• Chemical equilibrium: when the rates of the forward reaction and the rates of the reverse reaction are equal (there is no change in the concentrations of reactants and products)
  • Key Ideas:
  1. This does not mean the amount of product equals the amount of reactants                                                   
  1. The reaction has not stopped, but their concentrations are changing at a constant rate
  1. At equilibrium pressure will be constant; constant mass or temp does not indicate equilibrium
  • Heterogeneous equilibria: equilibria that involve more than one phase
  •  Homogeneous equilibria: systems in the gas phase, where all reactants and products are gases