The electrode potential of the following half cell at 298K X | X ^...

The net cell reaction can be written as follows,

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

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

${E}_{Cell}^{0} = 0 . 36 - \left(- 2 . 36\right) = 2 . 72V$

Now, the Nernst equation is,

${E}_{cell} = {E}_{cell}^{0} - \dfrac{0 . 06}{n}log\dfrac{\left[{X}^{2 +}\right]}{\left[{Y}^{2 +}\right]}$

$n =$The number of electrons involved in the net reaction.

${E}_{Cell} = 2 . 72 - \dfrac{0 . 06}{2}log\dfrac{0 . 001}{0 . 01}$

$= 2 . 72 + 0 . 03 = 2 . 75V$

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