$\begin{array}{r}{\mathrm{E}}_{{\mathrm{Cu}}^{2+}\mid \mathrm{Cu}}^0=+0.34\mathrm{V}\\ {\mathrm{E}}_{{\mathrm{Zn}}^{2+}\mid \mathrm{Zn}}^0=-0.76\mathrm{V}\end{array}$

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

Cathode has reduction, therefore it is negative whereas anode is positive because it corresponds to oxidation. 

$$\begin{gathered} {\mathrm{E}}_{\text{cell }}^{\circ }={\mathrm{E}}_{\mathrm{red}/\mathrm{cathode}}^{\circ }-{\mathrm{E}}_{\mathrm{red}/\mathrm{anode}}^{\circ } \\ {\mathrm{E}}_{\text{cell }}^{\circ }=-0.76 \mathrm{V}-0.34 \mathrm{V} \\ {\mathrm{E}}_{\text{cell }}^{\circ }<1.1 \mathrm{V} \end{gathered}$$

 ${\mathrm{E}}_{\mathrm{ext}}<1.1\mathrm{V}$  then zinc will act as cathode (Zn electrode) and Cu as anode (Cu electrode).