Explain how rusting of iron is envisaged as setting up of an electrochemical cell. 1 marks.

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Solution

Rusting of iron form an electrochemical cell.The reaction is take place in presence of water. An electrochemical cell is created on an iron object that has a distinct anode and cathode.
At one spot iron loses electrons (is oxidized) to form iron (II) ions.
Fe (s)â†’Fe²⁺ (aq) + 2e- (the anodic site of our electrochemical cell)
At another spot oxygen in the air combines with water and forms hydroxide ions.
½O₂ (g) + H₂O (l) + 2e-â†’ 2OH^- (aq)(the cathodic site of our electrochemical cell)
In the presence of oxygen iron further oxidizes at the anode (loses electrons) to become iron (III) ions.
Fe ²⁺ (aq)â†’ Fe³⁺ (aq) + e-
The iron (III) ions and the hydroxide combine to form rust.
2Fe ³⁺ (aq) + 6OH^- (aq)â†’ Fe₂O₃ (s) + 3 H₂O (l)

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