Electrochemistry

Assertion (A) For a Daniell cell \(\mathrm{Zn} / \mathrm{Zn}^{2+} \| \mathrm{Cu}^{2+} \mid \mathrm{Cu}\) with \(E_{\text {cell }}=1.1 \mathrm{~V}\), the application of opposite potential greater than \(1.1 \mathrm{~V}\) results into the flow of electrons from cathode to anode.

Reason (R) Zn is deposited at zinc electrode and \(\mathrm{Cu}\) is dissolved at copper electrode.