Identify the incorrect statement from the options below for the above cell :

$\mathrm{E}_{\text {cell }}^{0}=\mathrm{E}_{\mathrm{Cu}^{2+}}^{0}{\mid \mathrm{Cu}}^{-}-\mathrm{E}_{\mathrm{Zn}^{2+} \mid \mathrm{Zn}}^{0}=1.1 \mathrm{~V}$

So, if $\mathrm{E}_{\text {ext. }}=1.1 \mathrm{~V}$ no electron will flow

At, $\mathrm{E}_{\text {ext. }}>1.1 \mathrm{~V}$ cell act as electrolytic cell and electron will flow from $\mathrm{Cu}$ to $\mathrm{Zn}$.

At, $\mathrm{E}_{\text {ext. }}<1.1 \mathrm{~V}$ cell act as electrochemical cells so $\mathrm{Zn}$ dissolve and $\mathrm{Cu}$ deposit.