(A) At the anode,iron is oxidised: $2Fe(s) \to 2Fe^{2+}(aq) + 4e^-$.At the cathode,dissolved oxygen is reduced in the presence of water: $O_2(g) + 2H_

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$Fe$ is oxidised to $Fe^{2+}$ and dissolved oxygen in water is reduced to $OH^{-}$

(A) At the anode,iron is oxidised: $2Fe(s) \to 2Fe^{2+}(aq) + 4e^-$.At the cathode,dissolved oxygen is reduced in the presence of water: $O_2(g) + 2H_2O(l) + 4e^- \to 4OH^-(aq)$.The overall reaction is $2Fe(s) + O_2(g) + 2H_2O(l) \to 2Fe(OH)_2(s)$.$Fe(OH)_2$ is further oxidised by atmospheric oxygen to $Fe_2O_3 \cdot xH_2O$ (rust).

Class 12 Chemistry Electrochemistry Corrosion

Medium

Corrosion of iron is essentially an electrochemical phenomenon where the cell reactions are

A
$Fe$ is oxidised to $Fe^{2+}$ and dissolved oxygen in water is reduced to $OH^{-}$
B
$Fe$ is oxidised to $Fe^{3+}$ and $H_2O$ is reduced to $O_2^{2-}$
C
$Fe$ is oxidised to $Fe^{2+}$ and $H_2O$ is reduced to $O_2^-$
D
$Fe$ is oxidised to $Fe^{2+}$ and $H_2O$ is reduced to $O_2$