Steady-State Approximation
The steady-state approximation is a method used in chemical kinetics to simplify the analysis of complex reaction mechanisms.
Key Concepts
- Intermediate Species: Short-lived species formed in a reaction mechanism
- Steady-State Assumption: The concentration of the intermediate remains approximately constant during most of the reaction
- Rate of formation ≈ Rate of consumption
Applying the Steady-State Approximation
- Identify intermediate species in the mechanism
- Write rate expressions for formation and consumption of the intermediate
- Set the net rate of change of the intermediate to zero
- Solve for intermediate concentration
- Substitute into the overall rate law
Example
For the reaction: A → B → C
- B is an intermediate: d[B]/dt ≈ 0
- Steady-state approximation allows simplification of rate expressions to focus on A → C
Importance
- Simplifies mathematical treatment of multistep reactions
- Helps derive rate laws for complex mechanisms
- Widely used in enzymatic reactions and catalytic cycles
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