$5 \ A$ current is passed through a solution of zinc sulphate for $40 \ \text{minutes}$. Find the amount of zinc deposited at the cathode in $gm$.

$Assertion (A)$: $A$ 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 :

Electrolysis of dilute aqueous $NaCl$ solution was carried out by passing $10 \ mA$ current. The time required to liberate $0.01 \ mol$ of $H_2$ gas at the cathode is $(1 \ F = 96500 \ C \ mol^{-1})$

How much charge in coulombs is required for the reduction of one mole of $Al^{3+}$ to $Al$?

In the electrolysis of an aqueous $Ni(NO_3)_2$ solution using $Ni$ electrodes,upon passing $1$ equivalent of charge,the mass of the cathode $(Ni = 59)$ changes by:

If $0.5 \, A$ current is passed through an acidified silver nitrate solution for $10 \, min$,the mass of silver deposited on the cathode is ........... $g$ (equivalent weight of silver $= 108$).