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How rusting of iron is envisaged as setting up of an electrochemical cell?

Solution)

Rusting of Iron is due to corossion.

Rust is an Fe₂O₃.xH₂O

Theory of Rusting :

1. Water present on the metal surface dissolves CO2 and O2 from the air.

H₂O + CO₂ ---------> H₂CO₃

O₂ + 4H⁺ + 4e^- -------> 2H₂O

2. Fe in contact with dissolved CO2 and O2 undergoes oxidation.

Fe ------------> Fe²⁺ + 2e^- Anode (E_Fe⁺²/Fe = -0.44V)

3. Electrons lost by Fe are taken by H+

H⁺ + e^- ------------> H

4H+O₂ --------> 2H₂O

The dissolved O₂ can be take electrons directly also

O2 + 2H₂O + 4e^- -----------> 3OH^- cathode

Overall 2Fe_(s) + O_2(g) +4H⁺_(aq) -------------> 2Fe⁺² + 2H₂O

4. Fe⁺² react with dissolved O₂and water

Fe⁺² + 2OH^- -----------> Fe(OH)₂

4Fe(OH)₂ + O₂ +2H₂O ----------> 4Fe(OH)₃

2Fe(OH)₃ ---------> Fe₂O₃ + 3H₂O

Fe₂O₃ + XH2O ------------> Fe₂O₃.XH₂O

Rust (Hydrated ferric oxide)

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Chemistry, Academics

Category:- Chemistry
Reference No.:- M9527583

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