Describe the condition of equilibrium in a reversible reaction.
Describe how equilibrium concentrations are established experimentally.
Write the equilibrium constant expression in terms of concentrations,
Kc for a reaction and use the value of Kc and the concentrations
of all species but one to determine the equilibrium concentration of that
species.
Derive K values for situations where chemical equations are reversed,
multiplied through by constant coefficients, or added together.
Assess the relative importance of the forward and reverse reactions from the
magnitude of an equilibrium constant.
Write an equilibrium constant expression in terms of partial pressures of
gases, Kp; and relate a value of Kp to the corresponding value of
Kc.
Know that the concentrations of pure liquids and solids are omitted from
equilibrium constant expressions.
Calculate a numerical value of an equilibrium constant if equilibrium
conditions are given.
Predict the direction in which a reaction proceeds toward equilibrium by
comparing the reaction quotient, Qc to Kc.
Use the ideal gas law and Dalton's law of partial pressures in working with
Kp expressions.
Make qualitative predictions of how equilibrium conditions change when an
equilibrium mixture is disturbed. That is, apply Le Châtelier's
principle.
Calculate the final equilibrium condition in a reversible reaction from a
given set of initial conditions.
Calculate the new equilibrium concentrations or partial pressures after an
equilibrium system has adapted to changed conditions.