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Dynamic Equilibrium Simulator
Explore reversible reactions, Le Chatelier's
Principle, and the industrial Haber Process in a fully dynamic particle environment.
What you'll learn
- That chemical equilibrium is dynamic: both forward and reverse reactions
continue to occur at equal rates.
- How shifting conditions (Temperature, Pressure, Concentration) alter the rates, leading to a
new equilibrium state according to Le Chatelier's Principle.
- How to interpret live concentration-time graphs showing the characteristic plateau once
equilibrium is established.
- How the Haber Process (N₂ + 3H₂ ⇌ 2NH₃) is optimized industrially for maximum yield despite
conflicting rate/yield conditions.
How to use it
- Watch the individual Nitrogen (N₂) and Hydrogen (H₂) molecules collide and form Ammonia
(NH₃), while breaking down at the same time.
- Monitor the concentration graphs and rate counters to see the system hit equilibrium.
- Apply a stress to the system (add/remove chemicals, change pressure/volume, or change
temperature) and watch the rates respond.
- Try to find the optimal industrial conditions to maximize Ammonia production!
Notes
The Haber Process forward reaction is exothermic,
and converts 4 moles of gas into 2 moles of gas. Keep this in mind when manipulating temperature
and pressure!
