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 
flask to obtain a Cl
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 
flask to obtain a Cl
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 
flask to obtain a Cl
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.  
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
Answers 
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 
flask to obtain a Cl
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.  
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
Answers 
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. 
 
 
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