Question:
How many faradays of electricity are required to produce $12\,\mathrm{g}$ of magnesium from molten $\mathrm{MgCl_2}$?}
\[
(\text{Atomic weight of Mg}=24\,\mathrm{g\,mol^{-1}})
\]
How many faradays of electricity are required to produce $12\,\mathrm{g}$ of magnesium from molten $\mathrm{MgCl_2}$?}
\[
(\text{Atomic weight of Mg}=24\,\mathrm{g\,mol^{-1}})
\]
Show Hint
Number of Faradays required
\[
=\text{Moles of metal}\times\text{Valency}.
\]
Updated On: Jun 17, 2026
- 1
- 2
- 0.5
- 4
Show Solution
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The Correct Option is A
Solution and Explanation
Concept:
One faraday corresponds to one mole of electrons. During electrolysis,
\[
\mathrm{Mg}^{2+}+2e^-\rightarrow \mathrm{Mg}.
\]
Thus one mole of magnesium requires two faradays.
Step 1: Calculate moles of magnesium. \[ \text{Moles of Mg} = \frac{12}{24} = 0.5. \]
Step 2: Determine electron requirement. One mole Mg requires \[ 2F. \] Therefore \[ 0.5\ \text{mol Mg} \] requires \[ 0.5\times2=1F. \]
Step 3: Final answer. \[ \boxed{1\ \text{Faraday}} \]
Step 1: Calculate moles of magnesium. \[ \text{Moles of Mg} = \frac{12}{24} = 0.5. \]
Step 2: Determine electron requirement. One mole Mg requires \[ 2F. \] Therefore \[ 0.5\ \text{mol Mg} \] requires \[ 0.5\times2=1F. \]
Step 3: Final answer. \[ \boxed{1\ \text{Faraday}} \]
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