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CHXII03:ELECTROCHEMISTRY

330075 Electrode potential is

1 Potential difference develops between two electrodes

2 Potential difference develops between two different electrolytes

3 Potential difference develops between electrode and electrolyte

4 All of the above

CHXII03:ELECTROCHEMISTRY

330076 $E^{o} f o r F_{2} + 2 e \to 2 F^{-} i s 2.8 V,$
$E^{o} f o r \frac{1}{2} F_{2} + e \to F^{-} i s$

1 – 1.4 V

2 – 2.8 V

3 2.8 V

4 1.4 V

Explanation:

$E^{o}$ is intensive property and it does not depend on stoichiometry of $F_{2}$ taking part.

CHXII03:ELECTROCHEMISTRY

330077 By electromotive force we mean

1 The potential difference of a cell measured when there is a flow of current from the anode to the cathode and the cell is operating irreversibly.

2 The potential difference of a cell measured when there is a flow of current from the cathode to the anode and the cell is operating reversibly.

3 The potential difference of a cell when there is no flow of current and the cell is operating irreversibly

4 The potential difference of a cell when there is no flow of current and the cell is operating reversibly

CHXII03:ELECTROCHEMISTRY

330078 The standard reduction potentials for $Z n^{2 +} / Z n, N i^{2 +} / N i a n d F e^{2 +} / F e$ $a r e - 0 .76, - 0 .23 a n d - 0 .44 V$ respectively. The reaction $X + Y^{2 +} \to X^{2} + Y$ will be spontaneous when

1

X = Z n, Y = N i

2

X = N i, Y = F e

3

X = N i, Y = Z n

4

X = F e, Y = Z n

Explanation:

Lower SRP species undergo oxidation i.e., Zn(X). Higher SRP species undergo reduction i.e., $N i^{+ 2} (Y) .$

CHXII03:ELECTROCHEMISTRY

330079 Consider the following $E^{o}$ values:
$E_{F e^{3 +} / F e^{2 +}}^{o} = + 0 .77 V$
$E_{S n^{2 +} / S n}^{o} = + 0 .14 V$
Under standard conditions the potential for the reaction
$S n (s) + 2 F e^{3 +} (a q) \to 2 F e^{2 +} (s q) + S n^{2 +} (a q)$ is

1 0.91 V

2 0.63 V

3 1.40 V

4 1.68 V

Explanation:

$F o r S n_{(s)} + 2 F e_{(a q)}^{3 +} \to 2 F e_{(a q)}^{2 +} + S n_{(a q)}^{2 +}$
$E_{c e l l}^{o} = E_{S n / S n^{2 +}}^{o} + E_{F e^{3 +} / F e^{2 +}}^{o} = (0 .14) + (0 .77)$
$E_{c e l l} = 0 .91 V$

CHXII03:ELECTROCHEMISTRY

330075 Electrode potential is

1 Potential difference develops between two electrodes

2 Potential difference develops between two different electrolytes

3 Potential difference develops between electrode and electrolyte

4 All of the above

CHXII03:ELECTROCHEMISTRY

330076 $E^{o} f o r F_{2} + 2 e \to 2 F^{-} i s 2.8 V,$
$E^{o} f o r \frac{1}{2} F_{2} + e \to F^{-} i s$

1 – 1.4 V

2 – 2.8 V

3 2.8 V

4 1.4 V

Explanation:

$E^{o}$ is intensive property and it does not depend on stoichiometry of $F_{2}$ taking part.

CHXII03:ELECTROCHEMISTRY

330077 By electromotive force we mean

1 The potential difference of a cell measured when there is a flow of current from the anode to the cathode and the cell is operating irreversibly.

2 The potential difference of a cell measured when there is a flow of current from the cathode to the anode and the cell is operating reversibly.

3 The potential difference of a cell when there is no flow of current and the cell is operating irreversibly

4 The potential difference of a cell when there is no flow of current and the cell is operating reversibly

CHXII03:ELECTROCHEMISTRY

330078 The standard reduction potentials for $Z n^{2 +} / Z n, N i^{2 +} / N i a n d F e^{2 +} / F e$ $a r e - 0 .76, - 0 .23 a n d - 0 .44 V$ respectively. The reaction $X + Y^{2 +} \to X^{2} + Y$ will be spontaneous when

1

X = Z n, Y = N i

2

X = N i, Y = F e

3

X = N i, Y = Z n

4

X = F e, Y = Z n

Explanation:

Lower SRP species undergo oxidation i.e., Zn(X). Higher SRP species undergo reduction i.e., $N i^{+ 2} (Y) .$

CHXII03:ELECTROCHEMISTRY

330079 Consider the following $E^{o}$ values:
$E_{F e^{3 +} / F e^{2 +}}^{o} = + 0 .77 V$
$E_{S n^{2 +} / S n}^{o} = + 0 .14 V$
Under standard conditions the potential for the reaction
$S n (s) + 2 F e^{3 +} (a q) \to 2 F e^{2 +} (s q) + S n^{2 +} (a q)$ is

1 0.91 V

2 0.63 V

3 1.40 V

4 1.68 V

Explanation:

$F o r S n_{(s)} + 2 F e_{(a q)}^{3 +} \to 2 F e_{(a q)}^{2 +} + S n_{(a q)}^{2 +}$
$E_{c e l l}^{o} = E_{S n / S n^{2 +}}^{o} + E_{F e^{3 +} / F e^{2 +}}^{o} = (0 .14) + (0 .77)$
$E_{c e l l} = 0 .91 V$

CHXII03:ELECTROCHEMISTRY

330075 Electrode potential is

1 Potential difference develops between two electrodes

2 Potential difference develops between two different electrolytes

3 Potential difference develops between electrode and electrolyte

4 All of the above

CHXII03:ELECTROCHEMISTRY

330076 $E^{o} f o r F_{2} + 2 e \to 2 F^{-} i s 2.8 V,$
$E^{o} f o r \frac{1}{2} F_{2} + e \to F^{-} i s$

1 – 1.4 V

2 – 2.8 V

3 2.8 V

4 1.4 V

Explanation:

$E^{o}$ is intensive property and it does not depend on stoichiometry of $F_{2}$ taking part.

CHXII03:ELECTROCHEMISTRY

330077 By electromotive force we mean

1 The potential difference of a cell measured when there is a flow of current from the anode to the cathode and the cell is operating irreversibly.

2 The potential difference of a cell measured when there is a flow of current from the cathode to the anode and the cell is operating reversibly.

3 The potential difference of a cell when there is no flow of current and the cell is operating irreversibly

4 The potential difference of a cell when there is no flow of current and the cell is operating reversibly

CHXII03:ELECTROCHEMISTRY

330078 The standard reduction potentials for $Z n^{2 +} / Z n, N i^{2 +} / N i a n d F e^{2 +} / F e$ $a r e - 0 .76, - 0 .23 a n d - 0 .44 V$ respectively. The reaction $X + Y^{2 +} \to X^{2} + Y$ will be spontaneous when

1

X = Z n, Y = N i

2

X = N i, Y = F e

3

X = N i, Y = Z n

4

X = F e, Y = Z n

Explanation:

Lower SRP species undergo oxidation i.e., Zn(X). Higher SRP species undergo reduction i.e., $N i^{+ 2} (Y) .$

CHXII03:ELECTROCHEMISTRY

330079 Consider the following $E^{o}$ values:
$E_{F e^{3 +} / F e^{2 +}}^{o} = + 0 .77 V$
$E_{S n^{2 +} / S n}^{o} = + 0 .14 V$
Under standard conditions the potential for the reaction
$S n (s) + 2 F e^{3 +} (a q) \to 2 F e^{2 +} (s q) + S n^{2 +} (a q)$ is

1 0.91 V

2 0.63 V

3 1.40 V

4 1.68 V

Explanation:

$F o r S n_{(s)} + 2 F e_{(a q)}^{3 +} \to 2 F e_{(a q)}^{2 +} + S n_{(a q)}^{2 +}$
$E_{c e l l}^{o} = E_{S n / S n^{2 +}}^{o} + E_{F e^{3 +} / F e^{2 +}}^{o} = (0 .14) + (0 .77)$
$E_{c e l l} = 0 .91 V$

CHXII03:ELECTROCHEMISTRY

330075 Electrode potential is

1 Potential difference develops between two electrodes

2 Potential difference develops between two different electrolytes

3 Potential difference develops between electrode and electrolyte

4 All of the above

CHXII03:ELECTROCHEMISTRY

330076 $E^{o} f o r F_{2} + 2 e \to 2 F^{-} i s 2.8 V,$
$E^{o} f o r \frac{1}{2} F_{2} + e \to F^{-} i s$

1 – 1.4 V

2 – 2.8 V

3 2.8 V

4 1.4 V

Explanation:

$E^{o}$ is intensive property and it does not depend on stoichiometry of $F_{2}$ taking part.

CHXII03:ELECTROCHEMISTRY

330077 By electromotive force we mean

1 The potential difference of a cell measured when there is a flow of current from the anode to the cathode and the cell is operating irreversibly.

2 The potential difference of a cell measured when there is a flow of current from the cathode to the anode and the cell is operating reversibly.

3 The potential difference of a cell when there is no flow of current and the cell is operating irreversibly

4 The potential difference of a cell when there is no flow of current and the cell is operating reversibly

CHXII03:ELECTROCHEMISTRY

330078 The standard reduction potentials for $Z n^{2 +} / Z n, N i^{2 +} / N i a n d F e^{2 +} / F e$ $a r e - 0 .76, - 0 .23 a n d - 0 .44 V$ respectively. The reaction $X + Y^{2 +} \to X^{2} + Y$ will be spontaneous when

1

X = Z n, Y = N i

2

X = N i, Y = F e

3

X = N i, Y = Z n

4

X = F e, Y = Z n

Explanation:

Lower SRP species undergo oxidation i.e., Zn(X). Higher SRP species undergo reduction i.e., $N i^{+ 2} (Y) .$

CHXII03:ELECTROCHEMISTRY

330079 Consider the following $E^{o}$ values:
$E_{F e^{3 +} / F e^{2 +}}^{o} = + 0 .77 V$
$E_{S n^{2 +} / S n}^{o} = + 0 .14 V$
Under standard conditions the potential for the reaction
$S n (s) + 2 F e^{3 +} (a q) \to 2 F e^{2 +} (s q) + S n^{2 +} (a q)$ is

1 0.91 V

2 0.63 V

3 1.40 V

4 1.68 V

Explanation:

$F o r S n_{(s)} + 2 F e_{(a q)}^{3 +} \to 2 F e_{(a q)}^{2 +} + S n_{(a q)}^{2 +}$
$E_{c e l l}^{o} = E_{S n / S n^{2 +}}^{o} + E_{F e^{3 +} / F e^{2 +}}^{o} = (0 .14) + (0 .77)$
$E_{c e l l} = 0 .91 V$

CHXII03:ELECTROCHEMISTRY

330075 Electrode potential is

1 Potential difference develops between two electrodes

2 Potential difference develops between two different electrolytes

3 Potential difference develops between electrode and electrolyte

4 All of the above

CHXII03:ELECTROCHEMISTRY

330076 $E^{o} f o r F_{2} + 2 e \to 2 F^{-} i s 2.8 V,$
$E^{o} f o r \frac{1}{2} F_{2} + e \to F^{-} i s$

1 – 1.4 V

2 – 2.8 V

3 2.8 V

4 1.4 V

Explanation:

$E^{o}$ is intensive property and it does not depend on stoichiometry of $F_{2}$ taking part.

CHXII03:ELECTROCHEMISTRY

330077 By electromotive force we mean

1 The potential difference of a cell measured when there is a flow of current from the anode to the cathode and the cell is operating irreversibly.

2 The potential difference of a cell measured when there is a flow of current from the cathode to the anode and the cell is operating reversibly.

3 The potential difference of a cell when there is no flow of current and the cell is operating irreversibly

4 The potential difference of a cell when there is no flow of current and the cell is operating reversibly

CHXII03:ELECTROCHEMISTRY

330078 The standard reduction potentials for $Z n^{2 +} / Z n, N i^{2 +} / N i a n d F e^{2 +} / F e$ $a r e - 0 .76, - 0 .23 a n d - 0 .44 V$ respectively. The reaction $X + Y^{2 +} \to X^{2} + Y$ will be spontaneous when

1

X = Z n, Y = N i

2

X = N i, Y = F e

3

X = N i, Y = Z n

4

X = F e, Y = Z n

Explanation:

Lower SRP species undergo oxidation i.e., Zn(X). Higher SRP species undergo reduction i.e., $N i^{+ 2} (Y) .$

CHXII03:ELECTROCHEMISTRY

330079 Consider the following $E^{o}$ values:
$E_{F e^{3 +} / F e^{2 +}}^{o} = + 0 .77 V$
$E_{S n^{2 +} / S n}^{o} = + 0 .14 V$
Under standard conditions the potential for the reaction
$S n (s) + 2 F e^{3 +} (a q) \to 2 F e^{2 +} (s q) + S n^{2 +} (a q)$ is

1 0.91 V

2 0.63 V

3 1.40 V

4 1.68 V

Explanation:

$F o r S n_{(s)} + 2 F e_{(a q)}^{3 +} \to 2 F e_{(a q)}^{2 +} + S n_{(a q)}^{2 +}$
$E_{c e l l}^{o} = E_{S n / S n^{2 +}}^{o} + E_{F e^{3 +} / F e^{2 +}}^{o} = (0 .14) + (0 .77)$
$E_{c e l l} = 0 .91 V$

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