Question

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

Answer 1

Answer: 34

At anode
$Cu\to C{u}^{2+}+2e^{-}$
At cathode
$2A{g}^{+}+2e^{-}\to 2Ag$
$\text{ Cell reaction }\to Cu+2A{g}^{+}\to C{u}^{2+}+2Ag$
$E_{\text{cell }}=E_{\text{cell }}^0-\frac{0.06}{2}\log \frac{\left[C{u}^{2+}\right]}{{\left[A{g}^{+}\right]}^2}$
$0.43=E_{\text{cell }}^0-\frac{0.06}{2}\log \frac{(0.001)}{(0.01{)}^2}$
$E_{cell}^0=0.46$
$E_{cel{l}^0}^0=E_{A{g}^{+}/Ag}^0-E_{C{u}^{2+}/Cu}^0$
$0.46=0.80-E_{C{u}^{2+}/Cu}^0$
$E_{C{u}^{2+}/Cu}^0=0.34$ volt
$E_{C{u}^{2+/Cu}}^0=34\times 10^{-2}$