Le Chatelier's Principle
Explains the use of Le Chatelier's Principle in working out what happens to an equilibrium if you change the conditions (concentration, temperature, pressure or catalyst).
The Haber Process
Looks in detail at how the conditions for the Haber Process for the manufacture of ammonia are determined by the equilibrium between hydrogen, nitrogen and ammonia.
The Contact Process
Looks in detail at how the conditions for the Contact Process for the manufacture of sulfuric acid are determined by the equilibrium between sulfur dioxide, oxygen and sulfur trioxide.
Explains equilibrium constants expressed in terms of concentrations.
Explains equilibrium constants expressed in terms of partial pressures. Includes an explanation of the terms partial pressure and mole fraction.Before you read this page, you should have a reasonable understanding of Kc.
The effect of changing conditions
Looks at the way that equilibrium constants are changed (or not!) as you change the conditions for a reaction (concentration, temperature, pressure or catalyst), and how this ties in with Le Chatelier's Principle. This page assumes that you are fully confident about writing expressions for both kinds of equilibrium constants.