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ChemistryElectrochemistryGalvanic cells/Nernst Equation/Concentration CellsMedium2 minPYQ_2021

ChemistryMediumsingle choice

Which is the weight of A1 deposited at cathode when 1 ampere current is passed through molten $AlCl_{3}$ for 9650 seconds? (At mass of $Al = 27$ )

Options:

Answer:

Solution:

$Number of equivalents of Al deposited = \frac{I . t}{F} = \frac{1 \times 9650}{96500} = 0.1 Number. Of equivalents = moles \times n_{factor} AlCl_{3} ⟶ Al_{factor} = 3 + 3 0.1 = moles \times 3 moles of Al = 0.1/3 mass of Al = \frac{0.1}{3} \times 27 = 0.9 g$

Stream:MHT_CETSubject:ChemistryTopic:ElectrochemistrySubtopic:Galvanic cells/Nernst Equation/Concentration Cells

⏱ 2mℹ️ Source: PYQ_2021

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