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 |
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.
Another possibility is that the reaction occurs through more than one step. For example, a possible mechanism involves one step in which the two CH3NC molecules collide, resulting in the "activation" of one of them. In a second step, the activated molecule goes on to form the product. Determine which step must be rate determining in order for the kinetics of the reaction to be first order.
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