Disproportionation Reaction: A disproportionation reaction is a redox reaction where the same element undergoes both oxidation and reduction.
Analyzing the reaction:
* NH₄NO₃ → N₂O + 2H₂O
1. Nitrogen in NH₄NO₃: Nitrogen has an oxidation state of -3 in ammonium (NH₄⁺) and +5 in nitrate (NO₃⁻).
2. Nitrogen in N₂O: Nitrogen has an oxidation state of +1 in nitrous oxide (N₂O).
3. Nitrogen in H₂O: Nitrogen is not present in water.
Observation: In this reaction, nitrogen in the reactant (NH₄NO₃) is present in two different oxidation states (-3 and +5). In the product, nitrogen (N₂O) has an oxidation state of +1. This means:
* Nitrogen in ammonium (NH₄⁺) is oxidized: From -3 to +1.
* Nitrogen in nitrate (NO₃⁻) is reduced: From +5 to +1.
Conclusion: Because the same element (nitrogen) undergoes both oxidation and reduction in the reaction, it is classified as a disproportionation reaction.
