Some standard electrode potentials at 298K are given below: cases...

Since $X$ is getting dissolved, so reaction is

$$\begin{array}{ll}X \to {X}^{2 +} + 2{e}^{-}\left[Anode\right] \\ {Y}^{2 +} + 2{e}^{-} \to Y\left[cathode\right]\end{array}$${Y}^{2 +} + X \to {X}^{2 +} + Y$</p><p>${E}_{cell} = {E}_{cell}^{°} - \dfrac{0 . 06}{2}log\dfrac{{10}^{- 3}}{{10}^{- 1}}$</p><p>${E}_{cell} = {E}_{cell}^{°} + 0 . 06$</p><p>(A)$Cd \text{ and } Ni$</p> (=0.16+0.05912 \times 2)$=.16+0.0591$(=0.21(+\mathrm{ve})) <p>${E}_{cell} < 0$(Non-spontaneous)</p><p>(B)$Cd \text{ and } Fe$</p><p>${E}_{cell} = - 0 .044 - \left(- 0 .40\right) + 0 .06$</p><p>$= - 0 . 04 + 0 . 06$</p><p>$= 0 . 02V$</p><p>${E}_{cell} > 0$(Spontaneous)</p><p>(C)$Ni \text{ and } Pb$</p><p>${E}_{cell} = \left(- 0 .13 - \left(- 0 .24\right)\right) + 0 .06$</p><p>$= 0 . 11 + 0 . 06$</p><p>$= 0 . 17V$</p><p>${E}_{cell} > 0$(spontaneous)</p><p>(D)$Ni \text{ and } Fe$</p><p>${E}_{cell} = \left(- 0 .44 - \left(- 0 .24\right)\right) + 0 .06$</p><p>$= - 0 . 20 + 0 . 06$</p><p>$= - 0 . 14V$</p><p>${E}_{cell} < 0$ (Non-Spontaneous)