Chemistry - Electrochemistry Question with Solution | TestHub

$\mathrm{Pt}\left({\mathrm{H}}_2\right){\mathrm{P}}_1$ atm. $|\mathrm{HCl}|\mathrm{Pt}\left({\mathrm{H}}_2\right){\mathrm{P}}_2$ atm. For spontaneous reaction, $E_{\text{cell }}$ should be positive so $P_1>P_2$ $E_{\text{cell }}=\frac{0.059}{2}\log \frac{P_1}{P_2}$ Also, if $P_1>P_2$ oxidation occurs at L.H.S. electrode and reduction occurs at R.H.S. electrode.