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CHXII03:ELECTROCHEMISTRY

330058 Given below are half cell reactions :
$M n O_{4}^{-} + 8 H^{+} 5 e^{-} \to M n^{2 +} + 4 H_{2} O,$
$E_{M n^{2 +} {/ M n O}_{4}^{-}}^{o} = - 1 .510 V$
$\frac{1}{2} O_{2} + 2 H^{+} + 2 e^{-} \to H_{2} O$
$E_{O_{2} / H_{2} O}^{o} = + 1 .223 V$
Will the permanganate ion, ${M n O}_{4}^{-} l i b e r a t e O_{2}$ from water in the presence of an acid ?

1 No, because

E_{c e l l}^{o} = - 0 .287 V

2 Yes, because

E_{c e l l}^{o} = + 2 .733 V

3 No, because

E_{c e l l}^{o} = - 2 .733 V

4 Yes, because

E_{c e l l}^{o} = + 0 .287 V

Explanation:

supporting img
$C a t h o d e :$
${2 M n O}_{4}^{-} + 16 H^{+} + 10 e^{-} \to 2 M n^{2 +} + 8 H_{2} O;$
$E_{R P}^{o} = 1 .510 V$
$A n o d e :$
$5 H_{2} O \to \frac{5}{2} O_{2} + 10 H^{+} + 10 e^{-}$
$E_{O P}^{o} = - 1 .223 V$
$T a r g e t r e a c t i o n :$
${2 M n O}_{4}^{-} + 6 H^{+} \to 2 M n^{+ 2} + \frac{5}{2} O_{2} + 3 H_{2} O;$
$E_{c e l l}^{o} = {(S R P)}_{C a t h o d e} - {(S R P)}_{A n o d e}$
$E_{c e l l}^{o} = 1 .510 V - 1 .223 V$
$= 0 .287 V$
Yes the given cell reaction is possible.

NEET - 2022

CHXII03:ELECTROCHEMISTRY

330059 Assertion :
The potential difference between the two electrodes of a galvanic cell is called the cell potential.
Reason :
Cell potential is equal to the emf of a cell.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

CHXII03:ELECTROCHEMISTRY

330060 The difference between the electrode potentials of two electrodes when no current is drawn through the cell is called ....

1 Cell voltage

2 Cell difference

3 Cell potential

4 Cell emf

CHXII03:ELECTROCHEMISTRY

330061 I.
The potential of individual half-cell can be measured.
II.
Difference between the potentials of two half-cells can only be measured.
III.
$P t (s) | H_{2} (g) | H^{+} (a q)$ half-cell is called standard hydrogen electrode.
Select the correct statement(s) and choose the appropriate option.

1 I and II

2 II and III

3 III and I

4 I, II and III

Explanation:

The potential of individual half-cell cannot be measured. The difference between potentials of two half-cells give the emf of cell.
$P t (s) | H_{2} (g) | H^{+} (a q)$ half-cell is called standard hydrogen electrode. So, the option (2) is correct.

CHXII03:ELECTROCHEMISTRY

330058 Given below are half cell reactions :
$M n O_{4}^{-} + 8 H^{+} 5 e^{-} \to M n^{2 +} + 4 H_{2} O,$
$E_{M n^{2 +} {/ M n O}_{4}^{-}}^{o} = - 1 .510 V$
$\frac{1}{2} O_{2} + 2 H^{+} + 2 e^{-} \to H_{2} O$
$E_{O_{2} / H_{2} O}^{o} = + 1 .223 V$
Will the permanganate ion, ${M n O}_{4}^{-} l i b e r a t e O_{2}$ from water in the presence of an acid ?

1 No, because

E_{c e l l}^{o} = - 0 .287 V

2 Yes, because

E_{c e l l}^{o} = + 2 .733 V

3 No, because

E_{c e l l}^{o} = - 2 .733 V

4 Yes, because

E_{c e l l}^{o} = + 0 .287 V

Explanation:

supporting img
$C a t h o d e :$
${2 M n O}_{4}^{-} + 16 H^{+} + 10 e^{-} \to 2 M n^{2 +} + 8 H_{2} O;$
$E_{R P}^{o} = 1 .510 V$
$A n o d e :$
$5 H_{2} O \to \frac{5}{2} O_{2} + 10 H^{+} + 10 e^{-}$
$E_{O P}^{o} = - 1 .223 V$
$T a r g e t r e a c t i o n :$
${2 M n O}_{4}^{-} + 6 H^{+} \to 2 M n^{+ 2} + \frac{5}{2} O_{2} + 3 H_{2} O;$
$E_{c e l l}^{o} = {(S R P)}_{C a t h o d e} - {(S R P)}_{A n o d e}$
$E_{c e l l}^{o} = 1 .510 V - 1 .223 V$
$= 0 .287 V$
Yes the given cell reaction is possible.

NEET - 2022

CHXII03:ELECTROCHEMISTRY

330059 Assertion :
The potential difference between the two electrodes of a galvanic cell is called the cell potential.
Reason :
Cell potential is equal to the emf of a cell.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

CHXII03:ELECTROCHEMISTRY

330060 The difference between the electrode potentials of two electrodes when no current is drawn through the cell is called ....

1 Cell voltage

2 Cell difference

3 Cell potential

4 Cell emf

CHXII03:ELECTROCHEMISTRY

330061 I.
The potential of individual half-cell can be measured.
II.
Difference between the potentials of two half-cells can only be measured.
III.
$P t (s) | H_{2} (g) | H^{+} (a q)$ half-cell is called standard hydrogen electrode.
Select the correct statement(s) and choose the appropriate option.

1 I and II

2 II and III

3 III and I

4 I, II and III

Explanation:

The potential of individual half-cell cannot be measured. The difference between potentials of two half-cells give the emf of cell.
$P t (s) | H_{2} (g) | H^{+} (a q)$ half-cell is called standard hydrogen electrode. So, the option (2) is correct.

CHXII03:ELECTROCHEMISTRY

330058 Given below are half cell reactions :
$M n O_{4}^{-} + 8 H^{+} 5 e^{-} \to M n^{2 +} + 4 H_{2} O,$
$E_{M n^{2 +} {/ M n O}_{4}^{-}}^{o} = - 1 .510 V$
$\frac{1}{2} O_{2} + 2 H^{+} + 2 e^{-} \to H_{2} O$
$E_{O_{2} / H_{2} O}^{o} = + 1 .223 V$
Will the permanganate ion, ${M n O}_{4}^{-} l i b e r a t e O_{2}$ from water in the presence of an acid ?

1 No, because

E_{c e l l}^{o} = - 0 .287 V

2 Yes, because

E_{c e l l}^{o} = + 2 .733 V

3 No, because

E_{c e l l}^{o} = - 2 .733 V

4 Yes, because

E_{c e l l}^{o} = + 0 .287 V

Explanation:

supporting img
$C a t h o d e :$
${2 M n O}_{4}^{-} + 16 H^{+} + 10 e^{-} \to 2 M n^{2 +} + 8 H_{2} O;$
$E_{R P}^{o} = 1 .510 V$
$A n o d e :$
$5 H_{2} O \to \frac{5}{2} O_{2} + 10 H^{+} + 10 e^{-}$
$E_{O P}^{o} = - 1 .223 V$
$T a r g e t r e a c t i o n :$
${2 M n O}_{4}^{-} + 6 H^{+} \to 2 M n^{+ 2} + \frac{5}{2} O_{2} + 3 H_{2} O;$
$E_{c e l l}^{o} = {(S R P)}_{C a t h o d e} - {(S R P)}_{A n o d e}$
$E_{c e l l}^{o} = 1 .510 V - 1 .223 V$
$= 0 .287 V$
Yes the given cell reaction is possible.

NEET - 2022

CHXII03:ELECTROCHEMISTRY

330059 Assertion :
The potential difference between the two electrodes of a galvanic cell is called the cell potential.
Reason :
Cell potential is equal to the emf of a cell.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

CHXII03:ELECTROCHEMISTRY

330060 The difference between the electrode potentials of two electrodes when no current is drawn through the cell is called ....

1 Cell voltage

2 Cell difference

3 Cell potential

4 Cell emf

CHXII03:ELECTROCHEMISTRY

330061 I.
The potential of individual half-cell can be measured.
II.
Difference between the potentials of two half-cells can only be measured.
III.
$P t (s) | H_{2} (g) | H^{+} (a q)$ half-cell is called standard hydrogen electrode.
Select the correct statement(s) and choose the appropriate option.

1 I and II

2 II and III

3 III and I

4 I, II and III

Explanation:

The potential of individual half-cell cannot be measured. The difference between potentials of two half-cells give the emf of cell.
$P t (s) | H_{2} (g) | H^{+} (a q)$ half-cell is called standard hydrogen electrode. So, the option (2) is correct.

CHXII03:ELECTROCHEMISTRY

330058 Given below are half cell reactions :
$M n O_{4}^{-} + 8 H^{+} 5 e^{-} \to M n^{2 +} + 4 H_{2} O,$
$E_{M n^{2 +} {/ M n O}_{4}^{-}}^{o} = - 1 .510 V$
$\frac{1}{2} O_{2} + 2 H^{+} + 2 e^{-} \to H_{2} O$
$E_{O_{2} / H_{2} O}^{o} = + 1 .223 V$
Will the permanganate ion, ${M n O}_{4}^{-} l i b e r a t e O_{2}$ from water in the presence of an acid ?

1 No, because

E_{c e l l}^{o} = - 0 .287 V

2 Yes, because

E_{c e l l}^{o} = + 2 .733 V

3 No, because

E_{c e l l}^{o} = - 2 .733 V

4 Yes, because

E_{c e l l}^{o} = + 0 .287 V

Explanation:

supporting img
$C a t h o d e :$
${2 M n O}_{4}^{-} + 16 H^{+} + 10 e^{-} \to 2 M n^{2 +} + 8 H_{2} O;$
$E_{R P}^{o} = 1 .510 V$
$A n o d e :$
$5 H_{2} O \to \frac{5}{2} O_{2} + 10 H^{+} + 10 e^{-}$
$E_{O P}^{o} = - 1 .223 V$
$T a r g e t r e a c t i o n :$
${2 M n O}_{4}^{-} + 6 H^{+} \to 2 M n^{+ 2} + \frac{5}{2} O_{2} + 3 H_{2} O;$
$E_{c e l l}^{o} = {(S R P)}_{C a t h o d e} - {(S R P)}_{A n o d e}$
$E_{c e l l}^{o} = 1 .510 V - 1 .223 V$
$= 0 .287 V$
Yes the given cell reaction is possible.

NEET - 2022

CHXII03:ELECTROCHEMISTRY

330059 Assertion :
The potential difference between the two electrodes of a galvanic cell is called the cell potential.
Reason :
Cell potential is equal to the emf of a cell.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.

2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.

3 Assertion is correct but Reason is incorrect.

4 Assertion is incorrect but Reason is correct.

CHXII03:ELECTROCHEMISTRY

330060 The difference between the electrode potentials of two electrodes when no current is drawn through the cell is called ....

1 Cell voltage

2 Cell difference

3 Cell potential

4 Cell emf

CHXII03:ELECTROCHEMISTRY

330061 I.
The potential of individual half-cell can be measured.
II.
Difference between the potentials of two half-cells can only be measured.
III.
$P t (s) | H_{2} (g) | H^{+} (a q)$ half-cell is called standard hydrogen electrode.
Select the correct statement(s) and choose the appropriate option.

1 I and II

2 II and III

3 III and I

4 I, II and III

Explanation:

The potential of individual half-cell cannot be measured. The difference between potentials of two half-cells give the emf of cell.
$P t (s) | H_{2} (g) | H^{+} (a q)$ half-cell is called standard hydrogen electrode. So, the option (2) is correct.

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