Consider the cell $\mathrm{Pt}\left|\mathrm{Cl}_2\left(P_L\right)\right| \mathrm{HCl}(\mathrm{aq})\left|\mathrm{Cl}_2\left(P_R\right)\right| \mathrm{Pt}$, where $P_L$ and $P_R$ are the $\mathrm{Cl}_2$ pressures at the left and right electrodes. The standard electrode potential of $\mathrm{Cl}_2+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cl}^{-}$is 1.36 eV . The correct expression for electrode potential $(E)$ is $(\mathrm{F}$ is the Faraday constant)

• A

  $E=1.36-\frac{R T}{2 F} \ln \frac{P_L}{P_R}$
• Correct answer
  B

  $E=-\frac{R T}{2 F} \ln \frac{P_L}{P_R}$
• C

  $E=-1.36-\frac{R T}{2 F} \ln \frac{P_L}{P_R}$
• D

  $E=-\frac{R T}{F} \ln \frac{P_L}{P_R}$

Hence, the correct answer is option: 'B'.