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Lecturer(s)
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Berka Karel, doc. RNDr. Ph.D.
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Kvítek Libor, prof. RNDr. CSc.
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Course content
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1. Matter states of substances Gaseous state - ideal gas equation, ideal gas mixtures, real gases and their state behavior, critical state and liquefaction of gases. Solid state - crystal structure, X-ray analysis, crystal lattice defects, phase transformations. Liquid state - state behavior of liquids, vapor pressure over liquid, surface tension, viscosity. 2. Kinetic theory of ideal gas Gas pressure. Equipartition principle. Maxwell - Boltzmann distribution law. Intermolecular collisions. 3. Equilibrium thermodynamics - 1st theorem Theorem of thermodynamics. Volume work. Reversible and irreversible plot. Heat capacity. Enthalpie. Adiabatic action. Thermochemistry. Calorimetry. 4. Equilibrium thermodynamics - II. and III. sentence Theorem of thermodynamics. Thermal machines. Entropy and its statistical interpretation. Thermodynamic equilibrium. Helmholtz and Gibbs energy. Maxwell's equations. Dependence of Gibbs energy on pressure and temperature. Dependence of entropy on temperature. Theorem of thermodynamics. Entropy values according to the third law of thermodynamics. 5. Phase equilibria Homogeneous and heterogeneous systems and their characterization. Chemical potential. Phase rule. Phase diagrams of one-component systems. Phase transformations. Clapeyron and Clausius-Clapeyron equations. 6. Solutions and multicomponent systems Raoult's law and its consequences. Osmotic pressure. Solubility of solids. Phase diagrams of two-component systems. Three-component systems. Distribution equilibrium. Phase boundary equilibria - adsorption. 7. Chemical equilibrium Condition of chemical equilibrium. Equilibrium constant and its dependence on p, T. Reaction isotherm. Chemical equilibrium in non-ideal systems. Activity. 8. Equilibrium electrochemistry of bulk phase Faraday's laws of electrolysis. Electrolytic dissociation. Conductivity of electrolyte solutions. Activity and activity coefficient of electrolyte solutions. Ionic strength. Debye-Hückel theory. Weak electrolytes and their dissociation. Theory of acids and bases. Autoprotolysis. pH. Hydrolysis of salts. Buffers. Poorly soluble electrolytes. 9. Electrochemistry of equilibrated heterogeneous systems. Electrochemical potential. Galvanic cells. Nernst equation. Standard electrode potentials. Classification and examples of individual groups of reversible electrodes. Ion-selective electrodes. Electrode kinetics. 10. Chemical kinetics Basic concepts. Kinetic equations of 1st and 2nd order reactions. Determination of reaction order. Simultaneous reactions. Chain reactions. Influence of temperature on reaction rate. Collision theory. Theory of activated complex. Molecular dynamics. Homogeneous, heterogeneous and enzymatic catalysis. 11. Chemistry of colloidal systems Classification and description of colloidal systems. The most important properties of colloidal solutions. Phase and molecular colloids. Emulsion. Aerosols.
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Learning activities and teaching methods
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unspecified
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Learning outcomes
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The lecture is focused on an overview of the most important chapters of classical equilibrium physical chemistry with regard to practical needs of physicochemical knowledge in the field of material chemistry, analytical chemistry and other chemical branches. The main emphasis is placed on the connections between the main theses of classical physicochemical theory and practical consequences in the field of latent states, energetics of chemical reactions and electrochemistry. An important part is devoted to the chapters of chemical kinetics, either in terms of the description of the course of simple chemical reactions, including chemical catalysis.
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Prerequisites
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unspecified
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Assessment methods and criteria
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unspecified
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Recommended literature
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Atkins P., de Paula J. (2013). Fyzikální chemie. VŠCHT Praha.
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Brdička R., Dvořák J. (1977). Základy fysikální chemie. Academia Praha.
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Fischer, O. a kol. (1983). Fyzikální chemie. SPN, Praha.
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Moore, W. J. (1981). Fyzikální chemie. SNTL Praha.
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