How much current should be passed through acidified water for $100 \ s$ to liberate $0.224 \ L$ of $H_2$ gas at $STP$ (in $A$)?

What is the time (in $sec$) required for depositing all the silver present in $125 \ mL$ of $1 \ M \ AgNO_3$ solution by passing a current of $241.25 \ A$? $(1 \ F = 96500 \ C)$

The quantity of electricity needed to separately electrolyze $1 \ M$ solution of $ZnSO_{4}$, $AlCl_{3}$ and $AgNO_{3}$ completely is in the ratio of

$A$ current is passed for $2 \, \text{hours}$ through an acidic solution,liberating $11.2 \, L$ of oxygen at $NTP$ at the anode. What will be the amount of copper deposited at the cathode by the same current when passed through a solution of copper sulphate for the same duration? .......... $g$

$4.5 \ g$ of aluminium (atomic mass $27 \ amu$) is deposited at the cathode from an $Al^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at $STP$ from $H^{+}$ ions in the solution by the same quantity of electric charge will be .............. $L$.

How many atoms of calcium will be deposited from a solution of $CaCl_2$ by a current of $0.25 \, mA$ flowing for $60 \, s$?