The density of $Cu$ is $8.94 \, g \, cm^{-3}$. The quantity of electricity needed to plate an area $10 \, cm \times 10 \, cm$ to a thickness of $10^{-2} \, cm$ using $CuSO_4$ solution would be,if atomic mass of $Cu$ is $63.5$ .................. $C$

How much volume of oxygen at $STP$ will be liberated by $2$ $ampere$ flowing for $3$ $minutes$ and $13$ $seconds$ through acidified water? (in $cc$)

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

$1$ mole of electrons corresponds to how much Faraday,how much Coulomb,and how many electrons?

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

In the electrolysis of $CuCl_2$,a current of $2.0 \ A$ is passed through the solution at $1 \ bar$ pressure and $300 \ K$ temperature for $1 \ hour$. Calculate the amount of product obtained at the anode and cathode. $[Cu = 63.5, \ Cl = 35.5, \ R = 0.08314 \ L \ bar \ K^{-1} \ mol^{-1}]$