Question

Calculate the mass of $Mg$ and volume of chlorine gas at STP produced during electrolysis of molten $MgC{l}_2$ by the passage of $2$ amperes of current for $1$ hour. Molar masses for $Mg$ and $C{l}_2$ are respectively $24gmo{l}^{-1}$ and $71gmo{l}^{-1}$.

Answer 1

$W\left(Mg\right)=z.i.t=\left(\frac{24\times 2\times 1\times 60\times 60}{2\times 96500}\right)g$

$W\left(Mg\right)$ =0.8953g

$W\left({Cl}_2\right)=z.i.t=\left(\frac{71\times 2\times 1\times 60\times 60}{2\times 96500}\right)g$

$W(Cl{)}_2$ = 2.64g