| 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 |
We have seen a number of reactions in which a single reactant forms products. For example, consider the following first-order reaction: CH3NC(g) → CH3CN(g). However, we also learned that gas-phase reactions occur through collisions.
One possible explanation is that two molecules of CH3NC collide with each other and form two molecules of the product in a single elementary step. If that were the case, what reaction order would you expect?
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