The electric charge for electrode deposition of one equivalent of a substance is equal 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 $.7$)

During the electrolysis of acidified water, $16 \text{ g}$ of $O_2$ gas is formed at the anode. The volume of $H_2$ gas liberated at the cathode under $STP$ conditions is: (in $text{ L}$)

On passing electric current through molten aluminium chloride,$11.2 \ L$ of $Cl_2$ is liberated at $NTP$ at the anode. The quantity of aluminium deposited at the cathode is .............. $g$ (atomic weight of $Al = 27$).

When an electric current is passed through a silver nitrate solution using silver electrodes,$10.79 \ g$ of silver is deposited. If the same amount of electric current is passed through a copper sulfate solution using copper electrodes,how many grams of copper will be deposited at the cathode (in $g$)?

How many grams of cobalt metal will be deposited when a solution of cobalt $(II)$ chloride is electrolyzed with a current of $10 \ A$ for $109$ minutes? ($1 \ Faraday = 96,500 \ C$; Atomic mass of $Co = 59 \ u$)