Which of the following process represents disproportionation?
Correct answer: B. I2 + OH- → IO- + I- + H2O
- A. Cu + HNO3 → Cu(NO3)2 + NO + H2O
- B. I2 + OH- → IO- + I- + H2O
- C. Cl2 + I2 → 2ClI
- D. Zn + 2HCl → ZnCl2 + H2
Explanation
In a disproportionation reaction, a single element in one oxidation state is simultaneously oxidized and reduced to form two different products. In Option B, iodine (I2) undergoes disproportionation as it is both oxidized to IO- and reduced to I-. This demonstrates the key characteristic of disproportionation reactions. The other options involve redox reactions, but they do not involve a single element undergoing both oxidation and reduction.
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