Calculate the volume of $O_2$ gas liberated at the anode when a current of $2.5 \ A$ is passed for $1 \ hour$ through an aqueous solution of $Na_2SO_4$ using inert electrodes at $1 \ bar$ pressure and $300 \ K$ temperature. (Assume $1 \ mole$ of gas occupies $24.6 \ L$ at $1 \ bar$ and $300 \ K$) (in $mL$)

Which equation represents Faraday's first law of electrolysis? ($m \rightarrow$ mass,$c \rightarrow$ current,$t \rightarrow$ time,$z \rightarrow$ electrochemical equivalent)

The amount of copper metal deposited at cathode on passing electric current of $500 \ mA$ for $20 \ min$ in cupric chloride solution is ............ $g$

$Assertion (A)$: $A$ 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 :

The quantity of charge required to obtain $2$ moles of aluminium from $Al_2O_3$ is: (in $F$)

$96500 \ C$ of electric charge liberates how many grams of $Cu$ from $CuSO_4$ solution?