Problem: The following mechanism has been proposed for the reaction of NO with H2 to form N2O and H2O:NO(g) + NO(g)2 → N2O2 (g)N2 O2 (g) + H2 (g) → N2O(g) + H2O(g)The observed rate law is rate = k[NO]2 [H2 ]. If the proposed mechanism is correct, what can we conclude about the relative speeds of the first and second reactions?

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The following mechanism has been proposed for the reaction of NO with H2 to form N2O and H2O:

NO(g) + NO(g)2 → N2O2 (g)
N2 O2 (g) + H2 (g) → N2O(g) + H2O(g)

The observed rate law is rate = k[NO]2 [H2 ]. If the proposed mechanism is correct, what can we conclude about the relative speeds of the first and second reactions?

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