The number of electrons required to deposit $1 \ g$ atom of aluminium (at. wt. $= 27$) from a solution of aluminium chloride will be ............ $N$ (where $N$ is Avogadro's number).

During electrolysis of fused aluminium chloride,$0.9 \ g$ of aluminium was deposited on the cathode. The volume of chlorine liberated at the anode will be .............. $litres$ (at $STP$).

In the electrolysis of water,one Faraday of electrical energy would evolve

When the same quantity of electricity is passed through the aqueous solutions of the given electrolytes for the same amount of time,which metal will be deposited in maximum amount on the cathode?

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

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