Chemistry - Electrochemistry Question with Solution | TestHub

ChemistryElectrochemistryFaraday's Law of Electrolysis/Electrolytic CellsMedium2 minQB

ChemistryMediummultiple choice

4.5g of Al (atomic mass $= 27 amu$ ) is deposited at cathode from $Al^{+ 3}$ solution by a certain quantity of charge. The correct statement/s is are:

Options:(select one or more)

Answer:

A, C

Solution:

Al³⁺ + 3e⁻ → Al

Number of moles of Al produced = $\frac{4.5}{27} = 0.166$

Number of moles of electrons used = $3 \times 0.166$

H⁺ + e⁻ → 1/2 H₂

Number of moles of H₂ produced = $\frac{1}{2} \times 3 \times 0.166$

Volume of H₂ produced = $1.5 \times 0.166 \times 22.4 l = 5.57 = 5.6 l$

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

⏱ 2mℹ️ Source: QB

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