Subjects
Sections | |||
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Rate of Reaction | 11 mins | 0 completed | Learn Summary |
Average Rate of Reaction | 18 mins | 0 completed | Learn |
Arrhenius Equation | 16 mins | 0 completed | Learn Summary |
Rate Law | 38 mins | 0 completed | Learn Summary |
Integrated Rate Law | 52 mins | 0 completed | Learn Summary |
Collision Theory | 9 mins | 0 completed | Learn |
Additional Practice |
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Instantaneous Rate of Change |
Energy Diagram |
Catalyst |
Michaelis-Menten Equation |
Reaction Mechanism |
Identifying Reaction Order |
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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