Solutions of $Hg_{2}(ClO_{4})_{2}$,$Hg(ClO_{4})_{2}$,$CuSO_{4}$,and $AgNO_{3}$ are connected in series. If a current of $2.58 \ A$ is passed for $1 \ hour$,calculate the moles of metal liberated from each solution at the cathode.

The approximate time duration in hours to electroplate $30 \ g$ of calcium from molten calcium chloride using a current of $5 \ A$ is [At. mass of $Ca=40$]

What is the amount of chlorine evolved when $2 \ A$ of current is passed for $30 \ min$ in an aqueous solution of $NaCl$ (in $g$)?

How many faraday are needed to reduce a mole of $MnO_4^-$ to $Mn^{2+}$?

$A$ certain quantity of electricity is passed through an aqueous solution of $AgNO_3$ and a cupric salt solution connected in series. The amount of $Ag$ deposited is $1.08 \ g$. The amount of copper deposited is ............. $g$ (atomic weight of $Cu = 63.5$; $Ag = 108$).

Electricity is passed through an acidic solution of $Cu^{2+}$ until all the $Cu^{2+}$ is exhausted, leading to the deposition of $300 \ mg$ of $Cu$ metal. Subsequently, a current of $600 \ mA$ is passed through the same solution for another $28 \ minutes$ while keeping the total volume of the solution fixed at $200 \ mL$. The total volume of oxygen evolved at $STP$ during the entire process is . . . . . . $mL$. (Nearest integer) [Given: $Cu^{2+}_{(aq)} + 2e^{-} \rightarrow Cu_{(s)}$, $E_{red}^0 = +0.34 \ V$; $O_{2(g)} + 4H^{+} + 4e^{-} \rightarrow 2H_2O$, $E_{red}^0 = +1.23 \ V$; Molar mass of $Cu = 63.54 \ g \ mol^{-1}$; Faraday Constant $= 96500 \ C \ mol^{-1}$; Molar volume at $STP = 22.4 \ L$]