The electrode potential of the following half cell at 298   K X X 2 + 0 . 001 M ‖ Y 2 + 0 . 01 M…

The net cell reaction can be written as follows,

$\mathrm{X}+{\mathrm{Y}}^{2+}\to \mathrm{Y}+{\mathrm{X}}^{2+}$

${\mathrm{E}}_{\mathrm{cell}}^0={\mathrm{E}}_{\mathrm{cathode}}^0-{\mathrm{E}}_{\mathrm{anode}}^0$(Both are SRP values)

${\mathrm{E}}_{\mathrm{Cell}}^0=0.36-\left(-2.36\right)=2.72 \mathrm{V}$

Now, the Nernst equation is,

${\mathrm{E}}_{\mathrm{cell}}={\mathrm{E}}_{\mathrm{cell}}^0-\frac{0.06}{\mathrm{n}}\log \frac{\left[{\mathrm{X}}^{2+}\right]}{\left[{\mathrm{Y}}^{2+}\right]}$

$\mathrm{n}=$The number of electrons involved in the net reaction.

${\mathrm{E}}_{\mathrm{Cell}}=2.72-\frac{0.06}{2}\log \frac{0.001}{0.01}$

$=2.72+0.03=2.75 \mathrm{V}$

$=275\times {10}^{-2} \mathrm{V}$