A current of $\text{5}\text{.0}\text{A}$ flows for $\text{4}\text{.0}\text{h}$ through an electrolytic cell containing a molten salt of metal M. This results in deposition of $\text{0}\text{.25}\text{mol}$ of the metal $\text{M}$ at the cathode. The oxidation state of $\text{M}$ in the molten salt is $\text{+}\text{x}$. the value of '$\text{x}$' is ($\text{1}\text{Faraday}\text{=}\text{96000}\text{C}$ $\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$)