How much electricity is required in coulomb for the oxidation of:
(i) $1 m o l$ of $H_{2} O$ to $O_{2}$ ?
(ii) $1 m o l$ of $F e O$ to $F e_{2} O_{3}$ ?

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Solution

(i) $H_{2} O \to 2 H^{+} + \frac{1}{2} O_{2} + 2 e^{-}$
Oxidation of one mole of water will require $2 \times 96500 = 1.93 \times 10^{5} C$ .

(ii) $F e^{2 +} \to F e^{3 +}$
Oxidation of one mole of $F e^{2 +}$ will require $1 \times 96500 = 96500 C$ .

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

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

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