Dynamic Equilibrium Simulator

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 optimised industrially for useful yield despite conflicting rate/yield conditions.

How to use it

1. Watch the individual nitrogen (N₂) and hydrogen (H₂) molecules collide and form ammonia (NH₃), while breaking down at the same time.
2. Monitor the concentration graphs and rate counters to see the system hit equilibrium.
3. Apply a stress to the system (add/remove chemicals, change pressure/volume, or change temperature) and watch the rates respond.
4. Try to find industrial conditions that improve ammonia production while keeping the reaction practical.

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!