| 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 |
Reactions between certain haloalkanes (alkyl halides) and water produce alcohols. Consider the overall reaction for t-butyl bromide (2-bromo-2-methylpropane):
(CH3)3CBr(aq) + H2O(l) ⟶ (CH3)3COH(aq) + H+(aq) + Br-(aq)
The experimental rate law is rate = k[(CH3)3CBr]. The accepted mechanism for the reaction is
(1) (CH3)3C—Br(aq) ⟶ (CH3)3C+(aq) + Br-(aq) [slow]
(2) (CH3)3C+(aq) + H2O(l) ⟶ (CH3)3C—OH2+(aq) [fast]
(3) (CH3)3C—OH2+(aq) ⟶ H+(aq) + (CH3)3C—OH(aq) [fast]
(a) Why doesn’t H2O appear in the rate law?
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