Need help with this chemistry question:
NO(g) + O2(g) -> NO2(g) + O(g)
The experimentally determined rate law is found to be rate = k[NO]^a. Which of the following mechanisms is consistent with this rate law?
Mechanism I:
NO -> N + O (slow)
N + O3 -> NO + O (fast)
O + O -> O
Mechanism II:
O3 -> O + O
O + NO -> NO (slow)
(fast)
Based on the mechanism you chose in a:
i. Determine the molecularity of each step.
ii. What are the reaction intermediates?
iii. Is there a catalyst in the mechanism? If none, how can a catalyst speed up this reaction? Yes, there is a catalyst.
Sketch an energy diagram consistent with the reaction mechanism.