QBManager

ELECTROCHEMISTRY

275821 For the electrochemical cell,
${Ag}^{+} | AgCl | KCl | | {AgNO}_{3} ∣ {A g}^{+}$ , the overall cell reaction is

1

{Ag}^{+} + KCl \to AgCl (s) + K^{+}

2

Ag + AgCl \to 2 Ag + \frac{1}{2} {Cl}_{2}

3

AgCl (s) \to {Ag}^{+} + {Cl}^{-}

4

{Ag}^{+} + {Cl}^{-} \to AgCl (s)

Explanation:

For the electrochemical cell,
${Ag}^{-} | AgCl | KCl | | {AgNO}_{3} ∣ {Ag}^{+}$
The cell reaction is,
$AgCl (s) + e^{-} \to Ag + {Cl}^{-}$ (aq)
$Ag \to {Ag}^{+} (aq) + e^{-}$
Overall reaction
$AgCl (s) \to {Ag}^{+} + {Cl}^{-}$

JIPMER-2018

ELECTROCHEMISTRY

275822 If $E^{0} ({Zn}^{2 +}, Zn) = - 0.763 V$ and $E^{0} ({Fe}^{2 +}, Fe) =$ $- 0.44 V$ , then the emf of the cell $Zn ∣ {Zn}^{2 +} (a =$ 0.001) $| {Fe}^{2 +} (a = 0.005) | Fe$ is

1 equal to

0.323 V

2 less than

0.323 V

3 greater than

0.323 V

4 equal to

1.103 V

Explanation:

The cell reaction is-
$Zn + {Fe}^{2 +} ⟶ {Zn}^{2 +} + Fe$
From Nernst equation
$\begin{aligned} E_{cell} = E_{cell}^{o} - \frac{0.0591}{n} \log \frac{a_{{Zn}^{2 +}}}{a_{{Fe}^{2 +}}} \\ = (0.763 - 0.44) - \frac{0.0591}{1} \log \frac{0.001}{0.005} \\ = 0.364 V \end{aligned}$

JIPMER-2018

ELECTROCHEMISTRY

275823 For a cell involving two electron changes, $E_{cell}^{o} = 0.3 V$ at $25^{\circ} C$ . The equilibrium constant of the reaction is

1

10^{- 10}

2

3 \times 10^{- 2}

3 10

4

10^{10}

Explanation:

For $Δ G^{\circ}$ is related to $K_{sp}$ by the equation,
$\begin{aligned} Δ G^{o} = & - 2.303 RT \log K_{sp} \\ \log K_{sp} & = \frac{- Δ G^{o}}{2.303 RT} = \frac{{nFE}_{cell}^{o}}{2.303 RT} (at 25^{\circ} C) \\ = \frac{2 E_{cell}^{o}}{0.0591} = \frac{2 \times 0.3}{0.0591} = 10 \end{aligned}$
$\log K_{sp} = 10 \Rightarrow K_{sp} = 10^{10}$

Karnataka-CET-2018

ELECTROCHEMISTRY

275819 Assertion: When I M CusO $_{4}$ (aq) solution is electrolysed using copper electrodes, copper is dissolved at anode and copper gets deposites at cathode.
Reason: The standard oxidation potential of copper is less than the standard oxidation potential of water and standard reduction potential of copper is greater than the standard reduction potential of water.

1 If Assertion is correct but Reason is in correct.

2 If both the Assertion and Reason are incorrect.

3 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.

4 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.

Explanation:

Copper is dissolved at anode and deposited at cathode when $Cu$ electrodes are used and electrolyte is $1 M {CuSO}_{4} (aq)$ solution as standard oxidation potential of $Cu$ is higher than standard oxidation potential of water and standard reduction potential of $Cu$ is greater than standard reduction potential of water.

AIIMS-26 May

ELECTROCHEMISTRY

275821 For the electrochemical cell,
${Ag}^{+} | AgCl | KCl | | {AgNO}_{3} ∣ {A g}^{+}$ , the overall cell reaction is

1

{Ag}^{+} + KCl \to AgCl (s) + K^{+}

2

Ag + AgCl \to 2 Ag + \frac{1}{2} {Cl}_{2}

3

AgCl (s) \to {Ag}^{+} + {Cl}^{-}

4

{Ag}^{+} + {Cl}^{-} \to AgCl (s)

Explanation:

For the electrochemical cell,
${Ag}^{-} | AgCl | KCl | | {AgNO}_{3} ∣ {Ag}^{+}$
The cell reaction is,
$AgCl (s) + e^{-} \to Ag + {Cl}^{-}$ (aq)
$Ag \to {Ag}^{+} (aq) + e^{-}$
Overall reaction
$AgCl (s) \to {Ag}^{+} + {Cl}^{-}$

JIPMER-2018

ELECTROCHEMISTRY

275822 If $E^{0} ({Zn}^{2 +}, Zn) = - 0.763 V$ and $E^{0} ({Fe}^{2 +}, Fe) =$ $- 0.44 V$ , then the emf of the cell $Zn ∣ {Zn}^{2 +} (a =$ 0.001) $| {Fe}^{2 +} (a = 0.005) | Fe$ is

1 equal to

0.323 V

2 less than

0.323 V

3 greater than

0.323 V

4 equal to

1.103 V

Explanation:

The cell reaction is-
$Zn + {Fe}^{2 +} ⟶ {Zn}^{2 +} + Fe$
From Nernst equation
$\begin{aligned} E_{cell} = E_{cell}^{o} - \frac{0.0591}{n} \log \frac{a_{{Zn}^{2 +}}}{a_{{Fe}^{2 +}}} \\ = (0.763 - 0.44) - \frac{0.0591}{1} \log \frac{0.001}{0.005} \\ = 0.364 V \end{aligned}$

JIPMER-2018

ELECTROCHEMISTRY

275823 For a cell involving two electron changes, $E_{cell}^{o} = 0.3 V$ at $25^{\circ} C$ . The equilibrium constant of the reaction is

1

10^{- 10}

2

3 \times 10^{- 2}

3 10

4

10^{10}

Explanation:

For $Δ G^{\circ}$ is related to $K_{sp}$ by the equation,
$\begin{aligned} Δ G^{o} = & - 2.303 RT \log K_{sp} \\ \log K_{sp} & = \frac{- Δ G^{o}}{2.303 RT} = \frac{{nFE}_{cell}^{o}}{2.303 RT} (at 25^{\circ} C) \\ = \frac{2 E_{cell}^{o}}{0.0591} = \frac{2 \times 0.3}{0.0591} = 10 \end{aligned}$
$\log K_{sp} = 10 \Rightarrow K_{sp} = 10^{10}$

Karnataka-CET-2018

ELECTROCHEMISTRY

275819 Assertion: When I M CusO $_{4}$ (aq) solution is electrolysed using copper electrodes, copper is dissolved at anode and copper gets deposites at cathode.
Reason: The standard oxidation potential of copper is less than the standard oxidation potential of water and standard reduction potential of copper is greater than the standard reduction potential of water.

1 If Assertion is correct but Reason is in correct.

2 If both the Assertion and Reason are incorrect.

3 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.

4 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.

Explanation:

Copper is dissolved at anode and deposited at cathode when $Cu$ electrodes are used and electrolyte is $1 M {CuSO}_{4} (aq)$ solution as standard oxidation potential of $Cu$ is higher than standard oxidation potential of water and standard reduction potential of $Cu$ is greater than standard reduction potential of water.

AIIMS-26 May

ELECTROCHEMISTRY

275821 For the electrochemical cell,
${Ag}^{+} | AgCl | KCl | | {AgNO}_{3} ∣ {A g}^{+}$ , the overall cell reaction is

1

{Ag}^{+} + KCl \to AgCl (s) + K^{+}

2

Ag + AgCl \to 2 Ag + \frac{1}{2} {Cl}_{2}

3

AgCl (s) \to {Ag}^{+} + {Cl}^{-}

4

{Ag}^{+} + {Cl}^{-} \to AgCl (s)

Explanation:

For the electrochemical cell,
${Ag}^{-} | AgCl | KCl | | {AgNO}_{3} ∣ {Ag}^{+}$
The cell reaction is,
$AgCl (s) + e^{-} \to Ag + {Cl}^{-}$ (aq)
$Ag \to {Ag}^{+} (aq) + e^{-}$
Overall reaction
$AgCl (s) \to {Ag}^{+} + {Cl}^{-}$

JIPMER-2018

ELECTROCHEMISTRY

275822 If $E^{0} ({Zn}^{2 +}, Zn) = - 0.763 V$ and $E^{0} ({Fe}^{2 +}, Fe) =$ $- 0.44 V$ , then the emf of the cell $Zn ∣ {Zn}^{2 +} (a =$ 0.001) $| {Fe}^{2 +} (a = 0.005) | Fe$ is

1 equal to

0.323 V

2 less than

0.323 V

3 greater than

0.323 V

4 equal to

1.103 V

Explanation:

The cell reaction is-
$Zn + {Fe}^{2 +} ⟶ {Zn}^{2 +} + Fe$
From Nernst equation
$\begin{aligned} E_{cell} = E_{cell}^{o} - \frac{0.0591}{n} \log \frac{a_{{Zn}^{2 +}}}{a_{{Fe}^{2 +}}} \\ = (0.763 - 0.44) - \frac{0.0591}{1} \log \frac{0.001}{0.005} \\ = 0.364 V \end{aligned}$

JIPMER-2018

ELECTROCHEMISTRY

275823 For a cell involving two electron changes, $E_{cell}^{o} = 0.3 V$ at $25^{\circ} C$ . The equilibrium constant of the reaction is

1

10^{- 10}

2

3 \times 10^{- 2}

3 10

4

10^{10}

Explanation:

For $Δ G^{\circ}$ is related to $K_{sp}$ by the equation,
$\begin{aligned} Δ G^{o} = & - 2.303 RT \log K_{sp} \\ \log K_{sp} & = \frac{- Δ G^{o}}{2.303 RT} = \frac{{nFE}_{cell}^{o}}{2.303 RT} (at 25^{\circ} C) \\ = \frac{2 E_{cell}^{o}}{0.0591} = \frac{2 \times 0.3}{0.0591} = 10 \end{aligned}$
$\log K_{sp} = 10 \Rightarrow K_{sp} = 10^{10}$

Karnataka-CET-2018

ELECTROCHEMISTRY

275819 Assertion: When I M CusO $_{4}$ (aq) solution is electrolysed using copper electrodes, copper is dissolved at anode and copper gets deposites at cathode.
Reason: The standard oxidation potential of copper is less than the standard oxidation potential of water and standard reduction potential of copper is greater than the standard reduction potential of water.

1 If Assertion is correct but Reason is in correct.

2 If both the Assertion and Reason are incorrect.

3 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.

4 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.

Explanation:

Copper is dissolved at anode and deposited at cathode when $Cu$ electrodes are used and electrolyte is $1 M {CuSO}_{4} (aq)$ solution as standard oxidation potential of $Cu$ is higher than standard oxidation potential of water and standard reduction potential of $Cu$ is greater than standard reduction potential of water.

AIIMS-26 May

ELECTROCHEMISTRY

275821 For the electrochemical cell,
${Ag}^{+} | AgCl | KCl | | {AgNO}_{3} ∣ {A g}^{+}$ , the overall cell reaction is

1

{Ag}^{+} + KCl \to AgCl (s) + K^{+}

2

Ag + AgCl \to 2 Ag + \frac{1}{2} {Cl}_{2}

3

AgCl (s) \to {Ag}^{+} + {Cl}^{-}

4

{Ag}^{+} + {Cl}^{-} \to AgCl (s)

Explanation:

For the electrochemical cell,
${Ag}^{-} | AgCl | KCl | | {AgNO}_{3} ∣ {Ag}^{+}$
The cell reaction is,
$AgCl (s) + e^{-} \to Ag + {Cl}^{-}$ (aq)
$Ag \to {Ag}^{+} (aq) + e^{-}$
Overall reaction
$AgCl (s) \to {Ag}^{+} + {Cl}^{-}$

JIPMER-2018

ELECTROCHEMISTRY

275822 If $E^{0} ({Zn}^{2 +}, Zn) = - 0.763 V$ and $E^{0} ({Fe}^{2 +}, Fe) =$ $- 0.44 V$ , then the emf of the cell $Zn ∣ {Zn}^{2 +} (a =$ 0.001) $| {Fe}^{2 +} (a = 0.005) | Fe$ is

1 equal to

0.323 V

2 less than

0.323 V

3 greater than

0.323 V

4 equal to

1.103 V

Explanation:

The cell reaction is-
$Zn + {Fe}^{2 +} ⟶ {Zn}^{2 +} + Fe$
From Nernst equation
$\begin{aligned} E_{cell} = E_{cell}^{o} - \frac{0.0591}{n} \log \frac{a_{{Zn}^{2 +}}}{a_{{Fe}^{2 +}}} \\ = (0.763 - 0.44) - \frac{0.0591}{1} \log \frac{0.001}{0.005} \\ = 0.364 V \end{aligned}$

JIPMER-2018

ELECTROCHEMISTRY

275823 For a cell involving two electron changes, $E_{cell}^{o} = 0.3 V$ at $25^{\circ} C$ . The equilibrium constant of the reaction is

1

10^{- 10}

2

3 \times 10^{- 2}

3 10

4

10^{10}

Explanation:

For $Δ G^{\circ}$ is related to $K_{sp}$ by the equation,
$\begin{aligned} Δ G^{o} = & - 2.303 RT \log K_{sp} \\ \log K_{sp} & = \frac{- Δ G^{o}}{2.303 RT} = \frac{{nFE}_{cell}^{o}}{2.303 RT} (at 25^{\circ} C) \\ = \frac{2 E_{cell}^{o}}{0.0591} = \frac{2 \times 0.3}{0.0591} = 10 \end{aligned}$
$\log K_{sp} = 10 \Rightarrow K_{sp} = 10^{10}$

Karnataka-CET-2018

ELECTROCHEMISTRY

275819 Assertion: When I M CusO $_{4}$ (aq) solution is electrolysed using copper electrodes, copper is dissolved at anode and copper gets deposites at cathode.
Reason: The standard oxidation potential of copper is less than the standard oxidation potential of water and standard reduction potential of copper is greater than the standard reduction potential of water.

1 If Assertion is correct but Reason is in correct.

2 If both the Assertion and Reason are incorrect.

3 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.

4 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.

Explanation:

Copper is dissolved at anode and deposited at cathode when $Cu$ electrodes are used and electrolyte is $1 M {CuSO}_{4} (aq)$ solution as standard oxidation potential of $Cu$ is higher than standard oxidation potential of water and standard reduction potential of $Cu$ is greater than standard reduction potential of water.

AIIMS-26 May

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