When the same quantity of electricity is passed through aqueous solutions of $AgNO_3$ and $CuSO_4$,if the number of atoms of $Ag$ and $Cu$ deposited are $x$ and $y$ respectively,then determine the correct relationship.

Electricity is passed through an acidic solution of $Cu^{2+}$ until all the $Cu^{2+}$ is exhausted, leading to the deposition of $300 \ mg$ of $Cu$ metal. Subsequently, a current of $600 \ mA$ is passed through the same solution for another $28 \ minutes$ while keeping the total volume of the solution fixed at $200 \ mL$. The total volume of oxygen evolved at $STP$ during the entire process is . . . . . . $mL$. (Nearest integer) [Given: $Cu^{2+}_{(aq)} + 2e^{-} \rightarrow Cu_{(s)}$, $E_{red}^0 = +0.34 \ V$; $O_{2(g)} + 4H^{+} + 4e^{-} \rightarrow 2H_2O$, $E_{red}^0 = +1.23 \ V$; Molar mass of $Cu = 63.54 \ g \ mol^{-1}$; Faraday Constant $= 96500 \ C \ mol^{-1}$; Molar volume at $STP = 22.4 \ L$]

The unit of Faraday is

$A$ dilute solution of sulphuric acid is electrolysed using a current of $0.10 \ A$ for $2 \ hours$ to produce hydrogen and oxygen gas. The total volume of gases produced at $STP$ is $...... \ cm^3$. (Nearest integer) $[$ Given : Faraday constant $F = 96500 \ C \ mol^{-1}$ at $STP$,molar volume of an ideal gas is $22.7 \ L \ mol^{-1} ]$

The mass of a substance liberated when a charge $q$ flows through an electrolyte is proportional to

How much Faraday of electricity is required to reduce $1.5 \ mole$ of $KMnO_4$ into $MnO_2$ in a basic medium (in $F$)?