546-0507/02 – Physical Chemistry I (FCHI)
| Gurantor department | Department of Environmental Engineering | Credits | 3 |
| Subject guarantor | doc. Mgr. Eva Pertile, Ph.D. | Subject version guarantor | doc. Mgr. Eva Pertile, Ph.D. |
| Study level | undergraduate or graduate | Requirement | Compulsory |
| Year | 2 | Semester | winter |
| | Study language | Czech |
| Year of introduction | 2015/2016 | Year of cancellation | 2019/2020 |
| Intended for the faculties | HGF | Intended for study types | Bachelor |
Subject aims expressed by acquired skills and competences
The primary objective of lectures is to introduce students to the common principles of theoretical practice of different sciential discipline in a complete form, based on basic physical principles; and to broaden their knowledge about significant conclusions and applications, including current applications in science and technology. After successful completion of the course the student is expected to orient in problems of (chemical) thermodynamics and electrochemistry, their practical meaning and will be able to use acquired knowledge in other specialized courses, and also in solving application problems.
Teaching methods
Lectures
Individual consultations
Tutorials
Summary
Physical chemistry as a scientific discipline and its relations with other sciences. Utilization of physical chemistry to understand processes that influence our environment. The subject covers elementary parts of physical chemistry (basic terms and quantities, state behaviour, fundamentals of thermodynamics) which are followed by chapters of phase equlibria and chemical equilibria. The selected parts of behaviour and properties of electrolytes are introduced. The final part is devoted to kinetics of chemical reactions.
Compulsory literature:
ATKINS, Peter William - Julio de Paula. Physical chemistry for the Life Sciences. 1st ed. N.Y.: W. H. Freeman and Company, 2010, 699s. ISBN 0-1992-8065-9.
Recommended literature:
MALIJEVSKÝ A., et. al: Physical chemistry in brief. Institute of Chemical Technology, Prague, 2005. Dostupné z: http://old.vscht.cz/fch/en/tools/breviary-online.pdf.
RONIS David: Introductory Physical Chemistry I. McGill University.2015. Dostupné z: http://ronispc.chem.mcgill.ca/ronis/chem223/course_pac.pdf.
Way of continuous check of knowledge in the course of semester
Student knowledge is verified in written form, emphasis is given to understanding the subject and applying theoretical knowledge to solving practical problems. The evaluation also includes collective evaluation and self-assessment. An active assessment of the students is also included in the class. In the individual preparation, the student enriches the basic computations applied in physical chemistry on given examples. Based on the submission of the computation protocol, he / she will be awarded a credit.
E-learning
Other requirements
Elaboration of the calculation protocol.
Prerequisities
Subject has no prerequisities.
Co-requisities
Subject has no co-requisities.
Subject syllabus:
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.
Conditions for subject completion
Occurrence in study plans
Occurrence in special blocks
Assessment of instruction