Chemical Equilibrium 3D Lab

Dynamic equilibrium chamberPress Start. Both reactions will occur until their rates become equal.

Reaction chamber

Click a molecule to track it

Drag to pan · wheel to zoom · tap a molecule to track it

Choose a reversible reaction

N₂ + 3H₂ ⇌ 2NH₃ + heat

Run the simulation

Simulation speed1×

Equilibrium evidence

Not started

0.00Reaction quotient Q

1.00Equilibrium constant K

0.000Forward rate

0.000Reverse rate

Press Start to let molecular collisions begin.

Apply a stress

Watch Q change immediately. The reaction then shifts until Q approaches K again.

Temperature500 K

Container volume5.0 L

Estimated gas pressure0.0 atm

Add catalyst — speeds both directions

Concentrations

Select a formula here or on the chamber key to highlight that molecule.

Concentration versus time

View and tracking

Teacher demo tools

Show reaction flashes

Interactive teacher lecture

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The narration controls the chamber, stresses, molecules, highlights, and graph one concept at a time.

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Voice source

Teacher voice

Introduction to equilibrium0%

The lesson begins with particles reacting in both directions.

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Lesson chapters

Learning objectives

Distinguish static balance from dynamic equilibrium.
Use Q and K to predict the direction of shift.
Apply concentration, pressure, and temperature stresses.
Explain why a catalyst changes time but not equilibrium position.

Key concepts

At equilibrium, forward and reverse rates are equal—not zero.
Concentrations remain constant but are not necessarily equal.
If Q is below K, products form; if Q is above K, reactants form.
For an exothermic reaction, heat behaves like a product.

Suggested experiments

Reach equilibrium, add reactant, and follow Q back toward K.
Compress the Haber mixture and observe the side with fewer gas molecules.
Raise the temperature for the exothermic Haber reaction.
Repeat with and without catalyst and compare only the time taken.

Reaction library

Haber process and Contact process: exothermic industrial equilibria.
NO₂ dimerization: a visible molecular association example.
PCl₅ dissociation: an endothermic reaction that makes more gas particles.
Water-gas shift: equal gas molecules on both sides, so volume has little equilibrium effect.
Hydrogen iodide: a two-reactant, two-product comparison.

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