Electrolysis of aqueous copper (II) sulphate between Pt electrodes gives ' $X^{\prime}$ at anode and ' $Y^{\prime}$ at cathode. $X$ and $Y$ are respectively.

At 298 K , if emf of the cell corresponding to the reaction $\mathrm{Zn}(s)+2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Zn}^{2+}(0.01 \mathrm{M})+\mathrm{H}_2(g) (1 \mathrm{~atm})$ is 0.28 V , then the pH of the solution at the hydrogen electrode is $\left(\frac{2.303 R T}{F}=0.06 \mathrm{~V}\right)$, $\left(E_{\mathrm{Zn}^{2+} / \mathrm{Zn}}^{\circ}=-0.76 \mathrm{~V}\right)$

0.592 g of copper is deposited in 60 minutes by passing

0.5 A current through a solution of copper (II) sulphate. The electro chemical equivalent of copper (II) (in $\mathrm{gC}^{-1}$ ) is

( $F=96500 \mathrm{C} \mathrm{mol}^{-1}$ )