A solution containing chloride gives a white precipitate  with silver trioxonirate (V)solution. 
    
11. Mg2+(ag) + 2e–(aq) Eo(volts) = -2.370 The precipitate will be insoluble in dilute Zn2+(ag) + 2e–(aq)Zn(s) Eo(volts) = -0.763 A. HNO3 but solublein ammonia solution 
    

Cd2+  

Cu2+(ag) (ag) 

+ 2e– 

+ 2e–(aq) (aq) 

Cd(s) Cu(s) 

Eo(volts) = -0.403  Eo(volts) = +0.403 

1. HNO3 and in ammonia solution C. HCI but soluble in ammonia solution D. HCI and in ammonia solution. 
   

In the electrochemical series above the strongest  

reducing agent is 

36. Cu(s) B. Cd(s)
37. Zn(s) D. Mg(s)

In the diagram above, the activation energy for the  

backward reaction is 

1. +5kJ B. +15kJ 

In the experiment above, X could be a solution of A. Sodium, trioxonirate (V) and ammonium  chloride 

1. Sodium trioxonirate (111) and ammonium  chloride 
2. lead (11) trioxonirate (V) and copper turnings D. potassium, trioxonirate (V) and copper  turnings. 
3. +25kJ D. +30kJ 
4. The oxide that remains unchanged when heated in 
   
5. 2X(g)+ Y(g) Z(g)hydrogen is 
   

In the equation above the rate of formation of Z is  found to be independent of the concentration of Y and  to quadruple when rate equation for the reaction is A. R= k [X][Y] 

1. R= k [X]2[Y] 
2. R = k[X]2[Y]2
3. R = k[X]2[Y]0
4. CuO B. Fe2O3
5. PbO2 D. ZnO 
6. Whichof thefollowingisobservedwhenasolutionof  Iron(111) chlorideismixedwithasolutionof sodium  hydroxide? 
7. calcium B.aluminium 
8. iron D. zinc 
   

-1 39. Acommoncharacteristicsharedbyironandaluminum 

31. 2CI + 2H O 4HCI +O Ho = +115kJ mol 
    

2(g) 2 (g) (g) 2(g) 

In the above equilibrium reaction a decrease in  temperature will. 

1. favour the reverse reaction B. favour the forward reaction C. have no effect on the equilibriumstate D. double the rate of the reverse reaction 

is that both 

1. areextractedbyreductionmethods B. formonlybasicoxides 
2. showoxidationstatesof +2and+3 D. formsolublehydroxides.
3. Alloys are often used in preference to pure metals bacause A. metals are toohard 
4. metals are ductile 
5. metallic properties are improved in alloys D. alloys are a mixture of metals. 

OH 

41. CH3 CH2CHCH(CH3)2

The IUPAC nomenclature for the above compound is A. 4-methylpentan –3-ol 

1. 2-methylpentan –3-0l 
2. 3- methylpentan –3 –0l 
3. 1,1-dimenthylbutan-2-0l 
4. Dehydration of CH3 CH2 CH2 CH2 OH gives 
5. CH2 – CH – CH – CH2 – CH3
6. CH3CH– CH – CH2 – CH3
7. H – C – C – CH2 – CH3
8. CH3C-C-CH3
9. nCH2 =CH2 O2 (initiator) ( CH2 CH2 CH2 The above equation represents the manufacture of A. rubber B. polythene 
10. polystyrene D. butane 
11. One mole of a hydrocarbon contains 6 g of hydrogen.  If the molecular weight is 54, the hydrocarbon is an. A. alkanone B. alkane 
12. alkene D. alkyne 
13. The products obtained when a pure hydrocarbon is  burn in excess oxygen are 
14. carbon and hydrogen 
15. carbon and water 
16. carbon (11) oxide andhydrogen 
17. carbon (1V) oxide and water. 
18. How many structural isomers can be drawn for the non cyclic alkanol with molecular formula C4H10O 
19. 1 B. 2 
20. 3 D. 4 
21. On cracking medicinal paraffin, a gasis evolved which  gives a pop sound with a lighted splinter and a oily  liquid which decolourizes bromine solution is also  obtained. The products of the cracking are 
22. carbon (1V) oxide andalkyne 
23. carbon (11) oxide and alkane 
24. hydrogen gas and alkane 
25. hydrogen gas and alkane 
26. An example of aromatic compound is 
27. CH6H13OH 
28. C6H13CI 
29. C6H5OH 
30. C6H14
31. Terylene is synthesized from ethane –1, 2- diol and  benzene –1, 4- dicarboxylic acid by 
32. addition reaction 
33. consensation reaction 
34. elimination reaction 
35. substitution reaction. 
36. Which ofthe following istrue concerning the properties  of benezene and hexane? 
37. Both undergo subtitution reaction. 
38. Both undergo addtion reaction 
39. Both are solids 
40. Both can decolourize brominewater. 
    

Chemistry 1999 

1. 200 cm3 each of 0.1 M solution of lead (11) trioxonirate (V) and hydro chlorioc acid were mixed. Assuming that  lead (11) chloride is completely insoluble, calculate the  mass oflead (11) chloride that will be precipate. 
2. 2.78g B. 5.56g 
3. 8.34g D. 11.12g 

[Pb = 207, CI = 35.5, N = 14, O = 16] 

2. 56.00cm3 of a gas at s.t.p weighed 0.11 g, What isthe  vapour density of the gas? 
3. 11.00 B. 22.00 
4. 33.00 D. 44.00 

[Molar volume of a gas at s.t.p = 22.4 dm3] 

3. Which of the following gases will diffuse fastest  when passed through a porous plug? 
4. Propane B. Oxygen 
5. Methane D. Ammonia  

[H= 1, C= 12, N= 14, O = 16] 

4. Which of the following will have its mass increased  when heated in air? 
5. Helium B. Magnesium C. Copper pyrites D. Glass 
6. What is the temperature of a given mass of a gas  initially OoC and 9 atm, if the pressure is reduced to 3

atmosphere at constant volume? 

1. 91K B. 182K 
2. 273K D. 819K 

In the diagram above, the mixture of the two solid P  and Q can be separated by 

1. distillation 
2. fractional distillation 
3. crystallization 
4. fractional crystallization. 
5. Mg(s) +2HCl (aq) MgCl2(aq) + H2(g). From the  equation above, the mass of magnesium required to  react with 250cm3 of.5 M HCl is 
6. 0.3 g B. 1.5 g 
7. 2.4 g D. 3.0 g 

[ M = 27, Cl = 35.5] 

8. A gaseous metallic chloride MClx consist od 20.22%  of M by mass. The formula of the chloride is 
9. MCl B. MCl2
10. The element that is likely to participate in covalent  rather than ionic bonding is 
11. Z B. Y 
12. X D. W 
13. The least reactive elementsis 
14. W B. X 
15. Y D. Z 
16. ls22s22p63s23p63d74s2.An element with the electron  configuration above is a 
17. non-metal 
18. metal 
19. transition element 
20. group two element 
21. Given that electronegativity increases across a period  and decreases down a group in the periodic table, in  which of the following compounds will the molecules  be held together by the strongest hydrogen bond? A. HF(g) B. NH(g)
22. CH4(g) D. HCl(g)
23. 0.25 mole of hydrogen chloride was dissolved in distilled  water and the volume made up to 0.50dm3. If 15.00cm3  of the solution requires 12.50 cm3 of aqueous sodium  trioxocarbonate (1V0 for neutralization, calculate the  concentration of the alkalinesolution. 
24. 0.30 moldm-3 B. 0.40 moldm-3
    
25. MCl3 D. M2Cl6C. 0.50mol dm-3 D. 0.60 moldm-3 [M = 27, Cl = 35.5] 
26. In which of the following are water molecules in the  
    

most disorderlyarrangement? 

1. Ice at –10oC B. Ice atOoC 
2. Water at 100oC D. Steam at 100oC 
3. In order to remove one electron from 3s-orbital of  gaseous sodium atom, about 496 kJ mol-1 ofenergy  is required. This energy is referred to as 
4. electron affinity B. ionization energy C. activation energy D. electronegativity 
5. Nitrogen obtained from the liquefaction of air has a  higher density than that obtained from nitrogen  containing compounds because the former contains  A Water vapour B. Oxygen 
6. Carbon (1V) oxide D. Rare gases  Use the table below to answer question 13 and 14. 
7. The method that can be used to convert hard water  to soft water is 
8. Chlorination 

B Passage over activated charcoal 

1. the use of an ion exchange resin 
2. aeration 

Use the table below to answer question 13 and 14

18. The correct order of increasing oxidation number of  the transition metal ions for the compounds 

K Cr O , V O and KmnO is 

2 2 7 2 5 4 

1. V2O5 < K2Cr2O7, < KMnO4
2. K2Cr2O7, < KMnO4< V2O5
3. KMnO4 <K2Cr2O7, <V2O5
4. KMnO4< <V2O5< K2Cr2O7, 
5. The set of pollutants that is most likely to be  produced when petrol is accidentally spilled on  plastic materials and ignited is 
6. CO, CO2 andSO2
7. CO, HCl andSO2
8. CO, CO2 andHCl 
9. SO2, CO2 and HCl 
10. What is observed when aqueous solution of each of  tetraoxosulphate(V1) acid, potassium trioxides (V) and  potassium iodine are mixed together? 
11. white precipitate isformed 
12. a green precipitate isformed 
13. The mixture remains colourless 
14. The mixture turns reddish-brown. 
15. From the diagram above, the mass of crystals

deposited when 1 dm3 of a saturated solution of NaCl  is cooled from 80oC to 60oC is 

117. 117.00g B. 58.50g 
118. 11.70g D. 5.85g 

[Na = 23, Cl = 35.5] 

22. The solution with the lowest pH value is 
23. When a current 1 was passed through an electrolyte  solution for 40 minutes, a mass Xg of a univalent metal  was deposited at the cathode. What mass of the metal  will be deposited when a current 21 is passed through  the solution for 10 minutes? 
24. x/4 g B. x/2 g 
25. 2X g D. 4X g 
    
26. 5ml ofm/n HCl 30. RS(aq) + HF (aq)RF(s) + HS(aq) H =-65.7 kJ mol1. 
    
27. 10ml ofm/n HCl 
28. 15ml ofm/n HCl 
29. 20ml ofm/n HCl 
30. The solubility product of Cu(lO3)2 is 1.08 x 10-7.  Assuming that neither ions react appreciably with  water to form H+and OH–, what is the solubility of  this salt? 
31. 2.7 x 10-8mol dm-3
32. 9.0 x 10-8mol dm-3
33. 3.0 x 10-8mol dm-3
34. 9.0 x 10-8mol dm-3
35. The entropy and enthalpy of a system are a measure of A. degree of disorderliness and heat content  respectively 
36. heat content and degree of disorderliness  respectively 
37. heat content of a system only 
38. degree of disorderliness only. 
39. 2SO2(g) + O (g) 2NO2(g). In thechemical 2 

reaction above, the substance that will increase the  

From the equation above, it can be deduced that. A. the heat content of the reactants is lower than  that of the reactants ucts 

1. the heat content of the reactants is higher  than that of the products 
2. the reaction is slow 
3. a large amount of heat is absorbed. 
4. Which of the following statements is true of the  electrochemical series? 
5. Electropositivity of metals increase down the  series 
6. Electropositivity of non-metals decrease down  the series 
7. Electronegativity of non-metals increase down  the series 
8. Electropositivity of metal decreases down the  series 
9. The gasthat will form a white precipitate with acidified  silver trioxonirate (V)is 
10. NH3 B. SO2
    

rate of production of sulphur (V1) oxide is C. CO2 D. HCl 

1. manganese (1V)oxide 
2. finely dividedion 
3. vanadium (V0oxide 
4. nickel 
5. N2O4(g) 2NO2g). Increases in total pressure of  the equilibrium reaction abovewill 
6. Produce more of NO2(g) in the mixture 
7. Convert all of N2O4(g) to NO2(g) 
8. Have no effect on the concentrations of N2O4(g) andN2O4(g) 
9. Produce more odf N2O4g) in th mixture 
10. What quantity of electricitywill liberate 0.125 mole of  oxygen molecules during the electrolysis of dilute  sodium chloride solution? 
11. 24 125 coulombs 
12. 48 250 coulombs 
13. 72 375 coulombs 
14. 96 500 coulombs  

[F= 96 500Cmol-1] 

28. X +Y Z. The rate equation for the  chemical reaction above is – [X]=[X]2[Y] 

t  

The overall order of the reaction is 

1. 0 B. 1 
2. 2 D. 3 
3. Chlorine bromine and iodine resemble one another in  that they 
4. dissolve in alkalis 
5. react violentlywith hydrogen without heating C. are liquids 
6. displace one another from solutions of their  salts. 
7. The salt that reacts with dilute hydrochloric which  decolourizes acidified purple smelling gas which  decolourizes acidified purple potassium  tetraoxomanganate(V11) solution is 
8. Na2SO4 B. Na2SO3
9. Na2S D. Na2CO3
10. A pair of compounds that can be used to generate a  gas which physiological effect on human beings is A. sodium trioxonirate(V) and calcium chloride B. sodium dioxonitrate 

(111) and ammonium chloride 

1. sodiumtrioxonirate(V) an ammonium chloride D. sodium dioxonitrate (11l) and potassium  chloride. 
2. Hydrogen is used in oxy-hydrogen flames for melting  metals because it 
3. evolves a lot of heat when burnt 
4. combines explosively withoxygen 
5. is a very light gas 
6. is a rocketfuel.

In the diagram above Y is mixture of 

1. Calciumhydroxide and ammonium chloride B. Calcium hydroxide and sodiumchloride(V) C. Sodiumchlorideand ammoniumtrioxonirate(V) D. Sodium dioxonitrate(lll) and ammonium  chloride. 
2. What properties of duralumin make it more useful than  its constituent metals? 
3. it is heavy with a high melting point 
4. it is malleable andhas high density 
5. it is strong and light 
6. it is hard and ductile 
7. The pair ofmetalsin the reactivity seriesthat are usually  extracted by the electrolysis of their ores is 
8. Magnesium and zinc 
9. Magnesium andcalcium 
10. Copper and zinc 
11. Lead and calcium 
12. A metal that can be extracted from cassiterite is A. calcium B. magnesium C. tin D. copper 
13. Which of the following metals is passive to  concentrated trioxonirate(V) acid? 
14. iron B. tin 
15. copper D. zinc 
16. The hydrocarbon the burns in air with a sooty flameis A. C6H6 B. C3H6
17. C4H10 D. C6H6
18. 2-methylprop-1-ene is an isomerof 
19. but-2-ene 
20. pent-l-ene 
21. 2-methylbut-ene 
22. 2-methylbut-l-ene 
23. Which of the following is a solvent for perfumes?  A C5H12 B. C4H6
24. CH3COOH D. C2H5OH 
25. When excess ethanol is heated to 145oC in the presence  of concentrated H2SO4 the product is 
26. ethyne 
27. diethyl sulphate 
28. diethyl ether 
29. acetone 
30. How many grammes of bromine will saturate 5.2 g of  but-l-ene-3-yne? 
31. 64.0g B. 48.0 g 
32. 32.0g D. 16.0 g 

[C = 12, H= 1, Br = 80] 

47. Polyvinyl chloride is used to produced 
48. bread B. pencils C. ink D. pipes 
49. An organic compound that does not undergo a reaction  with both hydrogen cyanide and hydroxylamine can  be an 
50. alkenes B. alkanal 
51. alkanone D. Alkanoic acid 
52. When two end alkyl groups of ethyl ethanoate are  interchanged, the compound formed is known as A. methylethanoate 
53. ethyl propionate 
54. methylpronoste 
55. propel ethanoate. 

Which of the compounds above would react to take  up two molecules of bromine during bromination? A. 1 only 

1. 111 only 
2. 1 and 11only 
3. 11 and 111only
   

Chemistry 2000 

1. A mixture of iodine and sulphur crystals can be  separated by treatment with 
2. water of filter offsulphur 
3. carbon (1V) sulphide to filter offiodine C. ethanoic acid to filter offsulphur 
4. Elements in the same group have the  number of electron shells 
5. The non-metallic properties of the elements  tent to decrease across each period 
   
6. methanol to filter offiodine 10. The electron configuration of X2+ ion is 22
7. ls2 2s2 2p6 3s2 3p6 4s2 3d2
   
8. Sieving is a technique used to separate mixtures  containing solid particles of 
9. smallsizes B. large sizes 
10. different sizes D. the same size 
11. Which of the compounds is composed of Al, Si, O  and H? 
12. Epson salt B. Limestone 
13. Clay D. Urea 
14. 50cm3 of carbon (11) oxide was exploded with 150cm3 of air containing 20% oxygen by volume, which of  the reactants was in excess? 
15. Carbon (11) oxide 
16. Carbon (1V) oxide 
17. Oxygen 
18. Nitrogen 
19. Howmany moles of HCl will be required to react with  potassium heptaoxodichromate (V1) to produce 3  moles of chlorine? 
20. 14 B. 12 
21. 11 D. 10 
22. The ratio of the initial to the final pressure of a given  mass of gasis 1:1:5. Calculate the final volume of the  gas if the initial volume was 300cm3 at the same  temperature. 
23. 120cm3 B. 200cm3
24. 450cm3 D. 750cm3
25. The partial pressure of oxygen in a sample of air is  452mm Hg and the total pressure is 780mmHg. What  is the mole fraction ofoxygen? 
26. 0.203 B. 0.579 
27. ls2 2s2 2p6 3s2 3p6 4s2 3d1
28. ls2 2s2 2p6 3s2 3p6
29. ls2 2s2 2p6 3s2 3p6 4p2
30. Which of the following types of bonding does not  involves the formation of new substance? 
31. Metallic B. Covalent 
32. Co-ordinate D. Electrovalent 
33. The knowledge of half-life can be used to A. create an element 
34. detect an element 
35. split an element 
36. irradiate anelement 
37. The shape of CO ,H O and CH respectivelyare 2 2 4 
38. bent linear and tetrahedral 
39. bent tetrahedral and linear 
40. linear bent and tetrahedral 
41. tetrahedral, linear and bent. 
42. The distance between the nuclei of chlorine atoms in  a chlorine molecule is 0.914 nm. The atomic radius of  chlorine atom is 
43. 0.097nm 
44. 0.914nm 
45. 2.388nm 
46. 2.388nm 
47. The noble gas, argon, is used for 
48. electric arewelding 
49. welding brass 
50. underwater welding 
51. steal welding 
    
52. 2.030 D. 5.790 16. A side effect of soft water is that A. it gives offensive taste 
    
53. The fundamental difference between the three states  of matter isthe 
54. shape of theirparticles 
55. number of particles in each state 
56. shape of the container they occupy 
57. degree of movementof their particles 
58. Which of the following the following statements is  correct about the periodic table? 
59. Element in thesame period have the same  number of valence electrons 
60. The valence electrons of the elements in the  same period increase progressively across  

the period 

1. excess calcium sprecipitate 
2. it attacks lead contained in pipes 
3. it encourages the growth of bacteria 

17 Water molecules can be ligands especially when they  are bonded to. 

1. alkaline earthmetals 
2. alkalimetals 
3. transition metals 
4. group V11elements 
5. The air pollutant unknown in nature is A. NO B. CO 
6. HCHO D. DDT 
7. 10dm3 of distilled water used to wash 2.0 g of a  precipitate of AgCl. If the solubility product ofAgCl  is 2.0 x10-10 moldm-6, what quantity of silver waslost  in the process? 
8. 2.029 x10-3moldm-3
9. 1.414 x 10-3 mol dm-3
10. 2.029 x 10-5 mol dm-3
11. 1.414 x 10-5 mol dm-3
12. Hydration of ions in solution is associated with A. absorption ofheat 
13. reduction of heat 
14. conduction ofheat 
15. liberation of heat 

The diagram above is the solubility curve of solute, X. Find the amount of X deposited when 500cm3 of  solution of X is cooled from 60oC to 20oC 

1. 0.745mole B. 0.950mole 
2. 2.375moles D. 4.750moles. 
3. HCl(aq)+ H2O(1)+ 

3 (aq) + Cl–(aq) 

H O 

electricity required to discharge zinc 

1. 0.965 x104C B. 4.820x 104C C. 9.650 x104C D. 48.200x 104C [F = 96 500 C mol-1] 
2. Given that M is the mass of substance deposited in  an electrolysis and Q the quantity of electricity  consumed, then Faraday’s law can be written as A. M = Z  

Q 

1. M =Q

Z 

1. M = Z  

2Q 

1. M =QZ 

28 0.46g of ethanol when burned raised the temperature  of 50 g water by 14.3 K. Calculate the heat of  

combustion of ethanol. 

1. +3 000 kJmol-1
2. +300kJ mol-1
3. -300kJ mol-1
4. -3 000 kJmol-1

[C = 12, O = 16, H = 1] 

Specific heat capacity of water = 4.2 jg-1K-1 

29. Powdered marble reacts with hydrochloric acid  solution than the granular form because the  

powdered form has 

1. more molecules 
2. more atoms 
3. large surface are 
4. relatively largemass 

In the reaction above, Cl A. Conjugate acid B. Acid 

1. Conjugate base D. Base. 

(aq) is the 30. The graph that describes a zero order reaction is A. Rate 

23. In which order are the following salts sensitive to  light? 
24. Agl ›AgCl›AgBr 
25. AgCl ›Agl›AgBr 
26. AgBr ›AgCl ›AgI 
27. AgCl ›AgBr ›AgI 
28. Thee pOH of a solution of 0.25 mol dm-3 of  hydrochloric acid is 
29. 12.40 B. 13.40 
30. 14.40 D. 14.60 
31. MnO + 8H+’! Mn2+(aq)+4H O 4(aq) (aq) 2 (1) 

Y in the equation above represents 

1. 2e 
2. 3e 
3. 5e 
4. 7e 
5. Rate
6. Rate
7. Rate

Conc. Conc. 

Conc. 

26. ½Zn2+(aq)+e- ½Zn(s) Conc. In the reaction above, calculate the quantity of
    
27. A. increase the quantity of N2
28. increase the yield ofNO 
29. decrease the yield of NO 
30. decrease the quantity of O2
31. For a reaction in equilibrium, the species involved in  the equilibrium constant expressionare 
32. gaseous and solid species 
33. liquid and solid species 
34. solid and dissolved species 
35. gaseous and dissolved species 
36. A phenomenon where an element exists in different  forms in the same physical state is known as 
37. isomerism B. amorphism 
38. allotropy D. isotropy 
39. The substance often used for vulcanization of rubber is A. chlorine 
40. hydrogen peroxide 
41. sulphur 
42. tetraoxosulphate (V1) acid 
43. A gas that is not associated with global warming is A. CO2B. SO3
44. CH4 D. H2
45. The refreshing and characteristics taste of soda water  and other soft drinks is as a result of the presence in  them of 
46. carbon(1V)oxide 
47. carbon(11) oxide 
48. soda 
49. glucose 
50. A form of carbon used for absorbing poisonous gases  and purification of noble gases is 
51. wood charcoal’ 
52. animal charcoal 
53. carbon fibres 
54. carbon black. 
55. Synthesic gas is a mixture of 
56. CH4 andH2O 
57. CH4 and H2
58. CO2 and H2
59. CO and H2
60. Potassium vapour burns with a 
61. blue-flame 
62. brick-red flame 
63. violet flame 
64. golden-yellow flame 
65. A common characteristics of copper andsilver in their  usage as coinage metals is that they 
66. have high metalliclustre 
67. are not easily oxidized 
68. are easily oxidized 
69. are not easily reduced 
70. Haematite is an ore of 
71. Zinc B. Lead 
72. Iron E. copper. 
73. The least easily oxidized ofthe metals below is A. Ca B. Na 
74. Zn D. Al 
75. The repeating unit in natural rubber is 
76. alkynes 
77. isoprene 
78. n-propane 
79. neoprene 
80. Unsaturated organic compounds are identified by  decolourization of. 
81. silver bromide and potassium  tetraoxomanganate(v11)solution 
82. bromine water and acidified potassium  tetraoxomanganate(V11)solution 
83. silver bromine solution and bromine water D. bromine water and alkaline potassium  tetraoxomanganate (V11)solution. 
84. The conditions necessary for thee extraction of a water  molecule form two molecules of ethanol are. 
85. less acid and a lower temperature 
86. excess acid and a lower temperature 
87. excess acid and a higher temperature 
88. less acid and a higher temperature. 
89. The chlorinated alkane often used industrially  to remove grease is 
90. tetrachloromethane 
91. chloromethane 
92. trichloromethane 
93. dichloromethane. 
94. The reaction of carbide with water gives A. ethyne B. ethane 
95. ethane D. Ethanal  

O 

48. CH3-CH2-C–OCH2CH3

The compound above is an 

1. ether B. ester 
2. alkanal D. alkanol 
3. Alkanone are generally obtained by the oxidationof A. primary alkanols 
4. secondary alkanols 
5. tertiary alkanols 
6. alkanoic acid 
7. Sucrose is made up to 
8. glucose and glucose 
9. glucose and fructose 
10. fructose and fructose 
11. galactose and glucose.
    

Chemistry 2001 

1. 25cm3 of a gas X contains Z molecules at 15oC 
   

and 75 mm Hg. How many molecules will 25cm3 of another gas Y contain at the same temperature  and pressure? 

A, 2Y, B. 2Z. C. Y, D. Z. 

2. What mass of water is produced when 8.0g of  hydrogen reacts with excess oxygen? 
3. 72.0g, B. 36.0g, C. 16.0g, D. 8.0g 

Use the graph below to answer questions 3 and 4

3. How long does it take all the solid to melt? A. 6.0mins, B. 3.0mins, 
4. 2.5mins, D.1.0min 
5. If the gas is cooled, at what temperature will it  start to condense? 
6. 175oC, B. 250oC, 
7. 125oC, D. 150oC 
8. Four elementsW,X,Yand Z have atomic numbers  2,6,16 and 20 respectively. Which of these  

elements is ameal? 

1. X, B. Z, 
2. W, D. Y 
3. The diagram above represents the formation of A. a metallic bond, B. a covalent bond, 
4. an electrovalent bond. 

D a coordinate covalent bond 

7. An element X with relative atomic mass 16.2 contains  two isotopes 168X with relative abundance of 90% and m8X 

with relative abundance of 10%. The value of m is  A. 14, B. 12, 

1. 18, D. 16 
2. Cancerous growth are cured by exposure to A. x-rays, B. betta-rays, 
3. alpha-rays, D. gamma-rays 
4. Which of the following statement is correct about the  average kinetic energy of the molecules of agas? A. it increases with increase in pressure, 
5. it increases with increase in temperature, 
6. It increaseswith increase in volume, 
7. It increases at constant pressure. 
8. Millikan’s contribution to the development of atomic  theory is the determinationof 
9. positive rays, B. cathode rays, 
10. charge to massratio , D. charge onelectron. 
11. A particle that contains 9 protons, 10 neutrons and 10  electrons is 
12. positive ion B.neutral atom of a metal C. neutral atom of a non-metal 
13. negative ion. 
14. An oxide XO2 has a vapour density of 32. What is  the atomic massof X? 
15. 20 
16. 32 
17. 14 
18. 12 
19. The chemical used for coagulation in water  purification is 
20. copper tetraoxosulphate (VI) 
21. sodium tetraoxosulphate (VI) 
22. aluminium tetraoxosulphate(VI) 
23. calcium tetraoxosulphate (VI) 
24. Environment pollution is worsened by the release  from automobile exhaustsof 
25. heavy metals B. water vapour C. smoke D. steam 
26. Phosphorus is stored under water to prevent it from A. smelling B. dehydrating C. catching fire D. becoming inert 
27. Pure solvents are obtained by 
28. evaporation B. extraction 
29. condensation D. distillation
30. d K 

At what temperature are the solubilities of Lan  the same? 

26. As the concentration of an electrolyte reduces, the  conductivity 
27. decreases B. increases 
28. reduces to zero D. is unaffected. 27. C(s) + 2S(g) CS2 H =89kJmol-1 The chemical equation above implies that 
29. 89kJ of energy is absorbed 
30. each of carbon and sulphur has 89 kJ of energy C. both carbon and sulphur contribute 89kJ of energy 
    
31. 750C C. 900C 
32. D. 

1000C 820C 

1. 89 kJ of energy is released 
   
2. If 1 dm3 of a saturated solution of L at 600C is cooled  to 250C, what amount in mole willseparate? 
3. 0.25 B. 0.50 
4. 0.75 D. 1.00 
5. Deliquescent substance are used for 
6. drying B. melting 
7. wetting D. cooling 
8. What is the decrease in volume of air when  pyrogallol is shaken with 30.00cm3 of air?  
9. 0.63cm3 B………………….0.06cm3
10. 15.00cm3 D……………..6.30cm3
11. The pollution from petroleum spillage in rivers and  takes can best be dispersed by 
12. passing of ships through the area 
13. pouring detergents 
14. pouring organic solvents 
15. evaporation 
16. 3Cu(s) + 8HNO3(aq) 3Cu(NO3)2(aq) + 4H20(i)+2NO(g) 

In the equation above, copper is 

1. a base
2. an oxidizing agent 
3. a reducing agent 
4. an electron acceptor. 
5. NH3(g)+ HCI(g)’! NH4CI(s) 

The entropy change in the system above is 

1. zero B. indeterminate C. positive D. negative 
2. What current in amperes will deposit 2.7gof  aluminum in 2hours? 
3. 32 B. 16 
4. 8 D. 4 

{AI= 27, F 96 500C mol-1 

25. 2SO2(g)+O2(g) 2SO3(g) 

The equilibrium constant for the reaction above is increased by 

1. increasing the pressure of the system
2. increasing the temperature of the system 
3. increasing the surface area of the vessel 
4. the addition of a catalyst to the system 
5. Which of the following best explains the increase in  the rate of a chemical reaction as the temperature  rises? 
6. A lower proportion of the molecules has the  necessaryminimum energy to react 
7. The bonds in the reacting molecules are more  readily broken 
8. The collision frequency of the molecules  

increases 

1. The molecular collisions become more violent. 
2. In which of the following reaction have the oxidation  number of nitrogen increased? 
3. 2NO(g) +Br2(l) 2NOBr(1) 
4. FeSO4 (aq) + NO(g) Fe(NO)SO4(s) 
5. 2NO(g) + CI2(g) 2NOCI(l) 
6. 2NO(g) + O2(g) 2NO2(g) 
7. P(g) + Q(g) 3R(s)+S(g)

which of the following will increase the yield of R? A. Removing some S 

1. Using a larger closed vessel 
2. Adding a positive catalyst 
3. Increasing the temperature 

31 Ethanoic acid is 

1. tribasic B. unionizeable C. dibasic D. monobasic 
2. A metal M displaces zinc from zinc chloride solution.  This shows that 
3. M is more electronegative than zinc 
4. Zinc is above hydrogen in the series 
5. Electron flowfrom zinc to M 
6. M is more electropositive that zinc 
7. In which of the following reactions does reduction take  place? 
8. 2O2-——————O2 +4e
9. Fe2+– e———————Fe3+
10. 2H+-——————H 

2 

1. Cr – 2e———————Cr2+
2. When H is negative, a reaction is said to be A. Endothermic B. Exothermic 
3. Rerverisble D. Ionic.

ethyne? 

1. sp B. sp3
2. sp2d D. sp2
3. Protein in acid solution undergo 
4. Polymorphism 
5. Hydrolysis 
6. Fermentation 
7. Substitution 
8. Fermentation isthe 
9. breaking down of carbohydrate to glucose B. breaking down of sugar to carbohydrate C. conversion of sugar to alcohol in the presence  of yeast 
10. conversion of alcohol to sugar in the presence  of yeast. 
11. Catalytic hydrogenation of benzene produces 

function as 

1. a reducing agent B. a catalyst 
2. a dehydrating agent D. an oxidizing agent 
3. During the vulcanization ofrubber sulphur is added to A. lengthen the chain of rubber 
4. break down rubber polymer 
5. act as a catalyst 
6. bind rubber molecules together 
7. When sodium reacts with water,the resulting solution is A. Alkaline B. Acidic 
8. Neutral D. Weakly acidic. 
9. The general formula for the alkanalsis 
10. RCOOR1 B. R CO 

1 

1. RCHO D. ROH 
2. Which of the following metals burns with a brick red  flame? 
3. Ca B. Na 
   
4. Cyclohexene B. Oil C. Mg D. Pb C. Margarine D. Cyclohexane. 
   
5. A characteristics reaction of the compounds with the  general formulaCn2n is 
6. Substitution B. Esterification C. Decarboxylation D. Polymerization 
7. When chlorine is passed into water and the resulting  solution exposed to sunlight, the products formed are A. Chlorine gas and hydrogen 
8. Hydrochloric acid and oxygen 
9. Chlorine gas and oxochlorate (1) acid 
10. Oxygen and oxochlorate (1) acid 
11. The pair of organiccompounds that are isomers is A. But – 1-ene and but – 2-ene 
12. Ethanol and propanone 
13. Trichlorometheane and tetrachloromethane D. Benzene and methylbenzene 
14. C12H22O(s) + H2SO4(aq)———12C(s) + 11H2O(l) + H2SO4(aq) In the reaction above, tetraoxosulphate (VI) acid 
15. The gas that can best be collected by downward  displacement of airis 
16. Chlorine B. Sulphur (IV)oxide C. Carbon (IV) oxideD. Ammonia. 
17. A trihydric alkanol is 
18. Phenol B. Glycol 
19. Glycerol D. Ethanol 
20. The main impurity in iron ore during the extractionof  iron is 
21. Calcium trioxosilicate 
22. Silicon (IV) oxide 
23. Sulphur (II) oxide 
24. Carbon (IV) oxide. 
25. A burning candle produces water and 
26. carbon (IV) oxide 
27. carbon (IV) oxide 
28. oxygen 
29. hydrogen. 
30. molecular formula C. structuralformula D. general formula 

Chemistry 2002 

1. The formula CH2O for ethanoic acid is regarded as its 
2. edmispsoirlivcealifnoremacuhlaother in the column 
3. move at different speeds in thecolumn 
4. react with the solvent 
5. react with each other. 
6. Which of the following gases contains the least number  of atoms at s.t.p? 
7. 7 moles ofargon 
8. 4 moles ofchlorine 
9. 3 moles ofozone 
10. A compound contain 31.91% potassium, 28.93%  chlorine and the rest oxygen. What is the chemical  formula of thecompound? 
11. KClO B. KClO2
    
12. 1 mole of butane C. KClO3 D. KClO4
    
13. The chromatographic separation of ink is based on the  ability of the components to 
14. A little quantity oftrichloromethane (b.pt.60oC) was added  to a large quantity of ethanol ((b.pt.78oC). The most  probable boiling point of the resultant mixture is from. A. 60oC – 78oC B. 69 oC – 70oC
15. 70oC- 74oC D. 82oC – 84oC 
16. The gas that gives brown colouration in brown ring  test is 
17. CO B. NO 
18. CO2 D. NO2
19. Which ofthe following gives a precipitate when treated  with NaOH solution? 
20. NH4Cl B. Na2CO3
21. AlCl3 E. CH3COONa 
22. The reaction of an alkene with hydrogen in the presence  of a catalyst is 
23. a nucleophilic reaction 
24. an addition reaction 
25. a substitution reaction 
26. an oxidative reaction 
27. A rock sample was added to cold dilute HNO3. The gas  evolved was passed into a solution of acidified K2Cr2O7 and the solution turned green. 

The rock sample contains. 

1. SO 2- B. SO 2-

4 3 

1. NO3- D. Cl
2. The intermediate product formed when ethanol is  progressively oxidized to ethanoic acid with potassium  heptaoxodichromate (V1)is 
3. methanal B. propanal 
4. The boiling of fat and aqueous caustic soda is referred to  as. 
5. acidification B. hydrolysis 
6. saponification D. esterification. 
7. Ordinary glass is manufactured from silica, CaCO3and A. NaHCO3 B. K2SO4
8. K2CO3 D. Na2CO3
9. OH 

CH3– C-CH2-CH3 

CH3 

The major product of the dehydration of the compound above is 

A H 

CH3– C-CH2-CH3 

CH 

3 

1. CH3– C= CH2-CH3

CH3 

1. ethanal D. butanal C. CH3 – CH-CH-CH23
   
2. CH3 CH3 CH2–C-H 

OH 

The compound above is a 

CH3 

CH3 CH2CH2CH3  CH2

1. primary alkanols 
2. secondary alkanols 
3. tertiary alkanols 
4. glycol 

12, A red precipitate of copper (1) carbide is formed when  ammonium solution copper (1) chloride is introduced  into. 

1. CH3 – C =C -CH3
2. CH3 -CH2 -C a= CH3
3. CH2 =CH – CH2CH3

D CH3CH2 CH2CH3 

13. The most important use of hydrogen is in the A. manufacture of methyl alcohol 
14. manufacture of ethyl alcohol 
15. hydrogenation of oils 
16. manufacture ofammonia 
17. Which ofthe following polymersissuitable for packaging  and electrical insulation? 
18. Polyethene B. Polystyrene 
19. Polyamide D. Polycarbonate. 
20. The number of isomers formed byC6H14 is A. 2 B. 3 
21. 4 D. 5 
22. Which of these pairs are synthetic and natural  macromolecules respectively? 
23. Nylon and polyethylene, creatine and  haemoglobin 
24. Nylon and creative, polyethylene and  haemoglobin 
25. Polyethylene and creatine, nylon and  haemoglobin 
26. Haemoglobin and nylon, creatine and  polyethylene 
27. An example of an element that can catenate is A. nitrogen B. chlorine 
28. carbon D. bromine 
29. Ethanol can easily be produced by 
30. distillation of starch solution 
31. catalyst oxidation ofmethane 
32. destructive distillation of wood 
33. fermentation ofstarch. 
34. Hydrogen is readily released when dilute hydrochloric  acid reacts with 
35. Ag B. Au 
36. Cu D. Na 
37. Which of the following statement is true of a proton? A. The mass of a proton is 1.0008 g 
38. The mass of a proton is 
39. The mass of proton is 1840 times the mass of  an electron 
40. The total mass of the proton in a particular  nucleus is always half the nucleus is always  

half the nuclearmass. 

1. 0.44 atmosphere 
2. 0.55 atmosphere 
3. When H2S is passed into a solution ofiron (iii) chloride,  the solution turns 
4. brown B. pale green 
5. colourless D. pale red. 
6. Which ofthe following equationsshowsthat a reaction  is inequilibrium? 
7. G = H– T S 
8. G <O 
9. G =O 
10. G >O 
    
11. 14 C X + B 33. Cu S + O 2Cu + SO 6 2 (s) 2(g) (s) 2(g) 

X in the equation above represents. What is the change in the oxidation number ofcopper A. 14 N B. 13 C in the reaction above? 

7 

6 

1. 12 C D. 12 B A. 0 to+2 
   

6 5 

25. A gas X diffuses twice as fast as gas Y under the same condition. If the relative molecular mass of X is 28,  calculate the relative molecular mass of Y 
26. 14 B. 56 
28. 112 D. 120 
29. Which of the following chlorides would exhibit the least  ionic character? 
30. LiCl B. MgCl2
31. CaCl2 D. AlCl3
32. A fixed mass of gas has a volume of 92 cm3at 3oC. What  will be its volume at 18oC if the pressure remains  constant? 
33. 552.0cm3 B………………….97.0 cm3 C. 87.3cm3 D. 15.3cm3
34. The processes which return carbon(1V) oxide to the  atmosphere include 
35. Photosynthesis, respiration and transpiration B. Respiration, decay and combustion 
36. 0 to+1 
37. +1 to0 
38. +2 to+1

In the diagram above, the curve that represent  production of oxygen gas from the decompositi KClO3 in the presence of MnO2 catalyst is A. P 

1. Q 
2. R 
3. S 

s the  on of 

1. Photosynthesis, decay and respiration 
2. Ozone depletion, combustion and decay. 
3. The postulate of Dalton’s atomic theorywhich still hold  is that 
4. all element are made of small indivisible  particles 
5. particles of different elements combine in a  simple whole numberration 
6. atoms can neither be created nor destroy ed D. the particles of the same element are exactly  alike 
7. If 0.75 mole of cyclopropane and 0.66 mole of oxygen are  mixed in a vessel with a total pressure of 0.7 atmosphere,  what is the partial pressure of oxygen in the mixture? A. 0.22 atmosphere 
8. 0.33 atmosphere 
9. In the reaction E + F G + H, the backward reaction  is favoured if the concentration of 
10. E isreduced 
11. G isreduced 
12. F is increases 
13. E isincreased 
14. The products of the electrolysis of dilute sodium  hydroxide using platinum electrodes are 
15. sodium metal and oxygen gas 
16. hydrogen and oxygen gases 
17. water and hydrogen gas 
18. water and sodiummetal 
19. PCl5(g) PCl3(g) + Cl2(g)

In the reaction above, a decrease in pressure will A. increase the yield ofPCl3 

1. increase the yields ofPCl5
2. accelerate the reaction 
3. decelerate the reaction 
4. The Arrhenius equation expresses the relationship  between the speed of a reaction and its 
5. catalyst 
6. activation energy 
7. molecular collisions 
8. heat of reaction 
9. What amount of mercury would be liberated ifthe same  quantity of electricity that liberated 0.65 g of zinc is  supplied? 
10. 8.04g B. 4.02 g 
11. 2.01g D. 1.00 g 

[Zn = 65, Hg = 201] 

40. When dissolved in water, NaOH flakesshow A. a rapid reaction 
41. a slow reaction 
42. an exothermic change 
43. an endothermic change 
44. Steam changes the colour of anhydrous cobalt (11)  chloride from 
45. blue to white B. white to green C. blue to pink D. white to red 
46. Which of the following solutions containing only  hydroxyl ions will liberate hydrogen gas when reacted  with magnesium metal? 
47. 1.0 x 10-12 mol dm-3 B. 1.0 x 10-6 mol dm-3 C. 1.0 x 10-4 mol dm-3 D. 1.0 x 10-2 mol dm-3
48. The solubility of a salt of molar mass101 g at 20oC is  0.34mol dm-3. If 3.40 g ofthe salt is dissolved completely  in 250 cm3 of water in beaker, the resulting solution is A. saturated B. unsaturated 
49. supersaturated D. a suspension. 
50. 25 cm3 of a 0.2mol dm-3solution of Na CO requires 20cm3 2 3 

of a solution of HCl for neutralization. The concentration  of the HCl solution is 

1. 0.2mol dm-3 B. 0.4mol dm-3 C. 0.5mol dm-3 D. 0.6mol dm-3
2. When a salt loses its water of crystallization to the  atmosphere exposure, the process is said to be 
3. effervescence B. efflorescence C. fluorescence D. deliquescence 
4. Three drops of 1.0 mol dm-3solution of NaOH are added  to 20 cm-3 of a solution of pH 8.4. The pH of the resulting  solution will be 
5. less than 8.4 B. greater than 8.4 C. unaltered D. close to that of pure water. 
6. Tetraoxosulphate (Vl) acid burnsthe sk9in by A. dehydration B. hydrolysis 
7. hydration D. heating 
8. The substance least considered as a source of  environmental pollution is 
9. uranium 
10. lead compounds 
11. organphosphourous compounds 
12. silicateminerals. 
13. The propertywhich makes alcoholsolublein water isthe A. ionic character 
14. boiling point 
15. covalent nature 
16. hydrogen bonding 
17. The furring of kettlesis caused bythe presence in water  of 
18. calcium hydrogentrioxocarbonate (1V) 
19. calcium trioxocarbonate(1V) 
20. calcium tetraoxosulphate (V1) 
21. calcium hydroxide 
22. What volume of oxygen is produced from the 
23. Burning kerosene B. Freezing ice-cream 

Chemistry 2003 

decomposition of 2 moles of KClO3 at s.t.p  

22. 22.4dm3 B. 33.6 dm3
23. 44. 8 dm3 D. 67.2dm3

[Molar volume of a gas s.t.p = 22.4 dm3] 

1. evaporation D. absorption 
2. Which of the following is a physical change? 
3. Exposing white phosphorus toair 
4. Dissolving calcium inwater 
5. What is the percentage by mass of oxygen in  Al2(SO4)3.2H2O? 
6. 14.29% B. 25.39% 
7. 50.79% D. 59.25%  

[A= 27, S=32, H=1,O=16] 

4 The filter in a cigarette reducesthe nicotine content by A. burning B. adsorption 

5. 3Cu + pHNO33Cu(NO3)2 + 4H2O +xNO In the equation above, the values of p and x respectively 

are 

1. 1 and 3 B. 2 and3 
2. 6 and 2 D. 8 and2 
3. Neutral atoms of neon with atomic number 10 have the  same number of electrons as 
4. O2+ B. Ca2+
5. K+. D. Mg+
6. The noble gases owe their inactivity to A. octet configuration 
7. cyclic shape 
8. hexagonal shape 
9. obtuse configuration 
10. According to the kinetic theory, an increase in  temperature causes the kinetic energy of particles to A. decrease B. increase 
11. remain constant D. be zero 
12. 1. H =Is1

II N =Is22s22p3 

III O =Is22s22p4 

IV Zn = Is22s22p63s23p64s23d10 

From the above, which ofthe following pairsislikely to  be paramagnetic? 

1. I and II B. I and III 
2. I and IV D. I andIV 
3. A gas exerts pressure on its container because A. some of its molecules are moving faster than  others 
4. of the collision of the molecules with each  other 
5. of the mass of the molecules of gas 
6. the molecules of a gas collide with walls of the  container. 
7. When cathode rays are deflected onto the electrode of  an electrometer, the instrumentbecomes 
8. negatively charged B. positively charged C. neutral D. bipolar 
9. The weakest attractive forces that can be observed  between two molecules is 
10. ionic B. covalent 
11. coordinate covalent 
12. Van der Waals. 
13. A consequence of global warmingis 
14. air pollution 
15. water pollution 
16. 0.97g B. 9.70g 
17. 19.42g D. 97.10g 

[K CrO = 194.2 g mol dm-1] 

2 4 

18. Farmlands affected by crude-oil spillage can be  decontaminated by 
19. adding acidic solution 
20. using aerobic bacteria 
21. pouring water on the affected area 
22. burning off the oil from the area. 
23. When 10g of sodium hydroxide is dissolved in 100cm3 of water, the solution formed is approximately 
24. 0.01mol dm-3 B. 0.10moldm-1 C. 0.25mol dm-1 D. 0.50 mol dm-1 [Na = 23, H=1, O = 16] 
25. A change in the temperature of a saturated solution  disturbs the equilibrium between the 
26. dissolved solute and the solvent 
27. Solvent and the undissolved 
28. Dissolved solute and the undissolved solute D. Dissolved solute and the solution. 
29. If an equilibrium reaction has H > 0, the reaction will  proceed favourable in the forwarddirection. 
30. high temperature 
31. any temperature 
32. low temperature 
33. minimumtemperature 

2HCl(aq)+CaCO3 CaCl2(s) + CO2(g)+H2O(1) 

1. increased humidity D. flooding 

From the reaction above, which of the curves i 

n the  oxide 

14. Which of the following ionsis acidic? 
15. K+ B. NO –

3 

1. S2- D. H O+

3 

15. The structural component that makes detergent  dissolve more quickly in water than soap is 
16. -SO3-Na+ B. -COO– Na+ C. –SO –Na+ D. -COO–K+

4 

16. A liquid that will dissolve fat is 
17. hydrochloric acid 
18. calcium hydroxide 
19. kerosene 
20. water 
21. What a mass K CrO is required to prepare 250 cm3of 

diagram represents the production of carbon(IV)  as dilute HCl is added? 

1. L B. M 
2. N D. P 
3. s that 

The commonest feature of reaction at the anode i A. electrons are consumed 

1. oxidation isinvolved 
2. ions are reduced 
3. electrode dissolves 
4. Which of the following will change when a catalyst is  added to a chemicalreaction? 
5. The activation energy 
6. The potential energy of the reactants 
7. The heat of reaction 
8. The potential energy of the products.
9. If Y is an oxidizing agent that reactswith a reducing agent,  Z, which ofthe following is correct? 
10. Y increasesin oxidation number 
11. Y becomes reduced 
12. Z loses protons 
13. Z gains protons. 
14. When at equilibrium, which ofthe reactions below will  shift to the right if the pressure is increased and the  temperature is kept constant . 
15. 2SO3(g) 2SO2(g) + O2(g)
16. 2SO2(g) 2CO(g) + O2(g)
17. 2H2(g) +’!O2(g) 2H2O(g)
18. 2NO(g) N2(g) + O2(g)
19. In the electrolysis of a concentrated solution ofsodium  chloride using inert electrodes, which of the following  ions are discharge at the cathode and anode respectively?
20. Na+and Cl– B. Na+and OH C. H+and OH– D. H+and Cl
21. CO(g) + H2O(g) CO2(g) + H2(g)

From the reaction above, calculate the standard heat change ifthe standard enthalpies offormation ofCO2(g) 

1. Ca D. Sn 
2. Which of the following statements is true of sulphur  (1V)oxide? 
3. It formstetraoxosulphate(V1) acid with water B. It is an odourless gas 
4. It is an acidanhydride 
5. It forms white precipitate with acidified barium  chloride. 
6. The salt that will form a precipitate soluble in excess  ammonia solution is 
7. Ca(NO3)2B. Cu(NO3)2
8. Mg(NO3)2 D. Al(NO3)2
9. The metal liberates hydrogen from cold water in bubbles  only is 
10. Na B. K 
11. Ca D. Al 
12. Chlorine gas turns a damp starch-iodine paper A. pink B. colourless 
13. red D. dark blue 
14. The modern process of manufacturing steel form iron 
    

, H2O(g) and CO(g) in kJ mol-1are –394, -242 and –110 is by 

respectively. 

1. -262kJmol-1 B. –42 kJmol-1
2. +42 kJmol-1 D. +262 kJmol-1
3. When sugar is dissolved in a tea, the reaction is always  accompanied by 
5. positive entropy change 
6. negative entropy change 
7. no entropy change 
8. a minimum entropychange. 
9. Which of the following is an electrolyte? 
10. Alcohol 
11. Sodium acetate solution 
12. Solid potassium hydroxide 
13. Mercury 
14. Chlorine gas is prepared in the laboratory by A. adding concentrated hydrochloric acid to solid  manganese (1V)oxide 
15. adding concentrated tetraoxosulphate (V1)  

acid to solid sodiumchloride 

1. dropping concentrated hydrochloric acid onto  potassium tetraoxomanganate (V11) crystals 
2. oxidizing concentrated hydrochloric using  

potassium heptadichromate (V1) crystals. 

1. treatment with acids 
2. oxidation 
3. blast reduction 
4. treatment withalkalis 

In the diagram above, Y is 

1. NO B. NO2 C. N2 O5 D. N2O4

Ethene reacts with hydrogen bromide to give A. CH Br 

2 2 

1. CH3CH2Br 
2. C2 H2Br2
3. CHBr3
4. Metal of the transition series have special properties  which are different from those of groups 1 and 11 

elements because they have partially filled 

1. s orbitals B. p orbitals 
2. d orbitals D. f orbitals 
3. Hydrogen can be displace form a hot alkaline solution  by. 
4. Fe B. Cu 
5. Carbohydrates are compounds containing carbon  hydrogen and oxygen in the ration 
6. 3: 1:1 B. 2 : 1:1 
7. 1: 2:1 D. 1 : 1:1 

42 How many isomers does pentane have? 

1. 6 B. 5 
2. 4 D. 3 
3. The leachate of a certain plant ash is used in local soap  making because if contains
4. sodium hydroxide 
5. potassium hydroxide 
6. soluble carbonates and hydrogen carbonates. 
7. The formula for ethyl butanoate is 
8. C3H7COOC2H5 B. C2H5COOC3H7 C. C4H9COOC2H5 D. C2H5COOC4H9
9. The type of reaction that is peculiar to benzene is A. addition B. hydrolysis 
10. polymerization D. substitution 
11. Ethanol reacts with excess acidified K2Cr2O7 A. ethanedioc acid B. ethanol 
12. ethyl ethanoate D. ethanoic acid 
13. A compound contains 40.0% caron 6.7% hydrogen and  53.3% oxygen. If the molar mass of the compound is  180, find the molecular formula. 
14. CH2O B. C3H6O3
15. C6H12O6 D. C6H6O3

[ H = 1, C= 12, O = 16] 

48. The process by which atoms are rearrange into different  molecular structures in the petroleum refining process  is referred to as 
49. catalytic cracking B. hydrocracking 
50. plolymerization D. reforming 
51. Which of the following is found in cotton A. Starch B. Cellulose 
52. Fat D. Oil 
53. The principal constituent of natural gas is A. methane B. ethane 
54. propane D. butane. 
    

Chemistry 2004 

1. In the electrolysis of brine, the anode is A. Zinc 
2. Platinum 
3. Carbon 
4. Copper. 
5. Which of the following shows little or not net  reaction when the volume of the system is  decreased? 
6. 2O3(g) 3O2(g)
7. H2(g) + l2(g) 2Hl(g)
   
8. N 2NO2(g)C. 2NO2(g N2O4(g) D. PCl5(g PCl3(g) + Cl2(g

2O4(g)

In the endothermic reaction above, more product  

formation will be favoured by 2CO + O 2CO B. a decrease in volume 8. Given that2 2 

1. a decrease in pressure 
2. an increase in pressure 
3. a constant volume 
4. The oxidation state of Chlorine inHClO4 is  A. -1 B. 5 
5. +7 D. +1 
6. Which of the following hydrogen halides has the  highest entropy value? 
7. HBr B. HF 
8. Hl D. HCl 
9. The mass of silver deposited when a current of 10A  is passed through a solution of silver salt for 4830s  A. 54.0g B. 27.0g 
10. 13.5g D. 108.0g 

[Ag = 108, F = 96500 C mol-1] 

6. Which of the following acts as both a reducing and  an oxidizing agent? 
7. H S B. CO 

H [CO] is – 110.4kJmol-1and 

H[CO ]is –393o kJmol-1, the energy change for  2 

the reaction above is 

282. -282.6kJ B. +503.7 kJ C. –503.7 kJ D. +282.6 kJ 

ZnO + CO Zn + CO2 

9. In the reaction above, Zinc has been A. displaced B. oxidized 
10. reduced D. decomposed. 
11. What volume of gas is evolved at s.t.p. if 2g of  Calcium trioxocarbonate(iv) is added to a solution  of hydrochloric acid? 
12. 224cm3 B. 112cm3
13. 2240cm3 D. 448 cm3

[Ca = 40, C=12, O=16, Cl =35.5, H= 1, 

Molar volume of a gas at s.t.p =22.4 dm3] 

11. A chemical reaction is always associated with A. a change in the nature of the reactants B. the formation of newsubstances 
12. a change in the volume of the reactants 
    

C.2 2 D. an increase in the composition of one of H2 D. SO2the substances, 

12. When a solid substance disappears completely as a  gas on heating, the substance is said to have  undergone. 
13. Alkanol + Alkanoic acid Ester + Water The reverse reaction of the equation above is known as. 
    
14. sublimation B. crystallization A. saponification B. hydrolysis C. distillation D. evaporation C. fermentation D. hydration 
    
15. If a solution contains 4.9g oftetraoxosulphate (V1) acid,  calculate the amount of copper (11) oxide that will react  with it 
16. 40.0g B. 80.0g 
17. 0.8 g D. 4.0 g 

[Cu = 64, O =16, S =32, H =1] 

14. Vulcanization involvesthe removal of 
15. the single bond B. a double bond C. a polymer D. a monomer 
16. The alkyl group can be represented by the general  formula. 
17. CnH2n B. CnH2n-2
18. CnH2n+1 D. CnH2n+2
19. CH3COOH(g) CH4(g) + CO2(g)

The reaction above is 

1. acidification B. esterification C. decarboxylation D.carboxylation. 
2. A characteristic ofthe alkane family is 
3. substitution reaction 
4. neutralization reaction 
5. addition reaction 
6. elimination reaction. 
7. Pollution of underground water by metal ions is very  likely in a soil that has high 
8. alkalinity B. nitrate content C. acidity D. chloride content 
   
9. C H OH Conc. H Y 26. The solubility in mol dm-3 of 20g of CuSO dissolved in 2SO4

2 5 (aq)180oC4 100g of water at 180oC is 

In the reaction above, Y represent 

1. C2H5COOH B. CH4 C. CH3OCH3 D. C2H4
2. In the production ofsoap, concentrated sodium chloride  is added to 
3. saponify the soap 
4. emulsify the soap 
5. decrease the solubility of the soap 
6. increase the solubility of the soap 
7. Oxyacetylene flame is used for 1ron-welding because it A. evolves a tot heat when burnt 
8. dissociatesto produce carbon (1V) oxide and  oxygen 
9. makes the iron metal solidify very quickly  combines with oxygen give a pop sound. 
10. Which of these reagents can confirm the presence of a  triple bond? 
11. Bromine gas 
12. Brominewater 
13. Acidified KMnO4

Copper (1) chloride 

20. H CH3

H3C – C – C -CH2 – CH2-CH3  

CH3 H 

The IUPAC nomenclature of the compound above is A. 3,4 -dimethylhexane 

1. 2,3 –dimethylhexane 
2. 2 – ethylhexane 
3. 2 – ethylpentane 
4. An isomer of C5 H12 is 
5. 2 –ethyl butane 
6. butane 
7. 2- methyl butane  

2- methyl propane 

1. 0.25 B. 0.13 
2. 2.00 D. 1.25 

[Cu = 64, S =32, O = 16] 

27. Which of these compounds is a normalsalt? A. Na2CO3B. NaHCO3
28. NaHSO4 D. NaHS 
29. A carcinogenic substance is 
30. nitrogen (ll) oxide B. carbon (ll) oxide C. asbestos dust D. sawdust. 
31. What volumeof0.5moldm-3H SO will exactlyneutralize 2 4 

20 cm-3 of0.1moldm-3NaOHsolution?  

5. 5.0 cm-3
6. 6.8cm-3
7. 8.3cm-3
8. 2.0cm-3
9. Calcium tetraoxosulphate (V1) dissolvesin water only  sparingly to form a 
10. colloid B. solution 
11. suspension D. precipitate 

31 Hardness of water is caused by the presence of the  ions of 

1. calcium andmagnesium 
2. calcium andsodium 
3. magnesium and silver 
4. sodium and potassium 
5. It is difficult to achieve an orderly arrangement of the  molecules of a gas because they. 
6. can collide with one another in the container B. are too small in size 
7. have little force of attraction between them D. have no definite shape
8. The shape of the s-orbital is 
9. elliptical B. spiral 
10. circular D. spherical 
11. Which of the following mixtures of gases is likely to  burn in flame? 
12. Helium and neon 
13. Neon and nitrogen 
14. Neon and hydrogen 
15. Nitrogen andhelium 
16. The property of chlorine which cause hydrogen chloride  to be more ionic than the chlorine molecule is its. 
17. According toCharles’law, the volume of a gas becomes  zero at 
18. -100oC B. -273oC 
19. -373oC D. 0oC 
20. When steam is passed over red-hot carbon, the  substances produced are 
21. hydrogen and carbon(11) oxide 
22. hydrogen and carbon(1V) oxide 
23. hydrogen and trioxocarbonate (1V) acid D. hydrogen, oxygen andcarbon (1V) oxide 
24. Aluminum hydroxide is used in the dyeing industry as a 
    
25. electronegativity B. electropositivity A. dye B. dispersant C. electron affinity D. electrovalency. C. salt D. mordant 
27. Transition metals possess variable oxidation states  

because they have. 

1. electrons in the s orbitals 
2. electrons in the d orbitals 
3. partially filled p orbitals 
4. a variable number of electronsin the p orbitals. 
5. The allotrope of carbon used in the decolourization of  
   

In the experiment above, X is mixture of nitrogen,  carbon 1V) oxide and 

1. oxygen B. inert gas 
2. water D. impurities 
3. A given volumeof methane diffuses in 20s. How long  will it take same volume ofsulphur (V1) oxide to diffuse  under the same conditions? 
4. 40s B. 60s 
5. 20s D. 5s  

[C=12, H=1, S=32,O=16] 

38. Chlorine consisting of two isotopes of mass numbers  35 and 37 in the ratio 3:1 has an atomic mass of 35.5.  Calculate the relative abundance of the isotope of mass  number 37. 
39. 60 B. 20 
40. 75 D. 25 
41. An electron can be added to a halogen atom to form a  halide ion with 
42. 8 valence electrons 
43. 7 valence electron 
44. 2 valence electrons 
45. 3 valence electrons 
46. 226 Ra x Rn + alpha – particle 

88 86 

sugar is 

1. soot B. lampblack 
2. graphite D. charcoal 
3. Carbon is tetravalent because 
4. the 2s and 2p atomic orbital hybridized 
5. all the atomic orbitals of carbon hybridize C. the electrons in all the orbital of carbon are  equivalent 
6. the electrons in both the 2s and 2p orbital are  equivalent. 
7. Sodium metal is always kept under oil because it A. is reduced by atmospheric nitrogen 
8. readily reacts withwater 
9. reacts with oxygen and carbon(1V)oxide D. reacts vigorous on exposure to air. 
10. Alloys are best prepared by 
11. cooling a molten mixture of the metals 
12. reducing a mixture oftheir metallic oxides C. arc-welding 
13. electroplating 
14. Sulphur (1V) oxide bleaches by 
15. hydration B. reduction 
16. absorption D. oxidation. 
    
17. 226 50. Which of the following gases can be collected by the B. 220 method of downward delivery? C. 227 A. Oxygen B. Hydrogen D. 222 C. Chlorine D. Ammonia