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(B) The reduction reaction for magnesium is: $Mg^{2+} + 2e^- 	o Mg(s)$.One gram atom of $Mg$ corresponds to $1 \, 	ext{mole}$ of $Mg$ atoms.From the

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$2$

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(B) The reduction reaction for magnesium is: $Mg^{2+} + 2e^- 	o Mg(s)$.One gram atom of $Mg$ corresponds to $1 \, 	ext{mole}$ of $Mg$ atoms.From the balanced equation,$1 \, 	ext{mole}$ of $Mg^{2+}$ ions requires $2 \, 	ext{moles}$ of electrons to be reduced to $1 \, 	ext{mole}$ of $Mg$.Since $1 \, 	ext{mole}$ of electrons carries a charge of $1 \, 	ext{Faraday}$,$2 \, 	ext{moles}$ of electrons carry $2 \, 	ext{Faradays}$ of charge.Therefore,$2 \, 	ext{Faradays}$ are required.

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

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