Types Of Redox Reactions
Which of the following reactions is an example of a disproportionation reaction?
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About This Question
- Subject
- chemistry
- Chapter
- redox reactions and electrochemistry
- Topic
- types of redox reactions
- Difficulty
- Easy
- Year
- 2025
Solution
Correct Answer:
2H2O2(aq)→2H2O(l)+O2(g)
In a disproportionation reaction, the same element undergoes both oxidation and reduction simultaneously. In H₂O₂ decomposition, oxygen is in the −1 oxidation state in H₂O₂. In the products, oxygen in H₂O is −2 (reduction) and oxygen in O₂ is 0 (oxidation). Thus oxygen in H₂O₂ is simultaneously oxidised and reduced — the hallmark of disproportionation. Option B is a displacement reaction, option C is a combination reaction, and option D is a reduction of iron oxide by CO (a redox reaction but not disproportionation, since different elements are oxidised and reduced).
This easy difficulty chemistry question is from the chapter redox reactions and electrochemistry, covering the topic of types of redox reactions. It appeared in the 2025 exam.
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