The mass of silver (Molar mass of $Ag: 108 \ g \ mol^{-1}$) displaced by a quantity of electricity which displaces $5600 \ mL$ of $O_2$ at $S.T.P.$ will be . . . . . . $g$.

The same quantity of electricity was passed through solutions of salts of elements $X$,$Y$,and $Z$ with atomic masses $7$,$27$,and $48$ respectively. The masses of $X$,$Y$,and $Z$ deposited were $2.1 \ g$,$2.7 \ g$,and $7.2 \ g$ respectively. The valencies of $X$,$Y$,and $Z$ respectively are:

The laws of electrolysis were proposed by

In the process of electroplating,$m \ g$ of silver is deposited when $4 \ A$ of current flows for $2 \ \text{minutes}$. The amount (in $g$) of silver deposited by $6 \ A$ of current flowing for $40 \ \text{seconds}$ will be:

In an electroplating experiment,$m \ g$ of silver is deposited when $4 \ A$ of current flows for $2 \ min$. The amount (in $g$) of silver deposited by $6 \ A$ of current flowing for $40 \ s$ will be:

$A$ 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 $.7$)