Chemistry - Electrochemistry Question with Solution | TestHub

$\begin{array}{rl}& {\mathrm{Cu}}_{(\mathrm{s})}^{2+}+2{\mathrm{e}}^{-}⟶{\mathrm{Cu}}_{(\mathrm{s})}\\ & \text{ Mole ratio }=\frac{1\mathrm{mol}}{2{\mathrm{mole}}^{-}}\\ & \mathrm{W}=\frac{\mathrm{I}(\mathrm{A})\times \mathrm{t}(\mathrm{s})}{96500\left(\mathrm{C}/\mathrm{mol}{\mathrm{e}}^{-}\right)}\times \text{mole ratio }\times \text{ molar mass }\\ & 6.35\mathrm{g}=\frac{5\times \mathrm{t}}{96500\left(\mathrm{C}/\mathrm{mol}{\mathrm{e}}^{-}\right)}\times \frac{1\mathrm{mol}}{2\mathrm{mol}\mathrm{e}}\times 63.5\mathrm{g}{\mathrm{mol}}^{-1}\\ & \mathrm{t}=\frac{6.35\times 96500\times 2}{5\times 63.5}=3860\text{ seconds }\end{array}$