C3401 Physical Chemistry I

Faculty of Science
Autumn 2002
Extent and Intensity
2/0/0. 2 credit(s) (fasci plus compl plus > 4). Recommended Type of Completion: zk (examination). Other types of completion: k (colloquium).
Teacher(s)
prof. RNDr. Jan Vřešťál, DrSc. (lecturer)
Guaranteed by
prof. RNDr. Jan Vřešťál, DrSc.
Chemistry Section – Faculty of Science
Prerequisites
General chemistry, mathematics (C1400, C1460)
Course Enrolment Limitations
The course is also offered to the students of the fields other than those the course is directly associated with.
fields of study / plans the course is directly associated with
Course objectives
Course of physical chemistry deals with following topics: Perfect gas and real gas. Thermodyna-mics. First law and second law of thermodynamics. Gibbs function. Surfaces. Mixtures. Phase equilibria. Chemical equilibria. Introduction to the statistical thermodynamics. Equilibrium electrochemistry. Molecular interpretation of observed phenomena is emphasized. The aim of course is to present basic knowledge, which make it possible to solve practical problems in the field of phase, chemical and electrochemical equilibria.
Syllabus
  • 1. Physical chemistry as science. Charakteristics of states of matter. Microscopic and macroscopic phenomena. Perfect and real gas and their equation of state. Mixture of gases, partial pressures, critical state, principle of corresponding states. 2. Thermodynamics. System and its surroundings. Intensive and extensive properties, thermal equilibrium, temperature, pressure, zeroth law. 3. First law and its formulation for isolated and closed system, internal energy, heat, work. State functions. Thermodynamic reversibility. Enthalpy, heat capacity at constant pressure and volume. Exo- a endothermic processes. Standard states. Hess's law. Kirchhoff's law. Joule-Thomson effect. Calorimetry. 4. Second law. Irreversible processes. Entropy. Clausius inequality. Efficiency of heat engine. Carnot cycle. Third law. 5. Gibbs and Helmholtz function. Maximum work. Gibbs-Helmholtz equation. Reaction Gibbs function. Dependence of Gibbs function on pressure and temperature. 6. Chemical potential of perfect gas. Chemical potential and its dependence on composition. Fugacity and fugacity coefficients. Phase equilibria of pure substance. Phase transformations of pure substance. General condition of phase equilibrium. 7. Dependence of chemical potential of pure component on temperature and pressure. Phase stability. Phase diagram. Clapeyron and Clausius-Clapeyron equation. Clasification of phase transformations. 8. Surfaces. Surface energy. Bubbles, holes, drops, capillary action. Mixtures. Partial molar properties. Gibbs-Duhem equation. Raoult's and Henry's laws. Thermodynamics of mixing. Activities and activity coefficients, excess functions. Liquid solutions. 9. Colligative properties, ebulioscopy, cryoscopy. Phase equilibria in polycomponent systems. Gibbs phase rule. Izobaric phase diagrams of binary systems liquid-liquid and liquid-solid. Systems with chemical compound. Ternary phase diagrams. 10. Chemical equilibria. Dependence of Gibbs function on extent of reaction. Equilibrium constant and its dependence on pressure and temperature. Le Chatelier principle. Tabulated values of state functions. 11. Introduction to statistical thermodynamics. Configuration and its weight. Microstates and macrostates. Schroedinger equation and its solution. Energetic states of molecules. Boltzmann distribution, mole-cular partition function and its relation to internal energy and en-tropy. Canonical ensamble and its partition function. Sackur-Tetrode equation. Translational, rotational, vibrational and electronic con-tribution to partition function. Calculation of equilibrium constant. 12. Equilibrium electrochemistry. Equilibria in the ionic solutions. Activities of ions in solutions. Debye-Hückel theory of strong electrolytes, ionic atmosphere, ionic strenght. Solubility product. 13. Electrochemical cells. Galvanic and electrolytic cells. Standard electrode potential. Daniel cell. Electrodes, electromotive force and potentials of electrodes. Nernst equation. 14. Redox potentials. Liquid junctions and membrane potential. Thermodynamics of electrochemical cells. Dependence of electromotive force of cell on temperature, calculation of thermodynamic functions of reaction in the cell. pH and its measurement.
Literature
  • ATKINS, P. W. Physical chemistry. 6th ed. Oxford: Oxford University Press, 1998, 1014 s. ISBN 0198501013. info
Assessment methods (in Czech)
Výuka probíhá týdně, ukončení je písemnou (řešení příkladů) a ústní zkouškou.
Language of instruction
Czech
Further comments (probably available only in Czech)
The course can also be completed outside the examination period.
The course is taught annually.
The course is taught: every week.
Listed among pre-requisites of other courses
The course is also listed under the following terms Autumn 1999, Autumn 2000, Autumn 2001, Autumn 2003, Autumn 2004.
  • Enrolment Statistics (Autumn 2002, recent)
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