Catalysts speed up reactions by providing an alternate reaction pathway with a lower activation energy, making it easier for reactant molecules to form products.
Key points:
- Lower activation energy (Ea): Less energy is needed for collisions to be successful.
- Forward and reverse reactions: Catalysts increase the rate of both forward and reverse reactions equally.
- Not consumed: Catalysts are not used up in the reaction and can be used repeatedly.
- Does not change equilibrium: Catalysts do not affect the position of equilibrium or the equilibrium constant (K).
- Mechanism: They may provide a surface for the reaction or form intermediate complexes that make bond breaking/forming easier.
In short: Catalysts act like a “shortcut” for the reaction, helping it proceed faster without changing the final outcome.