Lawrie Ryan and Roger Norris Solutions for Chapter: Electrochemistry, Exercise 21: Questions

A half-cell containing $\mathrm{Sn}$ in $1.00 \mathrm{mol} {\mathrm{dm}}^{-3}$ ${\mathrm{Sn}}^{2+}$ ions is connected to another half-cell containing $\mathrm{Zn}$ in $1.00 \mathrm{mol} {\mathrm{dm}}^{-3}$ ${\mathrm{Zn}}^{2+}$ ions at $298 \mathrm{K}$. 

${\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}\stackrel{ }{\rightleftharpoons }\mathrm{Zn}\left(\mathrm{s}\right): {\mathrm{E}}^{°}=-0.76 \mathrm{V}$ and 

${\mathrm{Sn}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}\stackrel{ }{\rightleftharpoons }\mathrm{Sn}\left(\mathrm{s}\right): {\mathrm{E}}^{°}=-0.14 \mathrm{V}$

Which one of the following is the value of $\mathrm{E}$ when the concentration of both the ${\mathrm{Zn}}^{2+}$ ions and ${\mathrm{Sn}}^{2+}$ are changed to $0.1 \mathrm{mol} {\mathrm{dm}}^{-3}$?

An industrial process relies on a reaction that is impractically slow under normal conditions. How might you try to solve this problem? Use your knowledge of reaction rates to suggest several approaches.

Describe two limitations of using ${\mathrm{E}}^{°}$ values to predict the feasibility of a reaction.