BRAINCAKECollisions in Solution
Collision theory applies to reactions in solution just as it does to gases. Dissolved reactant particles (molecules or ions) move through the solvent, and a reaction happens only when two reactant particles collide with energy greater than or equal to the activation energy and in the correct orientation.
In solution, a reactant particle is surrounded by solvent molecules. Most of its collisions are with the solvent, not with the other reactant. The rate therefore depends on the concentration of the dissolved reactants in mol dm−3, which controls how often reactant particles meet. Changing the pressure has almost no effect, because liquids are almost incompressible.
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Key terms in this lesson
- activation energy
- The minimum energy that colliding particles must have for a reaction to occur.
- collision theory
- The theory that a reaction between particles occurs only when they collide with sufficient energy and the correct orientation.
More in Reaction Rates
- Steric Hindrance
- Effect of Concentration
- Effect of Pressure
- Effect of Surface Area
- Maxwell-Boltzmann Distribution Curve
- Effect of Temperature
- Effect of Catalysts
- Catalysts in Industry
All 12 lessons in Reaction Rates · All Edexcel AS-level Chemistry topics