In the electrolysis of $AgNO_3$,the mass of $Ag$ deposited is plotted against the charge. Slope of the line gives

Aluminium oxide may be electrolysed at $1000 \, ^\circ C$ to furnish aluminium metal (At. Mass $= 27 \, amu$; $1 \, F = 96,500 \, C$). The cathode reaction is $Al^{3+} + 3e^- \to Al^0$. To prepare $5.12 \, kg$ of aluminium metal by this method would require:

$A$ solution of aluminium chloride is electrolysed for $30$ minutes using a current of $2 \ A$. The amount of the aluminium deposited at the cathode is $.................$
[Given : molar mass of aluminium and chlorine are $27 \ g \ mol^{-1}$ and $35.5 \ g \ mol^{-1}$ respectively,Faraday constant $= 96500 \ C \ mol^{-1}$]. (in $g$)

Potassium chlorate is prepared by the electrolysis of $KCl$ in basic solution:
$6 OH^{-} + Cl^{-} \rightarrow ClO_{3}^{-} + 3 H_{2}O + 6 e^{-}$
If only $60\%$ of the current is utilized in the reaction,the time (rounded to the nearest hour) required to produce $10 \ g$ of $KClO_{3}$ using a current of $2 \ A$ is:
(Given: $F = 96,500 \ C \ mol^{-1}$,molar mass of $KClO_{3} = 122 \ g \ mol^{-1}$)

If a current of $0.4 \ A$ is passed through acidic water for $30 \ minutes$,calculate the volume of hydrogen gas produced at $STP$ in liters.

$A$ silver voltameter is connected in series with a water voltameter and an electric current is passed through them. At the end of electrolysis,the weight of the cathode in the silver voltameter increases by $0.108 \ g$. What is the volume of oxygen liberated at $STP$ in $mL$?