Equimolar solutions of zinc sulphate and ferric sulphate are subjected to electrolysis. What is the ratio of faradays of electricity required for deposition of one mole each of zinc and iron?

1 : 2

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2 : 3

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1 : 3

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3 : 2

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Solution

The correct option is C $2 : 3$
$Z n^{2 +} + 2 e^{-} \to Z n$
$F e^{3 +} + 3 e^{-} \to F e$

The number of faradays of electricity passed is directly proportional to number of moles of electrons.

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Equimolar solutions of zinc sulphate and ferric sulphate are subjected to electrolysis. What is the ratio of faradays of electricity required for deposition of one mole each of zinc and iron?

The correct option is C 2:3Zn2++2e−→ZnFe3++3e−→FeThe number of faradays of electricity passed is directly proportional to number of moles of electrons.

The correct option is C $2 : 3$
$Z n^{2 +} + 2 e^{-} \to Z n$
$F e^{3 +} + 3 e^{-} \to F e$

The number of faradays of electricity passed is directly proportional to number of moles of electrons.