Subject: Physical Chemistry · Chapter: Electrochemistry · Topic: Electrochemistry – General · Exam: NET DEC 2015 · Marks: 2 · Difficulty: Medium
Given that $\mathrm{E}^{\circ}\left(\mathrm{Cl}_{2} / \mathrm{Cl}^{-}\right)=1.35 \mathrm{V}$ and $\mathrm{K}_{\mathrm{sp}}(\mathrm{AgCl})=10^{-10}$ at $25^{\circ} \mathrm{C}$, $E^{0}$ corresponding to the electrode reaction $\frac{1}{2} \mathrm{Cl}_{2}(\mathrm{g})+\mathrm{Ag}^{+}($Soln. $)+\mathrm{e}^{-} \rightarrow \mathrm{AgCl}(\mathrm{s})$