How many coulombs are required for the oxidation of $2 \, mol$ of $H_2O_2$ to $O_2$?

Assertion $(A)$: The charge on one mole of electrons is one Faraday.
Reason $(R)$: The quantity of current required to deposit one mole of $Mg$ from $Mg^{2+}$ electrolyte solution is two Faradays.
The correct answer is

In the electrolysis of $AgNO_3$,the mass of $Ag$ deposited is plotted against the charge. Slope of the line gives

If a steady current of $4 \, A$ is maintained for $40 \, min$,depositing $4.5 \, g$ of zinc at the cathode,then the electrochemical equivalent $(Z)$ will be:

What is the total charge of one mole of electrons?

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