Write the cell reaction and calculate the standard $\mathrm{E}°$ of the cell.

$\mathrm{Zn}\left|{\mathrm{Zn}}^{2+}\right(1\mathrm{M}\left)\right|\left|{\mathrm{Cd}}^{2+}\right(1\mathrm{M}\left)\right|\mathrm{Cd}$

Given, $\mathrm{E}{°}_{\mathrm{Zn}/{\mathrm{Zn}}^{2+}}=0.763, \mathrm{E}{°}_{\mathrm{Cd}/{\mathrm{Cd}}^{2+}}=0.403\mathrm{V}$

The standard electrode potentials at $298 \mathrm{K}$ are given below:

$\mathrm{E}{°}_{{\mathrm{Zn}}^{2+}/\mathrm{Zn}}=-0.76\mathrm{V}, \mathrm{E}{°}_{{\mathrm{Fe}}^{2+}/\mathrm{Fe}}=-0.44\mathrm{V}$

${\mathrm{E}}_{{\mathrm{H}}^{+}/{\mathrm{H}}_2}^{\mathrm{o}} = 0.0\mathrm{V}, {\mathrm{E}}_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}^{\mathrm{o}} =+0.34\mathrm{V}$

Which of the two electrodes should be combined to form a cell having the highest emf? Identify the cathode and the anode and write the cell reaction.