Forward and reverse reactions occur simultaneously

Rates of forward and reverse reactions are equal

Concentrations of reactants and products remain constant

Ratio of product concentrations to reactant concentrations

Exponents are stoichiometric coefficients

Homogeneous reactions

Heterogeneous reactions

Indicator of the extent of reaction at equilibrium

Measuring concentrations at equilibrium

Q describes the ratio at any point in the reaction

System responds to stress by shifting equilibrium

Adding or removing reactants or products

Effect on equilibrium for reactions with gaseous components

Endothermic and exothermic reactions

Initial, Change, Equilibrium concentrations

Using K and the ICE table

Comparing Q to K

Haber process for ammonia synthesis

Contact process for sulfuric acid production

Acid rain formation

Ozone layer depletion

Hemoglobinoxygen binding

Enzymecatalyzed reactions