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Assertion (A): The charge on one mole of electrons is one Faraday.
Reason (R): The quantity of current required to deposit one mole of $\mathrm{Mg}$ from $\mathrm{Mg}^{2+}$ electrolyte solution is two Faradays.
The correct answer is
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Reason (R): The quantity of current required to deposit one mole of $\mathrm{Mg}$ from $\mathrm{Mg}^{2+}$ electrolyte solution is two Faradays.
The correct answer is
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Verified Answer
The correct answer is:
Both (A) and (R) are correct and (R) is the correct explanation of (A).
The quantity of current required to deposit one mole of $\mathrm{Mg}$ from $\mathrm{Mg}^{2+}$ electrolyte solution is two Faradays.
$$
\mathrm{Mg}^{2+}+2 e^{-} \longrightarrow \mathrm{Mg}
$$
$\therefore$ Quantity of electricity required $=2 \mathrm{~F}$
Thus, two mole of electrons produce one mole of $\mathrm{Mg}$. It can be concluded that if $n, c=1 \mathrm{~mol}$ electrons are involved in the electrod reaction, the passage of $n$ Faradays of electricity will liberate one mole of the substance, i.e. the charge on one mole of electrons is one Faraday.
$$
\mathrm{Mg}^{2+}+2 e^{-} \longrightarrow \mathrm{Mg}
$$
$\therefore$ Quantity of electricity required $=2 \mathrm{~F}$
Thus, two mole of electrons produce one mole of $\mathrm{Mg}$. It can be concluded that if $n, c=1 \mathrm{~mol}$ electrons are involved in the electrod reaction, the passage of $n$ Faradays of electricity will liberate one mole of the substance, i.e. the charge on one mole of electrons is one Faraday.
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