If nearly $10^5 \ C$ liberate $1 \ gm$ equivalent of aluminium,then the amount of aluminium (equivalent weight $9$) deposited through electrolysis in $20 \ minutes$ by a current of $50 \ A$ will be .............. $gm$.

$38.6 \ A$ of current is passed for $100 \ s$ through an aqueous $CuSO_4$ solution using platinum electrodes. The mass of copper deposited from the solution and the volume of gas liberated at $STP$ are respectively (molar mass of $Cu = 63.54 \ g \ mol^{-1}$)

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 $KClO_{3} = 122.6 \ g \ mol^{-1}, F = 96500 \ C \ mol^{-1}$)

In the electrolysis of an aqueous $NiI_2$ solution using $Ni$ electrodes,what happens to the mass of the cathode upon passing $1$ equivalent of charge? (Given: atomic mass of $Ni = 59$)

$A$ silver cup is plated with silver by passing $965 \ C$ of electricity. The amount of silver deposited is ............. $g$.

How many faraday of electricity is required to produce $10 \ g$ of calcium metal (molar mass $= 40 \ g \ mol^{-1}$) from calcium ions (in $F$)?