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.