$2.5 \, F$ of electricity are passed through a $CuSO_4$ solution. The number of gram equivalents of $Cu$ deposited on the cathode is $....$

$108 \ g$ of silver (molar mass $108 \ g \ mol^{-1}$) is deposited at the cathode from $AgNO_3(aq)$ solution by a certain quantity of electricity. The volume (in $L$) of oxygen gas produced at $273 \ K$ and $1 \ bar$ pressure from water by the same quantity of electricity is ............. $L$.

If current $(I)$ of an electrolytic cell is doubled and time $(t)$ for electrolysis is halved,then the $\frac{\text{mass}}{\text{eq. wt.}}$ ratio becomes :-

The anodic half-cell of a lead-acid battery is recharged using electricity of $0.05 \ F$. The amount of $PbSO_4$ electrolyzed in $g$ during the process is (Molar mass of $PbSO_4 = 303 \ g \ mol^{-1}$)

When the same quantity of electricity is passed through electrolytic cells containing different electrolytes connected in series,the amount of products obtained at the various electrodes is proportional to their:

When a certain amount of electricity is passed through a solution of $Al^{3+}$,$4.5 \ g$ of aluminum (atomic mass $27 \ amu$) is deposited at the cathode. If the same amount of electricity is passed through $H^{+}$ ions,what volume of hydrogen (in $L$) is produced at $STP$?