Le Chatelier's Principle

Le Chatelier's Principle

6 min read Updated Mar 26, 2026

You now know how to calculate K and Q, and how to predict which direction a reaction shifts. Le Chatelier’s principle is the conceptual framework that ties it all together - and it is tested on virtually every MCAT.

The Principle

Le Chatelier’s principle states: if a stress is applied to a system at equilibrium, the system will shift in the direction that partially relieves that stress.

The key word is “partially.” The system never completely undoes the change - it just moves toward a new equilibrium that partially offsets whatever you did.

Three Types of Stress

Le Chatelier’s principle applies to three types of changes:

  1. Changes in concentration (adding or removing a reactant or product)
  2. Changes in pressure or volume (for gas-phase reactions)
  3. Changes in temperature (the only one that changes K)

Each of the next three sections covers one of these in depth. Here is the summary table:

Stress appliedEquilibrium shifts…Does K change?
Add reactantToward products (right)No
Remove reactantToward reactants (left)No
Add productToward reactants (left)No
Remove productToward products (right)No
Increase pressure (decrease volume)Toward side with fewer moles of gasNo
Decrease pressure (increase volume)Toward side with more moles of gasNo
Increase temperatureToward endothermic directionYes
Decrease temperatureToward exothermic directionYes
Add catalystNo shiftNo
Add inert gas at constant volumeNo shiftNo

How to Think About It Using Q

Le Chatelier’s principle is really just Q vs. K logic in disguise:

  • Add reactant - the denominator of Q gets bigger, so Q decreases below K. Since Q < K, the reaction shifts forward.
  • Remove product - the numerator of Q gets smaller, so Q decreases below K. Since Q < K, the reaction shifts forward.
  • Add product - the numerator gets bigger, Q > K, so the reaction shifts backward.

Every Le Chatelier prediction can be confirmed by checking what happens to Q relative to K.

A system at equilibrium is stressed by adding more of one reactant. In which direction does the equilibrium shift, and does K change?
Click to reveal answer
The equilibrium shifts toward products (right). Adding reactant increases the denominator of Q, making Q < K. The forward reaction speeds up to consume the excess reactant. K does NOT change - only temperature changes K.
Does adding a catalyst shift the equilibrium position?
Click to reveal answer
No. A catalyst speeds up BOTH the forward and reverse reactions equally. It helps the system reach equilibrium faster, but it does not change the equilibrium position or the value of K.