Test: Thermodynamics of Electrochemistry

Question 1

Only One Option Correct Type

This section contains 15 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE is correct

Q.

Temperature coefficient of EMF of a cell in terms of entropy change is

Accepted Answer

&Delta;S/nF

Answer

-&Delta;S/nF

Answer

n/&Delta;S

Answer

nF/&Delta;S

Question 2

The standard reduction potential at 298 K of the reaction,

2H₂O + 2e^- H₂ + 2OH^- is 0.8277 V

Thus,thermodynamic equilibrium constant for the reaction.

2H₂O H₃O⁺ + OH^- at 298 K is

Accepted Answer

1.0 x 10^-14

Answer

1.0 x 10¹⁴

Answer

1.0 x 10^-7

Answer

1.0 x 10⁷

Question 3

Given ,

Thus ,equilibrium constant for the reaction in terms of log k is

2Fe³⁺ + 3I^- 2Fe²⁺ + I^-₃

Accepted Answer

7.78

Answer

3.89

Answer

-7.78

Answer

-3.89

Question 4

Given ,

Thus ,(log K_eq) for the reaction Cu²⁺ +In²⁺ Cu⁺ + In³⁺ is

Accepted Answer

10.0

Answer

9.2

Answer

7.8

Answer

11.2

Question 5

An excess of liquid mercury is added to an acidified solution of 1.0 x 10^-3 M Fe³⁺.Thus is if 5% of Fe³⁺ remains at equilibrium at 298 K

Accepted Answer

-0.793 V

Answer

+0.793 V

Answer

-0.397&#160;V

Answer

+0.397&#160;V

Question 6

EMF of the following cell is 0.2905 V

Zn/Zn²⁺(a = 0.1M)|| Fe²⁺ (a = 0.01M)| Fe

The equilibrium constant for the cell reaction is

[IIT JEE 2004]

Accepted Answer

10^0.32/0.0295

Answer

10^0.32/0.059

Answer

10^0.26/0.0295

Answer

10^0.32/0.295

Question 7

The half-cell reactions for rusting of iron are

ΔG^°(in kJ) for the reaction is

[IIT JEE 2005]

Accepted Answer

-322

Answer

-76

Answer

-122

Answer

-176

Question 8

The Gibbs free energy for the decomposition of Al₂O₃at 800 K is as follows :

2Al₂O₃→ 4Al + 3O₂ , Δ_rG = 2898kJ mol^-1

The potential difference needed for electrolytic reduction of Al₂O₃isat least

Accepted Answer

-2.5 V

Answer

4.5 V

Answer

3.0 V

Answer

5.0 V

Question 9

Given ,

The value of standard electrode potential for the half-reaction is

Fe³⁺(aq) + e^- → Fe²⁺(aq)

Accepted Answer

0.63 kJK^-1

Answer

-0.072 V

Answer

0.385 V

Answer

-0.63 kJK^-1

Question 10

For the reaction, 2H₂(g) + O₂(g) → 2H₂O(l), E⁰_cell = 1.23 V at 298 K

and ΔH⁰_f(H₂O) = - 285.8 kJ mol^-1 Thus, ΔS^°(standard entropy change ) is

Accepted Answer

-0.325 kJK^-1

Answer

+3.5 kJK^-1

Answer

0.63 kJK^-1

Answer

-0.63 kJK^-1

Question 11

For the reaction ,

Thus , for the reaction

Accepted Answer

1.70 V

Answer

5.09 V

Answer

0.28 V

Answer

0.84 V

Question 12

Consider the following equations for a cell reaction.

A+B C+ D, E⁰ = x volt, K_eq = K₁

2A +2B 2C+ 2D, E⁰ = y volt, K_eq = K₂

Then,

Accepted Answer

x = y , K₁² = K₂

Answer

x = y , K₁ = K₂

Answer

x = 2y , K₁ = 2K₂

Answer

x² = y , K₁² = K₂

Question 13

Which of the following statements about the spontaneous reaction occurring in a galvanic cell is always true?

Accepted Answer

E_cell > 0, ΔG< 0, Qeq

Answer

E⁰_cell > 0, ΔG⁰ < 0, Q < K_eq

Answer

E⁰_cell > 0, ΔG⁰ < 0, Q > K_eq

Answer

E⁰_cell > 0, ΔG⁰ > 0, Q > K_eq

Question 14

For a (Ag-Zn) button cell ,the net reaction is

Zn(s) + Ag₂O(s) → ZnO(s) + 2Ag(s)

ΔG⁰_f(Ag₂O) = -11.21kJmol^-1, ΔG⁰_f(ZnO) = - 318.3 kJ mol^-1

Hence, E^°_cell of the button cell is

Accepted Answer

1.591 V

Answer

3.182 V

Answer

1.71 V

Answer

-1.591 V

Question 15

For the reaction ,

Thus

Accepted Answer

-4.81 x 10³

Answer

-5.21 x 10³

Answer

-1.303 x 10³

Answer

-1.438 x 10³

Question 16

Matching List Type

Choices for the correct combination of elements from Column I and Column II are given as options (a), (b), (c) and (d), out of which one is correct

Q.

The standard reduction potential data at 298 K is given below:

Match E^° of a redox pair in Column I with the values given in Column II and select the corect answer using the codes given below:

Accepted Answer

d

Answer

a

Answer

b

Answer

c

Question 17

The standard potential of the following cell is 0.23 V at 288 K and 0.21 V at 308 K.

Match the parameters in Column I with their values in Column II and select the answer from the codes given below the list.

Accepted Answer

c

Answer

a

Answer

b

Answer

d

Question 18

Comprehension Type

This section contains a passage describing theory, experiments, data, etc. Two questions related to the paragraph have been given. Each question has only one correct answer out of the given 4 options (a), (b), (c) and (d)

Passage I

The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference across the cell is important in several process such as transmission of nerve impulses and maintaining the ion balance. A simple model for such a concentration cell involving a metal M is

M(s) | M⁺ (aq, 0.05M), || M⁺(aq) 1M|M(s) | E_cell| = 77mV

Q.

For the above cell,

Accepted Answer

E_cell > 0, ΔG < 0

Answer

E_cell < 0, ΔG < 0

Answer

E_cell < 0, ΔG > 0

Answer

None of these

Question 19

Passage I

The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference across the cell is important in several process such as transmission of nerve impulses and maintaining the ion balance. A simple model for such a concentration cell involving a metal M is

M(s) | M⁺ (aq, 0.05M), || M⁺(aq) 1M|M(s) | E_cell| = 77mV

Q.

If 0.05 M solution of M⁺ is replaced by 0.0025 M solution of M⁺,then |E_cell | would be

Accepted Answer

154 mV

Answer

35 mV

Answer

70 mV

Answer

700 mV

Question 20

Passage II

Given,

ΔG⁰_f(AgCl) = -109kJmol^-1, ΔG⁰_f(Cl^-) = -129kJmol^-1

ΔG⁰_f(Ag⁺) = 77kJmol^-1,

Thus E^°_cell of the cell reaction is

Ag⁺(aq) + Cl^-(aq) → AgCl(s) is

Accepted Answer

+0.59 V

Answer

-0.59 V

Answer

+0.29 V

Answer

-0.29 V

Question 21

Passage II

Given,

ΔG⁰_f(AgCl) = -109kJmol^-1, ΔG⁰_f(Cl^-) = -129kJmol^-1

ΔG⁰_f(Ag⁺) = 77kJmol^-1,

Q.

K_sp of AgCl is thus,

Accepted Answer

10-10

Answer

1010

Answer

-5

Answer

-10

Question 22

One Integer Value Correct Type

This section contains 3 questions, when worked out will result in an integer value from 0 to 9 (both inclusive)

Q.

A platinum electrode is immersed in a solution containing 0.1 M Fe²⁺and 0.1 M Fe³⁺.It iscoupled with SHE.Concentration Fe³⁺of increased to 0.1 M without change in [Fe²⁺], then the change in EMF (in centivolt) is

Accepted Answer

Question 23

Using Cr₂O₇^2-aqueous, solution
E⁰_red = 1.33V and ΔG⁰ = -770.07 kJmol^-1

What is the valency of the ion formed after reduction?

Accepted Answer

Question 24

Equilibriumconstant of the cell reaction,

Cu + 2Fe³⁺ 2Fe²⁺+ cu²⁺ is y x 10¹⁴

What is the value of y?

Accepted Answer

Thermodynamics of Electrochemistry - Free MCQ Practice Test with solutions,

MCQ Practice Test & Solutions: Test: Thermodynamics of Electrochemistry (24 Questions)

Only One Option Correct Type
This section contains 15 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE is correct
Q.
Temperature coefficient of EMF of a cell in terms of entropy change is

The standard reduction potential at 298 K of the reaction,
2H₂O + 2e^- H₂ + 2OH^- is 0.8277 V
Thus,thermodynamic equilibrium constant for the reaction.
2H₂O H₃O⁺ + OH^- at 298 K is

Given ,
Thus ,equilibrium constant for the reaction in terms of log k is
2Fe³⁺ + 3I^- 2Fe²⁺ + I^-₃

Given ,
Thus ,(log K_eq) for the reaction Cu²⁺ +In²⁺ Cu⁺ + In³⁺ is

An excess of liquid mercury is added to an acidified solution of 1.0 x 10^-3 M Fe³⁺.Thus is if 5% of Fe³⁺ remains at equilibrium at 298 K

EMF of the following cell is 0.2905 V
Zn/Zn²⁺(a = 0.1M)|| Fe²⁺ (a = 0.01M)| Fe
The equilibrium constant for the cell reaction is
[IIT JEE 2004]

The half-cell reactions for rusting of iron are

ΔG^°(in kJ) for the reaction is
[IIT JEE 2005]

The Gibbs free energy for the decomposition of Al₂O₃at 800 K is as follows :
2Al₂O₃→ 4Al + 3O₂ , Δ_rG = 2898kJ mol^-1
The potential difference needed for electrolytic reduction of Al₂O₃isat least

Given ,
The value of standard electrode potential for the half-reaction is
Fe³⁺(aq) + e^- → Fe²⁺(aq)

For the reaction, 2H₂(g) + O₂(g) → 2H₂O(l), E⁰_cell = 1.23 V at 298 K
and ΔH⁰_f(H₂O) = - 285.8 kJ mol^-1 Thus, ΔS^°(standard entropy change ) is

For the reaction ,
Thus , for the reaction

Consider the following equations for a cell reaction.
A+B  C+ D, E⁰ = x volt, K_eq = K₁
2A +2B  2C+ 2D, E⁰ = y volt, K_eq = K₂
Then,

Which of the following statements about the spontaneous reaction occurring in a galvanic cell is always true?

For a (Ag-Zn) button cell ,the net reaction is
Zn(s) + Ag₂O(s) → ZnO(s) + 2Ag(s)
ΔG⁰_f(Ag₂O) = -11.21kJmol^-1, ΔG⁰_f(ZnO) = - 318.3 kJ mol^-1
Hence, E^°_cell of the button cell is

For the reaction ,
Thus

The standard potential of the following cell is 0.23 V at 288 K and 0.21 V at 308 K.

Match the parameters in Column I with their values in Column II and select the answer from the codes given below the list.

Passage II
Given,
ΔG⁰_f(AgCl) = -109kJmol^-1, ΔG⁰_f(Cl^-) = -129kJmol^-1
ΔG⁰_f(Ag⁺) = 77kJmol^-1,
Thus E^°_cell of the cell reaction is
Ag⁺(aq) + Cl^-(aq) → AgCl(s) is

Passage II
Given,
ΔG⁰_f(AgCl) = -109kJmol^-1, ΔG⁰_f(Cl^-) = -129kJmol^-1
ΔG⁰_f(Ag⁺) = 77kJmol^-1,
Q.
K_sp of AgCl is thus,

Using Cr₂O₇^2-aqueous, solution
E⁰_red = 1.33V and ΔG⁰ = -770.07 kJmol^-1
What is the valency of the ion formed after reduction?

Equilibriumconstant of the cell reaction,
Cu + 2Fe³⁺ 2Fe²⁺+ cu²⁺ is y x 10¹⁴
What is the value of y?

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Thermodynamics of Electrochemistry - Free MCQ Practice Test with solutions,

MCQ Practice Test & Solutions: Test: Thermodynamics of Electrochemistry (24 Questions)

Only One Option Correct TypeThis section contains 15 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE is correctQ. Temperature coefficient of EMF of a cell in terms of entropy change is

The standard reduction potential at 298 K of the reaction, 2H2O + 2e- H2 + 2OH- is 0.8277 VThus,thermodynamic equilibrium constant for the reaction. 2H2O H3O+ + OH- at 298 K is

Given , Thus ,equilibrium constant for the reaction in terms of log k is2Fe3+ + 3I- 2Fe2+ + I-3

Given ,Thus ,(log Keq) for the reaction Cu2+ +In2+ Cu+ + In3+ is

An excess of liquid mercury is added to an acidified solution of 1.0 x 10-3 M Fe3+ .Thus is if 5% of Fe3+ remains at equilibrium at 298 K

EMF of the following cell is 0.2905 VZn/Zn2+ (a = 0.1M)|| Fe2+ (a = 0.01M)| Fe The equilibrium constant for the cell reaction is [IIT JEE 2004]

The half-cell reactions for rusting of iron are ΔG° (in kJ) for the reaction is [IIT JEE 2005]

The Gibbs free energy for the decomposition of Al2O3 at 800 K is as follows :2Al2O3 → 4Al + 3O2 , ΔrG = 2898kJ mol-1The potential difference needed for electrolytic reduction of Al2O3 is at least

Given , The value of standard electrode potential for the half-reaction isFe3+(aq) + e- → Fe2+(aq)

For the reaction, 2H2(g) + O2(g) → 2H2O(l), E0cell = 1.23 V at 298 K and ΔH0f (H2O) = - 285.8 kJ mol-1 Thus, ΔS° (standard entropy change ) is

For the reaction ,Thus , for the reaction

Consider the following equations for a cell reaction. A+B C+ D, E0 = x volt, Keq = K12A +2B 2C+ 2D, E0 = y volt, Keq = K2Then,

Which of the following statements about the spontaneous reaction occurring in a galvanic cell is always true?

For a (Ag-Zn) button cell ,the net reaction is Zn(s) + Ag2O(s) → ZnO(s) + 2Ag(s)ΔG0f(Ag2O) = -11.21kJmol-1, ΔG0 f(ZnO) = - 318.3 kJ mol-1Hence, E°cell of the button cell is

For the reaction ,Thus

The standard potential of the following cell is 0.23 V at 288 K and 0.21 V at 308 K. Match the parameters in Column I with their values in Column II and select the answer from the codes given below the list.

Passage II Given,ΔG0f(AgCl) = -109kJmol-1, ΔG0f(Cl-) = -129kJmol-1ΔG0f(Ag+) = 77kJmol-1,Thus E°cell of the cell reaction is Ag+(aq) + Cl-(aq) → AgCl(s) is

Passage II Given,ΔG0f(AgCl) = -109kJmol-1, ΔG0f(Cl-) = -129kJmol-1ΔG0f(Ag+) = 77kJmol-1,Q. Ksp of AgCl is thus,

Using Cr2O72- aqueous, solution E0red = 1.33V and ΔG0 = -770.07 kJmol-1What is the valency of the ion formed after reduction?

Equilibriumconstant of the cell reaction,Cu + 2Fe3+ 2Fe2+ + cu2+ is y x 1014 What is the value of y?

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Only One Option Correct Type
This section contains 15 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE is correct
Q.
Temperature coefficient of EMF of a cell in terms of entropy change is

The standard reduction potential at 298 K of the reaction,
2H₂O + 2e^- H₂ + 2OH^- is 0.8277 V
Thus,thermodynamic equilibrium constant for the reaction.
2H₂O H₃O⁺ + OH^- at 298 K is

Given ,
Thus ,equilibrium constant for the reaction in terms of log k is
2Fe³⁺ + 3I^- 2Fe²⁺ + I^-₃

Given ,
Thus ,(log K_eq) for the reaction Cu²⁺ +In²⁺ Cu⁺ + In³⁺ is

An excess of liquid mercury is added to an acidified solution of 1.0 x 10^-3 M Fe³⁺.Thus is if 5% of Fe³⁺ remains at equilibrium at 298 K

EMF of the following cell is 0.2905 V
Zn/Zn²⁺(a = 0.1M)|| Fe²⁺ (a = 0.01M)| Fe
The equilibrium constant for the cell reaction is
[IIT JEE 2004]

The half-cell reactions for rusting of iron are

ΔG^°(in kJ) for the reaction is
[IIT JEE 2005]

The Gibbs free energy for the decomposition of Al₂O₃at 800 K is as follows :
2Al₂O₃→ 4Al + 3O₂ , Δ_rG = 2898kJ mol^-1
The potential difference needed for electrolytic reduction of Al₂O₃isat least

Given ,
The value of standard electrode potential for the half-reaction is
Fe³⁺(aq) + e^- → Fe²⁺(aq)

For the reaction, 2H₂(g) + O₂(g) → 2H₂O(l), E⁰_cell = 1.23 V at 298 K
and ΔH⁰_f(H₂O) = - 285.8 kJ mol^-1 Thus, ΔS^°(standard entropy change ) is

For the reaction ,
Thus , for the reaction

Consider the following equations for a cell reaction.
A+B C+ D, E⁰ = x volt, K_eq = K₁
2A +2B 2C+ 2D, E⁰ = y volt, K_eq = K₂
Then,

For a (Ag-Zn) button cell ,the net reaction is
Zn(s) + Ag₂O(s) → ZnO(s) + 2Ag(s)
ΔG⁰_f(Ag₂O) = -11.21kJmol^-1, ΔG⁰_f(ZnO) = - 318.3 kJ mol^-1
Hence, E^°_cell of the button cell is

For the reaction ,
Thus

The standard potential of the following cell is 0.23 V at 288 K and 0.21 V at 308 K.

Match the parameters in Column I with their values in Column II and select the answer from the codes given below the list.

Passage II
Given,
ΔG⁰_f(AgCl) = -109kJmol^-1, ΔG⁰_f(Cl^-) = -129kJmol^-1
ΔG⁰_f(Ag⁺) = 77kJmol^-1,
Thus E^°_cell of the cell reaction is
Ag⁺(aq) + Cl^-(aq) → AgCl(s) is

Passage II
Given,
ΔG⁰_f(AgCl) = -109kJmol^-1, ΔG⁰_f(Cl^-) = -129kJmol^-1
ΔG⁰_f(Ag⁺) = 77kJmol^-1,
Q.
K_sp of AgCl is thus,

Using Cr₂O₇^2-aqueous, solution
E⁰_red = 1.33V and ΔG⁰ = -770.07 kJmol^-1
What is the valency of the ion formed after reduction?

Equilibriumconstant of the cell reaction,
Cu + 2Fe³⁺ 2Fe²⁺+ cu²⁺ is y x 10¹⁴
What is the value of y?