Review for Third Hour Exam

Chapters 5 & 6

Chapter 5. (last part)

1) Heterogeneous reactions (those involving, for example solid and gas phases)

2) Gibb's phase rule: F = C - N_p +2 , where C = N_s - R

Chapter 6. Phase equilibria

I. Single component systems

a) Phase diagrams

b) The Clapeyron equation: phase boundary (P vs. T) between 2 phases

c) Clausius-Clapeyron equation: apply approximations to Clapeyron eqn. and use for solid/gas and liquid/gas phase boundaries (vapor pressure vs. T)

d) Relation of the chemical potential to phase equilibria: T dependence, P dependence

e) Effects of surface tension on vapor pressure and particle nucleation

f) Ehrenfest classifications of phase transitions (1st order, 2nd order, etc.)

II. Binary liquid mixtures

a) Phase diagrams (bubble point line, dew point line)

b) Raoult's law and ideal solutions, chemical potential of an ideal solution

c) non-ideal liquids (i.e., positive and negative deviations from Raoult's law)

d) boiling point diagrams and distillation, lever rule

e) Henry's law for solutes; chemical potential of a dilute real solution and its standard state

f) Activities (a_i = P_i/P_i*) and activity coefficients (Raoult and Henry's law activity coefficients)

g) Qualitative aspects of colligative properties in terms of the chemical potential (mu is lower in the solution compared to the pure solvent)

h) Qualitative aspects of melting point phase diagrams of 2-component systems, cooling curves