In corrosion of iron, - Vidyadip

MCQ

In corrosion of iron,

A
Electrons flow from anode to cathode through the metal, while ions flow through the water droplets.
B
An electrochemical $(g$alvanic$)$ cell is formed in which $Fe$ acts as anode and $O_2$ is reduced at cathode.
C
Dissolved $\mathrm{O}_2$ oxidizes $\mathrm{Fe}^{2+}$ to $\mathrm{Fe}^{3+}$ before it is deposited as rust $(\mathrm{Fe}_2 \mathrm{O}_3 \cdot \mathrm{xH}_2 \mathrm{O}).$
✓
All of the above takes place.

✓

Answer

Correct option: D.

All of the above takes place.

The corrosion of iron is an electrochemical process. The anode region and cathode region are present in iron. Iron$(II)$ is oxidized to Iron$(\text{III})$ by oxygen and is then converted to rust. At the cathode, oxygen is reduced. The electron flow is from anode to cathode through metal. This is accompanied by the flow of ions through water droplets.

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