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CHM 101 CHM 101 Past Questions Objective Question
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Question

The rate law for the reaction 2NO₂ + O₃ → N₂O₅ + O₂ is rate = k[NO₂][O₃]. Which one of the following mechanisms is consistent with this rate law?
Options
A NO₂ + NO₂ → N₂O₄ (fast), N₂O₄ + O₃ → N₂O₅ + O₂ (slow)
B NO₂ + O₃ → NO₃ (fast), NO₃ + NO₂ → N₂O₅ + 5/2 O₂ (slow)
C NO₂ + O₃ → NO₃ + O₂ (slow), NO₃ + NO₂ → N₂O₅ (fast)
Correct Answer
D NO₂ + NO₂ → N₂O₂ + O₂ (slow), N₂O₂ + O₃ → N₂O₅ (fast)
Correct Answer

Option C is the correct answer.

Detailed Explanation

The rate law is determined by the slow step. In option C, the slow step is NO₂ + O₃ → products, which gives rate = k[NO₂][O₃], matching the given rate law.

Hint

The slow step (rate-determining step) must match the molecularity of the experimental rate law.

Question Info

Course: CHM 101
Topic: CHM 101 Past Questions
Type: Objective
Difficulty: Not specified
Question 1019 of 1872
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