Problem: The rate law for 2NO(g) + O2(g) ⟶ 2NO2(g) is rate = k[NO]2[O2]. In addition to the mechanism in the text (Section 16.6), the following ones have been proposed:I        2NO(g) + O2(g) ⟶2NO2(g)II       2NO(g) ⇌ N2O2(g)                          [fast]         N2O2(g) + O2(g) ⟶2NO2(g)           [slow]III      2NO(g) ⇌ N2(g) + O2(g)                  [fast]         N2(g) + 2O2(g) ⟶ 2NO2(g)            [slow](b) Which of these mechanisms is most reasonable? Why?

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Elementary steps of 1st and 3rd mechanisms are complicated compared to a bimolecular reaction.

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The rate law for 2NO(g) + O2(g) ⟶ 2NO2(g) is rate = k[NO]2[O2]. In addition to the mechanism in the text (Section 16.6), the following ones have been proposed:

I        2NO(g) + O2(g) ⟶2NO2(g)
II       2NO(g) ⇌ N2O2(g)                          [fast]
         N2O2(g) + O2(g) ⟶2NO2(g)           [slow]
III      2NO(g) ⇌ N2(g) + O2(g)                  [fast]
         N2(g) + 2O2(g) ⟶ 2NO2(g)            [slow]

(b) Which of these mechanisms is most reasonable? Why?

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