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The reaction of hydrogen and iodine monochloride is given as: H₂(g) + 2ICl(g) → 2HCl(g) + I₂(g) The reaction is first order with respect to H₂(g) and ICl(g), following mechanisms were proposed. Mechanism A: H₂(g) + 2ICl(g) → 2HCl(g) + I₂(g) Mechanism B: H₂(g) + ICl(g) → HI(g); slow HI(g) + ICl(g) → HCl(g) + I₂(g); fast Which of the above mechanism(s) can be consistent with the given information about the reaction?

1. A and B both
2. neither A nor B
3. A only
4. B only

Correct answer: B only

Solution

Mechanism B is consistent because the rate-determining step (slow step) involves one molecule of H₂ and one molecule of ICl, which aligns with the reaction being first order with respect to both. Mechanism A does not explain the observed rate law.

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