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1. Introduction to Catalysts
- A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process.
- Catalysts provide an alternative pathway with a lower activation energy.
- They do not alter the equilibrium position of a reversible reaction.
- Catalysts are classified as homogeneous (same phase as reactants) or heterogeneous (different phase).
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1. Introduction to Activation Energy
- Activation energy (Ea) is the minimum energy required for reactants to form products.
- It is a crucial concept in understanding how reactions proceed at the molecular level.
- Reactions with lower activation energy occur more quickly than those with higher activation energy.
- Transition state: Reactants must pass through a high-energy intermediate state before converting to products.
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1. Introduction to Chemical Kinetics
- Chemical kinetics is the branch of chemistry that studies the rate of chemical reactions and the factors affecting them.
- The rate of reaction refers to the change in concentration of reactants or products per unit time.
- It helps in understanding the mechanism of chemical processes.
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