The mass of ions deposited during a given interval of time in the process of electrolysis depends on

When a current of $0.6 \ A$ is passed through an aqueous solution of $CuSO_4$ for $7 \ minutes$,what is the total quantity of electricity passed in Faradays?

When $1 \ F$ (Faraday) of electricity is passed through an aqueous solution of $CuSO_4$,the amount of $Cu$ deposited is:

During the electrolysis of concentrated $H_2SO_4$,perdisulphuric acid $(H_2S_2O_8)$ and $O_2$ are formed in equimolar amounts. The amount of $H_2$ that will be formed simultaneously is $(2H_2SO_4 \rightarrow H_2S_2O_8 + 2H^+ + 2e^-)$

The anodic half-cell of a lead-acid battery is recharged using electricity of $0.05 \ F$. The amount of $PbSO_4$ electrolyzed in $g$ during the process is (Molar mass of $PbSO_4 = 303 \ g \ mol^{-1}$)

How many $Faradays$ are required to generate one gram atom of magnesium from $MgCl_2$?