$4.5 \ g$ of aluminium (atomic mass $27 \ amu$) is deposited at the cathode from an $Al^{3+}$ solution by a certain quantity of electric charge. The volume of hydrogen produced at $STP$ from $H^{+}$ ions in the solution by the same quantity of electric charge will be .............. $L$.

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?

Faraday's laws of electrolysis will fail when

Aqueous $CuSO_4$ solution was electrolysed by passing $2 \ A$ of current for $10 \ min$. What is the weight (in $g$) of copper deposited at the cathode? (Given: $Cu = 63 \ u$; $F = 96500 \ C \ mol^{-1}$)

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

When the same quantity of electricity is passed through electrolytic cells containing different electrolytes connected in series,the amount of products obtained at the various electrodes is proportional to their: