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

An electric current is passed through a silver voltameter connected to a water voltameter. The cathode of the silver voltameter weighed $0.108 \ g$ more at the end of the electrolysis. The volume of oxygen evolved at $STP$ is ............... $cm^{3}$.

What mass of silver (Atomic mass = $108 \text{ g/mol}$) is deposited by a quantity of electricity that displaces $5600 \text{ mL}$ of $O_2$ gas at $STP$ (in $\text{ g}$)?

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:

Calculate the quantity of electricity required to produce $0.42 \ g$ of $Ag$ at the cathode during the electrolysis of an $AgNO_3$ solution. (Molar mass of $Ag = 108 \ g \ mol^{-1}$) (in $C$)

The quantity of electricity needed to separately electrolyze $1 \ M$ solution of $ZnSO_{4}$, $AlCl_{3}$ and $AgNO_{3}$ completely is in the ratio of