The Faraday constant is $......$

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

$A$ current of $15.0 \ A$ is passed through a solution of $CrCl_2$ for $45 \ min$. The volume of $Cl_2$ (in $L$) obtained at the anode at $1 \ atm$ and $273 \ K$ is around ($1 \ F = 96500 \ C \ mol^{-1}$,At. wt. of $Cl=35.5$,$R=0.082 \ L \ atm \ K^{-1} \ mol^{-1}$) (in $.7$)

How much time is required for the complete decomposition of $2 \ mol$ of $H_2O$ using a current of $4 \ A$?

The quantity of electricity needed to liberate $0.5 \ g$ equivalent of an element is

For the oxidation of $0.2 \text{ M} \text{ FeSO}_4$ solution,$0.965 \text{ A}$ current is passed through it for $1 \text{ hour}$. The volume of the solution that is oxidised in $\text{mL}$ is: