Paper: CSIR-NET December 2015 · Subject: Physical Chemistry · Chapter: Electrochemistry · Topic: Electrochemistry – General · Marks: 2 · Difficulty: Medium
Given that $E^{o}\left(\mathrm{Cl_2}/\mathrm{Cl^{-}}\right)=1.35\,\mathrm{V}$ and $K_{sp}(\mathrm{AgCl})=10^{-10}$ at $25^{\circ}\mathrm{C}$, $E_0$ corresponding to the electrode reaction $\dfrac{1}{2}\mathrm{Cl_2}(g)+\mathrm{Ag^{+}}(\text{Soln.})+e^{-} \rightarrow \mathrm{AgCl}(s)$ is $\left[\dfrac{2.303RT}{F}=0.06\,V\right]$