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

What mass of $Mg$ is produced during electrolysis of molten $MgCl_2$ by passing $2 \ A$ current for $482.5 \ s$ (in $g$)? $(Molar \ mass \ Mg = 24 \ g \ mol^{-1})$

What is the time (in $sec$) required for depositing all the silver present in $125 \ mL$ of $1 \ M \ AgNO_3$ solution by passing a current of $241.25 \ A$? $(1 \ F = 96500 \ C)$

How much electricity is required in Faraday to produce $40.0 \ g$ of $Al$ from molten $Al_2O_3$? (Atomic mass of $Al = 27 \ g \ mol^{-1}$)

When $1 \ C$ of charge is passed through an electrolyte solution,the mass deposited is equal to:

When an electric current is passed through acidified water at $STP$,$112 \ mL$ of hydrogen gas is collected at the cathode in $965 \ s$. What is the current in amperes?