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WorksheetsPRACTISE QUESTIONS FOR SS2
Total questions: 50
Worksheet time: 8mins
Name
Class
Date
1.
Oil spillage could cause
a)
Soil pollution only
b)
water pollution only
c)
water and soil pollution
d)
air, water and soil pollution
2.
An organic compound with molecular mass 2 has an empirical formula CH. What is its molecular formula? (H = 1, C = 12)
a)
C₈H₈
b)
C₆H₆
c)
C₂H₂
d)
CH
3.
Consider the following reaction: 2HCl(aq) + CaCO₃ (s) → CaCl₂ (aq) + CO₂ (g) + H₂O(l) What happens to the frequency of collision between the calcium ions and the chloride ions as the reaction progresses? It would
a)
remain the same
b)
increase
c)
decrease
d)
double
4.
Exhaust fumes discharged from an electric generator gradually become invisible as a result of
a)
combustion
b)
adsorption
c)
emission
d)
diffusion
5.
The mass of water of crystallization in 1 mole of MgSO₄.6H₂O is (H = 1, O = 16)
a)
18
b)
108
c)
126
d)
246
6.
How many Faradays would be required to discharge one mole of oxygen gas?
a)
4
b)
3
c)
2
d)
1
7.
An increase in the kinetic energy of particles occurs in a reaction if
a)
a catalyst is added
b)
fine particles are used
c)
temperature is increased
d)
concentration is increased
8.
Which of the following reagents is used to distinguish between Al³⁺ and Zn²⁺?
a)
Ca(OH)₂
b)
HNO₃
c)
NaOH
d)
NH₃
9.
Which of the following representations of a cell reaction is correct?
a)
Zn(s)/Zn²⁺(aq)//Cu(s)/Cu²⁺(aq)
b)
Zn(s)/Zn²⁺(aq)//Cu²⁺(s)/Cu(aq)
c)
Zn²⁺(s)/Zn(aq)//Cu²⁺(s)/Cu(aq)
d)
Cu²⁺(s)/Cu(aq)/Zn(aq)/Zn²⁺(s)
10.
The following compounds are soluble in water except
a)
lead tetraoxosulphate(VI)
b)
sodium trioxocarbonate(IV)
c)
silver trioxonitrate(V)
d)
zinc chloride
11.
If a pink crystalline salt is found to be soluble and of high density, then the salt contains
a)
a halogen
b)
an alkaline
c)
a transition metal
d)
an amphoteric metal
12.
Which of the following salts crystallizes without water of crystallization?
a)
Na₂SO₄
b)
Na₂CO₃
c)
NaCl
d)
CaCl₂
13.
The basicity of ethanoic acid, CH₃COOH is
a)
1
b)
2
c)
3
d)
4
14.
An aqueous solution of pH 9.5 is
a)
acidic
b)
strongly acidic
c)
strongly alkaline
d)
slightly alkaline
15.
Melting of iceberg and flooding are environmental problems directly associated with
a)
Ozone layer depletion
b)
global warming
c)
use of fossil fuel
d)
use of fertilizers
16.
When equilibrium is attained in a chemical cell, the voltage is
a)
0
b)
greater than +1
c)
between 0 and -1
d)
between 0 and +1
17.
The gas absorbed when air is passed through a tube containing fused calcium chloride is
a)
argon
b)
carbon(IV) oxide
c)
water vapour
d)
nitrogen
18.
Water gas is a mixture of
a)
Hydrogen and carbon(II) oxide
b)
hydrogen and carbon(IV) oxide
c)
nitrogen and carbon(IV) oxide
d)
steam and carbon(II) oxide
19.
The volume of oxygen in one mole of air at s.t.p is (molar volume of a gas at s.t.p = 22.4dm³)
a)
4.7dm³
b)
16.0dm³
c)
22.4dm³
d)
32.0dm³
20.
Which of the following pairs of substances have a giant molecular structure?
a)
Diamond and iodine
b)
Diamond and silica
c)
Iodine and methane
d)
Methane and silica
21.
The volume occupied by 2 moles of ammonia at s.t.p is (molar volume of a gas at s.t.p = 22.4dm³)
a)
5.6dm³
b)
11.2dm³
c)
22.4dm³
d)
44.8dm³
22.
Permanent hardness of water may be caused by the presence of
a)
Mg(HCO₃)₂
b)
Ca(HCO₃)₂
c)
Na₂SO₄
d)
CaSO₄
23.
Chlorine does not undergo disproportionation when reacted with
a)
cold, dilute sodium hydroxide solution
b)
hot, concentrated sodium hydroxide
c)
potassium bromide
d)
water
24.
Which of the following compounds would not decompose when strongly heated?
a)
KClO₃
b)
KHCO₃
c)
K₂CO₃
d)
K₂O₂
25.
Which of the following substances is a strong electrolyte?
a)
Dilute magnesium chloride solution
b)
Distilled water
c)
Concentrated glucose solution
d)
Saturated ammonia solution
26.
Consider the following reaction equation: CH₄(g) + 2O₂(g) → 2H₂O(g) + CO₂(aq) What volume of steam would be produced by completely burning 15.0cm³ of methane?
a)
45.0cm³
b)
30.0cm³
c)
15.0cm³
d)
7.5cm³
27.
The volume of 0.05mol/dm³ Na₂CO₃ containing 2.65g of the salt is (Na₂CO₃ = 106)
a)
1.00dm³
b)
0.50dm³
c)
0.25dm³
d)
0.10dm³
28.
Which of the following oxide is insoluble in water?
a)
Zinc oxide
b)
Nitrogen(IV)oxide
c)
Potassium oxide
d)
Carbon (IV) oxide
29.
The halogen which usually exhibits only one oxidation state is
a)
bromine
b)
chlorine
c)
flourine
d)
iodine
30.
Group 8 elements in the periodic table are reactive because they
a)
Are gases at room temperature
b)
have stable electron configuration
c)
have large atomic radii
d)
have strong intermolecular forces
31.
Separation of petroleum into its fractions is possible because the fractions have
a)
different densities
b)
different solubilities
c)
complex mixtures
d)
different boiling points
32.
If the relative molecular mass of a gas is 71, its vapour densities at s.t.p is
a)
25
b)
35.5
c)
71
d)
142
33.
The best method of separating a mixture of kerosene and petrol is by
a)
The use of separating funnel
b)
simple distillation
c)
fractional distillation
d)
chromatography
34.
An atom of an element is electrically neutral, because it contains
a)
An equal number of electrons and protons
b)
more neutrons than protons
c)
more electrons than protons
d)
an equal number of electrons and neutrons
35.
A particle having 10 electrons, 8 protons and 8 neutrons is
a)
a noble gas
b)
an isotope of oxygen
c)
a metal
d)
an anion
36.
What is the non – S.I unit of atomic mass?
a)
amu
b)
kg
c)
dimensionless
d)
mole
37.
The important steps in the scientific method are
I. identifying the problem
II. examining the results of the experiment
III. using the conclusions to explain or predict
a)
I and II only
b)
I and III only
c)
II and III only
d)
I, II and III
38.
A metal oxide contains 54% of the metal. What mass of oxygen combines with 24g of the metal to form the oxide?
a)
28.2g
b)
20.4g
c)
47.0g
d)
103.5g
39.
How many orbitals are associated with the p – sub energy level?
a)
2
b)
3
c)
5
d)
6
40.
Group VIII elements are unreactive because
a)
they are non-metals
b)
they are monoatomic gases
c)
their highest occupied energy level is full
d)
their outermost shell contains equal number of electrons
41.
Elements in the same group of the periodic table have the same
a)
number of electron shells
b)
number of valence electrons
c)
physical properties
d)
atomic size
42.
The element with electron configuration 1s² 2s² 2p⁶ 3s² 3p¹ belongs to
a)
s – block, period 3, Group I
b)
s – block. Period 3, Group III
c)
p – block, period 3, Group II
d)
p – block, period 3, Group III
43.
Equal volumes of all gases under the same conditions of temperature and pressure contain the same number of molecules. This is an expression of
a)
Graham’s Law of diffusion
b)
Avogadro’s hypothesis
c)
Dalton’s atomic theory
d)
Boyle’s Law
44.
Why is cracking of petroleum an important industrial process?
a)
The length of carbon chain in the petroleum is increased
b)
It reduces knocking and smooth combustion
c)
It increases the quantity of petrol
d)
It decreases the octane number
45.
Which of the following oxides of nitrogen has oxidation number of +1?
a)
N₂O
b)
KNO₃
c)
NO
d)
N₂O₃
46.
If a catalyst is added to a system at equilibrium and the temperature and pressure remain constant, there would be no effect on the
a)
activation energy of the reaction
b)
rate of the forward reaction
c)
rate of the reverse reaction
d)
heat of reaction
47.
If 500cm³ of a saturated solution of a salt X contains 17.0g of X at 30⁰C, what would be the solubility of X at 30⁰ C. [X = 74.5g/mol]
a)
0.11
b)
0.15
c)
0.23
d)
0.46
48.
When Ca(OH)₂(aq) is added to NH₄Cl(s), the gas evolved
a)
turns moist red litmus paper blue
b)
bleaches damp blue litmus paper
c)
forms a white precipitate with AgNO₃(aq)
d)
forms a white precipitate with BaCl₂(aq)
49.
Which of the following equations represents an endothermic reaction?
a)
HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)
b)
NH₄Cl(s) → NH₃(s) + HCl(s)
c)
C(s) + O₂(g) → CO₂(g)
d)
2K(s) + 2H₂O(l) → 2KOH(aq) + H₂(g)
50.
The equation P = K/V illustrates
a)
Boyle’s law
b)
Dalton’s law
c)
Charles’ law
d)
Graham’s law
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