The quantity of electricity needed to separately electrolyze $1 \ M$ solution of $ZnSO_{4}$, $AlCl_{3}$ and $AgNO_{3}$ completely is in the ratio of

The mass deposited at an electrode during electrolysis is directly proportional to which of the following?

Match List $I$ with List $II$.

List $I$ (Conversion)	List $II$ (Number of Faraday required)
$A$. $1 \text{ mol of } H_2O \text{ to } O_2$	$I$. $3F$
$B$. $1 \text{ mol of } MnO_4^- \text{ to } Mn^{2+}$	$II$. $2F$
$C$. $1.5 \text{ mol of } Ca \text{ from molten } CaCl_2$	$III$. $1F$
$D$. $1 \text{ mol of } FeO \text{ to } Fe_2O_3$	$IV$. $5F$

Choose the correct answer from the options given below:

Copper sulphate solution is electrolysed between two platinum electrodes. $A$ current is passed until $1.6 \ g$ of oxygen is liberated at the anode. The amount of copper deposited at the cathode during the same period is .............. $g$ [At. mass of $Cu = 63.6$]

When an electric current is passed through a solution of $KCl$,$19.5 \ g$ of potassium (atomic mass $= 39$) is deposited. If the same amount of electric current is passed through a solution of $AlCl_3$,how many grams of aluminum will be liberated?

Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by $1 \ A$ current for $10 \ minutes$ in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same or different? Explain your answer.