From the solution of which of the following will one Faraday of electricity liberate one gram atom of metal?

$A$ current of $0.5 \ A$ is passed through molten $AlCl_3$ for $96.5 \ s$. The mass of aluminium deposited at cathode is $x \ mg$ and volume of chlorine liberated (at $STP$) at anode is $y \ mL$. $x$ and $y$ are respectively

The number of moles of electrons passed when a current of $2 \ A$ is passed through a solution of electrolyte for $20 \ minutes$ is

The weight of silver $(at. \ wt. = 108)$ displaced by a quantity of electricity which displaces $5600 \ mL$ of $O_2$ at $STP$ will be ............ $g.$

When $X$ amperes of current is passed through molten $AlCl_3$ for $96.5$ $s$,$0.09$ $g$ of aluminium is deposited. What is the value of $X$?

An electrolytic cell contains a solution of $Ag_{2}SO_{4}$ and has platinum electrodes. $A$ current is passed until $1.6 \ g$ of $O_{2}$ is liberated at the anode. The amount of silver deposited at the cathode would be ............ $g$.