CH 431/Lecture contents

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   * 1 LECTURE 1:Gas law
   * 2 Units
         o 2.1 Pressure units
         o 2.2 Volume units
         o 2.3 Temperature units
   * 3 Non-ideal behavior
         o 3.1 Compressibility
         o 3.2 Van der Waals
         o 3.3 Corresponding states
   * 1 LECTURE 2
   * 2 Probability distributions
         o 2.1 Discrete distributions
         o 2.2 Indistinguishable outcomes
         o 2.3 Moments of distributions
         o 2.4 Continuous distributions
   * 3 Energy levels
         o 3.1 Quantization
         o 3.2 Duality
         o 3.3 Standing waves in a 'box'
         o 3.4 Size changes
         o 3.5 Potential energy
         o 3.6 Ideal gases, 3D boxes
           * 3.6.1 Degeneracy
           * 3.6.2 Translational motion, degrees of freedom
         o 3.7 Rotational and vibrational energy states
   * 4 Statistical thermodynamics
         o 4.1 Thermal energy
         o 4.2 The Boltzmann probability factor
         o 4.3 Why the Boltzmann factor is an exponential
   * 1 LECTURE 3
         o 1.1 Partition functions
               + 1.1.1 Molecular partition functions versus system partition functions
               + 1.1.2 Translational partition function of a monatomic gas
                     # 1.1.2.1 Breakdown of Boltzmann statistics
         o 1.2 Other partition functions
               * 1.2.1 Electronic
               * 1.2.2 Vibrational
               * 1.2.3 Rotational
   * 1 LECTURE 4
         o 1.1 Classical thermodynamics
         o 1.2 Partial differentiation
         o 1.3 Exact and inexact differentials. State and path functions.
         o 1.4 The zeroth and first law of thermodynamics
         o 1.5 Heat and work
               + 1.5.1 Dissipation and the concept of energy
               + 1.5.2 Types of work
                     # 1.5.2.1 A special case: volume work
                     # 1.5.2.2 Sign conventions
         o 1.6 Compressing a gas in a cylinder
               + 1.6.1 Compression one (irreversible):
               + 1.6.2 Compression two (reversible).
         o 1.7 Reversible versus irreversible
         o 1.8 Work and heat are not state functions
         o 1.9 The more complete first law
   * 1 LECTURE 5: Isotherms and adiabats
         o 1.1 Isothermal expansion of an ideal gas
         o 1.2 Adiabatic expansion of an ideal gas
         o 1.3 Statistical interpretation
   * 1 LECTURE 6: Chemical thermodynamics
         o 1.1 Enthalpy
         o 1.2 Determining enthalpies from heat capacities.
               + 1.2.1 Scanning calorimetry
   * 2 Heat of chemical reactions
         o 2.1 Formation enthalpy
         o 2.2 Heat of combustion
         o 2.3 Hess's law
               + 2.3.1 Reaction-as-written convention (caution!)
               + 2.3.2 Reverse reactions
               + 2.3.3 Combining values
         o 2.4 Tabulation and standard states
              * 2.4.1 Standard states
              * 2.4.2 Tabulation
         o 2.5 Changing temperature
         o 2.6 Changing pressure
   * 1 LECTURE 7
         o 1.1 Spontaneity and entropy
         o 1.2 A new state function named entropy
               + 1.2.1 Circular integrals
         o 1.3 Spontaneity of an isolated system
               + 1.3.1 Entropy exchange of an open system
         o 1.4 Second law
               + 1.4.1 Vacuum expansion
               + 1.4.2 Mixing two gases
               + 1.4.3 Carnot cycles
               + 1.4.4 Efficiency
               + 1.4.5 Heat pumps
   * 1 LECTURE 8
         o 1.1 Two items left on our wish list
               + 1.1.1 Entropy on a microscopic scale
                     # 1.1.1.1 Permutations
         o 1.2 Changing the size of the box with the particles in it
               + 1.2.1 Partition functions and entropy
               + 1.2.2 Entropy versus temperature
                     # 1.2.2.1 Natural variables
                     # 1.2.2.2 Entropy and heat capacity
               + 1.2.3 Absolute entropies. The third law
   * 1 LECTURE 9
         o 1.1 One item that is left on our wish list
         o 1.2 Helmholtz energies
               + 1.2.1 Natural variables of A
         o 1.3 Gibbs energy
               + 1.3.1 Phase transitions
               + 1.3.2 Direction of the spontaneous change
               + 1.3.3 Meaning of the ΔG term
               + 1.3.4 Conjugate variables
               + 1.3.5 Natural variables of G
   * 1 LECTURE 10
         o 1.1 Partial derivatives as powerful machinery
               + 1.1.1 The partial differentials of first and second order. Maxwell relations
               + 1.1.2 'Measuring' entropy
                   * 1.1.2.1 Measuring entropy of an electrochemical reaction
               + 1.1.3 Energy U versus volume
         o 1.2 The relation between the heat capacities
   * 1 LECTURE 11
         o 1.1 Enthalpy H versus pressure
         o 1.2 Gibbs free energy G versus pressure
         o 1.3 The Gibbs-Helmholtz expression
         o 1.4 Gibbs free energy at function of T.
               + 1.4.1 Tabulation of H,S and G. Frozen entropy
         o 1.5 Transitions of order one and two
   * 1 LECTURE 12
   * 1 Phase diagrams
         o 1.1 Diagrams
         o 1.2 Thermodynamic stability
         o 1.3 Fluctuations
         o 1.4 Unary phase diagrams
               + 1.4.1 Liquid-vapor equilibrium
               + 1.4.2 Gas-solid
               + 1.4.3 Liquid-solid
               + 1.4.4 Putting the lines together
   * 2 Binary systems
         o 2.1 Number of moles
         o 2.2 Partial variables
         o 2.3 Thermodynamic potentials
               + 2.3.1 Thermodynamic and electrochemical potentials
         o 2.4 Gaseous mixtures
         o 2.5 Liquid mixtures
         o 2.6 Solid mixtures
         o 2.7 Ideal liquid-gas phase diagram
   * 1 LECTURE 13
         o 1.1 Mixtures
         o 1.2 Partial quantities and scaling
         o 1.3 Gaseous mixtures
         o 1.4 Liquid mixtures
         o 1.5 Solid mixtures
         o 1.6 Ideal liquid- ideal gas phase diagram
               + 1.6.1 The pressure diagram
               + 1.6.2 The temperature diagram
                     # 1.6.2.1 The lever rule
                     # 1.6.2.2 Distillation
   * 1 LECTURE 14
   * 2 Thermodynamics of solutions
         o 2.1 Thermodynamic potentials of solutions
               + 2.1.1 Thermodynamic potentials of ideal solutions
         o 2.2 Thermodynamics of ideal mixing
         o 2.3 Vapor pressures on non-ideal solutions
               + 2.3.1 Henry's law
               + 2.3.2 The other component
                     # 2.3.2.1 Gibbs-Duhem
                     # 2.3.2.2 Gibbs-Duhem in the ideal case
                     # 2.3.2.3 Gibbs-Duhem and Henry's law
               + 2.3.3 Margules functions
               + 2.3.4 Activity and activity coefficients
               + 2.3.5 Regular solutions
                     # 2.3.5.1 Gibbs free energy of regular solutions
         o 2.4 Real solutions
         o 2.5 Boiling non-ideal solutions
               + 2.5.1 Azeotropes
               + 2.5.2 Eutectics
   * 1 LECTURE 15
         o 1.1 Activities
               + 1.1.1 Raoult versus Henry
               + 1.1.2 Various concentration unit
               + 1.1.3 Non-volatile solutes
         o 1.2 Colligative properties
               + 1.2.1 Melting point depression
                     # 1.2.1.1 Determining molar masses nowadays
                     # 1.2.1.2 Purity analysis
               + 1.2.2 Osmosis
                     # 1.2.2.1 Semipermeable membranes
   * 1 LECTURE 16
         o 1.1 Ionic solutions
               + 1.1.1 Thermodynamic potentials versus the dissociation
               + 1.1.2 Mean ionic activity
               + 1.1.3 Activity coefficients
               + 1.1.4 Mean ionic molality
               + 1.1.5 Mean ionic activity coefficient
               + 1.1.6 Measuring mean ionic activity coefficients
               + 1.1.7 Debye-Hückel theory
                     # 1.1.7.1 Debye length
                           * 1.1.7.1.1 Ionic strength
               + 1.1.8 Ionic replacement
               + 1.1.9 Extension of the Debye theory
               + 1.1.10 Importance for colloids
   * 1 LECTURE 17
         o 1.1 Chemical reactions and the liquid problem
         o 1.2 Extent of reaction
               + 1.2.1 Measuring ξ
         o 1.3 Thermodynamic potentials
               + 1.3.1 Gas reactions
               + 1.3.2 ΔrG versus ΔfG
               + 1.3.3 Equilibrium constants
               + 1.3.4 Concentration
         o 1.4 Activity
         o 1.5 activities of pure condensed phases
         o 1.6 Le Chatelier
         o 1.7 K as a function of temperature
         o 1.8 Spontaneity
         o 1.9 Weak electrolytes
         o 1.10 Solubility products