$A$ solution of $Ni(NO_3)_2$ is electrolysed between platinum electrodes using $0.1 \ F$ electricity. How many moles of $Ni$ will be deposited at the cathode?

The quantity of electricity (in $C$) required to oxidize $1 \ mol$ of $H_2O$ to $O_2$ is approximately ..................... $\times 10^5 \ C$.

How much Faraday of electricity is required to reduce $1.5 \ mole$ of $KMnO_4$ into $MnO_2$ in a basic medium (in $F$)?

An electric current is passed through silver nitrate solution using silver electrodes. $10.79 \ g$ of silver was found to be deposited on the cathode. If the same amount of electricity is passed through copper sulphate solution using copper electrodes,the weight of copper deposited on the cathode is ............. $g$

For how much time,$10 \ A$ electric current should be passed through a dilute aqueous $NiSO_4$ solution during electrolysis using inert electrode,in order to get $5.85 \ g$ Nickel (in $s$)?
[At. mass of $Ni = 58.5 \ g/mol$]

$A$ current of $10.0 \, A$ flows for $2.00 \, h$ through an electrolytic cell containing a molten salt of metal $X$. This results in the decomposition of $0.250 \, mol$ of metal $X$ at the cathode. The oxidation state of $X$ in the molten salt is $(F = 96,500 \, C \, mol^{-1})$ (in $+$)