One gram of metal ion $M^{3+}$ is discharged by the passage of $1.81 \times 10^{23}$ electrons. What is the atomic weight of the metal?

In the Hall process,aluminium is produced by the electrolysis of molten $Al_2O_3$. How many seconds would it take to produce enough aluminium by the Hall process to make a case of $24$ cans of aluminium soft-drink,if each can uses $5.0 \ g$ of $Al$,a current of $9650 \ A$ is employed,and the current efficiency of the cell is $90.0 \ \%$?

Match the following and select the correct option for the quantity of electricity,in $C \ mol^{-1}$,required to deposit various metals at the cathode:

List-$I$	List-$II$
$a. \ Ag^{+}$	$i. \ 386000 \ C \ mol^{-1}$
$b. \ Mg^{2+}$	$ii. \ 289500 \ C \ mol^{-1}$
$c. \ Al^{3+}$	$iii. \ 96500 \ C \ mol^{-1}$
$d. \ Ti^{4+}$	$iv. \ 193000 \ C \ mol^{-1}$

The amount of charge required to liberate $11.5 \ g$ of sodium is .....

How much charge is required for the following reductions:
$(i)$ $1 \, mol$ of $Al^{3+}$ to $Al$.
$(ii)$ $1 \, mol$ of $Cu^{2+}$ to $Cu$.
$(iii)$ $1 \, mol$ of $MnO_{4}^{-}$ to $Mn^{2+}$.

One Faraday of electricity when passed through a solution of copper sulphate deposits: