1. Introduction. Gases. Ideal gases, fundamental laws. Real gases, compressibility factor, virial
coefficients, critical point,Van der Waals equation of state, theorem of corresponding states.
2. The chemical thermodynamics. Basic terms, thermodynamic system, thermodynamic properties,
thermodynamic process, thermodynamic state functions. Heat capacities of substances, variation of
heat capacities with temperature, difference in the molar heat capacities between the products and
reactants. The First law of thermodynamics, definition, signification. The work done by ideal gas. The
heat at constant pressure and volume. The fundamental thermodynamic function – enthalpy. The
thermodynamic definition of molar heat capacities.
3. The heating and cooling of substances. The heat of reaction. Laws of thermochemistry, theoretical
calculation of reaction heat. Kirchhoff’s law - variation of the reaction enthalpy with temperature. The
adiabatic reaction temperature.
4. The Second law of thermodynamics – definition and signification. The heat engine, Carnot heat engine.
The fundamental thermodynamic function – entropy (temperature and volume dependence for
homogeneous system, temperature and pressure dependence for a homogeneous system). The
statistical interpretation of entropy.
5. Thermodynamic potentials – Helmholtz and Gibbs free energy. Conditions of thermodynamic
equilibrium. Combined formulations of the first and second laws of thermodynamics, Maxwell relations.
The Gibbs and Helmholtz free energy – temperature dependence, Gibbs-Helmholtz equations,
significance and application.
6. Partial molar quantities – definition, properties. The Gibbs-Duhem equation. The chemical potential
and its significance. Chemical equilibrium. Conditions for chemical equilibrium. The Van´t Hoff
reaction isotherm, thermodynamic equilibrium constant. Types of equilibrium constant for
homogeneous and heterogeneous chemical reactions.
7. The calculation of equilibrium composition and degree of conversion. The effect of temperature on
chemical equilibrium, Van't Hoff reaction isochore and isobare . The effect of pressure on chemical
equilibrium. The Le Chatelier’s principle.
8. The phase equilibrium. The Gibbs phase rule, phase, state of aggregation, component, degree of
freedom. The phase diagram of a one-component system, triple point and critical point. Phase
equilibrium of pure substances, Clapeyron and Clausius-Clapeyron equation.
9. Two-component (binary) system. The third law of thermodynamics. Nernst's theorem, Planck's
postulate.
10. The chemical kinetics, significance. Homogeneous simple reactions. Basic terms, rate of chemical
reaction, order of reaction, molecularity, rate constant, reaction mechanism. First-order reactions,
reaction half-life, second-order reactions, nth-order reactions.
11. The mechanism of simultaneous chemical reactions, reversible, parallel and consecutive reactions,
mathematic analysis.
12. The temperature dependence of the rate of a chemical reaction, Arrhenius equation. The theory of
chemical kinetics - collision theory and theory of absolute reaction rates. The effect of pressure on
reactions rate.
13. Kinetics of heterogeneous chemical reactions, elementary steps in heterogenous reactions. The
molecular diffusion, Fick’s laws of diffusion, consecutive and parallel diffusion, principles of
analysis. The convection diffusion.
14. The adsorption, physical adsorption and chemisorption. Adsorption from gases on solids. Adsorption
isotherms, Freundlich and Langmuir isotherms, BET model of adsorption.
coefficients, critical point,Van der Waals equation of state, theorem of corresponding states.
2. The chemical thermodynamics. Basic terms, thermodynamic system, thermodynamic properties,
thermodynamic process, thermodynamic state functions. Heat capacities of substances, variation of
heat capacities with temperature, difference in the molar heat capacities between the products and
reactants. The First law of thermodynamics, definition, signification. The work done by ideal gas. The
heat at constant pressure and volume. The fundamental thermodynamic function – enthalpy. The
thermodynamic definition of molar heat capacities.
3. The heating and cooling of substances. The heat of reaction. Laws of thermochemistry, theoretical
calculation of reaction heat. Kirchhoff’s law - variation of the reaction enthalpy with temperature. The
adiabatic reaction temperature.
4. The Second law of thermodynamics – definition and signification. The heat engine, Carnot heat engine.
The fundamental thermodynamic function – entropy (temperature and volume dependence for
homogeneous system, temperature and pressure dependence for a homogeneous system). The
statistical interpretation of entropy.
5. Thermodynamic potentials – Helmholtz and Gibbs free energy. Conditions of thermodynamic
equilibrium. Combined formulations of the first and second laws of thermodynamics, Maxwell relations.
The Gibbs and Helmholtz free energy – temperature dependence, Gibbs-Helmholtz equations,
significance and application.
6. Partial molar quantities – definition, properties. The Gibbs-Duhem equation. The chemical potential
and its significance. Chemical equilibrium. Conditions for chemical equilibrium. The Van´t Hoff
reaction isotherm, thermodynamic equilibrium constant. Types of equilibrium constant for
homogeneous and heterogeneous chemical reactions.
7. The calculation of equilibrium composition and degree of conversion. The effect of temperature on
chemical equilibrium, Van't Hoff reaction isochore and isobare . The effect of pressure on chemical
equilibrium. The Le Chatelier’s principle.
8. The phase equilibrium. The Gibbs phase rule, phase, state of aggregation, component, degree of
freedom. The phase diagram of a one-component system, triple point and critical point. Phase
equilibrium of pure substances, Clapeyron and Clausius-Clapeyron equation.
9. Two-component (binary) system. The third law of thermodynamics. Nernst's theorem, Planck's
postulate.
10. The chemical kinetics, significance. Homogeneous simple reactions. Basic terms, rate of chemical
reaction, order of reaction, molecularity, rate constant, reaction mechanism. First-order reactions,
reaction half-life, second-order reactions, nth-order reactions.
11. The mechanism of simultaneous chemical reactions, reversible, parallel and consecutive reactions,
mathematic analysis.
12. The temperature dependence of the rate of a chemical reaction, Arrhenius equation. The theory of
chemical kinetics - collision theory and theory of absolute reaction rates. The effect of pressure on
reactions rate.
13. Kinetics of heterogeneous chemical reactions, elementary steps in heterogenous reactions. The
molecular diffusion, Fick’s laws of diffusion, consecutive and parallel diffusion, principles of
analysis. The convection diffusion.
14. The adsorption, physical adsorption and chemisorption. Adsorption from gases on solids. Adsorption
isotherms, Freundlich and Langmuir isotherms, BET model of adsorption.