1. Introduction. Gases. Ideal gases, fundamental laws. Real gases, compressibility factor, virial coefficients, critical state, 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's and Langmuir´s isotherms, BET model of adsorption isotherm.
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's and Langmuir´s isotherms, BET model of adsorption isotherm.