546-0855/01 – Physical chemistry (FCh)
Gurantor department | Department of Environmental Engineering | Credits | 5 |
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 | 2019/2020 | Year of cancellation | |
Intended for the faculties | HGF | Intended for study types | Bachelor |
Subject aims expressed by acquired skills and competences
- define thermodynamic quantities and thermodynamic laws
- be able to use basic thermodynamic quantities (enthalpy, entropy, Gibbs energy) to describe system behavior
- describe chemical equilibria - follow the equilibrium constant dependence on external factors (influence of temperature, pressure)
- describe phase equilibria - conditions of phase equilibrium, Gibbs phase law, phase equilibria of pure substances to define and use basic concepts of chemical kinetics - reaction of homogeneous and heterogeneous, rate of chemical reaction, kinetic equations, reaction order, rate constant
- monitor the dependence of reaction rate on temperature, pressure
describe basic elements of heterogeneous reactions - diffusion, adsorption; determination of the limiting link of a heterogeneous process
- apply the theoretical knowledge gained in theoretical exercises
Teaching methods
Lectures
Tutorials
Summary
The course covers elementary parts of physical chemistry (basic concepts and quantities, state behavior, fundamentals of thermodynamics) followed by topics from the field of phase equilibria, chemical equilibrium equilibria, selected parts of properties and behavior of systems containing electrolytes and description of chemical reaction rates.
Compulsory literature:
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. Mc Gill 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
Assesment methods and criteria linked to learning outcomes: Course-unit credit is awarded on the basis of point evaluation of individual calculation works (can be corrected max. Once). Repairs will be made in the credit week. Graded credit: - min. points 13 - credit of max. points 33. Evaluation of the exam: the minimum number of points necessary to obtain the exam is 27 points The maximum number of points earned on the exam is 67 points. The evaluation of the subject is obtained by the sum of points for the exercises and for passing the exam. The final classification is given by the conditions in the Study and Examination Regulations of VŠB TUO.
E-learning
Other requirements
Active participation in the lectures and the seminars, demonstration of
successful processing subtasks, entered continuously in the semester.
Elaboration of the calculation protocol.
Prerequisities
Subject has no prerequisities.
Co-requisities
Subject has no co-requisities.
Subject syllabus:
1. Physical chemistry, its meaning and basic division. Ideal and real gases.
2. Chemical thermodynamics. Heat capacities, heating and cooling of substances, selected thermodynamic concepts,
3. 1st theorem of thermodynamics, internal energy, enthalpy, heat of reaction and its dependence on temperature. Application of the 1st theorem of thermodynamics to an ideal gas, work of an ideal gas.
4. 2nd theorem of thermodynamics - Carnot's circular process, entropy, its interpretation and its dependence on state variables. Helmholtz and Gibbs energy, relationships between thermodynamic quantities, criteria for thermodynamic equilibrium, partial molar quantities, chemical potential, activity.
5. Chemical equilibria homogeneous and heterogeneous, equilibrium constant, reaction isotherm, Le Chatelier-Braun principle.
6. Phase equilibria - phase equilibrium conditions, Gibbs phase law, one component systems, two component systems, classification of solutions, ideal and real solutions.
7. Colligative properties - solutions of non-volatile substances. Binary liquid mixtures of immiscible, limitingly miscible and immiscible components.Partition equilibria - extraction.
8. Chemical kinetics - classification of reactions, basic concepts (reaction rate in homogeneous and heterogeneous systems, order of reaction, molecularity of reaction, mechanism of aggregate reaction).
9. Integrated kinetic equations of isolated reactions. Rate constant and its dependence on temperature. Basic elements of heterogeneous reactions.
10.Electrochemistry - electrolytes and electrolytic dissociation. Strong electrolytes - activity, activity coefficient, Debye - Hückel theory. Solubility product.
11.Equilibria in solutions of weak electrolytes - dissociation of weak acids and bases, hydrolysis of salts, buffers. Electrolysis, conversion numbers, electrical conductivity of electrolytes. Potentials in electrochemistry, electrodes, galvanic cells.
12.Colloid chemistry - classification of dispersion systems, degree of dispersion, particle size distribution function. Selected kinetic, electrical and optical properties of dispersion systems.
13.Heterogeneous dispersion systems (lyophobic salts, emulsions, foams, aerosols).
Conditions for subject completion
Occurrence in study plans
Occurrence in special blocks
Assessment of instruction