Le Chatelier's Principle Calculator

Le Chatelier's principle states that when a system at equilibrium is subjected to a change in concentration, temperature, pressure, or other factors, the equilibrium will shift in the direction that counteracts the imposed change to restore equilibrium.

For exothermic reactions, increasing temperature shifts equilibrium toward reactants (left), while decreasing temperature favors products (right). For endothermic reactions, the opposite occurs - higher temperature favors products, lower temperature favors reactants.

According to Le Chatelier's principle, increasing the concentration of a reactant will shift the equilibrium toward the products (right) to consume the excess reactant and restore equilibrium.

Increasing pressure (decreasing volume) shifts equilibrium toward the side with fewer gas molecules. Decreasing pressure (increasing volume) favors the side with more gas molecules. This only applies to reactions involving gases.

No, catalysts do not change the equilibrium position. They only increase the rate at which equilibrium is reached by lowering the activation energy for both forward and reverse reactions equally.

Adding an inert gas at constant volume has no effect on equilibrium position because it doesn't change the partial pressures of the reacting species. At constant pressure, it effectively decreases the pressure of reacting gases, shifting equilibrium toward more gas molecules.

Use Le Chatelier's principle: if you increase a substance's concentration, equilibrium shifts away from that substance. If you decrease a concentration, equilibrium shifts toward that substance to replace what was removed.

Phase labels (g), (l), (s), (aq) are crucial because Le Chatelier's principle applies differently to different phases. For example, pressure changes only affect gaseous species, and pure solids/liquids don't appear in equilibrium expressions.