Problem: The rate law for 2 NO(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](a) Which of these mechanisms is consistent with the rate law?
FREE Expert Solution
We are asked which of these mechanisms is consistent with the rate law.
2 NO(g) + O2(g) ⟶ 2 NO2(g)
rate = k[NO]2[O2]
Problem Details
The rate law for 2 NO(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]
(a) Which of these mechanisms is consistent with the rate law?
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