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Question: What is the quantity of electricity required to produce 4.8 g of Mg (molar mass = 24 g mol$^{-1}$) f...

What is the quantity of electricity required to produce 4.8 g of Mg (molar mass = 24 g mol−1^{-1}) from its salt solution?

A

10 F

B

4 F

C

1 F

D

0.4 F

Answer

0.4 F

Explanation

Solution

  1. Calculate moles of Mg:

    Moles of Mg=4.8 g24 g/mol=0.2 mol\text{Moles of Mg} = \frac{4.8\, \text{g}}{24\, \text{g/mol}} = 0.2\, \text{mol}

  2. Determine electrons required:

    The electrolytic reduction is:

    Mg2++2e−→Mg\text{Mg}^{2+} + 2e^- \rightarrow \text{Mg}

    So, 1 mole of Mg requires 2 moles of electrons. Therefore:

    Moles of electrons=0.2×2=0.4 mol\text{Moles of electrons} = 0.2 \times 2 = 0.4\, \text{mol}

  3. Convert moles of electrons to Faradays:

    Since 1 Faraday = 1 mole of electrons,

    Faradays required=0.4 F\text{Faradays required} = 0.4\, F