On passing $96500 \ C$ of charge through a $CuSO_4$ solution,the amount of copper liberated is:

Match List $I$ with List $II$.

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

Choose the correct answer from the options given below:

How much electricity is required in Faraday to produce $40.0 \ g$ of $Al$ from molten $Al_2O_3$? (Atomic mass of $Al = 27 \ g \ mol^{-1}$)

Three voltameters containing aqueous solutions of $H_2SO_4$,$CuSO_4$,and $AgNO_3$ are connected in series as shown. $A$ current was passed for $10 \ hours$. $10.8 \ g$ of $Ag$ was deposited at the cathode in the $(III)$ electrolytic cell during electrolysis. If the current efficiency is $50\%$,what is the magnitude of the current in amperes?

$2.5 \, F$ of electricity are passed through a $CuSO_4$ solution. The number of gram equivalents of $Cu$ deposited on the cathode is $....$

In the Hall-Heroult process,if a current of $10 \ A$ is passed for $8 \ \text{days}$ and $1 \ \text{hour}$,how many kilograms of carbon anode will be consumed?