546-0855/01 – Physical chemistry (FCh)

Gurantor departmentDepartment of Environmental EngineeringCredits5
Subject guarantordoc. Mgr. Eva Pertile, Ph.D.Subject version guarantordoc. Mgr. Eva Pertile, Ph.D.
Study levelundergraduate or graduateRequirementCompulsory
Study languageCzech
Year of introduction2019/2020Year of cancellation
Intended for the facultiesHGFIntended for study typesBachelor
Instruction secured by
LoginNameTuitorTeacher giving lectures
PER34 doc. Mgr. Eva Pertile, Ph.D.
Extent of instruction for forms of study
Form of studyWay of compl.Extent
Part-time Credit and Examination 8+8

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

Experimental work in labs


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:

ATKINS, P. W. a Julio DE PAULA. Atkins' physical chemistry. 9th ed. Oxford: Oxford University Press, c2010. ISBN 9780199543373.

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.


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.


Subject has no prerequisities.


Subject has no co-requisities.

Subject syllabus:

Physical chemistry, its importance and basic classification. Ideal and real gases. Chemical thermodynamics. Heat capacities, heating and cooling of substances, selected thermodynamic terms, 1st thermodynamic theorem, internal energy, enthalpy, reaction heat and its dependence on temperature. Application of the 1st law of thermodynamics to ideal gas, work of ideal gas. 2nd thermodynamic theorem - Carnot circle process, entropy, its interpretation and its dependence on state variables. Helmholtz and Gibbs energy, relations between thermodynamic quantities, criteria of thermodynamic equilibrium, partial molar quantities, chemical potential, activity. Homogeneous and heterogeneous chemical equilibria, equilibrium constant, reaction isotherm, Le Chatelier-Braun principle. Phase equilibria - conditions of phase equilibrium, Gibbs phase law, one-component systems, two-component systems, classification of solutions, ideal and real solutions. Colligative properties - solutions of non-volatile substances. Binary liquid mixtures of unlimited miscible, limited miscible and immiscible components. Partition equilibrium - extraction. Chemical kinetics - classification of reactions, basic concepts (reaction rate in homogeneous and heterogeneous systems, reaction order, reaction molecularity, aggregate reaction mechanism). Integrated kinetic equations of isolated reactions. Rate constant and its dependence on temperature. Basic elements of heterogeneous reactions. Electrochemistry - electrolytes and electrolytic dissociation. Strong electrolytes - activity, activity coefficient, Debye - Hückel theory. Solubility product. Equilibria in solutions of weak electrolytes - dissociation of weak acid and base, hydrolysis of salts, buffers. Electrolysis, gear numbers, electrical conductivity of electrolytes. Potentials in electrochemistry, electrodes, galvanic cells. Colloid chemistry - classification of dispersion systems, dispersion degree, particle size distribution function. Selected kinetic, electrical and optical properties of dispersion systems. Heterogeneous dispersion systems (lyophobic salts, emulsions, foams, aerosols).

Conditions for subject completion

Part-time form (validity from: 2019/2020 Winter semester)
Task nameType of taskMax. number of points
(act. for subtasks)
Min. number of pointsMax. počet pokusů
Credit and Examination Credit and Examination 100 (100) 51
        Credit Credit 33 (33) 15
                Výpočtový protokol Other task type 33  15
        Examination Examination 67  30 3
Mandatory attendence participation: The scope of compulsory education for the combined form of study is 8 h of lectures and 8 h exercises.

Show history

Conditions for subject completion and attendance at the exercises within ISP: As part of the ISP, the student is obliged to participate in individual consultations, which will be conducted in the form of a discussion on the topics studied. Exercise: The student submits a calculation report.

Show history

Occurrence in study plans

Academic yearProgrammeField of studySpec.ZaměřeníFormStudy language Tut. centreYearWSType of duty
2022/2023 (B0712A290001) Waste Management and Mineral Processing K Czech Ostrava 2 Compulsory study plan
2022/2023 (B0712A290001) Waste Management and Mineral Processing K Czech Most 2 Compulsory study plan
2021/2022 (B0712A290001) Waste Management and Mineral Processing K Czech Ostrava 2 Compulsory study plan
2021/2022 (B0712A290001) Waste Management and Mineral Processing K Czech Most 2 Compulsory study plan
2020/2021 (B0712A290001) Waste Management and Mineral Processing K Czech Most 2 Compulsory study plan
2020/2021 (B0712A290001) Waste Management and Mineral Processing K Czech Ostrava 2 Compulsory study plan
2019/2020 (B0712A290001) Waste Management and Mineral Processing K Czech Ostrava 2 Compulsory study plan
2019/2020 (B0712A290001) Waste Management and Mineral Processing K Czech Most 2 Compulsory study plan

Occurrence in special blocks

Block nameAcademic yearForm of studyStudy language YearWSType of blockBlock owner

Assessment of instruction

2021/2022 Winter
2020/2021 Winter