Catalysts

Definition

Catalysts are substances that increase the rate of a chemical reaction without being consumed in the process. They work by lowering the activation energy needed for the reaction to proceed.

5 Must Know Facts For Your Next Test

1. Catalysts lower the activation energy required for a reaction, making it easier for reactants to convert into products.
2. Catalysts do not alter the equilibrium position of a chemical reaction; they only help reach equilibrium faster.
3. Heterogeneous catalysts exist in a different phase than the reactants, while homogeneous catalysts exist in the same phase as the reactants.
4. Enzymes are biological catalysts that speed up biochemical reactions in living organisms.
5. A catalyst can be poisoned by impurities, which decreases its effectiveness and requires specific conditions for optimal performance.

Review Questions

• What is the primary function of a catalyst in a chemical reaction?
• How do heterogeneous and homogeneous catalysts differ?
• In what way does a catalyst affect the activation energy of a reaction?

Related terms

Activation Energy: The minimum amount of energy required for reactants to form products in a chemical reaction.

Reaction Rate: The speed at which reactants are converted into products in a chemical reaction, often measured as concentration change per unit time.

Enzyme: A type of protein that acts as a biological catalyst to accelerate biochemical reactions within living organisms.