QBManager

ELECTROCHEMISTRY

275941 An aqueous solution containing $6.5 g$ of $NaCl$ of $90 %$ purity was subjected to electrolysis. After the complete electrolysis, the solution was evaporated to get solid $NaOH$ . The volume of $1 M$ acetic acid required to neutralize $NaOH$ obtained above is

1

1000 {cm}^{3}

2

2000 {cm}^{3}

3

100 {cm}^{3}

4

200 {cm}^{3}

Explanation:

Given that,
Weight of pure $NaCl = 6.5 \times 0.9 = 5.85 g$
No. of equivalence of $NaCl = \frac{5.85}{58.5} = 0.1$
No. of equivalence of $NaOH$ obtained $= 0.1 \times$ volume of $1 M$ acetic acid required for the neutralisation of $NaOH = \frac{0.1 \times 1000}{1} = 100 {cm}^{3}$

Karnataka CET-2009

ELECTROCHEMISTRY

275961 The standard electrode potential of hydrogen electrode at $1 M$ concentration and hydrogen gas at 1 atmosphere pressure is

1 1 Volt

2 6 Volt

3 8 Volt

4 0 Volt

Explanation:

$E = 0 - \frac{0.059}{2} \log \frac{1}{(1)^{2}} = 0 V$
Standard electrode potential of hydrogen at $1 M$ concentration and $1 atm$ pressure is Zero Volts.

J and K CET-(2007)

ELECTROCHEMISTRY

275962 The standard oxidation potentials of $Zn, Cu$ , $Ag$ and $Ni$ electrodes are $+ 0.76, 0.34, - 0.80$ and $+ 0.25 V$ respectively. Which of the following reaction will provide maximum voltage?

1

Cu + 2 {Ag}^{+} (aq) \to {Cu}^{2 +} (aq) + 2 Ag

2

Zn + 2 {Ag}^{+} (aq) \to {Zn}^{2 +} (aq) + 2 Ag

3

H_{2} + {Ni}^{2 +}

(aq)

\to 2 H^{+} (aq) + Ni

4

Zn + {Cu}^{2 +} (aq) \to {Zn}^{2 +} (aq) + Cu

5

Zn + 2 H^{+} (aq) \to {Zn}^{2 +} (aq) + H_{2}

Explanation:

Oxidation potentials are given in the question. The reduction potentials are obtained by changing the sign, i.e. the reduction potentials of $Zn$ , $Cu, Ag$ and $Ni$ are, $- 0.76, - 0.34, + 0.80$ and $- 0.25 V$ respectively.
$E_{cell}^{o} = E_{Ag}^{o} - E_{Zn}^{o}$ $= 0.80 - (- 0.76) = 1.56 V$

Kerala-CEE-2007

ELECTROCHEMISTRY

275963 The standard $E_{red}^{\circ}$ values of $A, B$ and $C$ are $+ 0.68 V, - 2.54 V, - 0.50 V$ respectively. The order of their reducing power is

1

A > B > C

2

A > C > B

3

C > B > A

4

B > C > A

Explanation:

Greater in the negative value of standard reduction potential, stronger is the reducing character. Thus, order of reducing power-
$B (- 2.54 V) > C (- 0.50 V) > A (+ 0.68 V)$

MHT CET-2007

ELECTROCHEMISTRY

275965 In electrolytic cell, cathode acts as an/a

1 oxidising agent

2 reducing agent

3 either of the two

4 Neither (a) nor (b)

Explanation:

In electrolytic cell, cathode acts as a reducing agent.
At cathode, ${Na}^{+} + e^{-} \to Na$ (reduction)
At anode,
$\begin{aligned} {Na}^{+} + e^{-} \to Na (reduction) \\ {Cl}^{-} \to Cl + e^{-} (oxidation) \\ {Na}^{+} + {Cl}^{-} \to \underset{Cathode}{Na + \underset{Anode}{Cl}} \end{aligned}$

UP CPMT-2007

ELECTROCHEMISTRY

275941 An aqueous solution containing $6.5 g$ of $NaCl$ of $90 %$ purity was subjected to electrolysis. After the complete electrolysis, the solution was evaporated to get solid $NaOH$ . The volume of $1 M$ acetic acid required to neutralize $NaOH$ obtained above is

1

1000 {cm}^{3}

2

2000 {cm}^{3}

3

100 {cm}^{3}

4

200 {cm}^{3}

Explanation:

Given that,
Weight of pure $NaCl = 6.5 \times 0.9 = 5.85 g$
No. of equivalence of $NaCl = \frac{5.85}{58.5} = 0.1$
No. of equivalence of $NaOH$ obtained $= 0.1 \times$ volume of $1 M$ acetic acid required for the neutralisation of $NaOH = \frac{0.1 \times 1000}{1} = 100 {cm}^{3}$

Karnataka CET-2009

ELECTROCHEMISTRY

275961 The standard electrode potential of hydrogen electrode at $1 M$ concentration and hydrogen gas at 1 atmosphere pressure is

1 1 Volt

2 6 Volt

3 8 Volt

4 0 Volt

Explanation:

$E = 0 - \frac{0.059}{2} \log \frac{1}{(1)^{2}} = 0 V$
Standard electrode potential of hydrogen at $1 M$ concentration and $1 atm$ pressure is Zero Volts.

J and K CET-(2007)

ELECTROCHEMISTRY

275962 The standard oxidation potentials of $Zn, Cu$ , $Ag$ and $Ni$ electrodes are $+ 0.76, 0.34, - 0.80$ and $+ 0.25 V$ respectively. Which of the following reaction will provide maximum voltage?

1

Cu + 2 {Ag}^{+} (aq) \to {Cu}^{2 +} (aq) + 2 Ag

2

Zn + 2 {Ag}^{+} (aq) \to {Zn}^{2 +} (aq) + 2 Ag

3

H_{2} + {Ni}^{2 +}

(aq)

\to 2 H^{+} (aq) + Ni

4

Zn + {Cu}^{2 +} (aq) \to {Zn}^{2 +} (aq) + Cu

5

Zn + 2 H^{+} (aq) \to {Zn}^{2 +} (aq) + H_{2}

Explanation:

Oxidation potentials are given in the question. The reduction potentials are obtained by changing the sign, i.e. the reduction potentials of $Zn$ , $Cu, Ag$ and $Ni$ are, $- 0.76, - 0.34, + 0.80$ and $- 0.25 V$ respectively.
$E_{cell}^{o} = E_{Ag}^{o} - E_{Zn}^{o}$ $= 0.80 - (- 0.76) = 1.56 V$

Kerala-CEE-2007

ELECTROCHEMISTRY

275963 The standard $E_{red}^{\circ}$ values of $A, B$ and $C$ are $+ 0.68 V, - 2.54 V, - 0.50 V$ respectively. The order of their reducing power is

1

A > B > C

2

A > C > B

3

C > B > A

4

B > C > A

Explanation:

Greater in the negative value of standard reduction potential, stronger is the reducing character. Thus, order of reducing power-
$B (- 2.54 V) > C (- 0.50 V) > A (+ 0.68 V)$

MHT CET-2007

ELECTROCHEMISTRY

275965 In electrolytic cell, cathode acts as an/a

1 oxidising agent

2 reducing agent

3 either of the two

4 Neither (a) nor (b)

Explanation:

In electrolytic cell, cathode acts as a reducing agent.
At cathode, ${Na}^{+} + e^{-} \to Na$ (reduction)
At anode,
$\begin{aligned} {Na}^{+} + e^{-} \to Na (reduction) \\ {Cl}^{-} \to Cl + e^{-} (oxidation) \\ {Na}^{+} + {Cl}^{-} \to \underset{Cathode}{Na + \underset{Anode}{Cl}} \end{aligned}$

UP CPMT-2007

ELECTROCHEMISTRY

275941 An aqueous solution containing $6.5 g$ of $NaCl$ of $90 %$ purity was subjected to electrolysis. After the complete electrolysis, the solution was evaporated to get solid $NaOH$ . The volume of $1 M$ acetic acid required to neutralize $NaOH$ obtained above is

1

1000 {cm}^{3}

2

2000 {cm}^{3}

3

100 {cm}^{3}

4

200 {cm}^{3}

Explanation:

Given that,
Weight of pure $NaCl = 6.5 \times 0.9 = 5.85 g$
No. of equivalence of $NaCl = \frac{5.85}{58.5} = 0.1$
No. of equivalence of $NaOH$ obtained $= 0.1 \times$ volume of $1 M$ acetic acid required for the neutralisation of $NaOH = \frac{0.1 \times 1000}{1} = 100 {cm}^{3}$

Karnataka CET-2009

ELECTROCHEMISTRY

275961 The standard electrode potential of hydrogen electrode at $1 M$ concentration and hydrogen gas at 1 atmosphere pressure is

1 1 Volt

2 6 Volt

3 8 Volt

4 0 Volt

Explanation:

$E = 0 - \frac{0.059}{2} \log \frac{1}{(1)^{2}} = 0 V$
Standard electrode potential of hydrogen at $1 M$ concentration and $1 atm$ pressure is Zero Volts.

J and K CET-(2007)

ELECTROCHEMISTRY

275962 The standard oxidation potentials of $Zn, Cu$ , $Ag$ and $Ni$ electrodes are $+ 0.76, 0.34, - 0.80$ and $+ 0.25 V$ respectively. Which of the following reaction will provide maximum voltage?

1

Cu + 2 {Ag}^{+} (aq) \to {Cu}^{2 +} (aq) + 2 Ag

2

Zn + 2 {Ag}^{+} (aq) \to {Zn}^{2 +} (aq) + 2 Ag

3

H_{2} + {Ni}^{2 +}

(aq)

\to 2 H^{+} (aq) + Ni

4

Zn + {Cu}^{2 +} (aq) \to {Zn}^{2 +} (aq) + Cu

5

Zn + 2 H^{+} (aq) \to {Zn}^{2 +} (aq) + H_{2}

Explanation:

Oxidation potentials are given in the question. The reduction potentials are obtained by changing the sign, i.e. the reduction potentials of $Zn$ , $Cu, Ag$ and $Ni$ are, $- 0.76, - 0.34, + 0.80$ and $- 0.25 V$ respectively.
$E_{cell}^{o} = E_{Ag}^{o} - E_{Zn}^{o}$ $= 0.80 - (- 0.76) = 1.56 V$

Kerala-CEE-2007

ELECTROCHEMISTRY

275963 The standard $E_{red}^{\circ}$ values of $A, B$ and $C$ are $+ 0.68 V, - 2.54 V, - 0.50 V$ respectively. The order of their reducing power is

1

A > B > C

2

A > C > B

3

C > B > A

4

B > C > A

Explanation:

Greater in the negative value of standard reduction potential, stronger is the reducing character. Thus, order of reducing power-
$B (- 2.54 V) > C (- 0.50 V) > A (+ 0.68 V)$

MHT CET-2007

ELECTROCHEMISTRY

275965 In electrolytic cell, cathode acts as an/a

1 oxidising agent

2 reducing agent

3 either of the two

4 Neither (a) nor (b)

Explanation:

In electrolytic cell, cathode acts as a reducing agent.
At cathode, ${Na}^{+} + e^{-} \to Na$ (reduction)
At anode,
$\begin{aligned} {Na}^{+} + e^{-} \to Na (reduction) \\ {Cl}^{-} \to Cl + e^{-} (oxidation) \\ {Na}^{+} + {Cl}^{-} \to \underset{Cathode}{Na + \underset{Anode}{Cl}} \end{aligned}$

UP CPMT-2007

ELECTROCHEMISTRY

275941 An aqueous solution containing $6.5 g$ of $NaCl$ of $90 %$ purity was subjected to electrolysis. After the complete electrolysis, the solution was evaporated to get solid $NaOH$ . The volume of $1 M$ acetic acid required to neutralize $NaOH$ obtained above is

1

1000 {cm}^{3}

2

2000 {cm}^{3}

3

100 {cm}^{3}

4

200 {cm}^{3}

Explanation:

Given that,
Weight of pure $NaCl = 6.5 \times 0.9 = 5.85 g$
No. of equivalence of $NaCl = \frac{5.85}{58.5} = 0.1$
No. of equivalence of $NaOH$ obtained $= 0.1 \times$ volume of $1 M$ acetic acid required for the neutralisation of $NaOH = \frac{0.1 \times 1000}{1} = 100 {cm}^{3}$

Karnataka CET-2009

ELECTROCHEMISTRY

275961 The standard electrode potential of hydrogen electrode at $1 M$ concentration and hydrogen gas at 1 atmosphere pressure is

1 1 Volt

2 6 Volt

3 8 Volt

4 0 Volt

Explanation:

$E = 0 - \frac{0.059}{2} \log \frac{1}{(1)^{2}} = 0 V$
Standard electrode potential of hydrogen at $1 M$ concentration and $1 atm$ pressure is Zero Volts.

J and K CET-(2007)

ELECTROCHEMISTRY

275962 The standard oxidation potentials of $Zn, Cu$ , $Ag$ and $Ni$ electrodes are $+ 0.76, 0.34, - 0.80$ and $+ 0.25 V$ respectively. Which of the following reaction will provide maximum voltage?

1

Cu + 2 {Ag}^{+} (aq) \to {Cu}^{2 +} (aq) + 2 Ag

2

Zn + 2 {Ag}^{+} (aq) \to {Zn}^{2 +} (aq) + 2 Ag

3

H_{2} + {Ni}^{2 +}

(aq)

\to 2 H^{+} (aq) + Ni

4

Zn + {Cu}^{2 +} (aq) \to {Zn}^{2 +} (aq) + Cu

5

Zn + 2 H^{+} (aq) \to {Zn}^{2 +} (aq) + H_{2}

Explanation:

Oxidation potentials are given in the question. The reduction potentials are obtained by changing the sign, i.e. the reduction potentials of $Zn$ , $Cu, Ag$ and $Ni$ are, $- 0.76, - 0.34, + 0.80$ and $- 0.25 V$ respectively.
$E_{cell}^{o} = E_{Ag}^{o} - E_{Zn}^{o}$ $= 0.80 - (- 0.76) = 1.56 V$

Kerala-CEE-2007

ELECTROCHEMISTRY

275963 The standard $E_{red}^{\circ}$ values of $A, B$ and $C$ are $+ 0.68 V, - 2.54 V, - 0.50 V$ respectively. The order of their reducing power is

1

A > B > C

2

A > C > B

3

C > B > A

4

B > C > A

Explanation:

Greater in the negative value of standard reduction potential, stronger is the reducing character. Thus, order of reducing power-
$B (- 2.54 V) > C (- 0.50 V) > A (+ 0.68 V)$

MHT CET-2007

ELECTROCHEMISTRY

275965 In electrolytic cell, cathode acts as an/a

1 oxidising agent

2 reducing agent

3 either of the two

4 Neither (a) nor (b)

Explanation:

In electrolytic cell, cathode acts as a reducing agent.
At cathode, ${Na}^{+} + e^{-} \to Na$ (reduction)
At anode,
$\begin{aligned} {Na}^{+} + e^{-} \to Na (reduction) \\ {Cl}^{-} \to Cl + e^{-} (oxidation) \\ {Na}^{+} + {Cl}^{-} \to \underset{Cathode}{Na + \underset{Anode}{Cl}} \end{aligned}$

UP CPMT-2007

ELECTROCHEMISTRY

275941 An aqueous solution containing $6.5 g$ of $NaCl$ of $90 %$ purity was subjected to electrolysis. After the complete electrolysis, the solution was evaporated to get solid $NaOH$ . The volume of $1 M$ acetic acid required to neutralize $NaOH$ obtained above is

1

1000 {cm}^{3}

2

2000 {cm}^{3}

3

100 {cm}^{3}

4

200 {cm}^{3}

Explanation:

Given that,
Weight of pure $NaCl = 6.5 \times 0.9 = 5.85 g$
No. of equivalence of $NaCl = \frac{5.85}{58.5} = 0.1$
No. of equivalence of $NaOH$ obtained $= 0.1 \times$ volume of $1 M$ acetic acid required for the neutralisation of $NaOH = \frac{0.1 \times 1000}{1} = 100 {cm}^{3}$

Karnataka CET-2009

ELECTROCHEMISTRY

275961 The standard electrode potential of hydrogen electrode at $1 M$ concentration and hydrogen gas at 1 atmosphere pressure is

1 1 Volt

2 6 Volt

3 8 Volt

4 0 Volt

Explanation:

$E = 0 - \frac{0.059}{2} \log \frac{1}{(1)^{2}} = 0 V$
Standard electrode potential of hydrogen at $1 M$ concentration and $1 atm$ pressure is Zero Volts.

J and K CET-(2007)

ELECTROCHEMISTRY

275962 The standard oxidation potentials of $Zn, Cu$ , $Ag$ and $Ni$ electrodes are $+ 0.76, 0.34, - 0.80$ and $+ 0.25 V$ respectively. Which of the following reaction will provide maximum voltage?

1

Cu + 2 {Ag}^{+} (aq) \to {Cu}^{2 +} (aq) + 2 Ag

2

Zn + 2 {Ag}^{+} (aq) \to {Zn}^{2 +} (aq) + 2 Ag

3

H_{2} + {Ni}^{2 +}

(aq)

\to 2 H^{+} (aq) + Ni

4

Zn + {Cu}^{2 +} (aq) \to {Zn}^{2 +} (aq) + Cu

5

Zn + 2 H^{+} (aq) \to {Zn}^{2 +} (aq) + H_{2}

Explanation:

Oxidation potentials are given in the question. The reduction potentials are obtained by changing the sign, i.e. the reduction potentials of $Zn$ , $Cu, Ag$ and $Ni$ are, $- 0.76, - 0.34, + 0.80$ and $- 0.25 V$ respectively.
$E_{cell}^{o} = E_{Ag}^{o} - E_{Zn}^{o}$ $= 0.80 - (- 0.76) = 1.56 V$

Kerala-CEE-2007

ELECTROCHEMISTRY

275963 The standard $E_{red}^{\circ}$ values of $A, B$ and $C$ are $+ 0.68 V, - 2.54 V, - 0.50 V$ respectively. The order of their reducing power is

1

A > B > C

2

A > C > B

3

C > B > A

4

B > C > A

Explanation:

Greater in the negative value of standard reduction potential, stronger is the reducing character. Thus, order of reducing power-
$B (- 2.54 V) > C (- 0.50 V) > A (+ 0.68 V)$

MHT CET-2007

ELECTROCHEMISTRY

275965 In electrolytic cell, cathode acts as an/a

1 oxidising agent

2 reducing agent

3 either of the two

4 Neither (a) nor (b)

Explanation:

In electrolytic cell, cathode acts as a reducing agent.
At cathode, ${Na}^{+} + e^{-} \to Na$ (reduction)
At anode,
$\begin{aligned} {Na}^{+} + e^{-} \to Na (reduction) \\ {Cl}^{-} \to Cl + e^{-} (oxidation) \\ {Na}^{+} + {Cl}^{-} \to \underset{Cathode}{Na + \underset{Anode}{Cl}} \end{aligned}$

UP CPMT-2007

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