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CHXII03:ELECTROCHEMISTRY

330424 For the reduction of silver ions with copper metal, the standard cell potential is 0.46 V at $25^{\circ} C$ . The value of standard Gibbs energy $Δ G^{o}$ will be

1

- 44 .5 V

2

- 98 .0 k J

3

- 89 .0 k J

4

- 89 .0 J

Explanation:

$Δ G^{o} = - n E^{o} F (f o r C u + 2 A g^{+} \to C u^{2 +} + 2 A g)$
$= - 2 \times 0 .46 \times 96500$
$= - 88788 J = - 89 .0 k J$

CHXII03:ELECTROCHEMISTRY

330425 For the cell $Mg (s) | {Mg}^{2 +} (aq) | | {Ag}^{+} (aq) | Ag (s)$ , the maximum work that can be obtained during operation of cell at $25^{\circ} C$ is ____.
Given $E_{Mg / {Mg}^{2 +}}^{0} = + 2.37 V$ and $E_{{Ag}^{+} / Ag}^{\circ} = + 0.80 V$

1

6.118 \times 10 k J

2

6.118 \times 10^{2} k J

3

6.118 \times 10^{3} k J

4

6.118 \times 10^{4} k J

Explanation:

$E_{cell} = (0.059 / 2) log K_{c}$
$∵ E_{cell} = E_{O P_{Mg}}^{\circ} + E_{R P_{Ag}}^{\circ}$ for the change
$Mg + 2 {Ag}^{+} \to {Mg}^{2 +} + 2 Ag$
or $E_{O P_{Mg}} + E_{R P_{Ag}}^{\circ} = (0.059 / 2) log K_{c}$
or $2.37 + 0.80 = (0.059 / 2) log K_{c}$
or $\log K_{c} = 107.457$ and $E_{cell} = 3.17 V$
For maximum work
$- Δ G^{\circ} = W_{max}$
$W_{max} = nF \times E^{\circ} = 2 \times 96500 \times 3.17$
$= 6.118 \times 10^{5}$ joule
$= 6.118 \times 10^{2} kJ$

CHXII03:ELECTROCHEMISTRY

330426 $Δ G^{o}$ of the cell reaction $AgCl(s) + \frac{1}{2} H_{2} (g) ⇌ Ag(s) + H^{+} + C l^{-}$ $i s - 21 .52 k J$ .
$Δ G^{o} of 2AgCl(s) + H_{2} (g) ⇌ 2Ag(s) + 2 H^{+} + 2C l^{-}$ is

1 -21.52 kJ

2 43.04 kJ

3 -10.76 kJ

4 -43.04 kJ

Explanation:

$K_{C_{2}} {= K}_{C_{1}}^{2}$
$∴ Δ G = - n F E^{o} = - R T l n K_{C}$
$∴ Δ G_{2} = 2 \times (- 21 .52) = - 43 .04 k J$

CHXII03:ELECTROCHEMISTRY

330427 Assertion :
In equation $Δ_{r} G = - {nFE}_{cell}$ , value of $Δ_{r} G$ depends on $n$ .
Reason :
$E_{cell}$ is an intensive property and $Δ_{r} G$ is an extensive property.

1 Both Assertion and Reason are true and Reason is not the correct explanation of Assertion.

2 Assertion is true but Reason is false.

3 Assertion is false but Reason is true.

4 Both Assertion and Reason are true and Reason is the correct explanation of Assertion.

Explanation:

$Δ_{r} G = - {nFE}_{cell}$
$E_{cell}$ is an intensive property and $Δ_{r} G$ is an extensive property as it depends on number of $e^{⊖}$ transferred in cell reaction

NEET - 2023

CHXII03:ELECTROCHEMISTRY

330428 How many kJ of energy is spent when a current of 4 amp passes for 200 second under a potential of 115 V?

1 72 kJ

2 82 kJ

3 52 kJ

4

- 92 k J

Explanation:

$Δ G = - n F E = - Q E$
$= - 4 \times 200 \times 115 \times 1 0^{- 3} k J$
$Δ G = - 92 k J$

CHXII03:ELECTROCHEMISTRY

330424 For the reduction of silver ions with copper metal, the standard cell potential is 0.46 V at $25^{\circ} C$ . The value of standard Gibbs energy $Δ G^{o}$ will be

1

- 44 .5 V

2

- 98 .0 k J

3

- 89 .0 k J

4

- 89 .0 J

Explanation:

$Δ G^{o} = - n E^{o} F (f o r C u + 2 A g^{+} \to C u^{2 +} + 2 A g)$
$= - 2 \times 0 .46 \times 96500$
$= - 88788 J = - 89 .0 k J$

CHXII03:ELECTROCHEMISTRY

330425 For the cell $Mg (s) | {Mg}^{2 +} (aq) | | {Ag}^{+} (aq) | Ag (s)$ , the maximum work that can be obtained during operation of cell at $25^{\circ} C$ is ____.
Given $E_{Mg / {Mg}^{2 +}}^{0} = + 2.37 V$ and $E_{{Ag}^{+} / Ag}^{\circ} = + 0.80 V$

1

6.118 \times 10 k J

2

6.118 \times 10^{2} k J

3

6.118 \times 10^{3} k J

4

6.118 \times 10^{4} k J

Explanation:

$E_{cell} = (0.059 / 2) log K_{c}$
$∵ E_{cell} = E_{O P_{Mg}}^{\circ} + E_{R P_{Ag}}^{\circ}$ for the change
$Mg + 2 {Ag}^{+} \to {Mg}^{2 +} + 2 Ag$
or $E_{O P_{Mg}} + E_{R P_{Ag}}^{\circ} = (0.059 / 2) log K_{c}$
or $2.37 + 0.80 = (0.059 / 2) log K_{c}$
or $\log K_{c} = 107.457$ and $E_{cell} = 3.17 V$
For maximum work
$- Δ G^{\circ} = W_{max}$
$W_{max} = nF \times E^{\circ} = 2 \times 96500 \times 3.17$
$= 6.118 \times 10^{5}$ joule
$= 6.118 \times 10^{2} kJ$

CHXII03:ELECTROCHEMISTRY

330426 $Δ G^{o}$ of the cell reaction $AgCl(s) + \frac{1}{2} H_{2} (g) ⇌ Ag(s) + H^{+} + C l^{-}$ $i s - 21 .52 k J$ .
$Δ G^{o} of 2AgCl(s) + H_{2} (g) ⇌ 2Ag(s) + 2 H^{+} + 2C l^{-}$ is

1 -21.52 kJ

2 43.04 kJ

3 -10.76 kJ

4 -43.04 kJ

Explanation:

$K_{C_{2}} {= K}_{C_{1}}^{2}$
$∴ Δ G = - n F E^{o} = - R T l n K_{C}$
$∴ Δ G_{2} = 2 \times (- 21 .52) = - 43 .04 k J$

CHXII03:ELECTROCHEMISTRY

330427 Assertion :
In equation $Δ_{r} G = - {nFE}_{cell}$ , value of $Δ_{r} G$ depends on $n$ .
Reason :
$E_{cell}$ is an intensive property and $Δ_{r} G$ is an extensive property.

1 Both Assertion and Reason are true and Reason is not the correct explanation of Assertion.

2 Assertion is true but Reason is false.

3 Assertion is false but Reason is true.

4 Both Assertion and Reason are true and Reason is the correct explanation of Assertion.

Explanation:

$Δ_{r} G = - {nFE}_{cell}$
$E_{cell}$ is an intensive property and $Δ_{r} G$ is an extensive property as it depends on number of $e^{⊖}$ transferred in cell reaction

NEET - 2023

CHXII03:ELECTROCHEMISTRY

330428 How many kJ of energy is spent when a current of 4 amp passes for 200 second under a potential of 115 V?

1 72 kJ

2 82 kJ

3 52 kJ

4

- 92 k J

Explanation:

$Δ G = - n F E = - Q E$
$= - 4 \times 200 \times 115 \times 1 0^{- 3} k J$
$Δ G = - 92 k J$

CHXII03:ELECTROCHEMISTRY

330424 For the reduction of silver ions with copper metal, the standard cell potential is 0.46 V at $25^{\circ} C$ . The value of standard Gibbs energy $Δ G^{o}$ will be

1

- 44 .5 V

2

- 98 .0 k J

3

- 89 .0 k J

4

- 89 .0 J

Explanation:

$Δ G^{o} = - n E^{o} F (f o r C u + 2 A g^{+} \to C u^{2 +} + 2 A g)$
$= - 2 \times 0 .46 \times 96500$
$= - 88788 J = - 89 .0 k J$

CHXII03:ELECTROCHEMISTRY

330425 For the cell $Mg (s) | {Mg}^{2 +} (aq) | | {Ag}^{+} (aq) | Ag (s)$ , the maximum work that can be obtained during operation of cell at $25^{\circ} C$ is ____.
Given $E_{Mg / {Mg}^{2 +}}^{0} = + 2.37 V$ and $E_{{Ag}^{+} / Ag}^{\circ} = + 0.80 V$

1

6.118 \times 10 k J

2

6.118 \times 10^{2} k J

3

6.118 \times 10^{3} k J

4

6.118 \times 10^{4} k J

Explanation:

$E_{cell} = (0.059 / 2) log K_{c}$
$∵ E_{cell} = E_{O P_{Mg}}^{\circ} + E_{R P_{Ag}}^{\circ}$ for the change
$Mg + 2 {Ag}^{+} \to {Mg}^{2 +} + 2 Ag$
or $E_{O P_{Mg}} + E_{R P_{Ag}}^{\circ} = (0.059 / 2) log K_{c}$
or $2.37 + 0.80 = (0.059 / 2) log K_{c}$
or $\log K_{c} = 107.457$ and $E_{cell} = 3.17 V$
For maximum work
$- Δ G^{\circ} = W_{max}$
$W_{max} = nF \times E^{\circ} = 2 \times 96500 \times 3.17$
$= 6.118 \times 10^{5}$ joule
$= 6.118 \times 10^{2} kJ$

CHXII03:ELECTROCHEMISTRY

330426 $Δ G^{o}$ of the cell reaction $AgCl(s) + \frac{1}{2} H_{2} (g) ⇌ Ag(s) + H^{+} + C l^{-}$ $i s - 21 .52 k J$ .
$Δ G^{o} of 2AgCl(s) + H_{2} (g) ⇌ 2Ag(s) + 2 H^{+} + 2C l^{-}$ is

1 -21.52 kJ

2 43.04 kJ

3 -10.76 kJ

4 -43.04 kJ

Explanation:

$K_{C_{2}} {= K}_{C_{1}}^{2}$
$∴ Δ G = - n F E^{o} = - R T l n K_{C}$
$∴ Δ G_{2} = 2 \times (- 21 .52) = - 43 .04 k J$

CHXII03:ELECTROCHEMISTRY

330427 Assertion :
In equation $Δ_{r} G = - {nFE}_{cell}$ , value of $Δ_{r} G$ depends on $n$ .
Reason :
$E_{cell}$ is an intensive property and $Δ_{r} G$ is an extensive property.

1 Both Assertion and Reason are true and Reason is not the correct explanation of Assertion.

2 Assertion is true but Reason is false.

3 Assertion is false but Reason is true.

4 Both Assertion and Reason are true and Reason is the correct explanation of Assertion.

Explanation:

$Δ_{r} G = - {nFE}_{cell}$
$E_{cell}$ is an intensive property and $Δ_{r} G$ is an extensive property as it depends on number of $e^{⊖}$ transferred in cell reaction

NEET - 2023

CHXII03:ELECTROCHEMISTRY

330428 How many kJ of energy is spent when a current of 4 amp passes for 200 second under a potential of 115 V?

1 72 kJ

2 82 kJ

3 52 kJ

4

- 92 k J

Explanation:

$Δ G = - n F E = - Q E$
$= - 4 \times 200 \times 115 \times 1 0^{- 3} k J$
$Δ G = - 92 k J$

CHXII03:ELECTROCHEMISTRY

330424 For the reduction of silver ions with copper metal, the standard cell potential is 0.46 V at $25^{\circ} C$ . The value of standard Gibbs energy $Δ G^{o}$ will be

1

- 44 .5 V

2

- 98 .0 k J

3

- 89 .0 k J

4

- 89 .0 J

Explanation:

$Δ G^{o} = - n E^{o} F (f o r C u + 2 A g^{+} \to C u^{2 +} + 2 A g)$
$= - 2 \times 0 .46 \times 96500$
$= - 88788 J = - 89 .0 k J$

CHXII03:ELECTROCHEMISTRY

330425 For the cell $Mg (s) | {Mg}^{2 +} (aq) | | {Ag}^{+} (aq) | Ag (s)$ , the maximum work that can be obtained during operation of cell at $25^{\circ} C$ is ____.
Given $E_{Mg / {Mg}^{2 +}}^{0} = + 2.37 V$ and $E_{{Ag}^{+} / Ag}^{\circ} = + 0.80 V$

1

6.118 \times 10 k J

2

6.118 \times 10^{2} k J

3

6.118 \times 10^{3} k J

4

6.118 \times 10^{4} k J

Explanation:

$E_{cell} = (0.059 / 2) log K_{c}$
$∵ E_{cell} = E_{O P_{Mg}}^{\circ} + E_{R P_{Ag}}^{\circ}$ for the change
$Mg + 2 {Ag}^{+} \to {Mg}^{2 +} + 2 Ag$
or $E_{O P_{Mg}} + E_{R P_{Ag}}^{\circ} = (0.059 / 2) log K_{c}$
or $2.37 + 0.80 = (0.059 / 2) log K_{c}$
or $\log K_{c} = 107.457$ and $E_{cell} = 3.17 V$
For maximum work
$- Δ G^{\circ} = W_{max}$
$W_{max} = nF \times E^{\circ} = 2 \times 96500 \times 3.17$
$= 6.118 \times 10^{5}$ joule
$= 6.118 \times 10^{2} kJ$

CHXII03:ELECTROCHEMISTRY

330426 $Δ G^{o}$ of the cell reaction $AgCl(s) + \frac{1}{2} H_{2} (g) ⇌ Ag(s) + H^{+} + C l^{-}$ $i s - 21 .52 k J$ .
$Δ G^{o} of 2AgCl(s) + H_{2} (g) ⇌ 2Ag(s) + 2 H^{+} + 2C l^{-}$ is

1 -21.52 kJ

2 43.04 kJ

3 -10.76 kJ

4 -43.04 kJ

Explanation:

$K_{C_{2}} {= K}_{C_{1}}^{2}$
$∴ Δ G = - n F E^{o} = - R T l n K_{C}$
$∴ Δ G_{2} = 2 \times (- 21 .52) = - 43 .04 k J$

CHXII03:ELECTROCHEMISTRY

330427 Assertion :
In equation $Δ_{r} G = - {nFE}_{cell}$ , value of $Δ_{r} G$ depends on $n$ .
Reason :
$E_{cell}$ is an intensive property and $Δ_{r} G$ is an extensive property.

1 Both Assertion and Reason are true and Reason is not the correct explanation of Assertion.

2 Assertion is true but Reason is false.

3 Assertion is false but Reason is true.

4 Both Assertion and Reason are true and Reason is the correct explanation of Assertion.

Explanation:

$Δ_{r} G = - {nFE}_{cell}$
$E_{cell}$ is an intensive property and $Δ_{r} G$ is an extensive property as it depends on number of $e^{⊖}$ transferred in cell reaction

NEET - 2023

CHXII03:ELECTROCHEMISTRY

330428 How many kJ of energy is spent when a current of 4 amp passes for 200 second under a potential of 115 V?

1 72 kJ

2 82 kJ

3 52 kJ

4

- 92 k J

Explanation:

$Δ G = - n F E = - Q E$
$= - 4 \times 200 \times 115 \times 1 0^{- 3} k J$
$Δ G = - 92 k J$

CHXII03:ELECTROCHEMISTRY

330424 For the reduction of silver ions with copper metal, the standard cell potential is 0.46 V at $25^{\circ} C$ . The value of standard Gibbs energy $Δ G^{o}$ will be

1

- 44 .5 V

2

- 98 .0 k J

3

- 89 .0 k J

4

- 89 .0 J

Explanation:

$Δ G^{o} = - n E^{o} F (f o r C u + 2 A g^{+} \to C u^{2 +} + 2 A g)$
$= - 2 \times 0 .46 \times 96500$
$= - 88788 J = - 89 .0 k J$

CHXII03:ELECTROCHEMISTRY

330425 For the cell $Mg (s) | {Mg}^{2 +} (aq) | | {Ag}^{+} (aq) | Ag (s)$ , the maximum work that can be obtained during operation of cell at $25^{\circ} C$ is ____.
Given $E_{Mg / {Mg}^{2 +}}^{0} = + 2.37 V$ and $E_{{Ag}^{+} / Ag}^{\circ} = + 0.80 V$

1

6.118 \times 10 k J

2

6.118 \times 10^{2} k J

3

6.118 \times 10^{3} k J

4

6.118 \times 10^{4} k J

Explanation:

$E_{cell} = (0.059 / 2) log K_{c}$
$∵ E_{cell} = E_{O P_{Mg}}^{\circ} + E_{R P_{Ag}}^{\circ}$ for the change
$Mg + 2 {Ag}^{+} \to {Mg}^{2 +} + 2 Ag$
or $E_{O P_{Mg}} + E_{R P_{Ag}}^{\circ} = (0.059 / 2) log K_{c}$
or $2.37 + 0.80 = (0.059 / 2) log K_{c}$
or $\log K_{c} = 107.457$ and $E_{cell} = 3.17 V$
For maximum work
$- Δ G^{\circ} = W_{max}$
$W_{max} = nF \times E^{\circ} = 2 \times 96500 \times 3.17$
$= 6.118 \times 10^{5}$ joule
$= 6.118 \times 10^{2} kJ$

CHXII03:ELECTROCHEMISTRY

330426 $Δ G^{o}$ of the cell reaction $AgCl(s) + \frac{1}{2} H_{2} (g) ⇌ Ag(s) + H^{+} + C l^{-}$ $i s - 21 .52 k J$ .
$Δ G^{o} of 2AgCl(s) + H_{2} (g) ⇌ 2Ag(s) + 2 H^{+} + 2C l^{-}$ is

1 -21.52 kJ

2 43.04 kJ

3 -10.76 kJ

4 -43.04 kJ

Explanation:

$K_{C_{2}} {= K}_{C_{1}}^{2}$
$∴ Δ G = - n F E^{o} = - R T l n K_{C}$
$∴ Δ G_{2} = 2 \times (- 21 .52) = - 43 .04 k J$

CHXII03:ELECTROCHEMISTRY

330427 Assertion :
In equation $Δ_{r} G = - {nFE}_{cell}$ , value of $Δ_{r} G$ depends on $n$ .
Reason :
$E_{cell}$ is an intensive property and $Δ_{r} G$ is an extensive property.

1 Both Assertion and Reason are true and Reason is not the correct explanation of Assertion.

2 Assertion is true but Reason is false.

3 Assertion is false but Reason is true.

4 Both Assertion and Reason are true and Reason is the correct explanation of Assertion.

Explanation:

$Δ_{r} G = - {nFE}_{cell}$
$E_{cell}$ is an intensive property and $Δ_{r} G$ is an extensive property as it depends on number of $e^{⊖}$ transferred in cell reaction

NEET - 2023

CHXII03:ELECTROCHEMISTRY

330428 How many kJ of energy is spent when a current of 4 amp passes for 200 second under a potential of 115 V?

1 72 kJ

2 82 kJ

3 52 kJ

4

- 92 k J

Explanation:

$Δ G = - n F E = - Q E$
$= - 4 \times 200 \times 115 \times 1 0^{- 3} k J$
$Δ G = - 92 k J$