Chemistry - Electrochemistry Question with Solution | TestHub

To a beaker containing $0.1\mathrm{M}-\mathrm{HCl}$, pure solid AgCl is added. Both a silver and a hydrogen electrode (${\mathrm{p}}_{{\mathrm{H}}_2}=1.0$ bar = constant) are then placed in the solution. The value of $E_{cell}$ (in volts) at $298\mathrm{K}$ is:

$[E_{\frac{A{g}^{+}}{Ag}}^0=0.80\mathrm{V},$, $K_{sp}(\mathrm{AgCl})=10^{-10}$, $\frac{2.303RT}{F}=0.06\mathrm{F}]$