How many seconds of current at $9.65 \ A$ must be passed through a solution of $Al^{3+}$ to obtain $1 \ \text{millimole}$ of $Al$ metal?

When $1 \ F$ (Faraday) of electricity is passed through an aqueous solution of $CuSO_4$,the amount of $Cu$ deposited is:

Passage of a current for $548 \, s$ through a silver coulometer results in the deposition of $0.746 \, g$ of silver. What is the current (in $A$)?

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

$6.5 \, g$ of $Mg$ is deposited during the electrolysis of fused $MgCl_2$. What will be the volume of chlorine gas (in $L$) discharged at the electrode at $STP$?

Mass in grams of copper deposited by passing $9.6487 \ A$ current through a voltmeter containing copper sulphate solution for $100 \ s$ is (Given : Molar mass of $Cu: 63 \ g \ mol^{-1}, 1 \ F=96487 \ C$ ) (in $g$)