Font size
S
M
L
XL
WorksheetsSS2 CHEMISTRY 2ND TERM REVISION
Total questions: 100
Worksheet time: 33mins
Name
Class
Date
1.
The suitable method for the separation of a mixture of miscible liquids with close temperature range is
a)
decantation
b)
fractional distillation
c)
filtration
d)
simple distillation
2.
A bomb calorimeter is used to determine the heat of
a)
combustion
b)
formation
c)
neutralization
d)
solution
3.
The following processes are involved in the treatment of town water supply except
a)
chlorination
b)
coagulation
c)
dehydration
d)
filtration
4.
An example of amorphous carbon is
a)
diamond
b)
dolomite
c)
fullerene
d)
lampblack
5.
The suitable indicator for titration of strong base against weak acid is
a)
litmus
b)
methyl orange
c)
methyl red
d)
phenolphthalein
6.
In the reaction I₂ + H₂ ⇌ 2HI, if the equilibrium of I₂, H₂ and HI are 2.4, 1.8 and 16.2 mol/dm³ respectively. Calculate the equilibrium constant.
a)
62.4
b)
60.8
c)
58.0
d)
38.5
7.
In the fractional distillation of crude oil, the order of collection is
a)
diesel, kerosene and petrol
b)
kerosene, diesel and petrol
c)
kerosene, petrol and diesel
d)
petrol, kerosene and diesel
8.
An example of a co- ordinate covalent compound is
a)
Cl₂
b)
Cu²⁺
c)
H₂O
d)
H₃O⁺
9.
When a crystal was added to its solution, it did not dissolve and the solution remained unchanged. This shows that it is
a)
concentrated
b)
diluted
c)
saturated
d)
supersaturated
10.
How many molecules of oxygen are present in 8g of oxygen gas? [ O = 16, Avogadro’s number = 6.02 x 10²³]
a)
1.51 x 10²³
b)
3.01 x 10²³
c)
4.82 x 10²³
d)
9.63 x 10²³
11.
Which of the following metals does not react with water to produce hydrogen?
a)
Calcium
b)
Lithium
c)
Magnesium
d)
Potassium
12.
How many faraday(s) of electricity is required to liberate 9g of aluminium? [Al = 27, 1 F = 96500 C]
a)
0.1
b)
0.3
c)
1.0
d)
2.7
13.
The type of bond that exists in ammonia is
a)
covalent
b)
dative
c)
electrovalent
d)
hydrogen
14.
Elements X and Y have electronic configuration 2, 1 and 2, 8, 7 respectively. Which of the following statements is correct?
a)
The bond between X and Y will be a coordinate bond
b)
The bond between X and Y will be covalent
c)
The bond between X and Y will be electrovalent
d)
X and Y are in the same period of the periodic table
15.
The IUPAC name for NaHCO₃ is
a)
sodium bicarbonate
b)
sodium hydrogen carbonate
c)
sodium hydrogen sulphide
d)
sodium hydrogen trioxocarbonate(IV)
16.
What defines the pH of a solution?
a)
Calcium ion
b)
Copper ion
c)
Hydrogen ion
d)
Oxygen ion
17.
The corrosion of metals result from the combined action of water and
a)
atmospheric nitrogen
b)
atmospheric oxygen
c)
copper(II) oxide
d)
hydrogen
18.
What is the oxidation number of Y in YO₄³⁻?
a)
+2
b)
+3
c)
+4
d)
+5
19.
When ΔH is negative, the reaction is said to be
a)
catalytic
b)
endothermic
c)
exothermic
d)
ionic
20.
The rate of a chemical reaction can be altered by the following factors except
a)
concentration of the reactants
b)
heat change accompanying the reaction
c)
physical state of the reactants
d)
presence of a catalyst
21.
The elements ¹²₆R and ¹³₆R exhibit
a)
allotropy
b)
esterification
c)
isomerism
d)
isotopy
22.
An element X forms a chloride XCl₄, in which group of the periodic table is X?
a)
II
b)
III
c)
IV
d)
V
23.
Ammonia is manufactured from nitrogen and hydrogen by
a)
action of iron on steam
b)
electrolysis of brine
c)
decomposition of ammonium trioxonitrate (V)
d)
Haber process
24.
A is 0.02 mol/dm³ of H₂SO₄, B is Sodium trioxocarbonate(IV) solution. If 18.5cm³ of the acid was required to neutralize 9.0cm³ of sodium trioxocarbonate(IV), calculate the concentration of B in mol/dm³
a)
0.02
b)
0.04
c)
6.04
d)
18.04
25.
The ideal gas equation(PV = nRT) holds for all gases at
a)
high pressure only
b)
high temperature only
c)
low pressure and high temperature
d)
low pressure and low temperature
26.
When chlorine water is exposed to sunlight, the products formed are
a)
chlorine gas and oxochlorate (I) acid
b)
hydrochloric acid and oxygen
c)
hydrogen and oxygen
d)
oxygen and oxochlorate (I) acid
27.
A given mass of gas occupies 288.4cm³ at 36°C and 750mmHg. What will be its volume in cm³ at 47°C and 900mmHg?
a)
186
b)
232
c)
249
d)
380
28.
Calculate the mass of carbon(IV) oxide formed, when 3g of carbon is completely burnt in oxygen [ C = 12, O = 16]
a)
14
b)
13
c)
12
d)
11
29.
When 100cm³ of a gas diffuses in 12 seconds, calculate the rate of diffusion of the gas.
a)
10.3
b)
9.3
c)
8.3
d)
7.3
e)
6.3
30.
Temporary hardness of water is removed by
a)
boiling
b)
coagulation
c)
filtration
d)
neutralization
31.
The power of an atom to attract electrons is called
a)
electron affinity
b)
electronegativity
c)
electron positivity
d)
ionization energy
32.
What is the molar mass of an alkene compound with a molecular formula C₆H₁₄? [C = 12, H = 1]
a)
86g
b)
92g
c)
98g
d)
110g
33.
Which of the following gases could be prepared in a kipp’s apparatus?
a)
Ethane
b)
Oxygen
c)
Carbon (IV) oxide
d)
Dinitrogen (I) Oxide
34.
Sodium chloride would be soluble in a
a)
polar solvent
b)
non-polar solvent
c)
saturated solvent
d)
neutral solvent
35.
The compound that has hydrogen bonding between its molecule is
a)
HI
b)
HF
c)
HCl
d)
HBr
36.
The number of replaceable hydrogen atoms in one molecule of an acid is its
a)
atomicity
b)
basicity
c)
acidity
d)
alkalinity
37.
Consider the reaction equation:Cl₂(g) + 2KBr(aq) → Br₂(aq) + 2KCl(aq). Chlorine is
a)
oxidizing agent
b)
reducing agent
c)
electron donor
d)
substance oxidized
38.
Consider the following cell notations:
Mg²⁺ + 2e⁻ → Mg E° = - 2.37v
Zn²⁺ + 2e⁻ → Zn E° = - 0.76v
Determine the cell voltage
a)
- 3.13v
b)
-1.61v
c)
+ 1.61v
d)
+3.13v
39.
Which of the following factors does not affect an equilibrium reaction?
a)
Temperature
b)
Concentration
c)
Pressure
d)
Catalyst
40.
If the atomic number of an element, J is 11 and that of nitrogen is 7, the most likely formula of the nitride of J is
a)
J₃N
b)
JN₃
c)
J₃N₂
d)
N₂J
41.
All pure samples of a chemical substance contain the same element combined together in the same proportion by mass. This is a statement of the
a)
Law of definite proportions
b)
law of multiple proportions
c)
law of reciprocal proportions
d)
law of conservation of mass
42.
Chlorine turns moist litmus paper colourless. This is a/an
a)
Observation
b)
theory
c)
hypothesis
d)
law
43.
The gas that cannot be dried using concentrated tetraoxosulphate (VI) acid is
a)
CO₂
b)
NH₃
c)
HCl
d)
H₂S
44.
Which of the following molecules has a linear shape?
a)
CO₃
b)
SiO₂
c)
H₂O
d)
NH₃
45.
The substance with the least change in solubility with change in temperature is
a)
Na₂SO₄
b)
KClO₃
c)
NaCl
d)
KCl
46.
Ammonium chloride was heated with an aqueous solution of a substance X to produce an ammonia gas. X is likely to be
a)
sodium hydroxide
b)
sodium tetraoxosulphate (VI)
c)
sodium trioxocarbonate (IV)
d)
sodium chloride
47.
Temporary hard water contains
a)
Ca(HCO₃)₂
b)
MgSO₄
c)
CuSO₄
d)
CaCO₃
48.
An oxide that shows both acidic and basic properties in aqueous solution is called
a)
a neutral oxide
b)
an acidic oxide
c)
a basic oxide
d)
an amphoteric oxide
49.
The surface area of a reactant in a chemical reaction can be increased by
a)
breaking into chips
b)
altering the direction of reactants
c)
using reactants of different densities
d)
subjecting the reactant to high pressure
50.
Which of the following aqueous solutions is neutral to litmus paper?
a)
NH₄Cl
b)
Na₂CO₃
c)
FeCl₃
d)
NaCl
51.
The following processes are involved in the treatment of town water supply except
a)
chlorination
b)
dehydration
c)
coagulation
d)
filtration
52.
An example of amorphous carbon is
a)
diamond
b)
limestone
c)
lampblack
d)
fullerene
53.
Which of the following is an unsaturated compound?
a)
Benzene
b)
Cyclohexane
c)
Pentane
d)
Octane
54.
In the reaction I₂ + H₂ ⇌ 2HI, if the equilibrium concentration of I₂, H₂ and HI are 2.4, 1.8 and 16.2 mol/dm³ respectively. Calculate the equilibrium constant.
a)
62.4
b)
60.8
c)
58.0
d)
38.5
55.
In the fractional distillation of crude oil, the order of collection is
a)
diesel, kerosene and petrol
b)
kerosene, diesel and petrol
c)
kerosene, petrol and diesel
d)
petrol, diesel and kerosene
56.
Given that H = x, S = 318.2JK⁻²mol ⁻² T = 90°C. Calculate the value of x in joules.
a)
115506.0
b)
113306.0
c)
114406.0
d)
112206.0
57.
Which of the following explains vulcanization of rubber?
a)
Hardening the rubber through cross - linkage
b)
Increasing the solubility of the rubber
c)
Removing Sulphur from the rubber
d)
Softening the rubber through cross - linkage
58.
How many faraday(s) of electricity is required to liberate 9g of aluminium? [Al = 27, 1F = 96500C]
a)
0.3
b)
1.0
c)
2.7
d)
3.0
59.
The rate of a chemical reaction can be altered by the following factors except
a)
concentration of the reactants
b)
heat change accompanying the reaction
c)
physical state of the reactants
d)
temperature of the system
60.
The maximum number of electrons that can be accommodated by the K – Shell is
a)
2
b)
4
c)
8
d)
18
61.
The general gas law is derived from the combination of
a)
Avogadro’s law and Dalton’s law
b)
Boyle’s law and Avogadro’s law
c)
Boyle’s law and Charles’ law
d)
Charles’ law and Dalton’s law
62.
Under what conditions do real gases behave like ideal gases?
a)
Low temperature and high pressure
b)
High temperature and low pressure
c)
Low pressure and low temperature
d)
High pressure and high temperature
63.
Which of the following statements is correct about the electrolysis of concentrated CuSO₄ solution using copper electrodes?
a)
The concentration of the electrolyte is unchanged
b)
The electrolyte becomes more acidic
c)
The colour of the solution gradually fades
d)
Oxygen
64.
An application of electrochemistry in which a cheap metal is coated with a less reactive and most often more expensive metal is
a)
metal purification
b)
galvanization
c)
redox reaction
d)
electroplating
65.
The most electronegative element on the periodic table can be found in
a)
group 1, period 1
b)
group 1, period 2
c)
group VII, period 2
d)
group VII, period 3
66.
The position of equilibrium in a reversible reaction is affected
a)
particle size of the reactants
b)
change in concentration of the reactants
c)
maintaining size of the reaction vessel
d)
vigorous stirring of the reaction mixture
67.
The amount of heat energy produced by a system is known as
a)
enthalpy
b)
entropy
c)
exothermic
d)
endothermic
68.
Which of the following quantum numbers gives the number of orbitals present in each energy sub – level?
a)
Spin
b)
Magnetic
c)
Subsidiary
d)
Principal
69.
Consider the reaction below: N₂O₄(g) ⇌ 2NO₂(g) H = +ve. A decrease in temperature of the system would
a)
shift equilibrium position to the right
b)
favour reactant formation
c)
favour product formation
d)
decrease the concentration of reactant and product
70.
If a mixture of 2 moles of helium and 1 mole of neon are contained in a 10dm³ at stp. What would be the partial pressure of helium gas? [PT = 1.01 X 10⁵Nm⁻²]
a)
3.67 x 10⁶ Nm⁻²
b)
6.73 x 10⁶ Nm⁻²
c)
1.52 x 10⁵ Nm⁻²
d)
1.15 x 10⁴ Nm⁻²
71.
Which of the following salts is an acid salt?
a)
NaHSO₄
b)
Na₂SO₄
c)
CaCO₃
d)
NaCl
72.
When P₄O₁₀ is dissolved in water it forms
a)
a hydrated salt
b)
bubbles of oxygen
c)
a basic salt
d)
a weak acid
73.
A saturated solution of a salt R at 30°C contains 0.28g of the salt in 100cm³ of solution. What is the solubility of the salt? [Relative Molar Mass of R = 56]
a)
0.05mol/dm³
b)
0.10mol/dm³
c)
2.80mol/dm³
d)
5.60mol/dm³
74.
Arrange the following gases in order of increasing rate of diffusion: H₂S, NH₃, SO₃, CO₂
[H = 1, C = 12, N = 14, S = 32]
a)
H₂S < NH₃ < SO₃ < CO₂
b)
NH₃ < H₂S < CO₂ < SO₃
c)
SO₃ < CO₂ < H₂S < NH₃
d)
CO₂ < SO₃ < NH₃ < H₂S
75.
A hydrocarbon with a vapour density of 28 contains 14.3% hydrogen by mass. What is the molecular formula of the compound? [H = 1, C = 12]
a)
C₄H₈
b)
C₄H₆
c)
C₂H₄
d)
CH₂
76.
Chemicals produced in small amounts are called
a)
pure chemicals
b)
rare chemicals
c)
fine chemicals
d)
heavy chemicals
77.
Which of the following metals does not show variable oxidation state?
a)
Cr
b)
Ni
c)
Mn
d)
Zn
78.
During crystallization. It is important
a)
to evaporate to near dryness to get pure crystals
b)
to attach gas syringe to collect fumes
c)
not to evaporate water of crystallization
d)
to use high flames
79.
How many electrons are present in the ion ³²₁₆X²⁻?
a)
32
b)
18
c)
16
d)
14
80.
Which of the factors favours the formation of ionic bonds?
a)
Metals with high ionization energy and non – metals with low ionization energy
b)
Low electronegativity difference between bonding atoms
c)
Metals with low ionization energy and non – metals with electron affinity
d)
The bonding atoms must belong to different periods of the periodic table
81.
When S and P block elements react the bond formed is
a)
electrovalent
b)
covalent
c)
metallic
d)
dative - covalent
82.
The types of bond that exist in NH₄Cl are
a)
covalent and ionic bonds
b)
covalent, ionic and hydrogen bonds
c)
ionic and dative bonds
d)
ionic, dative and covalent bonds
83.
A certain volume of a gas is found to weigh 4.4g. An equal volume of hydrogen weighs 0.20g, the relative molar mass of the gas is
a)
44
b)
22
c)
28
d)
64
84.
Change of state of matter can occur when there is change in
a)
mass
b)
volume
c)
density
d)
temperature
85.
The orbital with the lowest energy
a)
3d
b)
4s
c)
4d
d)
4p
86.
Chemistry is often described as a central science because it is
a)
classified as a pure science
b)
used to change one substance to another
c)
classifies as an applied science
d)
featured in all the pure science
87.
Which of the following methods can be used to separate a mixture of two miscible liquids with different boiling points?
a)
Filtration
b)
Evaporation
c)
Decantation
d)
Distillation
88.
Group VII elements in their combined states are called
a)
cations
b)
anions
c)
halogens
d)
halides
89.
Which of the following halogens is most reactive?
a)
Fluorine
b)
Iodine
c)
Bromine
d)
Chlorine
90.
Consider the following reaction equation:
C₃H₄(g) + 2H₂(g) → C₃H₈(g)
The volume of hydrogen that would be required to react completely with 0.65 moles of C₃H₄ at stp is [Molar Volume of a gas at stp = 22.4 dm³]
a)
11.20 dm³
b)
29.12 dm³
c)
33.60 dm³
d)
58.24 dm³
91.
A solute would not dissolve in its solution if the solution is
a)
concentrated
b)
unsaturated
c)
saturated
d)
diluted
92.
Which of the following statements about indicators is always correct?
a)
The midpoint of the pH range of an indicator is 7
b)
The pH of an indicator is lower than its pKa value
c)
The colour red indicate an acidic solution
d)
The pKa value of an indicator is equal to pH value
93.
Which of the following statements about the periodic table is correct?
a)
Group numbers can be used to predict charges of ions.
b)
Metallic character increases from left to right across the period
c)
Elements are arranged in order of decreasing proton number
d)
Group number is the number of electron shells in an atom of the elements.
94.
Factors that affect the speed of chemical reactions does not include
a)
pressure
b)
temperature
c)
volume of gas
d)
change in mass
95.
Which of the following conditions can affect the amount of substance produced in an equilibrium
system?
I. Pressure
II. Catalyst
III. Concentration
IV. Temperature
a)
I and II only
b)
III and IV only
c)
I, III and IV only
d)
I, II, III and IV
96.
Which of the following statements about silver plating is correct?
a)
The electrolyte must contain ions of a more reactive metal
b)
The anode releases silver ions into the electrolyte
c)
The cathode must be a bar of silver
d)
It is only used in plating silver wares
97.
The high boiling point of water is a property arising from the existence of
a)
hydrogen bonding
b)
lattice structure
c)
high density
d)
low volatility
98.
The Faraday’s laws are associated with
a)
temperature and pressure
b)
pressure of gases
c)
reaction of gases
d)
electrolysis
99.
When chlorine water is exposed to sunlight, the products formed are
a)
chlorine gas and hydrogen
b)
chlorine gas and oxochlorate (I) acid
c)
hydrochloric acid and oxygen
d)
oxygen and oxochlorate (I) acid
100.
Arrange the following halogens in order of increasing reactivity: bromine, chlorine, iodine
a)
bromine, chlorine, iodine
b)
iodine, bromine, chlorine
c)
chlorine, bromine, iodine
d)
iodine, chlorine, bromine
Reset
