During electrolysis,the amount of ions discharged is $NOT$ proportional to which of the following?

The amount of charge required to liberate $9 \ g$ of aluminium (atomic weight = $27$ and valency = $3$) in the process of electrolysis is ......... $coulombs$ (Faraday's constant $= 96500 \ C \ mol^{-1}$)

When a current of $10800 \ C$ is passed through an electrolyte,$2.977 \ g$ of a metal is deposited. If the molar mass of the metal is $106.4 \ g \ mol^{-1}$,what is the charge on the metal cation?

What is the amount of chlorine evolved when $2 \ A$ of current is passed for $30 \ min$ in an aqueous solution of $NaCl$ (in $g$)?

The value of one Faraday is .............. $C \ mol^{-1}$.

$A$ 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 $.7$)