What you’ll learn10 learning objectivesChoose one objective for a focused lesson, or study the complete topic.7.1.1What is meant by a reversible reaction• Reactions being equal and the concentration of reactants and products remaining constant- (a) understand what is meant by a reversible reaction- (b) understand what is meant by dynamic equilibrium in terms of the rate of forward and reverse- (c) understand the need for a closed system in order to establish dynamic equilibriumSyllabus objective7.1.2Le Chatelier’s principle as: if a change• Define Le Chatelier’s principle as: if a change is made to a system at dynamic equilibrium, the position of equilibrium moves to minimise this changeSyllabus objective7.1.3Le Chatelier’s principle to deduce (from• Use Le Chatelier’s principle to deduce qualitatively (from appropriate information) the effects of changes in temperature, concentration, pressure or presence of a catalyst on a system at equilibriumSyllabus objective7.1.4Expressions for equilibrium constants• Deduce expressions for equilibrium constants in terms of concentrations, K cSyllabus objective7.1.5The terms mole fraction and partial pressure• Use the terms mole fraction and partial pressureSyllabus objective7.1.6Expressions for equilibrium constants• Deduce expressions for equilibrium constants in terms of partial pressures, K p (use of the relationship between Kp and Kc is not required)Syllabus objective7.1.7The Kc and Kp expressions to carry out• Use the Kc and Kp expressions to carry out calculations (such calculations will not require the solving of quadratic equations)Syllabus objective7.1.8The quantities present at equilibrium• Calculate the quantities present at equilibrium, given appropriate dataSyllabus objective7.1.9Whether changes in temperature, concentration• State whether changes in temperature, concentration or pressure or the presence of a catalyst affect the value of the equilibrium constant for a reactionSyllabus objective7.1.10Conditions used in the Haber process• Describe/explain: the conditions used in the Haber process and the Contact process, as examples of the importance of an understanding of dynamic equilibrium in the chemical industry and the application of Le Chatelier’s principleSyllabus objective