Chemistry - Electrochemistry Question with Solution | TestHub

ChemistryElectrochemistryFaraday's Law of Electrolysis/Electrolytic CellsMedium2 minQB

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Through molten $AlCl_{3}$ , a charge equal to the charge of 1 mole $N^{3 -}$ ion was passed. Volume of $Cl_{2}$ evolved at anode when measured at NTP will be

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Answer:

Solution:

Hence, Charge passed = $1.6 \times 1 0^{- 19} \times 3 \times 6.02 \times 1 0^{23}$

$= 1.6 \times 3 \times 6.02 \times 1 0^{4}$ coulomb.

Number of gram equivalents of Cl₂ formed = $\frac{1.6 \times 3 \times 6.02 \times 1 0 ^{4}}{96500} = 3$

The number of moles of Cl₂ formed = $\frac{3}{2}$ .

Volume of Cl₂ at NTP = $22.4 \times \frac{3}{2} = 33.6$ L.

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

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