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Faraday's First Law

How much elec...

Question

How much electricity is required in coulomb for the oxidation of ?

(i) 1 mole of $H_{2} O t o O_{2}$ ?

(ii) 1 mole of $F e O t o F e_{2} O_{3}$ ?

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Solution

(i) $H_{2} O 1 m o l \to 2 H^{+} + \frac{1}{2} O_{2} + 2 e^{-} 2 F$

Electricity required to oxidise $1 m o l H_{2} O t o O_{2} = 2 F$

$= 2 \times (96500 C) = 1, 93, 000 C$

$= 1.93 \times 10^{5} C$

(ii) $2 F e O + \frac{1}{2} O_{2} \to F e_{2} O_{3}$

$2 F e^{2 +} 2 m o l \to 2 F e^{3 +} + 2 e^{-} 2 F$

Electricity required to oxidise 2 moles $F e O t o F e_{2} O_{3} = 2 F$

Electricity required to oxidise 2 moles FeO to

$F e_{2} O_{3} = 1 F = 96, 500 C$

$= 9.65 \times 10^{4} C$

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Faraday's First Law

Standard XII Chemistry

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