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Electrochemical Cells, Galvanic Cells

Which of the ...

Question

Which of the following cells can be used to experimentally determine the reduction potential of Zinc?

A

Z n (s) | Z n^{2 +} (a q) | | H^{+} (a q) | H_{2} (g), P t

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B

P t, H_{2} (g) | H^{+} (a q) | | Z n (s) | Z n^{2 +} (a q)

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C

Z n (s) | Z n^{2 +} (a q) | | C u^{2 +} (a q) | C u (s)

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D

any one of these

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Solution

The correct option is A $Z n (s) | Z n^{2 +} (a q) | | H^{+} (a q) | H_{2} (g), P t$
SRP of zinc is -0.76 volts.
SRP of hydrogen is 0.
Since SRP of zinc is less than SRP of hydrogen hence, Zn acts as a cathode.
To find the reduction potential of the element we make the anode of the metal and cathode of $H^{+}$ as the standard reduction potential of $H^{+} | H_{2} = 0$ .
$∴$ The cell is $Z n (s) | Z n^{2 +} (a q) | | H^{+} (a q) | H_{2} (g), P t$

Hence, option A is correct.

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Similar questions

Q. For the cell,

Z n (s) | Z n^{2 +} (a q) | | C u^{2 +} (a q) | C u (s)

The cell potential

E_{c e l l}

can be increased:

E_{C e l l}^{o}

value of the following reactions:

Z n (s) + C u^{2 +} (a q) \to Z n^{2 +} (a q) + C u (s)

E_{C u^{2 +} / C u}^{\circ} = 0.34 V, E_{Z n^{2 +} / Z n}^{\circ} = - 0.76 V

E^{\circ}

{Zn(s)|Zn}^{2 +} (aq) | | {Cu}^{2 +} (aq)|Cu(s)

1.10

25^{\circ} C

. The equilibrium constant for the reaction,

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

1.94 \times 10^{x}

x

$E^{0}$ for the cell, $Z n | Z n {^{2 +}}_{(a q)} | | C u {^{2 +}}_{(a q)} | C u$ is $1.10 V$ at $25^{0} C$ . The equilibrium constant for $Z n + C u {^{2 +}}_{(a q)} \to Z n {^{2 +}}_{(a q)} + C u$ the cell reaction is of the order of :

Consider the cell:

Z n | Z n^{2 +} (a q) (1.0 M) | | C u^{2 +} (a q) (1.0 M) | | C u

The standard reduction potential are

0.350

C u^{2 +} (a q) + 2 e^{-} \to C u

- 0.763

Z n^{2 +} (a q) + 2 e^{-} \to Z n

The cell reaction is:

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