During the electrolysis of acidified water, $16 \text{ g}$ of $O_2$ gas is formed at the anode. The volume of $H_2$ gas liberated at the cathode under $STP$ conditions is: (in $text{ L}$)

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:

What is the volume of $H_2$ gas produced at $S.T.P.$ when $1 \ Faraday$ of electricity is passed through a dilute solution of acid (in $mL$)?

On passing a current of $1.2 \ A$ through a solution of salt of copper for $40 \ min$,$0.96 \ g$ of copper was deposited. The equivalent weight of copper in $g$ is

Charge required to liberate $11.5 \ g$ of sodium is:

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?