Saturday, 2 March 2019



1. Which question Paper Type of Chemistry is given to you?
A. Type A
B. Type B
C. Type C
D. Type D

2. What is the concentration of a solution containing 2g of NaOH in 100cm3 of solution?
[Na = 23, O = 16, H = 1]
A. 0.40 mol dm-3
B. 0.50 mol dm-3
C.  0.05 mol dm-3
D. 0.30 mol dm-3

3. Which of the following properties is NOT peculiar to matter?
A. kinetic energy of particles increases from solid to gas
B. Random motion of particles increases from liquid to gas
C. Orderliness of particles increases from gas to liquid
D. Random motion of particles increases from gas to solid

4.  The principle of column chromatography is based on the ability of the constituents to __.
A.  move at different speeds in the column
B.  dissolve in each other in the column
C.   react with the solvent in the column
D.   react with each other in the column

5. From the diagram above, an ideal can be represented by __. 
A. M
B.  N
C.  K
D.  L

6.  Which of the following questions is correct about the periodic table?
A.  The non-metallic properties of the elements tend to decrease across each period
B. The valence electrons of the elements increase progressively across the period
C. Elements in the same group have the same number of electron shells
D. Elements in the same period have the number of valence electrons

7. The relative atomic mass of a naturally occurring lithium consisting of 90% Li and 10% Li is
A. 6.9
B. 7.1
C. 6.2
D. 6.8

8. An isotope has an atomic number of 15 and a mass number of 31. The number of protons it contain is __.
A. 16
B. 15
C.  46
D.  31

9.  The molecular lattice of iodine is held together by __.
A. dative bond
B.  metallic bond
C.  hydrogen bond
D.  van der Waal's forces

10.          The arrangement of particles in crystal lattices can be studied using
A.              X - rays
B.              γ - rays
C.              α - rays
D.             β – rays

11.    From the diagram above, find the amount of solute deposited when 200 cm3 of the solution is cooled from 55oC to 40oC
A. 0.10 mole
B.  0.20mole
C.  0.01 mole
D.  0.02 mole

12. The importance of sodium aluminate (III) in the treatment of water is to __.
A. cause coagulation
B.  neutralize acidity
C.  prevent goitre and tooth decay
D.  kill germs

13.  What type of bond exits between an element X with atomic number 12 and Y with atomic number 17?
A.  Electrovalent
B.  Metallic
C.  Covalent
D.  Dative

14. Hardness of water is mainly due to the presence of __.
A. calcium hydroxide or magnesium hydroxide
B. calcium trioxocarbonate (IV) or calcium tetraoxosulphate (VI)
C. sodium hydroxide or magnesium Hydroxide
D. calcium chloride or sodium chloride salts

15. A suitable solvent for iodine and nephthalene is __.
A.  carbon (IV) sulphide
B.   ethanol
C.   water
D.   benzene

16. Which of the following noble gases is commonly found in the atmosphere?
A.  Xenon
B.  Neon
C.  Helium
D.   Argon

17.          N2O4(g)   2NO2(g)     H = +ve
In the reaction above, an increase in temperature will __.
A.  increase the value of the equilibrium constant
B.  decreases the value of the equilibrium constant
C.  increase in the reactant production
D.  shift the equilibrium to the left

18.  CH3COOH(aq) + OH-(aq) CH3COO-(aq) + H2O(l)
In the reaction above, CH3COO-(aq) is
A.  conjugate base
B.  acid
C. base
D. conjugate acid

19.  How many cations will be produced from a solution of potassium aluminium tetraoxosulphate (VI)?
A.   3
B.   4
C.  1
D.  2

20. Which of the following is NOT an alkali?
A.  NH3
B.   Mg(OH)2
C.  Ca(OH)2
D.  NaOH

21. An effect of thermal pollution on water bodies is that the __.
A. volume of water reduces
B. volume of chemical waste increase
C.  level of oxides of nitrogen increase
D.   level of oxygen reduces

22. Which of the following is a deliquescent compound?
A.  Na2CO3
B. CaCl2
C.  CuO
D.  Na2CO3. 10H2O

23. A chemical reaction which the hydration energy is greater than the lattice energy is referred to as __.
A. a spontaneous reaction
B. an endothermic reaction
C.  an exothermic reaction
D.  a reversible reaction

24. The function of zinc electrode in a galvanic cell is that it __.
A.  undergoes reduction
B.  serves as the positive electrode
C.  production electrons
D.  uses up electrons

25.   CH4(g) + Cl2(g)  CH3 Cl(s) + HCl(g)
The major factor that influence the rate of the reaction above is 
A.  catalyst
B.  temperature
C.  concentration
D.  light

26.  The condition required for corrosion to take place is the presence of __.
A. water and carbon (IV) oxide
B. water, carbon (IV) oxide and oxygen
C.  oxygen and carbon (IV) oxide
D.  water and oxygen

27. In the diagram above, X is the
A.  enthalpy
B.  enthalpy change
C.  activation energy
D.  activated complex
28.   The diagram above best illustrates the effect of decrease in __.
A. concentration
B.  temperature
C.  surface area
D.  pressure

29.  MnO-4(aq) + Y + 5Fe2+(aq)  Mn2+(aq) + 5Fe2+(aq) + 4H2O(l)
In the equation above, Y is
A.  5H+(aq)
B. 4H+(aq)
C. 10H+(aq)
D. 8H+(aq)

30.          Given that M is the mass of a substance deposited during electrolysis and Q is the quantity of electricity consumed, then Faraday's first law can be written as
[Electrochemical equivalent]

31. The impurities formed during the laboratory preparation of chlorine gas are removed by
A. H2O
B. NH3
C. H2SO4
D.  HCl

32. The effect of the presence of impurities such as carbon and sulphur on iron is that they __.
A. give it high tensile strength
B.  make it malleable and ductile
C.  increase its melting point
D.  lower its melting point

33. A few drops of concentrated HNO3 is added to an unknown solution and boiled for a while. If this produces a brown solution, the cation presents are likely to be __.
A.  Pb2+
B.  Cu2+
C.  Fe3+
D.  Fe2+

34. The bleaching action of chlorine gas is effective due to the presence of __.
A.  hydrogen chloride
B.  water
C.   air
D.  oxygen

35. In the laboratory preparation of oxygen, dried oxygen is usually collected over __.
A. hydrochloric acid
B. mercury
C. calcium chloride
D.  tetraoxosulphate (VI) acid

36. The property of concentrated H2SO4 that makes it suitable for preparing HNO3 is its __.
A. boiling point
B. density
C. oxidizing properties
D. dehydrating properties

37. Bronze is preferred to copper in the making of medals because it __.
A.  is stronger
B.  can withstand low temperature
C.  is lighter
D.  has low tensile strength

38. The constituents of baking powder that makes the dough to rise is __.
B.  NaOH
C. Na2CO3
D.  NaCl

39. Which of the following compound is used as a gaseous fuel?
A.   CH3 – C = CH
B.   CH3 – CH2 – CH3
C.   CH3 – CH2 – CH2 – COOH
D.  CH3 – CH2 – CH2 – CH3

40.  The ability of carbon to form long chains is referred to as  __.
A. alkylation
B.  acylation
C.  catenation
D.  carbonation

41. Which of the following compounds will undergo polymerization reaction?
A. C2H4
C.  C2H6

42.  The compound above exhibits  __.
A. geometric isomerism
B. optical isomerism
C.  structural isomerism
D.  positional isomerism

43. An organic compound has an empirical formula CH2O and vapour density of 45.
What is the molecular formula?
[C = 12, H = 1, O = 16]
A.  C3H7OH
B.  C2H5OH
C.  C3H6O3
D.  C2H4O2

 44. The reaction above represented by the equation above is useful in the production of  __.
A. propanol
B. butanol
C.  methanol
D.  ethanol

45.The number of isomers that can be obtained from C4H10 is  __.
A. 3
B.  4
C. 1
D.   2
46.  The functional groups present in the compound above are  __.
A. alkene and halo-group
B.  hydroxyl and chloro-group
C.  alkene and chloro-group
D.  hydroxyl and halo-group

47.   Which of the following is a primary amine?

48. Two organic compounds K and L were treated with a few drops of Fehling's solutions respectively. K formed a brick-red precipitate while L, remains unaffected. The compound K is an __.
A.  alkanol
B.  alkane
C.  alkanal
D.  alkanone

49.  Which of the following statements is true about 2-methylpropane and butane ?
A. They are members of the same homologous series
B. They have the same boiling point
C. They have different number of carbon atoms
D.   They have the same chemical properties

The reaction above is best described as __.
A.  esterification
B.  condensation
C.  saponification
D.  neutralization

1.              B
2.              B
3.              D
4.              A
5.              B
6.              B
8.              B
9.              D
10.          A
11.          B
12.          A
13.          A
14.          B
15.          B
16.          D
17.          A
18.          A
19.          D
20.          A
21.          D
22.          B
23.          C
24.          C
25.          D
26.          D
27.          B
28.          A
29.          A
30.          B
31.          A
32.          D
33.          D
34.          B
35.          D
36.          C
37.          C
38.          A
39.          D
40.          C
41.          A
42.          B
43.          C
44.          D
45.          D
46.          B
47.          B
48.          C
49.          A
50.          A

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