Courses

# CHEMICAL KINETICS, EQUILIBRIUM and ELECTROCHEMISTRY - Sample Test Notes | EduRev

## : CHEMICAL KINETICS, EQUILIBRIUM and ELECTROCHEMISTRY - Sample Test Notes | EduRev

``` Page 1

CHEMICAL KINETICS, EQUILIBRIUM & ELECTROCHEMISTRY
(SET -B) TEST-4
1. The rate of chemical reaction is doubled for
every 10 °C rise in temperature because of
(a) increase in the activation energy
(b) decrease in the activation energy
(c) increase in the number of molecular collision
(d) increase in the number of activated
molecules
2. The velocity of a reaction is doubled for every
10 °C rise in temperature. If temperature is raised
by 50 °C the reaction velocity increases by about
(a) 12 times  (b) 16 times
(c) 32 times   (d) 50 times
3. If the rate of the reaction is equal to the rate
constant, the order of the reaction is
(a) 1   (b) 2
(c) 3   (d) 0
4. For a first order reaction, the half life period is
independent of
(a) initial concentration
(b) cube root of initial concentration
(c) first power of final concentration
(d) square root of final concentration
5. If initial concentration is reduced to 1/4
th
in a
zero order reaction, the time taken for half the
reaction to complete
(a) remains same   (b) becomes 4 times
(c) becomes one-fourth (d) doubles
6. The reaction,
N 2
O
5
(In CCl
4
) ? 2NO
2
+
2
1
O
2
(g)
is first order in N
2
O
5
with the rate constant
6.2 x 10
–4
s
–1
. What is the value of rate of reaction
when [N
2
O
5
] = 1.25 mol L
–1

(a) 7.75 x 10
–4
mol L
–1
s
–1

(b) 6.35 x 10
–3
mol L
–1
s
–1

(c) 5.15 x 10
–5
mol L
–1
s
–1

(d) 3.85 x 10
–4
mol L
–1
s
–1

7. When we increase the temperature, the rate of
reaction increases because of
(a) more number of collisions
(b) decrease in mean free path
(c) more number of energetic electrons
(d) less number of energetic electrons
8. Which of the following has been used to explain
the subject of chemical kinetics
(a) Collision theory of biomolecular reactions
(b) The activated complex theory
(c) Arrhenius equation
(d) All of these
9. In gaseous equilibrium the correct relation
between K c
and K
p
is
(a) K
c
= K
p
(RT)
?
n
(b) K
p
= K
c
(RT)
?
n

(c)
n
p
c
) K (
RT
K
?
=  (d)
n
c
p
) K (
RT
K
?
=
10. Of the given anions, the strongest Bronsted base
is
(a) C ? O
–
(b) C ? O
2
–

(c) C ? O
3
–
(d) C ? O
4
–

11. If 1.0 mole of I
2
is introduced into 1.0 litre flask
at 1000 K, at equilibrium (K
c
= 10
–6
), which one
is correct
(a) [I
2
(g)] > [I
–
(g)]  (b) [I
2
(g)] < [I
–
(g)]
(c) [I
2
(g)] = [I
–
(g)]  (d) [I
2
(g)] =
2
1
[I
–
(g)]
12. The K
sp
of CuS, Ag
2
S and HgS are 10
–31
. 10
–44

and 10
–54
respectively. The solubility of these
sulphides are
(a) Ag
2
S > CuS > HgS
(b) Ag
2
S > HgS > CuS
(c) HgS > Ag
2
S > CuS
(d) CuS > Ag
2
S > HgS
13. 1 mole of N
2
and 2 moles of H
2
are allowed to
react in 1 dm
3
vessel. At equilibrium 0.8 moles of
NH
3
is formed. The concentration of H
2
in the
vessel is
(a) 0.6 moles  (b) 0.8 mole
(c) 0.2 mole  (d) 0.4 mole
14. Dissociation constant of NH
4
OH is 1.8 x 10
–5
.
The hydrolysis constant of NH
4
Cl would be
(a) 1.80 x 10
–19
(b) 5.55 x 10
–10

(c) 5.55 x 10
–5
(d) 1.80 x 10
–5

15. For the reaction C(s) + CO
2
(g)     2CO(g), the
partial pressures of CO
2
and CO are 2.0 and 4.0
atm respectively at equilibrium. The Kp for the
reaction is
(a) 0.5   (b) 4.0
(c) 8.0   (d) 32.0
16. K c
for PCl
5
(g) ? PCl
3
(g) + Cl
2
(g) is 0.04 at 250 °C.
How many moles of PCl
5
must be added to a 3 L
2
concentration of 0.15 M
(a)  4.2 moles  (b)  2.1 moles
(c)  5.5 moles  (d)  6.3 moles
17. 1.08 g of pure silver was converted into silver
nitrate and its solution was taken in a beaker. It
was electrolysed using platinum cathode and
silver anode. 0.01 Faraday of electricity was
passed using 0.15 volt above the decomposition
potential of sliver. The silver content of the
beaker after the above shall be
(a) 0 g   (b) 0.108 g
(c) 0.0108 g   (d) 0.00108 g
18. A current of 2.0 A passed for 5 hours through a
molten metal salt deposits 22.2 g metal (At. wt. =
177). The oxidation state of the metal in the
metal salt is
(a) +1   (b) +2
(c) +3   (d) +4

Page 2

CHEMICAL KINETICS, EQUILIBRIUM & ELECTROCHEMISTRY
(SET -B) TEST-4
1. The rate of chemical reaction is doubled for
every 10 °C rise in temperature because of
(a) increase in the activation energy
(b) decrease in the activation energy
(c) increase in the number of molecular collision
(d) increase in the number of activated
molecules
2. The velocity of a reaction is doubled for every
10 °C rise in temperature. If temperature is raised
by 50 °C the reaction velocity increases by about
(a) 12 times  (b) 16 times
(c) 32 times   (d) 50 times
3. If the rate of the reaction is equal to the rate
constant, the order of the reaction is
(a) 1   (b) 2
(c) 3   (d) 0
4. For a first order reaction, the half life period is
independent of
(a) initial concentration
(b) cube root of initial concentration
(c) first power of final concentration
(d) square root of final concentration
5. If initial concentration is reduced to 1/4
th
in a
zero order reaction, the time taken for half the
reaction to complete
(a) remains same   (b) becomes 4 times
(c) becomes one-fourth (d) doubles
6. The reaction,
N 2
O
5
(In CCl
4
) ? 2NO
2
+
2
1
O
2
(g)
is first order in N
2
O
5
with the rate constant
6.2 x 10
–4
s
–1
. What is the value of rate of reaction
when [N
2
O
5
] = 1.25 mol L
–1

(a) 7.75 x 10
–4
mol L
–1
s
–1

(b) 6.35 x 10
–3
mol L
–1
s
–1

(c) 5.15 x 10
–5
mol L
–1
s
–1

(d) 3.85 x 10
–4
mol L
–1
s
–1

7. When we increase the temperature, the rate of
reaction increases because of
(a) more number of collisions
(b) decrease in mean free path
(c) more number of energetic electrons
(d) less number of energetic electrons
8. Which of the following has been used to explain
the subject of chemical kinetics
(a) Collision theory of biomolecular reactions
(b) The activated complex theory
(c) Arrhenius equation
(d) All of these
9. In gaseous equilibrium the correct relation
between K c
and K
p
is
(a) K
c
= K
p
(RT)
?
n
(b) K
p
= K
c
(RT)
?
n

(c)
n
p
c
) K (
RT
K
?
=  (d)
n
c
p
) K (
RT
K
?
=
10. Of the given anions, the strongest Bronsted base
is
(a) C ? O
–
(b) C ? O
2
–

(c) C ? O
3
–
(d) C ? O
4
–

11. If 1.0 mole of I
2
is introduced into 1.0 litre flask
at 1000 K, at equilibrium (K
c
= 10
–6
), which one
is correct
(a) [I
2
(g)] > [I
–
(g)]  (b) [I
2
(g)] < [I
–
(g)]
(c) [I
2
(g)] = [I
–
(g)]  (d) [I
2
(g)] =
2
1
[I
–
(g)]
12. The K
sp
of CuS, Ag
2
S and HgS are 10
–31
. 10
–44

and 10
–54
respectively. The solubility of these
sulphides are
(a) Ag
2
S > CuS > HgS
(b) Ag
2
S > HgS > CuS
(c) HgS > Ag
2
S > CuS
(d) CuS > Ag
2
S > HgS
13. 1 mole of N
2
and 2 moles of H
2
are allowed to
react in 1 dm
3
vessel. At equilibrium 0.8 moles of
NH
3
is formed. The concentration of H
2
in the
vessel is
(a) 0.6 moles  (b) 0.8 mole
(c) 0.2 mole  (d) 0.4 mole
14. Dissociation constant of NH
4
OH is 1.8 x 10
–5
.
The hydrolysis constant of NH
4
Cl would be
(a) 1.80 x 10
–19
(b) 5.55 x 10
–10

(c) 5.55 x 10
–5
(d) 1.80 x 10
–5

15. For the reaction C(s) + CO
2
(g)     2CO(g), the
partial pressures of CO
2
and CO are 2.0 and 4.0
atm respectively at equilibrium. The Kp for the
reaction is
(a) 0.5   (b) 4.0
(c) 8.0   (d) 32.0
16. K c
for PCl
5
(g) ? PCl
3
(g) + Cl
2
(g) is 0.04 at 250 °C.
How many moles of PCl
5
must be added to a 3 L
2
concentration of 0.15 M
(a)  4.2 moles  (b)  2.1 moles
(c)  5.5 moles  (d)  6.3 moles
17. 1.08 g of pure silver was converted into silver
nitrate and its solution was taken in a beaker. It
was electrolysed using platinum cathode and
silver anode. 0.01 Faraday of electricity was
passed using 0.15 volt above the decomposition
potential of sliver. The silver content of the
beaker after the above shall be
(a) 0 g   (b) 0.108 g
(c) 0.0108 g   (d) 0.00108 g
18. A current of 2.0 A passed for 5 hours through a
molten metal salt deposits 22.2 g metal (At. wt. =
177). The oxidation state of the metal in the
metal salt is
(a) +1   (b) +2
(c) +3   (d) +4

19. The equivalent conductance at infinite dilution
of a weak acid such as HF
(a)  can be determined by extrapolation of
measurement on dilute solutions of HCl, HBr
and HI
(b) can be determined by measurement on very
dilute HF solutions
(c) can best be determined from measurements
on dilute solutions of NaF, NaCl and HCl
(d) is an undefined quantity
20. In the cell, Zn|Zn
2+
||Cu
2+
|Cu, the negative
terminal is
(a) Cu   (b) Cu
2+

(c) Zn   (d) Zn
2+

21. The emf of the cell
Ni/Ni
2+
(1.0M)||Au
3+
(1.0 M)/Au is [E ° for
Ni
2+
/Ni = – 0.25V; E ° for Au
3+
/Au = 1.5 V]
(a) + 1.25 V   (b) + 1.75 V
(c) – 1.25 V   (d) – 1.75 V
22. E° of a cell aA + bB ?? cC +dD is
(a) E + RTlog
D C
B A
] d [ ] c [
] b [ ] a [

(b) E +
b a
d c
] B [ ] A [
] D [ ] C [
log
nF
RT

(c) E +
B A
D c
] B [ ] A [
] d [ ] C [
log
nF
RT

(d) E +
D C
B A
] d [ ] C [
] B [ ] a [
log
nF
RT

23. Prevention of corrosion of iron by Zn coating is
called
(a) Galvanisation
(b) Cathodic protection
(c) Electrolysis
(d) Photoelectrolysis
24. In the electrolytic cell, flow of electrons is from
(a) Cathode to anode in solution
(b) Cathode to anode through external supply
(c) Cathode to anode through internal supply
(d) Anode to cathode through internal supply
25. For a cell reaction involving a two –electron
change, the standard e.m.f. of the cell is found to
be 0.295 V at 25 °C. The equilibrium constant of
the reaction at 25 °C will be
(a)  29.5 × 10
–2
(b)  10
(c)  1 ×10
10
(d)  1 × 10
–10

Assertion –Reason
In every question a statement of ASSERTION
is followed by a statement of REASON .Mark
the correct answer out of the following choices:
(a) If both ASSERTION and REASON are
true and reason is the correct explanation of
the assertion.
(b) If both ASSERTION and REASON are
true but reason is not the correct explanation of
the assertion
(c) If ASSERTION is true but REASON is
false
(d) If both ASSERTION and REASON are
false.
26. Assertion : Rate constant and rate of reaction
may have same units.
Reason : For first order reactions they have
same units.
27.  Assertion : The decomposition of HI on the
surface of gold is first order when the
concentration is low while zero order at higher
concentration.
Reason : The rate of reaction is proportional to
the first power of the concentration of the
reactant for first order reaction.
28. Assertion : A solution of pH = 1 has hydrogen
ion concentration hundred times than that of a
solution of pH = 3
Reason : pH = log
] O H [
1
3
+

29. Assertion :Hydrolysis of sodium acetate results
in an acidic solution.
Reason :It produces H
+
ions in the solution.
30. Assertion : Iron rusts slower in pure water than
in saline water
Reason : Corrosion accelerates in presence of air
and moisture.

Page 3

CHEMICAL KINETICS, EQUILIBRIUM & ELECTROCHEMISTRY
(SET -B) TEST-4
1. The rate of chemical reaction is doubled for
every 10 °C rise in temperature because of
(a) increase in the activation energy
(b) decrease in the activation energy
(c) increase in the number of molecular collision
(d) increase in the number of activated
molecules
2. The velocity of a reaction is doubled for every
10 °C rise in temperature. If temperature is raised
by 50 °C the reaction velocity increases by about
(a) 12 times  (b) 16 times
(c) 32 times   (d) 50 times
3. If the rate of the reaction is equal to the rate
constant, the order of the reaction is
(a) 1   (b) 2
(c) 3   (d) 0
4. For a first order reaction, the half life period is
independent of
(a) initial concentration
(b) cube root of initial concentration
(c) first power of final concentration
(d) square root of final concentration
5. If initial concentration is reduced to 1/4
th
in a
zero order reaction, the time taken for half the
reaction to complete
(a) remains same   (b) becomes 4 times
(c) becomes one-fourth (d) doubles
6. The reaction,
N 2
O
5
(In CCl
4
) ? 2NO
2
+
2
1
O
2
(g)
is first order in N
2
O
5
with the rate constant
6.2 x 10
–4
s
–1
. What is the value of rate of reaction
when [N
2
O
5
] = 1.25 mol L
–1

(a) 7.75 x 10
–4
mol L
–1
s
–1

(b) 6.35 x 10
–3
mol L
–1
s
–1

(c) 5.15 x 10
–5
mol L
–1
s
–1

(d) 3.85 x 10
–4
mol L
–1
s
–1

7. When we increase the temperature, the rate of
reaction increases because of
(a) more number of collisions
(b) decrease in mean free path
(c) more number of energetic electrons
(d) less number of energetic electrons
8. Which of the following has been used to explain
the subject of chemical kinetics
(a) Collision theory of biomolecular reactions
(b) The activated complex theory
(c) Arrhenius equation
(d) All of these
9. In gaseous equilibrium the correct relation
between K c
and K
p
is
(a) K
c
= K
p
(RT)
?
n
(b) K
p
= K
c
(RT)
?
n

(c)
n
p
c
) K (
RT
K
?
=  (d)
n
c
p
) K (
RT
K
?
=
10. Of the given anions, the strongest Bronsted base
is
(a) C ? O
–
(b) C ? O
2
–

(c) C ? O
3
–
(d) C ? O
4
–

11. If 1.0 mole of I
2
is introduced into 1.0 litre flask
at 1000 K, at equilibrium (K
c
= 10
–6
), which one
is correct
(a) [I
2
(g)] > [I
–
(g)]  (b) [I
2
(g)] < [I
–
(g)]
(c) [I
2
(g)] = [I
–
(g)]  (d) [I
2
(g)] =
2
1
[I
–
(g)]
12. The K
sp
of CuS, Ag
2
S and HgS are 10
–31
. 10
–44

and 10
–54
respectively. The solubility of these
sulphides are
(a) Ag
2
S > CuS > HgS
(b) Ag
2
S > HgS > CuS
(c) HgS > Ag
2
S > CuS
(d) CuS > Ag
2
S > HgS
13. 1 mole of N
2
and 2 moles of H
2
are allowed to
react in 1 dm
3
vessel. At equilibrium 0.8 moles of
NH
3
is formed. The concentration of H
2
in the
vessel is
(a) 0.6 moles  (b) 0.8 mole
(c) 0.2 mole  (d) 0.4 mole
14. Dissociation constant of NH
4
OH is 1.8 x 10
–5
.
The hydrolysis constant of NH
4
Cl would be
(a) 1.80 x 10
–19
(b) 5.55 x 10
–10

(c) 5.55 x 10
–5
(d) 1.80 x 10
–5

15. For the reaction C(s) + CO
2
(g)     2CO(g), the
partial pressures of CO
2
and CO are 2.0 and 4.0
atm respectively at equilibrium. The Kp for the
reaction is
(a) 0.5   (b) 4.0
(c) 8.0   (d) 32.0
16. K c
for PCl
5
(g) ? PCl
3
(g) + Cl
2
(g) is 0.04 at 250 °C.
How many moles of PCl
5
must be added to a 3 L
2
concentration of 0.15 M
(a)  4.2 moles  (b)  2.1 moles
(c)  5.5 moles  (d)  6.3 moles
17. 1.08 g of pure silver was converted into silver
nitrate and its solution was taken in a beaker. It
was electrolysed using platinum cathode and
silver anode. 0.01 Faraday of electricity was
passed using 0.15 volt above the decomposition
potential of sliver. The silver content of the
beaker after the above shall be
(a) 0 g   (b) 0.108 g
(c) 0.0108 g   (d) 0.00108 g
18. A current of 2.0 A passed for 5 hours through a
molten metal salt deposits 22.2 g metal (At. wt. =
177). The oxidation state of the metal in the
metal salt is
(a) +1   (b) +2
(c) +3   (d) +4

19. The equivalent conductance at infinite dilution
of a weak acid such as HF
(a)  can be determined by extrapolation of
measurement on dilute solutions of HCl, HBr
and HI
(b) can be determined by measurement on very
dilute HF solutions
(c) can best be determined from measurements
on dilute solutions of NaF, NaCl and HCl
(d) is an undefined quantity
20. In the cell, Zn|Zn
2+
||Cu
2+
|Cu, the negative
terminal is
(a) Cu   (b) Cu
2+

(c) Zn   (d) Zn
2+

21. The emf of the cell
Ni/Ni
2+
(1.0M)||Au
3+
(1.0 M)/Au is [E ° for
Ni
2+
/Ni = – 0.25V; E ° for Au
3+
/Au = 1.5 V]
(a) + 1.25 V   (b) + 1.75 V
(c) – 1.25 V   (d) – 1.75 V
22. E° of a cell aA + bB ?? cC +dD is
(a) E + RTlog
D C
B A
] d [ ] c [
] b [ ] a [

(b) E +
b a
d c
] B [ ] A [
] D [ ] C [
log
nF
RT

(c) E +
B A
D c
] B [ ] A [
] d [ ] C [
log
nF
RT

(d) E +
D C
B A
] d [ ] C [
] B [ ] a [
log
nF
RT

23. Prevention of corrosion of iron by Zn coating is
called
(a) Galvanisation
(b) Cathodic protection
(c) Electrolysis
(d) Photoelectrolysis
24. In the electrolytic cell, flow of electrons is from
(a) Cathode to anode in solution
(b) Cathode to anode through external supply
(c) Cathode to anode through internal supply
(d) Anode to cathode through internal supply
25. For a cell reaction involving a two –electron
change, the standard e.m.f. of the cell is found to
be 0.295 V at 25 °C. The equilibrium constant of
the reaction at 25 °C will be
(a)  29.5 × 10
–2
(b)  10
(c)  1 ×10
10
(d)  1 × 10
–10

Assertion –Reason
In every question a statement of ASSERTION
is followed by a statement of REASON .Mark
the correct answer out of the following choices:
(a) If both ASSERTION and REASON are
true and reason is the correct explanation of
the assertion.
(b) If both ASSERTION and REASON are
true but reason is not the correct explanation of
the assertion
(c) If ASSERTION is true but REASON is
false
(d) If both ASSERTION and REASON are
false.
26. Assertion : Rate constant and rate of reaction
may have same units.
Reason : For first order reactions they have
same units.
27.  Assertion : The decomposition of HI on the
surface of gold is first order when the
concentration is low while zero order at higher
concentration.
Reason : The rate of reaction is proportional to
the first power of the concentration of the
reactant for first order reaction.
28. Assertion : A solution of pH = 1 has hydrogen
ion concentration hundred times than that of a
solution of pH = 3
Reason : pH = log
] O H [
1
3
+

29. Assertion :Hydrolysis of sodium acetate results
in an acidic solution.
Reason :It produces H
+
ions in the solution.
30. Assertion : Iron rusts slower in pure water than
in saline water
Reason : Corrosion accelerates in presence of air
and moisture.

1 D 6 A 11 A 16 B 21 B 26 C
2 C 7 A 12 A 17 A 22 B 27 B
3 D 8 D 13 B 18 C 23 A 28 A
4 A 9 B 14 B 19 C 24 C    29 D
5 C 10 A 15 C 20 C 25 C 30 A

Solutions
1. (D)  With temperature the number of activated
molecules increase.
2. (C)  There are 5 tens hence (2)
5
= 32.
3. (D) Rate = K[A]
0

? Rate = K for zero order.
4. (A) t
1/2
for first order is independent to initial
concentration.
5. (C)  t =
K
a
for zero order, t =
K 4
1
and t
1
=
K 2
1
,
? t
1
= 2t
6. (A) Rate = K[N
2
O
5
] = 6.2 x 10
–4
x 1.25
= 7.75 x 10
–4
mol L
–1
S
–1

7. (A) Increase in number of effective collisions.
8. (D)  All the statements are correct
9. (B) Relation is K
p
= K
c
(RT)
?
n

10. (A) The weaker the conjugate acid, the stronger
is the base and vice versa. HClO is a weak acid,
hence C ? O
–
is a strong base
11. (A)         I
2
2I
–

1 – x     2x
K
c
=
6
2
10
) x 1 (
) x 2 (
-
=
-

12. (A) For CuS solubility is (10
–31
)
1/2

For Ag
2
S =
3 / 1
44
3 / 1
sp
4
10
4
K
?
?
?
?
?
?
?
?
=
?
?
?
?
?
?
?
?
-
and for
HgS = (10
–54
)
1/2

13. (B)           N
2
+         3H
2
2NH
3

Initial mole     1                   2               0
Moles at eqm.1 – 0.4 = 0.6   2 – 3 x 0.4 = 0.8     0.8
14. (B) K
h
=
5
14
b
w
10 x 8 . 1
10
K
K
-
-
= = 5.5 x 10
–10

15. (C) Kp =
2
4 x 4
Kp ;
P
co P
2
CO
2
= = 8; C(s) = 1; the
concentration of solids and liquids are taken as
unity.
16. (B) At equilibrium the moles of Cl
2
must be
= 0.15 × 3= 0.45
PCl
5
? PCl
3
+ Cl
2

3
45 . 0 x -
3
45 . 0

3
45 . 0
Equilibrium conc.
? 0.04 =
3 / ) 45 . 0 x (
15 . 0 15 . 0
-
×

?  x = 2.1 moles
17. (A) Ag
+
+
g 108
F 1
Ag e ?
-

1 F = 1 mole of electrons = 96500 C
0.01 F = 1.08 g Ag;   Ag left = 1.08 – 1.08 = 0
18. (C)  m =
96500
xQ . Wt . E

? E. wt. = 3 . 60
60 x 60 x 5 x 2
96500 x 2 . 22
Q
96500 mx
= =
Oxidation state = 3
3 . 60
177
. wt . Eq
. wt . At
= =
19. (C) Kohlrausch law. ? eq (NaF) + ? eq(HCl) – ?
eq(NaCl) = ? eq (HF)
20. (C) Negative pole is Zn
21. (B) ) Ni ( E ) Au ( E E
0
oxi
0
d Re
0
cell
+ = = 1.5 + 0.25
= 1.75 V
22. (B) E
cell
=
0
cell
E –
b a
d c
] B [ ] A [
] D [ ] C [
In
nF
RT

Hence
0
cell
E = E
cell
+
b a
d c
] B [ ] A [
] D [ ] C [
In
nF
RT

23. (A) Galvanization.
24. (C)  In electrolytic cell the flow of electrons is
from cathode to anode through internal supply.
25. (C) The equilibrium  constant is related to the
standard emf of cell by the expression
log K =
059 . 0
2
295 . 0
059 . 0
n
E
0
cell
× = ×
log K =
59
590
= 10
K = 1 × 10
10

26. (C) Assertion is true but reason is false
For zero order reactions, rate constant and rate
of reaction have the same units.
27. (B) Both assertion and reason are true but reason
is not the correct explanation of assertion
When gas is adsorbed on the surface of a solid
catalyst , the fraction of the surface of catalyst
covered by the reactant is proportional to the
concentration at low values and hence order of
reaction is first order .While at higher
concentrations , the surface of catalyst gets
covered fully & hence rate of reaction becomes
independent of concentration and so zero order
reaction.
28. (A) Both assertion and reason are true and
reason is correct explanation of assertion.
Page 4

CHEMICAL KINETICS, EQUILIBRIUM & ELECTROCHEMISTRY
(SET -B) TEST-4
1. The rate of chemical reaction is doubled for
every 10 °C rise in temperature because of
(a) increase in the activation energy
(b) decrease in the activation energy
(c) increase in the number of molecular collision
(d) increase in the number of activated
molecules
2. The velocity of a reaction is doubled for every
10 °C rise in temperature. If temperature is raised
by 50 °C the reaction velocity increases by about
(a) 12 times  (b) 16 times
(c) 32 times   (d) 50 times
3. If the rate of the reaction is equal to the rate
constant, the order of the reaction is
(a) 1   (b) 2
(c) 3   (d) 0
4. For a first order reaction, the half life period is
independent of
(a) initial concentration
(b) cube root of initial concentration
(c) first power of final concentration
(d) square root of final concentration
5. If initial concentration is reduced to 1/4
th
in a
zero order reaction, the time taken for half the
reaction to complete
(a) remains same   (b) becomes 4 times
(c) becomes one-fourth (d) doubles
6. The reaction,
N 2
O
5
(In CCl
4
) ? 2NO
2
+
2
1
O
2
(g)
is first order in N
2
O
5
with the rate constant
6.2 x 10
–4
s
–1
. What is the value of rate of reaction
when [N
2
O
5
] = 1.25 mol L
–1

(a) 7.75 x 10
–4
mol L
–1
s
–1

(b) 6.35 x 10
–3
mol L
–1
s
–1

(c) 5.15 x 10
–5
mol L
–1
s
–1

(d) 3.85 x 10
–4
mol L
–1
s
–1

7. When we increase the temperature, the rate of
reaction increases because of
(a) more number of collisions
(b) decrease in mean free path
(c) more number of energetic electrons
(d) less number of energetic electrons
8. Which of the following has been used to explain
the subject of chemical kinetics
(a) Collision theory of biomolecular reactions
(b) The activated complex theory
(c) Arrhenius equation
(d) All of these
9. In gaseous equilibrium the correct relation
between K c
and K
p
is
(a) K
c
= K
p
(RT)
?
n
(b) K
p
= K
c
(RT)
?
n

(c)
n
p
c
) K (
RT
K
?
=  (d)
n
c
p
) K (
RT
K
?
=
10. Of the given anions, the strongest Bronsted base
is
(a) C ? O
–
(b) C ? O
2
–

(c) C ? O
3
–
(d) C ? O
4
–

11. If 1.0 mole of I
2
is introduced into 1.0 litre flask
at 1000 K, at equilibrium (K
c
= 10
–6
), which one
is correct
(a) [I
2
(g)] > [I
–
(g)]  (b) [I
2
(g)] < [I
–
(g)]
(c) [I
2
(g)] = [I
–
(g)]  (d) [I
2
(g)] =
2
1
[I
–
(g)]
12. The K
sp
of CuS, Ag
2
S and HgS are 10
–31
. 10
–44

and 10
–54
respectively. The solubility of these
sulphides are
(a) Ag
2
S > CuS > HgS
(b) Ag
2
S > HgS > CuS
(c) HgS > Ag
2
S > CuS
(d) CuS > Ag
2
S > HgS
13. 1 mole of N
2
and 2 moles of H
2
are allowed to
react in 1 dm
3
vessel. At equilibrium 0.8 moles of
NH
3
is formed. The concentration of H
2
in the
vessel is
(a) 0.6 moles  (b) 0.8 mole
(c) 0.2 mole  (d) 0.4 mole
14. Dissociation constant of NH
4
OH is 1.8 x 10
–5
.
The hydrolysis constant of NH
4
Cl would be
(a) 1.80 x 10
–19
(b) 5.55 x 10
–10

(c) 5.55 x 10
–5
(d) 1.80 x 10
–5

15. For the reaction C(s) + CO
2
(g)     2CO(g), the
partial pressures of CO
2
and CO are 2.0 and 4.0
atm respectively at equilibrium. The Kp for the
reaction is
(a) 0.5   (b) 4.0
(c) 8.0   (d) 32.0
16. K c
for PCl
5
(g) ? PCl
3
(g) + Cl
2
(g) is 0.04 at 250 °C.
How many moles of PCl
5
must be added to a 3 L
2
concentration of 0.15 M
(a)  4.2 moles  (b)  2.1 moles
(c)  5.5 moles  (d)  6.3 moles
17. 1.08 g of pure silver was converted into silver
nitrate and its solution was taken in a beaker. It
was electrolysed using platinum cathode and
silver anode. 0.01 Faraday of electricity was
passed using 0.15 volt above the decomposition
potential of sliver. The silver content of the
beaker after the above shall be
(a) 0 g   (b) 0.108 g
(c) 0.0108 g   (d) 0.00108 g
18. A current of 2.0 A passed for 5 hours through a
molten metal salt deposits 22.2 g metal (At. wt. =
177). The oxidation state of the metal in the
metal salt is
(a) +1   (b) +2
(c) +3   (d) +4

19. The equivalent conductance at infinite dilution
of a weak acid such as HF
(a)  can be determined by extrapolation of
measurement on dilute solutions of HCl, HBr
and HI
(b) can be determined by measurement on very
dilute HF solutions
(c) can best be determined from measurements
on dilute solutions of NaF, NaCl and HCl
(d) is an undefined quantity
20. In the cell, Zn|Zn
2+
||Cu
2+
|Cu, the negative
terminal is
(a) Cu   (b) Cu
2+

(c) Zn   (d) Zn
2+

21. The emf of the cell
Ni/Ni
2+
(1.0M)||Au
3+
(1.0 M)/Au is [E ° for
Ni
2+
/Ni = – 0.25V; E ° for Au
3+
/Au = 1.5 V]
(a) + 1.25 V   (b) + 1.75 V
(c) – 1.25 V   (d) – 1.75 V
22. E° of a cell aA + bB ?? cC +dD is
(a) E + RTlog
D C
B A
] d [ ] c [
] b [ ] a [

(b) E +
b a
d c
] B [ ] A [
] D [ ] C [
log
nF
RT

(c) E +
B A
D c
] B [ ] A [
] d [ ] C [
log
nF
RT

(d) E +
D C
B A
] d [ ] C [
] B [ ] a [
log
nF
RT

23. Prevention of corrosion of iron by Zn coating is
called
(a) Galvanisation
(b) Cathodic protection
(c) Electrolysis
(d) Photoelectrolysis
24. In the electrolytic cell, flow of electrons is from
(a) Cathode to anode in solution
(b) Cathode to anode through external supply
(c) Cathode to anode through internal supply
(d) Anode to cathode through internal supply
25. For a cell reaction involving a two –electron
change, the standard e.m.f. of the cell is found to
be 0.295 V at 25 °C. The equilibrium constant of
the reaction at 25 °C will be
(a)  29.5 × 10
–2
(b)  10
(c)  1 ×10
10
(d)  1 × 10
–10

Assertion –Reason
In every question a statement of ASSERTION
is followed by a statement of REASON .Mark
the correct answer out of the following choices:
(a) If both ASSERTION and REASON are
true and reason is the correct explanation of
the assertion.
(b) If both ASSERTION and REASON are
true but reason is not the correct explanation of
the assertion
(c) If ASSERTION is true but REASON is
false
(d) If both ASSERTION and REASON are
false.
26. Assertion : Rate constant and rate of reaction
may have same units.
Reason : For first order reactions they have
same units.
27.  Assertion : The decomposition of HI on the
surface of gold is first order when the
concentration is low while zero order at higher
concentration.
Reason : The rate of reaction is proportional to
the first power of the concentration of the
reactant for first order reaction.
28. Assertion : A solution of pH = 1 has hydrogen
ion concentration hundred times than that of a
solution of pH = 3
Reason : pH = log
] O H [
1
3
+

29. Assertion :Hydrolysis of sodium acetate results
in an acidic solution.
Reason :It produces H
+
ions in the solution.
30. Assertion : Iron rusts slower in pure water than
in saline water
Reason : Corrosion accelerates in presence of air
and moisture.

1 D 6 A 11 A 16 B 21 B 26 C
2 C 7 A 12 A 17 A 22 B 27 B
3 D 8 D 13 B 18 C 23 A 28 A
4 A 9 B 14 B 19 C 24 C    29 D
5 C 10 A 15 C 20 C 25 C 30 A

Solutions
1. (D)  With temperature the number of activated
molecules increase.
2. (C)  There are 5 tens hence (2)
5
= 32.
3. (D) Rate = K[A]
0

? Rate = K for zero order.
4. (A) t
1/2
for first order is independent to initial
concentration.
5. (C)  t =
K
a
for zero order, t =
K 4
1
and t
1
=
K 2
1
,
? t
1
= 2t
6. (A) Rate = K[N
2
O
5
] = 6.2 x 10
–4
x 1.25
= 7.75 x 10
–4
mol L
–1
S
–1

7. (A) Increase in number of effective collisions.
8. (D)  All the statements are correct
9. (B) Relation is K
p
= K
c
(RT)
?
n

10. (A) The weaker the conjugate acid, the stronger
is the base and vice versa. HClO is a weak acid,
hence C ? O
–
is a strong base
11. (A)         I
2
2I
–

1 – x     2x
K
c
=
6
2
10
) x 1 (
) x 2 (
-
=
-

12. (A) For CuS solubility is (10
–31
)
1/2

For Ag
2
S =
3 / 1
44
3 / 1
sp
4
10
4
K
?
?
?
?
?
?
?
?
=
?
?
?
?
?
?
?
?
-
and for
HgS = (10
–54
)
1/2

13. (B)           N
2
+         3H
2
2NH
3

Initial mole     1                   2               0
Moles at eqm.1 – 0.4 = 0.6   2 – 3 x 0.4 = 0.8     0.8
14. (B) K
h
=
5
14
b
w
10 x 8 . 1
10
K
K
-
-
= = 5.5 x 10
–10

15. (C) Kp =
2
4 x 4
Kp ;
P
co P
2
CO
2
= = 8; C(s) = 1; the
concentration of solids and liquids are taken as
unity.
16. (B) At equilibrium the moles of Cl
2
must be
= 0.15 × 3= 0.45
PCl
5
? PCl
3
+ Cl
2

3
45 . 0 x -
3
45 . 0

3
45 . 0
Equilibrium conc.
? 0.04 =
3 / ) 45 . 0 x (
15 . 0 15 . 0
-
×

?  x = 2.1 moles
17. (A) Ag
+
+
g 108
F 1
Ag e ?
-

1 F = 1 mole of electrons = 96500 C
0.01 F = 1.08 g Ag;   Ag left = 1.08 – 1.08 = 0
18. (C)  m =
96500
xQ . Wt . E

? E. wt. = 3 . 60
60 x 60 x 5 x 2
96500 x 2 . 22
Q
96500 mx
= =
Oxidation state = 3
3 . 60
177
. wt . Eq
. wt . At
= =
19. (C) Kohlrausch law. ? eq (NaF) + ? eq(HCl) – ?
eq(NaCl) = ? eq (HF)
20. (C) Negative pole is Zn
21. (B) ) Ni ( E ) Au ( E E
0
oxi
0
d Re
0
cell
+ = = 1.5 + 0.25
= 1.75 V
22. (B) E
cell
=
0
cell
E –
b a
d c
] B [ ] A [
] D [ ] C [
In
nF
RT

Hence
0
cell
E = E
cell
+
b a
d c
] B [ ] A [
] D [ ] C [
In
nF
RT

23. (A) Galvanization.
24. (C)  In electrolytic cell the flow of electrons is
from cathode to anode through internal supply.
25. (C) The equilibrium  constant is related to the
standard emf of cell by the expression
log K =
059 . 0
2
295 . 0
059 . 0
n
E
0
cell
× = ×
log K =
59
590
= 10
K = 1 × 10
10

26. (C) Assertion is true but reason is false
For zero order reactions, rate constant and rate
of reaction have the same units.
27. (B) Both assertion and reason are true but reason
is not the correct explanation of assertion
When gas is adsorbed on the surface of a solid
catalyst , the fraction of the surface of catalyst
covered by the reactant is proportional to the
concentration at low values and hence order of
reaction is first order .While at higher
concentrations , the surface of catalyst gets
covered fully & hence rate of reaction becomes
independent of concentration and so zero order
reaction.
28. (A) Both assertion and reason are true and
reason is correct explanation of assertion.

A solution of pH = 1 has hydrogen ion
concentration 100 times than that of a  solution
of pH = 3
pH = - log [H
3
O
+
] =
] O H log[
1
3
+

29. (D) Both assertion and reason are false.
Sodium acetate (CH
3
COONa) is a salt of a
weak acid (CH
3
COOH) and a strong base
(NaOH).Salts of weak acids and strong bases
on hydrolysis  result in an alkaline solution
because OH
-
ions are formed
CH
3
COONa + H
2
O ?CH
3
COOH +NaOH
or
CH
3
COO
-
+Na
+
+H
2
O ?CH
3
COOH +Na
+
OH
-

or
CH
3
COO
-
+ H
2
O ?CH
3
COOH + OH
-

30. (a) Both assertion and reason are true and
reason is the correct explanation of assertion.
As electrolytes increase the rate of corrosion
and therefore iron rusts faster in saline water
than in pure water.

```
Offer running on EduRev: Apply code STAYHOME200 to get INR 200 off on our premium plan EduRev Infinity!