Collision Theory Simulator

Collision Theory Statement

For a chemical reaction to occur, three conditions must be met:

1. Particles must collide with each other
2. Collisions must have sufficient energy ≥ activation energy (Ea)
3. Collisions must have correct orientation (proper geometry)

Activation Energy (Ea)

The minimum energy required for a reaction to occur. Particles with E < Ea bounce off without reacting. The activation energy barrier determines the rate at a given temperature.

k = A · e^(-Ea/RT)    (Arrhenius equation)

Factors Affecting Reaction Rate

Temperature: Higher T → particles move faster → more collisions with E ≥ Ea → rate increases.

Concentration: Higher [ ] → more particles per unit volume → more frequent collisions → rate increases.

Surface Area: Smaller particles → greater exposed surface → more collision sites → rate increases.

Catalyst: Provides alternative pathway with lower Ea → more particles have sufficient energy → rate increases. Catalyst is not consumed.

Maxwell-Boltzmann Distribution

At any temperature, particles have a range of kinetic energies. The distribution shows the fraction of particles at each energy level.

As temperature increases, the peak shifts right and flattens — a greater proportion of particles exceed Ea.

Successful vs Unsuccessful Collisions

Most collisions are unsuccessful because particles lack sufficient energy or wrong orientation. Only a small fraction result in reaction.

Rate ∝ (collision frequency) × (fraction with E ≥ Ea) × (orientation factor)