When the same quantity of electricity is passed through aqueous $H_2SO_4$ and molten $MgSO_4$,what is the ratio of the weights of hydrogen and magnesium deposited?

$A$ 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 $.7$)

The quantity of electricity required to liberate $112 \, cm^3$ of hydrogen at $STP$ from acidified water is

In the electrolysis of $AgNO_3$,the mass of $Ag$ deposited is plotted against the charge. Slope of the line gives

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

If the electrochemical equivalent of a substance is $0.0006735 \ g/C$,what is its equivalent weight?