1. Introduction: Physical Chemistry from the viewpoint of major applications for analytical chemistry and technology used in environmental engineering. Basic terminology, thermodynamic system, thermodynamic process, state properties. Substances and their systems. Chemical and physical phenomena. Expressing condition and composition of the system.
2. States of matter: State gas - the ideal gas, a mixture of ideal gases, real gases and their state behavior, critical state, and gas liquefaction.
3. State liquid - state behavior of liquids, vapor pressure above the liquid surface tension, viscosity. Solid phase - crystal structure, X-ray analysis, lattice defects, band model solids.
4. Equilibrium Thermodynamics: Selected thermodynamic concepts, heat capacity, I.věta thermodynamics. Internal energy. Volume work. Reversible and irreversible process. Adiabatic process. Heat capacity. Enthalpy.
5. Thermochemistry. Calorimetry. Application of the first sentence on the thermodynamic ideal gas, ideal gas work. II.věta thermodynamics. Thermal machines.
6. Entropy and its dependence on pressure and temperature. Helmholtz and Gibbs energy. Gibbs energy dependence on pressure and temperature.
7. Thermodynamic equilibrium. Helmholtz and Gibbs energy relations between the thermodynamic variables, criteria of thermodynamic equilibrium, partial molar quantities, chemical potential, activity.
8. Chemical equilibria: homogeneous and heterogeneous system. Terms of chemical equilibrium. Reaction isotherm. The equilibrium constant, the possibility of its expression and its dependence on p, T.
9. Principle of moving equilibrium. Le Chatelier's principle. Possibilities of influencing the yield of chemical reactions. Chemical equilibrium in non-ideal systems.
10. Phase Equilibrium: Conditions of phase equilibrium. Chemical potential. Gibbs Law of phases. Phase diagrams of one-component systems. Phase transformations. Clapeyron and Clausius-Clapeyron equation.
11. Solutions and multicomponent systems: classification solution, ideal and real, thermodynamic functions solutions. Raoult law and its consequences. Osmotic pressure. Solubility of solids. Henry's law.
12. Phase diagrams of binary systems: solid - liquid, liquid - liquid (or unlimited. Partially miscible, immiscible), solid - solid (miscible or immiscible in the solid phase, the formation of compounds in solid phase). Distillation, rectification, steam distillation, crystallization intermittent.
13. Colligative properties - Solutions solids. Binary mixtures unlimitedly miscible liquid, sparingly miscible and immiscible components.
14. Partition equilibrium, Nernst distribution law, extraction, simpler and more complex distributive balance.
2. States of matter: State gas - the ideal gas, a mixture of ideal gases, real gases and their state behavior, critical state, and gas liquefaction.
3. State liquid - state behavior of liquids, vapor pressure above the liquid surface tension, viscosity. Solid phase - crystal structure, X-ray analysis, lattice defects, band model solids.
4. Equilibrium Thermodynamics: Selected thermodynamic concepts, heat capacity, I.věta thermodynamics. Internal energy. Volume work. Reversible and irreversible process. Adiabatic process. Heat capacity. Enthalpy.
5. Thermochemistry. Calorimetry. Application of the first sentence on the thermodynamic ideal gas, ideal gas work. II.věta thermodynamics. Thermal machines.
6. Entropy and its dependence on pressure and temperature. Helmholtz and Gibbs energy. Gibbs energy dependence on pressure and temperature.
7. Thermodynamic equilibrium. Helmholtz and Gibbs energy relations between the thermodynamic variables, criteria of thermodynamic equilibrium, partial molar quantities, chemical potential, activity.
8. Chemical equilibria: homogeneous and heterogeneous system. Terms of chemical equilibrium. Reaction isotherm. The equilibrium constant, the possibility of its expression and its dependence on p, T.
9. Principle of moving equilibrium. Le Chatelier's principle. Possibilities of influencing the yield of chemical reactions. Chemical equilibrium in non-ideal systems.
10. Phase Equilibrium: Conditions of phase equilibrium. Chemical potential. Gibbs Law of phases. Phase diagrams of one-component systems. Phase transformations. Clapeyron and Clausius-Clapeyron equation.
11. Solutions and multicomponent systems: classification solution, ideal and real, thermodynamic functions solutions. Raoult law and its consequences. Osmotic pressure. Solubility of solids. Henry's law.
12. Phase diagrams of binary systems: solid - liquid, liquid - liquid (or unlimited. Partially miscible, immiscible), solid - solid (miscible or immiscible in the solid phase, the formation of compounds in solid phase). Distillation, rectification, steam distillation, crystallization intermittent.
13. Colligative properties - Solutions solids. Binary mixtures unlimitedly miscible liquid, sparingly miscible and immiscible components.
14. Partition equilibrium, Nernst distribution law, extraction, simpler and more complex distributive balance.