Effects of Catalysts on Chemical Reactions
Key Concepts
- Collision Theory: Chemical reactions occur only when reacting particles collide with sufficient energy.
- The rate of a chemical reaction is determined by the frequency of successful collisions (collisions per second).
- Activation Energy: The minimum amount of energy particles need to react.
Catalysts
- Definition: Catalysts increase the rate of chemical reactions without being consumed in the reaction.
- Importance:
- Allow reactions to occur quickly without increasing temperature, saving money.
- Can be reused multiple times as they are not used up during the reaction.
How Catalysts Work
- Provide an alternative reaction pathway with a lower activation energy.
- Result in more particles having sufficient energy to collide successfully.
- Increase the rate of the reaction by allowing more successful collisions per second.
Key Points About Catalysts
- Exclusion from Chemical Equations:
- Catalysts are not included in the chemical equation as they are not consumed.
- Specificity:
- Different reactions require different catalysts.
- Biological Catalysts:
- Enzymes act as catalysts in living organisms (to be discussed in detail in biology topics).
Study Resources
- Additional questions on catalysts and their effects are available in the revision workbook.
By understanding these concepts, you should be able to describe the effect of catalysts on the rate of chemical reactions.