BRAINCAKEEffect of Catalysts
A catalyst is a substance that increases the rate of a reaction without being used up. It is chemically unchanged at the end of the reaction.
A catalyst works by providing an alternative reaction pathway with a lower activation energy. It often does this by forming an intermediate with a reactant, or by holding reactant molecules on its surface where bonds are weakened.
The effect is shown on a Maxwell-Boltzmann distribution. The curve itself does not change, because the temperature is the same. But the catalysed activation energy, Ecat, is to the left of the uncatalysed Ea, so a much larger area lies to the right of it.
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Key terms in this lesson
- activation energy
- The minimum energy that colliding particles must have for a reaction to occur.
More in Reaction Rates
- Steric Hindrance
- Effect of Concentration
- Effect of Pressure
- Effect of Surface Area
- Maxwell-Boltzmann Distribution Curve
- Effect of Temperature
- Collisions in Solution
- Catalysts in Industry
All 12 lessons in Reaction Rates · All Edexcel AS-level Chemistry topics