How many $L$ of chlorine gas will be deposited at $NTP$ when a current of $100 \, A$ is passed through molten $NaCl$ for $5 \, hours$?

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.

$A$ current of $19296 \ C$ is passed through an aqueous solution of copper sulphate using copper electrodes. What is the mass (in $g$) of copper deposited at the cathode? (Molar mass of $Cu = 63.5 \ g \ mol^{-1}$)

Salts of $A, B$ and $C$ were electrolysed under identical conditions using the same quantity of electricity. It was found that when $2.1 \ g$ of $A$ was deposited,the weights of $B$ and $C$ deposited were $2.7 \ g$ and $9.6 \ g$. If the atomic mass of $A, B$ and $C$ are $7, 27$ and $64$ respectively,then the valencies of $A, B$ and $C$ respectively are:

How much electricity in terms of Faraday is required to reduce $2 \ mol$ of $MnO_4^{-}$ into $Mn^{2+}$?

The number of moles of electrons passed when a current of $2 \ A$ is passed through a solution of electrolyte for $20 \ minutes$ is