Molten $\mathrm{Ni}{\left({\mathrm{NO}}_3\right)}_2$ is electrolysed between platinum electrodes using 0.1 Faraday of electrical charge. The number of moles of Nickel deposited at the cathode  is

Each NI⁺² ion accepts 2 electrons during its reduction

$$\begin{gathered} \mathrm{So}, \mathrm{g} \mathrm{eq} \mathrm{wt} \mathrm{of} \mathrm{Ni}=\frac{\mathrm{Mass} \mathrm{of} \mathrm{one} \mathrm{mole} \mathrm{of} \mathrm{Ni}}{\mathrm{No}. \mathrm{of} {\mathrm{e}}^{-1} \mathrm{accepted} \mathrm{by} \mathrm{each} {\mathrm{Ni}}^{2+} \mathrm{ion} =2} \\ \mathrm{i}.\mathrm{e}., \mathrm{No}.\mathrm{of} \mathrm{g} \mathrm{eq} \mathrm{is} \mathrm{twice} \mathrm{No}.\mathrm{of} \mathrm{mole} \\ \mathrm{No}. \mathrm{of} \mathrm{mole}=\frac{\mathrm{No}. \mathrm{of} \mathrm{g} \mathrm{eq}}{2} \\ 0.1 \mathrm{Faraday} \mathrm{of} \mathrm{charge} \mathrm{deposits} 0.1 \mathrm{g} \mathrm{eq} \mathrm{of} \mathrm{substance} \mathrm{or} \frac{0.1}{2}=0.05 \mathrm{mole} \end{gathered}$$