Le Chatelier Predictor
Select a reaction type and a stress condition to instantly see which direction the equilibrium shifts and why.
Reaction
Stress Applied
Stress Details
No further configuration needed — catalysts don't change equilibrium position.
Inert gas at constant volume — partial pressures of reactants/products are unchanged.
Step-by-step Reasoning
Effect on Kc
Quick Reference
| Stress | Shift Direction | K changes? |
|---|---|---|
| Add reactant | Forward → | No |
| Add product | ← Reverse | No |
| Remove reactant | ← Reverse | No |
| Remove product | Forward → | No |
| Increase pressure (gas) | Toward fewer gas moles | No |
| Decrease pressure (gas) | Toward more gas moles | No |
| Increase temp (exo) | ← Reverse | Kc decreases |
| Increase temp (endo) | Forward → | Kc increases |
| Add catalyst | No shift | No |
| Add inert gas (const. vol.) | No shift | No |
Summary
Select a reaction type and a stress condition to instantly see which direction the equilibrium shifts and why.
How it works
- Select a preset reaction or choose "Custom" to describe your own equilibrium.
- Pick the type of stress: concentration change, pressure/volume change, or temperature change.
- Configure the stress details — which species, which direction, and for temperature reactions, whether the reaction is exo- or endothermic.
- Click "Predict Shift" to see the direction (forward, reverse, or no shift) and the reasoning.
- Review the color-coded result and the step-by-step explanation below the result panel.
Use cases
- Check equilibrium shift predictions during exam prep or homework.
- Verify intuition when designing industrial chemical processes (e.g., Haber process).
- Understand how a catalyst affects equilibrium position (it doesn't).
- Explore how removing a product drives a reaction forward.
- See why increasing pressure favors the side with fewer moles of gas.
- Confirm the effect of adding an inert gas at constant volume.
Frequently Asked Questions
Last updated: 2026-06-18 ·
Reviewed by Nham Vu