How many Faraday of electricity is required to produce $5 \mathrm{~g}$ of magnesium from magnesium chloride? (Molar mass Mg $=24 \mathrm{~g} \mathrm{~mol}^{-1}$ )

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Aicharya · Accepted Answer

$\begin{aligned} & \mathrm{Mg}^{+2}+2 \mathrm{e}^{-} ightarrow \mathrm{Mg} \ & 2 \mathrm{~mol} \quad 1 \mathrm{~mol} \ & \frac{5}{24}=0.208 \mathrm{~mol} \mathrm{Mg} \ & 	herefore 	ext { Mol of charge required or faraday of change required } \ & =0.208 	imes 2 \ & =0.416 \mathrm{~F} \ & \end{aligned}$

How many Faraday of electricity is required to produce $5 \mathrm{~g}$ of magnesium from magnesium chloride?…

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