1. Which of the following raw materials is used in the plastic industry?
A. ethene
B. methane
C. Sulphur
D. Hydrogen
2. Which of the following organic compounds can undergo both additon and substitutions reactions?
A. Pentane
B. Benzene
C. Propane
D. Haxane
3. Which of the following equation represents a redox reaction?
A. $AgNO_{3(aq)}$ + $KClP_{(ag)}\longrightarrow AgCl_{(s)}$ + $KNO_{3(aq)}$
B. $HNO_{3(aq)}$ + $NaOH_{(ag)}\longrightarrow NaNO_{3(aq)}$ + ${H_2}O_{(l)}$
C. $CaCO_{3(s)}\longrightarrow CaO_{(s)}$ + $CO_{2(g)} $
D. $2H_2S_{(g)}$ + $SO_{2(g)}\longrightarrow 2H_2O_{(l)}$ + $3S_{(g)}$
4. The process of extraction of iron from its ore is
A. decomposition
B. oxidation
C. reduction
D. sublimation
5. What is the solubility of a salt if 0.4g of it is obtained on evaporating $200cm^3$ of its saturated solution to its dryness?
A. $0.08gdm^{-3}$
B. $2.00gdm^{-3}$
C. $8.00gdm^{-3}$
D. $80.00gdm^{-3}$
6. An acidic salt has
A. a single cation in its aqueous solution
B. double anions in its aqueous solution
C. hydrogen ion in its aqueous solution
D. hydrogen atoms in its aqueous solution
7. A reaction is endothermic if the
A. enthalpy change is negative
B. reaction vessel fells cool during the reaction
C. bond forming energy exceeds bond braking energy
D. heta off formationof reactants exceeds heat of formation of products
8. In which of the following compounds does hydrogen form ionic compound
A. $CH_4$
B. $HCl$
C. $NH_3$
D. $NaH$
9. Consider the following reaction equation: $Br_2$ + 2Kl $\longrightarrow$ 2KBr + $I_2$ bromine is reacting as
A. an oxidizing agent
B. a reducing agent
C. an acid
D. a base
10. An organic compound has the empirical fkrmula $CH_2$. If its molar mass is $42gmol^{-1}$, what is its molecular formula? [H = 1.0, C = 12.0]
A. $C_2H_4$
B. $C_3H_4$
C. $C_3H_6$
D. $C_4H_8$
11. Ethene is produced from ethanol by
A. decomposition
B. hydrolysis
C. ozonolysis
D. dehydrationbr>
12. See pages for figures
13. What is the mass of solute in $500cm^3$ of $0.005moldm^{-3}$ $H_2SO_4$?
A. $0.490g$
B. $0.049$
C. $0.245$
D. $0.0245$
14. Pure water can be made to boil at a tempersture lower than 0 by
A. reduce its quantity
B. decreasing the external pressure
C. distilling it
D. increasing the external pressure
15. See pages for figures
16. When salt added to its saturated solution, the salt
A. dissolves and the solution becomes super saturated
B. dissolves and the solution becomes unsaturated
C. precipitates and the solution remains unchanged
D. dissolves and crystals are formed
17. When substance X was added to a solution of bromine water, the solution becomes colorless. X is likely to be
A.propane
B. propanoic acid
C. propyne
D. propanol
18. The preferential discharge of ions during electrolysis is influenced by the
A. mechanism of electrolysis
B. electrolytic reaction
C. nature of electrode
D. type of electrolytic cell.
19. The valence electrons of $_{12}Mg$ are in the
A. 3s orbital
B. 2px orbital
C. 2s orbital
D. 1s orbital
20.Stainless steel is an alloy comprising of
A. Fe and C
B. Fe and Ni
C. Fe, C and Ni
D. Fe, C and Al
21. The number of hydrogen ions in $1.0dm^3$ of $0.02moldm^{-3}$ tetraoxosulphate (VI) acid is [$N_A$ = 6.02 x $10^{23}$]
A. $1.2 \times 10^{22}$
B. $1.2 \times 10^{23}$
C. $2.4 \times 10^{22}$
D. $2.4 \times 10^{23}$
22. The most suitable substance for putting out petrol fire is
A. Water
B. carbon(IV)oxide
C. fire blanket
D. sand
23. The following factors would contribute to environmental pollution except
A. Production of ammonia
B. Manufacture of cement
C. Photosynthesis
D. combustion
24.The position of equilibrum in a reversible reaction is affected by
A. Particle size of the reactants
B.Vigorous stirring of the reaction mixture
C. Presence of a catalyst
D.Change in concentration of reactants
25. See Pages for figures
26. Which of the following statements best explains the differences between a gas and a vapour?
A.Unlike gases, vapours are liquid at room temprature
B.Unlike gases, vapour can easily be condensed into liquids
C.Unlike gases, vapour is readily converted into solids
D.Vapours are generally denser than gases.
27. Consider the following reaction equations: 2HCL + $Ca(OH)_2$ $\longrightarrow$ $CaCl_2$ +$H_20$. what is the volume of $0.1moldm^{-3}$ HCl that would completely neutralize 25cm3 of $0.3moldm^{-3}$ $Ca(OH)_2$?
A. $150cm^3$
B. $75cm^3$
C. $30cm^3$
D. $25cm^3$
28. Cu and $HN{O_3}$ are not suitable for preparing hydrogen gas because of their
A.Reactivity and oxidation
B.Conductivity and corrosiveness respectively
C.Melting point and reduction respectively
D. Electronegativity and solubility respectively
29. Which of the following formula cannot be empirical formula?
A. $CH$
B. $_2$
C. $_{25}$
D. $_{24}$
30. One of the criteria for confirming the purity of benzene is to determine its
A. heat capacity
B. boiling point
C. mass
D. colour
31. When chlorine is passed through a sample of water, the pH of the water sample would be
A. $< 7 $
B. $>7$
C. $=7$
D. $0$
32. How many atoms are contained in 0.2 moles of nitrogen? [$N_A$ =6.02 x $10^{23}$]
A. $1.20 \times 10^{23}$
B. $2.41 \times 10^{23}$
C. $3.62 \times 10^{23}$
D. $4.82 \times 10^{23}$
33.The strength of metallic bonds depends on the
A. Charge density of the atoms
B. Ductility of the metal
C.Number of valence electrons
D.Total number of electrons in the atom.
34. When is added to $_3$ solution, crystals of silver forms on surface. This indicates that is
A. Oxidized
B. Reduced
C. Decomposed
D. Dissiciated.
35. The emperical formula of a compund containing 0.067 molCu and 0.066 mol O is [Cu = 63.5, 0 =16]
A. $Cu_2O$
B. $CuO$
C. $CuO_2$
D. $Cu_2O_2$
36. The change in oxidation state of iron in the reaction represented by the equation below is $2FeCl{_3} + H{_2}S\longrightarrow {_ 2}$
A. +2 to +3
B. +3 to +2
C. 0 to +2
D. +3 to 0.
37. Which of the following methods can be used to separate blood cells from plasma?
A. Centrifugation
B. Filtration
C. Chromatography
D. Distillation
38. Which of the following statements about ionic radius is correct? Ionic radius
A. Increase as nuclear charge increases
B.Decreases as nuclear charge increases
C. Decreases as nuclear charge decreases
D. Remains constant as nuclear charge increases
39. Analysis of a hydrocarbon shows that it contains 0.93g of carbon per gram of the compund. The mole ratio of carbon to hydrogen in the compound is
[H = 1.0, C = 12.0, O = 16.0]
A. 1:1
B. 1:2
C. 2:1
D. 2:3
40. The law of definite proportions states that
A. Pure samples of the same compund contains the same elements combined in the same proportion by mass
B. Pure samples of substances are in the same proportion by mass
C. Chemical compunds are pure because they contain the same elements
D. Matter can neither be created or destroyed.
41. What is the relative molecular mass of a compund which has emperical formula CH2O? [H =1.0, C = 12.0, O =16.0]
A. 42
B. 45
C. 126
D. 180
42. Atoms are electrically neutral because they
A. Do not conduct electricity
B. Contain equal number of protons and electrons
C. Are composed of neutrons and electrons
D. Cannot be attracted by electromagnetic field.
43. Common salt (Nacl) is used for preserving foods. Which of thee following properties could be used to determine its purity before use?
A. Solubility in water
B. Melting point
C. Relative density
D. Cryslalline nature
44. Which of the following electron configurations represents the transition element chromium $(24Cr)$?
A. $1{s}^2 2{s}^2 2{p}^6 3{s}^2 3{p}^6 4{s}^2 3{d}^4$
B. $1{s}^2 2{s}^2 2{p}^6 3{s}^2 3{p}^6 3{d}^6$
C. $1{s}^2 2{s}^2 2{p}^6 3{s}^2 3{p}^4$
D. $1{s}^2 2{s}^2 2{p}^6 3{s}^2 3{p}^6 4{s}^1 3{d}^5$
45. The atomic number of an isotope of hydrogen is equal to its mass number because it
A. Has a totally filled valence shell
B. Has a high charge to mass ratio
C. Does not contain neutrons
D. Exhibits isotopy
Q46 See pages for figures
47. The bonding pair of electrons in a hydrogen chloride molecule is pulled towards the chlorine atom because
A. Chlorine has a larger atomic size
B. Chlorine has a larger atomic mass
C. Chlorine is more electronegative
D.There is no bonding orbitals within the hydrogen atom.
48. The solubility of $CO_2$ in water can be accounted for by
A. Van der Waal forces
B. Ionic attraction
C. Dipole attraction
D. Covalent bonding
49. Which of the following properties would not influence electrovalent bond formation?
A. Electronagativity
B. Electron affinity
C. Ionization potential
D. Catalytic ability
50. Particles in a solid exhibit
A. Vibrational motion only
B. Vibrational and Transitional motion
C. Vibrational and random motion
D. Random and translational motion.
ANSWER
1
A
21
A
41
B
2
B
22
B
42
A
3
D
23
C
43
B
4
C
24
D
44
A
5
B
25
B
45
C
6
C
26
B
46
D
7
A
27
A
47
C
8
D
28
A
48
C
9
A
29
D
49
D
10
C
30
B
50
B
11
D
31
A
12
A
32
A
13
A
33
C
14
B
34
A
15
B
35
B
16
A
36
B
17
C
37
A
18
C
38
B
19
A
39
A
20
C
40
A
