Assertion (A): The charge on one mole of elec | vedclass

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(A) The reaction for the deposition of $Mg$ from $Mg^{2+}$ is:$Mg^{2+} + 2e^{-} \longrightarrow Mg$This shows that $2 \ 	ext{moles}$ of electrons are

Vedclass · Accepted Answer

Both $(A)$ and $(R)$ are correct and $(R)$ is the correct explanation of $(A)$.

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(A) The reaction for the deposition of $Mg$ from $Mg^{2+}$ is:$Mg^{2+} + 2e^{-} \longrightarrow Mg$This shows that $2 \ 	ext{moles}$ of electrons are required to deposit $1 \ 	ext{mole}$ of $Mg$.Since $1 \ 	ext{mole}$ of electrons carries a charge of $1 \ F$,$2 \ 	ext{moles}$ of electrons carry a charge of $2 \ F$.Thus,the quantity of electricity required to deposit $1 \ 	ext{mole}$ of $Mg$ is $2 \ F$,making the Reason $(R)$ correct.Furthermore,the definition of Faraday's constant is the charge on $1 \ 	ext{mole}$ of electrons,which is approximately $96500 \ C$. Therefore,Assertion $(A)$ is also correct.Since the definition of the charge on one mole of electrons (Assertion) is the fundamental principle used to calculate the electricity required for the deposition (Reason),$(R)$ is the correct explanation of $(A)$.

Assertion $(A)$: The charge on one mole of electrons is one Faraday.
Reason $(R)$: The quantity of current required to deposit one mole of $Mg$ from $Mg^{2+}$ electrolyte solution is two Faradays.
The correct answer is

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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 $Mg$ from $Mg^{2+}$ electrolyte solution is two Faradays.The correct answer is