When the same quantity of electricity is passed through aqueous $H_2SO_4$ and molten $MgSO_4$,what is the ratio of the weights of hydrogen and magnesium deposited?

$Assertion (A)$: $A$ 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 :

$A$ steady current of $5 \, A$ is maintained for $45 \, min$. During this time,it deposits $4.572 \, g$ of zinc at the cathode of a voltameter. The $E.C.E.$ of zinc is:

The mass of silver (Molar mass of $Ag: 108 \ g \ mol^{-1}$) displaced by a quantity of electricity which displaces $5600 \ mL$ of $O_2$ at $S.T.P.$ will be . . . . . . $g$.

The charge required for the reduction of $1 \ \text{mole}$ of $MnO_4^{-}$ to $MnO_2$ is (in $F$)

The mass of copper deposited from a solution of $CuSO_4$ by passage of $5 \ A$ current for $965 \ s$ is ............ $g$ (Mol. wt. of Copper $= 63.5$)