Catalysts

A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the reaction itself. In other words, it speeds up the reaction without undergoing any permanent change.

Key Concepts

• Activation Energy: Catalysts work by lowering the activation energy required for a reaction to occur. This reduces the energy barrier and allows the reaction to proceed more rapidly.
• Types of Catalysts: Catalysts can be classified as homogeneous (in the same phase as the reactants) or heterogeneous (in a different phase from the reactants).
• Enzyme Catalysts: Enzymes are biological catalysts that facilitate biochemical reactions in living organisms.
• Promoters and Inhibitors: Some substances can enhance the catalytic activity of a catalyst (promoters), while others can decrease or stop the activity (inhibitors).

Examples of Catalysts

Common catalysts include:

1. Platinum in catalytic converters: Used to convert harmful gases in car exhaust into less harmful substances.
2. Iron in the Haber process: Aiding the production of ammonia from nitrogen and hydrogen.
3. Enzymes in digestion: Helping to break down food in the digestive system.

Study Tips

When studying catalysts, it's important to:

1. Understand the concept of activation energy and how catalysts affect it.
2. Recognize the different types of catalysts and their applications in various chemical processes.
3. Learn about the role of enzymes as biological catalysts in living organisms.
4. Explore how promoters and inhibitors influence the activity of catalysts.

Additionally, practicing with sample problems and real-world applications can help reinforce your understanding of catalysts and their impact on chemical reactions.