$A$ current of $0.25 \, A$ is passed through $CuSO_4$ solution placed in a voltameter for $45 \, minutes$. The amount of $Cu$ deposited on the cathode is ............. $g$ $(At. \, weight \, of \, Cu = 63.6)$.

The negative $Zn$ pole of a Daniel cell,sending a constant current through a circuit,decreases in mass by $0.13 \ g$ in $30$ minutes. If the electrochemical equivalent of $Zn$ and $Cu$ are $32.5$ and $31.5$ respectively,the increase in the mass of the positive $Cu$ pole in this time is .............. $g$.

How much current should be passed through acidified water for $100 \ s$ to liberate $0.224 \ L$ of $H_2$ gas at $STP$ (in $A$)?

By passing electric current,$NaClO_{3}$ is converted into $NaClO_{4}$ according to the following equation:
$NaClO_{3} + H_{2}O \rightarrow NaClO_{4} + H_{2}$
How many moles of $NaClO_{4}$ will be formed when $3 \ F$ of charge is passed through $NaClO_{3}$?

How much electricity in terms of Faraday is required to produce:
$(i)$ $20.0 \, g$ of $Ca$ from molten $CaCl_2$?
$(ii)$ $40.0 \, g$ of $Al$ from molten $Al_2O_3$?

Clarify the stoichiometry of the reactions occurring on the electrodes of an electrolytic cell and its relationship with the quantity of electricity.