Le Chatelier's Principle

• Le Chatelier's Principle is about how the position of equilibrium is affected by temperature, pressure and concentration
• If you change the conditions of a reversible reaction the position of equilibrium will shift to try and counteract the change
• Negative energy changes mean the reaction is exothermic
• If we were to decrease the temperature of a forward exothermic reaction the position of equilibrium would be pushed to the right. (more products produced)
• If we were to increase the temperature of a forward exothermic reaction the position of equilibrium would be pushed to the left. (less products produced)
• If we increase the pressure the equilibrium will move to whichever side reduces the pressure back down. To lower the pressure the equilibrium will move to the side with the fewest molecules.
• If we decrease the pressure the equilibrium will move to whichever side brings the pressure back up. To rise the pressure the equilibrium will move to the side with the most molecules.
• If we increase the concentration of a product, the equilibrium will shift right to make more reactants