What is the number of Faraday's of charge, that should be required to convert one mole of $\mathrm{FeCr}_2 \mathrm{O}_4$ to $\mathrm{Fe}^{3+}$ an $\mathrm{CrO}_4^{2-}$ through an electrolytic oxidation process consider the current efficiency to be $87.5 \%$ ?

NEET UG CHEMISTRY MCQ: ELECTRO CHEMISTRY

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Analyzing +4 | -1

What is the number of Faraday's of charge, that should be required to convert one mole of

\mathrm{FeCr}_2 \mathrm{O}_4

\mathrm{Fe}^{3+}

\mathrm{CrO}_4^{2-}

through an electrolytic oxidation process consider the current efficiency to be

87.5 \%

View answer and explanation

Correct option: A

Option A is correct. The number of Faradays required to convert one mole of

\mathrm{FeCr}_2 \mathrm{O}_4

\mathrm{Fe}^{3+}

and

\mathrm{CrO}_4^{2-}

is 8, considering the current efficiency.

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