For a cell, $\mathrm{Cu}\left(\mathrm{s}\right)\mid {\mathrm{Cu}}^{2+}\left(0.001\mathrm{M}\left|\right|{\mathrm{Ag}}^{+}(0.01\mathrm{M})\mid \mathrm{Ag}\left(\mathrm{s}\right)\right.$ the cell potential is found to be 0.43V at 298 K. The magnitude of standard electrode potential for ${\mathrm{Cu}}^{2+}/\mathrm{Cu} \mathrm{is} \mathrm{\_\_\_\_\_\_\_}\times {10}^{-2} \mathrm{V}.$
[Given : ${\mathrm{E}}_{{\mathrm{Ag}}^{+};\mathrm{Ag}}^{\ominus }=0.80\mathrm{V}$ and $\left.\frac{2.303\mathrm{RT}}{\mathrm{F}}=0.06\mathrm{V}\right]$

$\mathrm{Anode}: \mathrm{Cu}\left(\mathrm{s}\right)\to {\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}$
Cathode: $\left.{\mathrm{Ag}}^{+}+{\mathrm{e}}^{-}\to \mathrm{Ag}\left(\mathrm{s}\right)\right]2$
$\overline{\mathrm{Cus}\left(\mathrm{s}\right)+2{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)\to {\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)+2\mathrm{Ag}\left(\mathrm{s}\right)}$
$\begin{array}{l}{\mathrm{E}}_{\text{cell }}={\mathrm{E}}_{\text{cell }}^{\mathrm{o}}-\frac{0.06}{2}\log \frac{\left[{\mathrm{Cu}}^{2+}\right]}{{\left[{\mathrm{Ag}}^{+}\right]}^2}\\ 0.43={\mathrm{E}}_{\text{cell }}^{\mathrm{o}}-\frac{0.06}{2}\log \left(\frac{{10}^{-3}}{{\left({10}^{-2}\right)}^2}\right)\\ 0.43={\mathrm{E}}_{\mathrm{cell}}^{\mathrm{o}}-0.03\log 10\\ {\mathrm{E}}_{\text{cell }}^{\mathrm{o}}=0.46\mathrm{V}\\ {\mathrm{E}}_{\mathrm{cell}}^{\mathrm{o}}={\mathrm{E}}_{{\mathrm{Ag}}^{+}/\mathrm{Ag}}^{\mathrm{l}}-{\mathrm{E}}_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}^{\mathrm{o}}\\ {\mathrm{E}}_{{\mathrm{Cu}}^{2+}/{\mathrm{Cu}}^{\mathrm{o}}}^{\mathrm{o}}=(0.80-0.46)=0.34\mathrm{V}=34\times {10}^{-2}\end{array}$