MHT CET · Chemistry · Electrochemistry
What mass of \(\mathrm{Mg}\) is produced during electrolysis of molten \(\mathrm{MgCl}_2\) by passing \(2 \mathrm{amp}\) current for 482.5 second?
\(\left(\right.\) Molar mass \(\mathrm{Mg}=24 \mathrm{~g} \mathrm{~mol}^{-1}\) )
- A \(0.12 \mathrm{~g}\)
- B \(0.24 \mathrm{~g}\)
- C \(1.2 \mathrm{~g}\)
- D \(0.4 \mathrm{~g}\)
Answer & Solution
Correct Answer
(A) \(0.12 \mathrm{~g}\)
Step-by-step Solution
Detailed explanation
\(\mathrm{Mg}_{(\mathrm{s})}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Mg}_{(\mathrm{s})} \)
\( \text { Mole ratio }=\frac{1 \mathrm{~mol}}{2 \mathrm{~mole}^{-}} \)
\( \mathrm{W}=\frac{\mathrm{I}(\mathrm{A}) \times \mathrm{t}(\mathrm{s})}{96500\left(\mathrm{C} / \mathrm{mol} \mathrm{e}^{-}\right)} \times \text { mole ratio } \times\) \(\text{molar mass} \)
\( \mathrm{W}=\frac{2 \times 482.5}{96500\left(\mathrm{C} / \mathrm{mol} \mathrm{e}^{-}\right)} \times \frac{1 \mathrm{~mol}}{2 \mathrm{~mol} \mathrm{e}^{-}} \times 24 \mathrm{~g} \mathrm{~mol}^{-1} \)
\( \mathrm{~W}=0.12 \mathrm{~g}\)
\( \text { Mole ratio }=\frac{1 \mathrm{~mol}}{2 \mathrm{~mole}^{-}} \)
\( \mathrm{W}=\frac{\mathrm{I}(\mathrm{A}) \times \mathrm{t}(\mathrm{s})}{96500\left(\mathrm{C} / \mathrm{mol} \mathrm{e}^{-}\right)} \times \text { mole ratio } \times\) \(\text{molar mass} \)
\( \mathrm{W}=\frac{2 \times 482.5}{96500\left(\mathrm{C} / \mathrm{mol} \mathrm{e}^{-}\right)} \times \frac{1 \mathrm{~mol}}{2 \mathrm{~mol} \mathrm{e}^{-}} \times 24 \mathrm{~g} \mathrm{~mol}^{-1} \)
\( \mathrm{~W}=0.12 \mathrm{~g}\)
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