Question

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

• A. $Fe$ is oxidised to $F{e}^{2+}$ and dissolved oxygen in water is reduced to $O^{2-}$
• B. $Fe$ is oxidised to $F{e}^{3+}$ and $H_{2}O$ is reduced to $O_2^{2-}$
• C. $Fe$ is oxidised to $F{e}^{2+}$ and $H_{2}O$ is reduced to $O_2^{-}$
• D. $Fe$ is oxidised to $F{e}^{2+}$ and $H_{2}O$ is reduced to $O_2$

Answer 1

The correct option is A $Fe$ is oxidised to $F{e}^{2+}$ and dissolved oxygen in water is reduced to $O^{2-}$

$Anode:Fe\left(s\right)\to F{e}^{2+}\left(aq\right)+2e^{-}$
$Cathode:4H^{+}+O_2+4e^{-}\to 2H_{2}O$