$4.5 \ g$ 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 .............. $L$.

Two different electrolytic cells filled with molten $Cu(NO_3)_2$ and molten $Al(NO_3)_3$ respectively are connected in series. When electricity is passed,$2.7 \ g$ of $Al$ is deposited on the electrode. Calculate the weight of $Cu$ deposited on the cathode. [Atomic mass: $Cu = 63.5$,$Al = 27.0 \ g \ mol^{-1}$] (in $g$)

Calculate the quantity of electricity required to liberate $0.224 \ dm^3$ of chlorine at $STP$ during the electrolysis of fused sodium chloride (in $C$)?

When a current of $10800 \ C$ is passed through an electrolyte,$2.977 \ g$ of a metal is deposited. If the molar mass of the metal is $106.4 \ g \ mol^{-1}$,what is the charge on the metal cation?

The electrochemical equivalent of a metal is $x \ g \ C^{-1}$. The equivalent weight of the metal is:

How much time is required for complete decomposition of $4 \, \text{moles}$ of water using $4 \, \text{A}$ current?