Chemistry - Electrochemistry Question with Solution | TestHub

ChemistryElectrochemistryFaraday's Law of Electrolysis/Electrolytic CellsMedium2 minPYQ_2021

ChemistryMediumnumerical

Consider the following reaction

${MnO}_{4}^{-} + 8 H^{+} + 5 e^{-} \to {Mn}^{+ 2} + 4 H_{2} O, E ° = 1.51 V$

The quantity of electricity required in Faraday to reduce five moles of ${MnO}_{4}^{-}$ is

Answer:

25.00

Solution:

For this balanced reaction, the change in oxidation number of the metal ion is ${Mn}^{+ 7} \to {Mn}^{+ 2}$ .

Therefore one mole $Mn$ required $5$ Faraday

Hence, for five mole $Mn$ required $25$ Faraday.

Stream:JEESubject:ChemistryTopic:ElectrochemistrySubtopic:Faraday's Law of Electrolysis/Electrolytic Cells

⏱ 2mℹ️ Source: PYQ_2021

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