Select the most appropriate Nernst equation for Daniell cell containing ${Cu}^{2 +} and {Zn}^{2 +} ions .$

Moderate

A

$E_{({cu}^{2 +} / Cu)} = E_{({Cu}^{2 +} / Cu)}^{o} - \frac{RT}{F} In \frac{1}{[{Cu}^{2 +} (aq)]}$
B

$E_{({Zn}^{2 +} / Zn)} = E_{({Zn}^{2 +} / Zn)}^{o} - \frac{RT}{2 F} In \frac{1}{[{Zn}^{2 +} (aq)]}$
C

$E_{cell} = E_{cell}^{o} - \frac{RT}{2 F} In \frac{[{Zn}^{2 +}]}{[{Cu}^{2 +}]}$
D

All of the above

Solution

In Daniell cell, the electrode potential for concentration of Cu²⁺ and Zn²⁺ ions can be written as
For cathode
$E_{({Cu}^{2 +} / Cu)} = E_{({Cu}^{2 +} / Cu)}^{o} - \frac{RT}{2 F} In \frac{1}{[{Cu}^{2 +} (aq)]}$
For anode
$E_{({Zn}^{2 +} / Zn)} = E_{({Zn}^{2 +} / Zn)}^{o} - \frac{RT}{2 F} In [{Zn}^{2 +} (aq)] E_{cell} = E_{{Cu}^{2 +} / Cu} - E_{{Zn}^{2 +} / Zn} E_{cell} = E_{cell}^{o} - \frac{RT}{2 F} In \frac{[{Zn}^{2 +}]}{[{Cu}^{2 +}]}$

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