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Catalysis

Catalysis is the process in which a substance, called a catalyst, increases the rate of a chemical reaction without being consumed in the reaction.

Key Concepts​

  • Catalyst: Speeds up a reaction by lowering the activation energy
  • Homogeneous Catalysis: Catalyst and reactants are in the same phase
  • Heterogeneous Catalysis: Catalyst and reactants are in different phases
  • Enzyme Catalysis: Biological catalysts that are highly specific and efficient

How Catalysts Work​

  • Provide an alternative reaction pathway with lower activation energy
  • Increase the frequency of effective collisions
  • Do not change the overall thermodynamics (ΔG, ΔH remain the same)

Example​

  • Decomposition of hydrogen peroxide:
    2 H₂O₂ → 2 H₂O + O₂
    • Without catalyst: slow reaction
    • With MnO₂ (catalyst): reaction speeds up, MnO₂ remains unchanged

Importance​

  • Catalysts are essential in industrial processes (e.g., Haber process, catalytic converters)
  • Enable biochemical reactions in living organisms
  • Reduce energy consumption and waste in chemical manufacturing

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