A student proposes the following two-step mechanism for the reaction below:
H+ + I- + H2O2 🡪 H2O + HOI r = k[H+][I-]
Step 1: H+ + H+ + H2O2 🡪 H4O22+ (slow)
Step 2: H4O22+ + I- 🡪 H2O + HOI + H+ (fast)
Would you agree or disagree with this proposed mechanism? Explain your answer with reference to all the rules for a valid
reaction mechanism proposal.
I found this on Google: "the sum of each elementary step in a reaction mechanism must yield the overall reaction equation. The rate law of the rate-determining step must agree with the experimentally determined rate law."
I would disagree because
1. the sum of the elementary steps does NOT add up to the chemical reaction.
2. the rate law for step 1 involves H2O2 but the experimentally determined rate law does not depend on H2O2.