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:

$A$ metal surface of $100 \, cm^2$ area has to be coated with a nickel layer of thickness $0.001 \, mm$. $A$ current of $2 \, A$ was passed through a solution of $Ni(NO_3)_2$ for '$x$' seconds to coat the desired layer. The value of $x$ is $.........$. (Nearest integer)
($\rho_{Ni}$ (density of Nickel) is $10 \, g \cdot cm^{-3}$,Molar mass of Nickel is $60 \, g \cdot mol^{-1}$,$F = 96500 \, C \cdot mol^{-1}$)

$108 \ g$ of silver (molar mass $108 \ g \ mol^{-1}$) is deposited at the cathode from $AgNO_3(aq)$ solution by a certain quantity of electricity. The volume (in $L$) of oxygen gas produced at $273 \ K$ and $1 \ bar$ pressure from water by the same quantity of electricity is ............. $L$.

The amount of ion discharged during electrolysis is not directly proportional to

During electrolysis of an aqueous solution of $Na_{2}SO_{4}$,$2.4 \, L$ of $O_{2}$ at $STP$ was liberated at the anode. The volume of $H_{2}$ at $STP$ liberated at the cathode is ............. $L$.

$A$ constant current was passed through a solution of $AuCl_4^-$ ion between gold electrodes. After a period of $10.0 \ \text{minutes}$,the increase in mass of cathode was $1.314 \ \text{g}$. The total charge passed through the solution is . . . . . . $\times 10^{-2} \ \text{F}$. (Given atomic mass of $Au = 197$)