Le Chatelier's principle: push an equilibrium and it pushes back
This animation depicts the Haber process equilibrium, N2 + 3H2 in balance with 2NH3, showing four gas molecules on the reactant side converting to two on the product side. Increasing system pressure compresses the container, and the equilibrium visibly shifts toward the side with fewer gas molecules, producing more ammonia. It helps students see how Le Chatelier's principle predicts shifts in reversible reactions and is useful for chemistry courses covering equilibrium, reaction stress, and industrial synthesis.
Narrated · 16:9 · every frame verified for overlaps, spacing and edges before rendering
The prompt that made it
Nitrogen and hydrogen in equilibrium with ammonia: four gas molecules on the left become two on the right. Increasing the pressure stresses the system, and the equilibrium shifts toward the side with fewer molecules, making more ammonia.
Make the next one in this series
- Show how increasing temperature shifts the ammonia equilibrium in an exothermic reaction
- Animate the effect of adding a catalyst on reaction rate without shifting equilibrium position
- Compare concentration changes and their effect on shifting equilibrium in a reversible reaction
