(a) Calculate for the following reaction at 298K :
$2\mathrm{Al}\left(\mathrm{}\mathit{s}\right)+3{\mathrm{Cu}}^{2+}\left(0.01\mathrm{M}\right)\to$ $2{\mathrm{Al}}^{3+}\left(0.01\mathrm{M}\right)+3\mathrm{Cu}\left(\mathrm{}\mathit{s}\right)$

(b) Using the ${\mathrm{E}}^{\circ }$ values of $\mathrm{A}$ and $\mathrm{B}$, predict which is better for coating the surface of iron [${\mathrm{E}}^{\circ }{}_{\left({\mathrm{Fe}}^{2+}∕\mathrm{Fe}\right)}$ $=-0.44\mathrm{V}]$ to prevent corrosion and why ?
Given : $\mathrm{E}{°}_{\left({\mathrm{A}}^{2+}∕\mathrm{A}\right)}=-2.37\mathrm{V}$ $\mathrm{}:\mathrm{}\mathrm{E}{°}_{\left({\mathrm{B}}^{2+}∕\mathrm{B}\right)}=-0.14\mathrm{V}$
OR
(a) The conductivity of $0.001\mathrm{mol}{\mathrm{L}}^{-1}$ solution of ${\mathrm{CH}}_3\mathrm{COOH}$ is $3.905\times {10}^{-5}\mathrm{S}{\mathrm{cm}}^{-1}$. Calculate its molar conductivity and degree of dissociation $\left(\mathit{\alpha }\right)$.
Given ${\mathit{\lambda }}^0\left({\mathrm{H}}^{+}\right)=349.6\mathrm{S}\mathrm{cm}{\mathrm{mol}}^{-1}$ and ${\mathit{\lambda }}^0$ $\left({\mathrm{CH}}_3{\mathrm{COO}}^{-}\right)=40.9\mathrm{S}{\mathrm{cm}}^2{\mathrm{mol}}^{-1}$
(b) Define electrochemical cell. What happens if external potential applied becomes greater than of electrochemical cell ?