Physical chemistry 0600-S1-CM-CF

The physical chemistry course includes 30 hours of lecture and 45 hours of laboratory.
The lecture covers the following content

1. Introduction (scope of the subject, mathematical foundations)

2. States of matter

3. Gaseous state
1) gas laws,
2) equation of state of an ideal gas;
3) equations of state of real gases (van der Waals, virial);
3) principle of corresponding states;
4) condensation of gases;
5) kinetic theory of gases;
6) diffusion, effusion.

4. Thermodynamics: First law of thermodynamics
1) basic concepts (system, heat, work, energy);
2) internal energy of the system;
3) First law of thermodynamics;
4) determination of changes in internal energy (calorimetric bomb), heat capacity;
5) adiabat;
6) enthalpy;
7) determination of enthalpy changes (calorimeter), heat capacity;
8) interpretation of heat capacity at the molecular level;
9) enthalpy of physical changes;
10) standard state;
11) enthalpy of chemical reactions;
12) Hess's law;
13) Kirchhoff's equation.

5. Thermodynamics: 2nd law of thermodynamics
1) Carnot cycle;
2) entropy (direction of spontaneous process; entropy and 2nd law of thermodynamics; entropy change);
3) calculation of entropy changes;
4) absolute entropy and 3rd law of thermodynamics;
5) entropy and spontaneity of reactions;
6) consequences of 2nd law of thermodynamics – free energy, free enthalpy, conditions of spontaneity of process;

6. Thermodynamics: thermodynamic functions
1) relationship between thermodynamic functions;
2) extensive, intensive quantities;
3) partial molar quantities;
4) important thermodynamic equations (Gibbs-Duhem equation et al.).

7. Non-ideality of gases, gas mixtures, liquid solutions
1) chemical potential of a component of the mixture;
2) volatility and volatility coefficient (gases);
3) activity and activity coefficients;
4) chemical potential of a non-ionic substance in solution;
5) chemical potential of an electrolyte in solution;
6) electrochemical potential of ions in solution;
7) chemical potential of the solvent.

8. Phase equilibria – single-component systems
1) phase transitions of the first and second kind;
2) theoretical description of a phase transition of the first kind;
3) phase diagram and characteristic points;
4) thermal analysis;
5) Gibbs phase rule;
6) examples of phase diagrams

9. Phase equilibria – binary systems
1) Gibbs phase rule;
2) solutions of volatile liquids (fractional distillation, azeotropic solutions);
3) phase diagrams of liquid-liquid systems;
4) phase diagrams of liquid-solid systems;
5) thermal analysis;
6) phase diagrams of systems containing amphiphilic compounds.

10. Phase equilibria – ternary systems
1) Gibbs phase rule;
2) Gibbs triangle;
3) examples of phase diagrams;
4) Nernst partition law.

11. Solutions – colligative properties
1) lowering the vapor pressure above the solution (Raoult's law, Henry's law);
2) increasing the boiling point, lowering the freezing point;
3) osmotic pressure, osmometry.

12. Solutions – solubility of substances
1) dissolution (effect of the molecular structure of the substance);
2) solubility product, the effect of various factors on the solubility of the substance.

13. Electrolyte solutions – equilibrium
1) methods for determining activity coefficients – discussion of the isopiestic method;
2) Debye–Hückel theory (ion cloud, ionic cloud thickness, Debye–Hückel limiting law);
3) equilibria in electrolyte solutions (ion product of water, Brønsted-Lowry theory of acids and bases, acid dissociation constants, bases);
4) ampholytes (ordinary, zwitterionic, isoelectric point);
5) acid-base titration;
6) buffers, buffer capacity;
7) acid-base indicators;

14. Chemical reactions – thermodynamics
1) free enthalpy of reaction;
2) spontaneity of reaction;
3) coupled reactions;
4) chemical equilibrium constants;
5) influence of T, p on equilibrium constants,
6) Le Chatelier-Braun's rule of contradiction.

15. Chemical kinetics, part 1
1) rate of chemical reaction;
2) kinetic laws;
3) order of reaction;
4) elementary reaction, molecularity;
5) irreversible n-order reactions, n = 0, 1, 2; differential and integral equations, half-life;
6) reversible reactions and equilibrium;
7) series reactions;
8) parallel reactions;
9) creation of differential equations for several interrelated reactions;
10) determination of the order of reaction;
11) experimental techniques;
12) collision theory;
13) theory of absolute reaction rate;
14) derivation of kinetic equations;
15) equilibrium approximation;
16) Lindemann-Christiansen mechanism;
17) chain reactions;
18) branched chain reactions, explosions;
19) oscillatory reactions;
20) photochemical reactions.

16. Chemical Kinetics, Part 2: Catalysis
1) Types of Catalysis;
2) Homogeneous Catalysis;
3) Enzymatic Reactions;
4) Competitive Inhibition in Enzymatic Catalysis;
5) Heterogeneous Catalysis;
6) Adsorption;
7) Langmuir-Hinshelwood Kinetics;
8) Catalyst Deactivation.

17. Surface phenomena
1) interfacial layer;
2) surface tension, interfacial;
3) curved surfaces;
4) wetting;
5) surface films;
6) adsorption at the liquid-gas interface;
7) adsorption on the surface of solids.

18. Viscosity
1) definition of viscosity;
2) viscosity of solutions - related quantities;
3) viscosity average molecular weight;
4) flow in a capillary - Hagen-Poiseuille equation;
5) measurement of viscosity;
6) rheological behavior of materials.

19. Intermolecular interactions
1) interactions between ions;
2) interactions between permanent dipoles - Keesom energy;
3) interactions between induced dipoles - Debye energy; 4) interactions between electrically neutral molecules – dispersion energy (London energy),
5) atomic repulsion forces;
6) interparticle interactions

20. Electrochemistry: transport in electrolyte solutions

1) ion transport equation (Nernst-Planck equation) and its components, diffusion coefficient, mobility;
2) basic quantities (current density, electrolytic conductivity, ion transference number, electrolyte molar conductivity);
3) determination of electrolyte conductivity, conductometric probe constant;
4) dependence of electrolytic conductivity, molar conductivity on electrolyte concentration;
5) Debye-Hückel-Onsager theory of electrolyte conductivity;
6) Wien effects;
7) measurement of ion transference number using Hittorf's method; 8) electrolyte diffusion (Fick's I and II laws).

21. Equilibrium electrochemistry: galvanic cells
1) cells, half-cells;
2) half-reactions and total reactions of a cell;
3) Stockholm convention.
4) types of electrodes, types of half-cells;
5) notation of cells and half-cells;
6) series of standard half-cell potentials;
7) thermodynamic description of an electrochemical cell;
8) Nernst equation;

22. Electrochemistry: current flow
1) exchange current and Butler-Volmer equation;
2) overvoltage in electrolysis;
3) Tafel equations.

23. Electrochemical corrosion.