The quantity of electricity required to liberate $112 \, cm^3$ of hydrogen at $STP$ from acidified water is

On passing electric current through molten aluminium chloride,$11.2 \ L$ of $Cl_2$ is liberated at $NTP$ at the anode. The quantity of aluminium deposited at the cathode is .............. $g$ (atomic weight of $Al = 27$).

Potassium chlorate is prepared by electrolysis of $KCl$ in basic solution as shown by the following equation:
$6 OH^{-} + Cl^{-} \rightarrow ClO_{3}^{-} + 3 H_{2}O + 6 e^{-}$
$A$ current of $x \ A$ has to be passed for $10 \ h$ to produce $10.0 \ g$ of potassium chlorate. The value of $x$ is $.......$ (Nearest integer).
(Molar mass of $KClO_{3} = 122.6 \ g \ mol^{-1}, F = 96500 \ C \ mol^{-1}$)

How many seconds of current at $241.25 \ A$ must be passed to deposit all the silver present in $125 \ mL$ of $1 \ M \ AgNO_3$ solution? $(1 \ F = 96500 \ C)$

If $1$ mole of electrons is passed through the solutions of $AlCl_3$,$AgNO_3$,and $MgSO_4$,in what ratio will $Al$,$Ag$,and $Mg$ be deposited at the electrodes?

How many coulombs of electricity is required to produce $1 \ g$ of $Na$ metal from its ions (in $C$)? (Atomic mass of $Na = 23 \ g/mol$)