Chemistry - Electrochemistry Question with Solution | TestHub

The given standard reduction potential is $E_{\text{red}}^{\circ }=+0.34\text{ V}$.

The required reaction is an oxidation reaction:
${\mathrm{Cu}}_{(\mathrm{s})}\to {\mathrm{Cu}}_{(\mathrm{aq})}^{+2}(0.1\text{ M})+2{\mathrm{e}}^{-}$

The standard oxidation potential is:
$E_{\text{ox}}^{\circ }=-E_{\text{red}}^{\circ }=-0.34\text{ V}$

Using the Nernst equation for the oxidation potential at $298\text{ K}$:
$E_{\text{ox}}=E_{\text{ox}}^{\circ }-\frac{0.0592}{n}{\log }_{10}[{\mathrm{Cu}}^{+2}]$

Here, the number of electrons transferred is $n=2$ and $[{\mathrm{Cu}}^{+2}]=0.1\text{ M}$.

$E_{\text{ox}}=-0.34-\frac{0.0592}{2}{\log }_{10}(0.1)$

$E_{\text{ox}}=-0.34-0.0296\times (-1)$

$E_{\text{ox}}=-0.34+0.0296$

$E_{\text{ox}}=-0.3104\text{ V}$

Answer: -0.3104 V