CHAPTER 8: Chemical Equilibria

Learning outcomes:

explain, in terms of rates of the forward and reverse reactions, what is meant by a reversible reaction and dynamic equilibrium
state Le Chatelier’s Principle and apply it to deduce qualitatively (from appropriate information) the effects of changes in temperature, concentration or pressure, on a system at equilibrium.
state whether changes in concentration, pressure or temperature or the presence of a catalyst affect the value of the equilibrium constant for a reaction
deduce expressions for equilibrium constants in terms of concentrations, ftc, and partial pressures, ftp. [treatment of the relationship between ftp and ftc is not required]
calculate the values of equilibrium constants in terms of concentrations or partial pressures from appropriate data
calculate the quantities present at equilibrium, given appropriate data (such calculations will not require the solving of quadratic equations).
describe and explain the conditions used in the Haber process and the Contact process, as examples of the importance of an understanding of chemical equilibrium in the chemical industry.
show understanding of, and use, the Brønsted-Lowry theory of acids and bases, including the use of the acid-I, base-II concept
explain qualitatively the differences in behaviour between strong and weak acids and bases and the pH values of their aqueous solutions in terms of the extent of dissociation