Model equilibrium responses with clear chemistry-based decision support. Compare multiple disturbances for balanced reaction insights. See shift, Q versus K, and gas effects instantly.
| Reaction | K | Current State | Disturbance | Expected Shift |
|---|---|---|---|---|
| N2O4(g) ⇌ 2NO2(g) | 0.150 | Q = 0.0625 | Increase pressure | Left from pressure, right from Q < K |
| H2(g) + I2(g) ⇌ 2HI(g) | 50.0 | Q = 80.0 | Remove product | Left from Q > K, right from product removal |
| N2(g) + 3H2(g) ⇌ 2NH3(g) | 6.0 | Near equilibrium | Decrease volume | Right toward fewer gas moles |
| Heat + N2O4(g) ⇌ 2NO2(g) | 0.150 | Q = K | Increase temperature | Right for endothermic behavior |
This calculator combines reaction quotient analysis with standard equilibrium response rules from Le Chatelier’s principle. It estimates the dominant direction after one or more disturbances.
Concentration rules: adding reactants or removing products favors products. Removing reactants or adding products favors reactants.
Pressure and volume rules: increasing pressure or decreasing volume favors the side with fewer gaseous moles. Decreasing pressure or increasing volume favors the side with more gaseous moles.
Temperature rules: treat heat as a reactant for endothermic reactions and as a product for exothermic reactions. Only temperature changes alter K directly.
Inert gas rule: at constant volume there is usually no shift for ideal gases. At constant pressure, the side with more gaseous moles is favored.
It estimates the likely equilibrium shift direction after selected disturbances. It compares Q with K and then adds standard Le Chatelier responses for concentration, pressure, volume, temperature, and inert gas changes.
No. It is a directional diagnostic tool. It tells whether the system tends left, right, or stays balanced. Finding exact new equilibrium concentrations requires solving equilibrium equations separately.
The coefficients become exponents in the reaction quotient expression. Without correct coefficients, Q will be wrong, and the predicted shift based on Q versus K can be misleading.
Pressure changes matter mainly for gaseous equilibria. A change in pressure or volume favors the side with fewer or more gaseous moles, depending on the disturbance direction.
Not always. At constant volume, ideal-gas equilibria usually show no shift. At constant pressure, the volume expands and may favor the side with more gaseous moles.
Temperature is the only common disturbance that changes the equilibrium constant itself. Concentration, pressure, and volume mainly change Q or the direction favored during re-equilibration.
Tolerance sets how close Q must be to K before the calculator treats the mixture as nearly at equilibrium. A larger tolerance makes no-shift outcomes more likely.
Yes. Use values consistently. If your equilibrium constant is based on pressure, enter partial pressures. If it is based on concentration, enter concentration values instead.
Important Note: All the Calculators listed in this site are for educational purpose only and we do not guarentee the accuracy of results. Please do consult with other sources as well.