Reaction Rates & Collision Theory

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About this simulation

Run a particle experiment, change temperature, concentration, surface area and catalyst, and compare conversion curves.

What students can explore

Save a run without a catalyst. Add a catalyst: what changes in the curve and energy diagram?
Illustrative excess-reagent model: X=1−exp(−kt). Arrhenius kinetics use barriers of 50 or 45 kJ/mol; concentration and surface area scale k. Particle motion illustrates collisions rather than calculating them. This is an irreversible model, not an equilibrium solver.

Learning objectives

1Save a run without a catalyst. Add a catalyst: what changes in the curve and energy diagram?

Questions teachers ask

Save a run without a catalyst. Add a catalyst: what changes in the curve and energy diagram?

The barrier falls and conversion becomes faster. Reactant and product energy levels and the final conversion stay the same.

About the model

Illustrative excess-reagent model: X=1−exp(−kt). Arrhenius kinetics use barriers of 50 or 45 kJ/mol; concentration and surface area scale k. Particle motion illustrates collisions rather than calculating them. This is an irreversible model, not an equilibrium solver.

Embed this simulation

Drop it into your LMS, blog, or class site — free.

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