How much electricity is required in coulomb for the oxidation of
$(i)$ $1 \, mol$ of $H_2O$ to $O_2?$
$(ii)$ $1 \, mol$ of $FeO$ to $Fe_2O_3?$
$(i)$ $1 \, mol$ of $H_2O$ to $O_2?$
$(ii)$ $1 \, mol$ of $FeO$ to $Fe_2O_3?$
(N/A) $(i)$ The oxidation reaction is: $H_2O \longrightarrow 2H^+ + \frac{1}{2} O_2 + 2e^-$.
Thus,$2 \, mol$ of electrons are required for the oxidation of $1 \, mol$ of $H_2O$.
Electricity required $= 2 \, F = 2 \times 96487 \, C = 192974 \, C$.
$(ii)$ The oxidation reaction is: $FeO + \frac{1}{2} H_2O \longrightarrow \frac{1}{2} Fe_2O_3 + H^+ + e^-$.
Thus,$1 \, mol$ of electrons is required for the oxidation of $1 \, mol$ of $FeO$.
Electricity required $= 1 \, F = 96487 \, C$.
Thus,$2 \, mol$ of electrons are required for the oxidation of $1 \, mol$ of $H_2O$.
Electricity required $= 2 \, F = 2 \times 96487 \, C = 192974 \, C$.
$(ii)$ The oxidation reaction is: $FeO + \frac{1}{2} H_2O \longrightarrow \frac{1}{2} Fe_2O_3 + H^+ + e^-$.
Thus,$1 \, mol$ of electrons is required for the oxidation of $1 \, mol$ of $FeO$.
Electricity required $= 1 \, F = 96487 \, C$.
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