1. Chapter 6 Chemical Equilibrium

2. Material Equilibrium • Chemical equilibrium, which is equilibrium with respect to conversion of one set of chemical species to another set. • Phase equilibrium, which is equilibrium with respect to transport of matter between phases of system.

3. 2NO2(g) →N2O4(g)

4. H2O+CO → H2+CO2

5. H2O+CO → H2+CO2

6. Equilibrium Constant • Ka: acid dissociation constant (HA H++A-) • Kb=Kw/Ka (A-+H2O HA+OH-) • Kw=1×10-14 (H2O H++OH-) • Ksp: solubility product constant

7. The Standard Concentration Equilibrium Constant Kc: equilibrium constant expressed by concentration Kp: equilibrium constant expressed by pressure aA+bB→cC+dD△n=(c+d)-(a+b)

9. Nonideal MixtureActivity and Activity Coefficients

10. Heterogeneous Equilibra

11. Application of the Equilibrium Constant－Reaction Quotient 1. Q=K, equilibrium 2. Q>K, the system shifts to the left 3. Q<K, the system shifts to the right

13. Le Châtelier’s Principle • If a change in conditions is imposed on a system at equilibrium, the equilibrium position will shift in a direction that tends to reduce that change in conditions. • If a reactant or product is added to a system at equilibrium, the system will shift away from the added component. If a reactant or product is removed, the system will shift toward the removed component

14. The Effect of a Change in Concentration • If a reactant or product is added to a system at equilibrium, the system will shift away from the added component. If a reactant or product is removed, the system will shift toward the removed component.