The steady-state approximation is a useful idea in chemical kinetics for simplifying the study of complex reactions. Here’s a explanation:
1. What it means
- In some reactions, intermediates are formed and then quickly used up.
- Their concentration stays very small and nearly constant during most of the reaction.
- The steady-state approximation assumes that the rate of formation of the intermediate = the rate of its consumption.
2. Why it is useful
- It makes the math much simpler when working with complicated multi-step reactions.
- Instead of tracking every intermediate exactly, we assume they don’t build up.
3. Where it is applied
- Used in chain reactions and enzyme kinetics (like the Michaelis–Menten model).
- Common in atmospheric chemistry, combustion, and biological reaction mechanisms.
In short: The steady-state approximation assumes that the amount of an intermediate stays nearly constant because it is made and used up at the same rate. This makes it easier to calculate reaction rates.