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

Faraday's laws of electrolysis state that the mass deposited on an electrode is proportional to:

$A$ current of $16\, A$ flows through molten $NaCl$ for $10\, min$. The amount of metallic sodium that appears at the negative electrode would be ............ $g$.

According to the first law of Faraday,the weight of a substance discharged at the electrode is:

On passing $C$ ampere of current for time $t$ seconds through $1 \ L$ of $2 \ M$ $CuSO_4$ solution (atomic weight of $Cu = 63.5$), the amount $m$ of $Cu$ (in grams) deposited on the cathode will be:

During electrolysis of fused aluminium chloride,$0.9 \ g$ of aluminium was deposited on the cathode. The volume of chlorine liberated at the anode will be .............. $litres$ (at $STP$).