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

In a copper voltameter experiment,current is decreased to one-fourth of the initial value but it is passed for four times the earlier duration. The amount of copper deposited will be:

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 $\text{ F}$)?

What current strength is required to deposit $36 \ g$ of $Ag$ in $7 \ minute$ from $AgNO_3$ solution by electrolysis (in $A$)? (Atomic mass $Ag = 108$)

When $1 \ C$ of electricity is passed through an electrolytic solution,the mass deposited on the electrode is equal to which of the following?

What will be the weight of $Al$ deposited at the cathode when $0.5 \ F$ of electricity is passed through an aqueous solution of $AlCl_3$ (in $g$)? (Atomic mass of $Al = 27$)