To deposit one litre of hydrogen at $22.4 \text{ atmosphere}$ from acidulated water,the quantity of electricity that must pass through is ............. $coulomb$.

$A$ 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 $22.7 \ L \ mol^{-1} ]$

If current $(I)$ of an electrolytic cell is doubled and time $(t)$ for electrolysis is halved,then the $\frac{\text{mass}}{\text{eq. wt.}}$ ratio becomes :-

The quantity of electricity required to liberate $5600 \ mL$ of $H_2$ at $STP$ is the same as that required to liberate how many grams of silver (equivalent weight = $108$)?

$Assertion (A)$: $A$ current of $96.5 \ A$ is passed into aqueous $AgNO_3$ solution for $100 \ s$. The weight of silver deposited is $10.8 \ g$ (At. wt. of $Ag = 108$).
$Reason (R)$: The mass of a substance deposited during the electrolysis of an electrolyte is inversely proportional to the quantity of electricity passing through the electrolyte.
The correct answer is :

When a copper voltameter is connected with a battery of $e.m.f.$ $12 \ V$,$2 \ g$ of copper is deposited in $30 \ minutes$. If the same voltameter is connected across a $6 \ V$ battery,then the mass of copper deposited in $45 \ minutes$ would be ............. $g$.