WASSCE CHEMISTRY MAY/JUNE 2016 (SSCE WAEC MAY/JUNE 2016 CHEMISTRY)
1. The following atoms of carbon 126C, 136C and 146C can be described as?
A. Allotropes
B. Isomers
C. Isotopes
D. Isotones
2. An atom X consist of 6 protons, 6 electrons and 7 neutrons. Which of the following representations of the atom is correct?
A. 136X
B. 137X
C. 196X
D. 197X
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3. How many electron are present in $_{4}^{9}B{{e}^{2+}}$
A. 2
B. 4
C. 5
D. 6
4. When element 20Y combines with element 8 Z
A. A covalent compound , YZ is formed
B. A covalent compound, ZY is formed
C. An ionic compound, YZ is formed
D. An ionic compound, ZY is formed
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5. The boiling points of HF, H2O and NH3 increase in the order of
A. NH3
B. H2O < HF
C. HF < NH3 < H2O
D. NH3 < HF < H2O
6. Chemicals that are produced in small quantities and with very degree of purity are
A. Bulk chemicals
B. Fine chemicals
C. Heavy chemicals
D. Light chemicals
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7. The mass of potassium hydroxide required to make 300.ocm3 of 0.4 moldm-3 solution is
{KOH = 56.0}
A. 26.88g
B. 13.44g
C. 6.72g
D. 3.36g
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8. Metals can be stretched into wires because they are
A. Ductile
B. Good conductors
C. Lustrous
D. Malleable
9. Aluminium is used in the manufacture or aircraft because it
A. Is hard and brittle
B. Is light and resists corrosion
C. Has high density and conducts electricity
D. Is malleable and ductile
10. An unsaturated solution differs from a saturated solution at a given temperature because it
A. Cannot dissolve more solute
B. Can hold more solute than it can actually dissolve
C. Can still dissolve more solute at given temperature
D. Form crystal more easily on cooling
11. Which of the following arrangements shows increasing order of reactivity of the halogens?
A. F2 > Cl2 > Br2 >I2
B. I2 < Br2 < Cl2
C. F2 < Cl2 < Br2
D. I2 > Br2 > Cl2 > F2
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12. The shape of the water molecule is_______?
A. Linear
B. Pyramidal
C. Tetrahedral
D. V-shaped
13. Which of the following elements would produce coloured ion in aqueous solution?
A. Calcium
B. Copper
C. Magnesium
D. Sodium
14 The minimum amount of energy required for effective collisions between reacting particles is known as
A. Activation energy
B. Bond energy
C. Kinetic energy
D. Potential energy
15. The bond formed between H2O and H+ to form the hydroxonium H3O+ is
A. Dative
B. Covalent
C. Electrovalent
D. Ionic
16. An element X forms the following oxides X2O, XO and XO2. This phenomenon illustrates the law of________?
A. Conservation of mass
B. Definite proportion
C. Mass action
D. Multiple proportion
17. How many moles of oxygen would contain 1.204 × 1024 molecules?
[Avogadro's constant (NA) = 6.02 × 1023]
A. 1
B. 2
C. 3
D. 4
18. Which of the following statements about solids is correct?
A. Solid particles are less orderly than those of a liquid
B. Solid have lower densities than liquids
C. Solid particles have greater kinetic energies than those of liquids
D. Solid particles cannot be easily compressed
19. Which of the following apparatus can be used to measure a specific volume of a liquid accurately?
A. Beaker
B. Conical flask
C. Measuring cylinder
D. Pipette
20. The general gas equation $\frac{PV}{T}=K$ is a combination of
A. Boyle's and Charles' laws
B. Boyle's and Graham's laws
C. Charles' and Graham's laws
D. Dalton's and Graham's laws
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21. The spreading of the scent of a flower in a garden is an example of_____?
A. Brownian motion
B. Diffusion
C. Osmosis
D. Tynadal effect
22. Propane carbon(IV)oxide diffuse at the same rate because [H = 1.00, C = 12.0, O = 16.0]
A. They are both gases
B. Their molecules contain carbon
C. They have the same relative molecular mass
D. Both are denser than air
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23. The energy which accompanies the addition of an electron to an isolated gaseous atom is
A. Atomization
B. Electronegativity
C. Electron affinity
D. Ionization
24. An aqueous solution of (NH4)2 SO4 is
A. Acidic
B. Alkaline
C. Amphoteric
D. Neutral
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25. When NH4Cl(s) is dissolved in water, the container feels cold to touch. This implies
A. The process is endothermic
B. The process is exothermic
C. NH4Cl forms a saturated solution
D. NH4Cl is highly soluble in water
26. The pH of four solutions M, N, Q and R are 2, 6, 8 and 11 respectively.
Which of the following deductions about the solutions is correct?
A. The pH of N is increased when the solution is diluted
B. The pH of Q is increased when the solution is evaporated
C. M is the most alkaline solution
D. R is the most acidic solution
27. Consider the following reaction equation
H3O+(aq) + OH(aq) → 2H2O(1)
The reaction represents
A. Esterification
B. Hydrolysis
C. Neutralization
D. Redox
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28. The refreshing characteristic taste of fizzy drinks is due to the presence of
A. Carbon(IV)oxide
B. Glucose
C. Hydrogen
D. Sodium Citrate
29. Chemical equilibrium is attained when
A. All the reactants have been completely used up
B. The reaction goes to completion
C. The concentration of reactants and products remain constant
D. The concentration of reactants and products are equal
30. Which of the following factors will affect the rate of the reaction represented by the following equation?
2HCl(aq) + CaCO3(s) → CaCl2(aq) + H2O(1) + CO2(g)
I. Pressure
II.Concentration
III. Nature of reactants
IV. Temperature
A. I and II only
B. II, III and IV only
C. I, II and III only
D. I, II. III and IV
31. On evaporation to dryness, 3503 of saturated solution of salt Z gave 55.5g of salt. What is the solubility of the salt? [Z = 101]
A. 1.57 moldm-3
B. 3.14 moldm-3
C. 6.28 moldm-3
D. 12.56 moldm-3
32. Which of the following salts when dissolved in water will form a solution that will change blue litmus to red?
A. CH3COONa
B. NH4Cl
C. NaCl
D. KCl
33. Which of the following bonds are broken when ethanol is boiled?
I. Covalent bonds
II. Ionic bonds
III. Hydrogen bonds
A. I only
B. II only
C. III only
D. I, II, III
34. A compound with molecular formula CH2O2 is
A. A Carbohydrate
B. A Carboxylic acid
C. An alkanol
D. An ester
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35. The quality of electricity required to discharge 1 mole of univalent ion is
A. 9600C
B. 48250C
C. 96500C
D. 193000C
36. Chlorine water is used as a bleaching agent because it is
A. An acidic solution
B. An alkaline solution
C. An oxidizing agent
D. A reducing agent
37. Which of the following substances is a non-electrolyte?
A. H2SO4
B. CH3COOH
C. C6H12O6
D. NH4Cl
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38. The oxidation number of sulphur is +4 in
A. Na2S2O3
B. H2SO3
C. H2SO4
D. SO3
39. Consider the following ionic equation:
Cr2O72- + 14H+ + ne- → 2Cr3+ + 7H2O.
The value of n in the equation is_______?
A. 7
B. 6
C. 3
D. 2
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40. Consider the following half-cell reactions.
Al(s) → Al3+(aq) + 3e-
Cu2+(aq) + 2e- → Cu(s)
The overall equation for the reaction is
A. Al(s) + Cu2+(aq) → Al3+(aq) + Cu(s)
B. 2Al(s) + Cu2+(aq) → 2Al(aq) + Cu(s)
C. 2Al(s) + 3Cu2+(aq) → 3Cu(s) + 2Al3+(aq)
D. 3Al(s) + 2Cu2+(aq) → Cu(s) + 3Al3+(aq)
41. Amino acids are obtained from proteins by
A. Hydrolysis
B. Oxidation
C. Polymerization
D. Reduction
42. When a compound X is heated with concentrated tetraoxosulphate(VI)acid, it produces an alkene. X is an
A. Alkane
B. Alkanol
C. Alkanoate
D. Alkyne
43. Ripening of fruits is hastened by using
A. Ethanol
B. Ethane
C. Ethene
D. Ethyne
44. The compound that makes palm wine taste sour after exposure to the air for few days is
A. Ethanol
B. Ethanoic acid
C. Methanol
D. Methanoic acid
45. Which of the following compounds is/are secondary alkanols?
i) CH3CH(CH3)CH3OH
ii) CH3CH2CH(OH)CH3
iii) CH3C(OH)(CH3)CH3
A. I only
B. II only
C. I and III only
D. II and III only
46. Consider the following reaction equation
C2H4(g) + 3O2(g) →→ 2CO2(g) + 2H2O(l).
The volume of oxygen at s.t.p that will be required to burn 14g of ethene is
[C2H4 = 28; Molar volume of gas at s.t.p = 22.4dm3
A. 64.2dm3
B. 33.6dm3
C. 11.2dm3
D. 3.73dm3
47. Which of the following sources of energy contributes to green-house effect?
A. Natural gas
B. Nuclear
C. Wind
D. Solar
48. A consequences of global warming is
A. Air pollution
B. Flooding
C. Increased humidity
D. Water pollution
49. Which of the following metals is common to both brass and bronze?
A. Aluminium
B. Copper
C. Lead
D. Iron
50. The alkanol obtained from the production of soap is
A. Dihydric Alkanol
B. Tertiary Alkanol
C. Trihydric Alkanol
D. Monohydric Alkanol