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

Aluminum oxide is electrolyzed at $1000^\circ C$ to produce aluminum metal. The cathode reaction is $Al^{3+} + 3e^- \rightarrow Al$. What quantity of electricity is required to produce $5.12 \ kg$ of aluminum metal? (Given: $1 \ Faraday = 96500 \ C$)

$A$ solution of copper sulphate is electrolysed for $10 \text{ minutes}$ with a current of $1.5 \text{ amperes}$. The mass of copper deposited at the cathode is:
(Given: Molar mass of $Cu = 63 \text{ g mol}^{-1}$; $1F = 96487 \text{ C mol}^{-1}$)

Consider the reaction: $Cr_{2}O_{7}^{2-} + 14H^{+} + 6e^{-} \rightarrow 2Cr^{3+} + 7H_{2}O$. What is the quantity of electricity in coulombs needed to reduce $1 \ mol$ of $Cr_{2}O_{7}^{2-}$?

When the same quantity of electricity is passed through aqueous solutions of $AgNO_3$ and $CuSO_4$,if the number of atoms of $Ag$ and $Cu$ deposited are $x$ and $y$ respectively,then determine the correct relationship.

The charge required for the reduction of $1 \ \text{mole}$ of $MnO_4^{-}$ to $MnO_2$ is (in $F$)