| Sections | |||
|---|---|---|---|
| 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 |
|---|
| 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]
(a) Which of these mechanisms is consistent with the rate law?
Enter your friends' email addresses to invite them:
Join thousands of students and gain free access to 46 hours of Chemistry videos that follow the topics your textbook covers.