$A$ solution of $CuSO_4$ is electrolysed for $10$ minutes with a current of $1.5$ amperes. What is the mass of copper deposited at the cathode (in $g$)?

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

The ratio of weights of hydrogen gas liberated and magnesium deposited by passing the same amount of electricity from aqueous $H_2SO_4$ and fused $MgSO_4$ are :

The electrochemical equivalent of magnesium is $0.126 \ mg/C$. $A$ current of $5 \ A$ is passed in a suitable solution for $1 \ hour$. The mass of magnesium deposited will be ........... $gm$.

What is the charge on tin if $7.375 \ g$ of metallic tin is deposited by the passage of $24125 \ C$ through a solution containing the ion? [Atomic weight of $Sn = 118 \ g/mol$]

How much charge is required for the following reductions:
$(i)$ $1 \, mol$ of $Al^{3+}$ to $Al$.
$(ii)$ $1 \, mol$ of $Cu^{2+}$ to $Cu$.
$(iii)$ $1 \, mol$ of $MnO_{4}^{-}$ to $Mn^{2+}$.