The mass of a substance liberated when a charge $q$ flows through an electrolyte is proportional to

$A$ $4 \ A$ current is passed through a solution of zinc sulphate for $50 \ min$. Find the amount of zinc deposited at the cathode in $g$.

During the electrolysis of acidified water, $16 \text{ g}$ of $O_2$ gas is formed at the anode. The volume of $H_2$ gas liberated at the cathode under $STP$ conditions is: (in $text{ L}$)

How much electricity in terms of Faraday is required to produce $40.0 \text{ g}$ of $\text{Al}$ from molten $\text{Al}_2\text{O}_3$ (in $\text{ F}$)?

When electricity is passed through a solution of $AlCl_3$,$13.5 \ g$ of $Al$ is deposited. What is the number of Faradays used?

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