How much volume of oxygen at $STP$ will be liberated by $2$ $ampere$ flowing for $3$ $minutes$ and $13$ $seconds$ through acidified water? (in $cc$)

Faraday's laws of electrolysis state that the mass deposited on an electrode is proportional to:

Potassium chlorate is prepared by the electrolysis of $KCl$ in basic solution:
$6 OH^{-} + Cl^{-} \rightarrow ClO_{3}^{-} + 3 H_{2}O + 6 e^{-}$
If only $60\%$ of the current is utilized in the reaction,the time (rounded to the nearest hour) required to produce $10 \ g$ of $KClO_{3}$ using a current of $2 \ A$ is:
(Given: $F = 96,500 \ C \ mol^{-1}$,molar mass of $KClO_{3} = 122 \ g \ mol^{-1}$)

The mass of zinc produced by the electrolysis of zinc sulphate solution with a steady current of $0.015 \ A$ for $15$ minutes is . . . . . . $ \times 10^{-4} \ g$. (Atomic mass of zinc $= 65.4 \ amu$)

The mass of copper deposited from a solution of $CuSO_4$ by passage of $5 \ A$ current for $965 \ s$ is ............ $g$ (Mol. wt. of Copper $= 63.5$)

The number of electrons required to deposit $1 \ g$ atom of aluminium (at. wt. $= 27$) from a solution of aluminium chloride will be ............ $N$ (where $N$ is Avogadro's number).