Chemistry - Electrochemistry Question with Solution | TestHub

The given cell reaction is ${\mathrm{Zn}}_{(\mathrm{s})}+{\mathrm{Cu}}_{(\mathrm{aq})}^{+2}\to {\mathrm{Zn}}_{(\mathrm{aq})}^{+2}+{\mathrm{Cu}}_{(\mathrm{s})}$

The number of electrons transferred in the reaction is $n=2$.

Using the Nernst equation at 298 K:

$E_{\text{cell}}=E_{\text{cell}}^{\circ }-\frac{0.0592}{n}{\log }_{10}\frac{[{\mathrm{Zn}}^{+2}]}{[{\mathrm{Cu}}^{+2}]}$

Substituting the given values:

$E_{\text{cell}}=1.1-\frac{0.0592}{2}{\log }_{10}\left(\frac{0.1}{0.1}\right)$

$E_{\text{cell}}=1.1-\frac{0.0592}{2}{\log }_{10}(1)$

Since ${\log }_{10}(1)=0$:

$E_{\text{cell}}=1.1-0=1.1\text{ V}$

Answer: 1.1 V