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What are the steps to apply the steady-state approximation when the first step is fast and reversible?
1. Identify the intermediate. 2. Set up equilibrium for the fast, reversible step. 3. Solve for the intermediate's concentration. 4. Substitute the intermediate's expression into the slow step's rate law.
What are the differences between intermediates and catalysts?
Intermediates: Produced then consumed, don't appear in overall reaction. | Catalysts: Used then regenerated, appear in reactants and products.
What is a reaction mechanism?
A series of elementary steps showing how a reaction occurs at the molecular level.
Define an elementary step.
A single molecular event (e.g., collision, bond breaking/forming).
What are intermediates?
Species produced in one step and consumed in a later step; they don't appear in the overall reaction.
What are catalysts?
Species that speed up a reaction but are not consumed in the overall reaction; they appear in reactants and products.
Define the rate-determining step.
The slowest step in a reaction mechanism; it determines the overall reaction rate.
What is the steady-state approximation?
The assumption that the concentration of intermediates remains constant because their rate of formation equals their rate of consumption.