K L Chugh Solutions for Chapter: Electrochemistry, Exercise 11: Follow Up Problems

Calculate ${\mathrm{\Delta G}}^{\mathrm{\Theta }}$ and the equilibrium constant for the cell reaction:

${\mathrm{Cl}}_2+2{\mathrm{I}}^{-}⟶2{\mathrm{Cl}}^{-}+{\mathrm{I}}_2$

Given that ${\mathrm{E}}^{\mathrm{\Theta }}\left({\mathrm{Cl}}_2, {\mathrm{Cl}}^{-}\right)=1.36 \mathrm{V}; {\mathrm{E}}^{\mathrm{\Theta }}\left({\mathrm{I}}_2, {\mathrm{I}}^{-}\right)=0.536 \mathrm{V}$

$$Determine the equilibrium constant of the reaction at $298 \mathrm{K},$ 

given $$\begin{gathered} {{\mathrm{E}}^{°}}_{{\mathrm{Fe}}^{3+}/{\mathrm{Fe}}^{2+}}=0.771 \mathrm{V} \\ {{\mathrm{E}}^{°}}_{{\mathrm{Sn}}^{2+}/\mathrm{Sn} =}+0.150 \mathrm{V} \end{gathered}$$

for chemical reaction $2{\mathrm{Fe}}^{3+}+{\mathrm{Sn}}^{2+}\rightleftharpoons 2{\mathrm{Fe}}^{2+}+{\mathrm{Sn}}^{4+}$.

From the obtained value of the equilibrium constant, predict whether ${\mathrm{Sn}}^{2+}$ ions can reduce ${\mathrm{Fe}}^{3+}$ to ${\mathrm{Fe}}^{2+}$ quantitatively or not