619-3001/01 – Advanced Physical Chemistry (VKFCH)

Gurantor departmentDepartment of Physical Chemistry and Theory of Technological ProcessesCredits7
Subject guarantorprof. Ing. Kamila Kočí, Ph.D.Subject version guarantorprof. Ing. Bedřich Smetana, Ph.D.
Study levelundergraduate or graduateRequirementCompulsory
Study languageCzech
Year of introduction2015/2016Year of cancellation2019/2020
Intended for the facultiesFMTIntended for study typesFollow-up Master
Instruction secured by
LoginNameTuitorTeacher giving lectures
ZAL041 Ing. Monika Kawuloková, Ph.D.
PER40 RNDr. Kristina Peřinová
VIT155 Ing. Silvie Rosypalová, Ph.D.
SME06 prof. Ing. Bedřich Smetana, Ph.D.
Extent of instruction for forms of study
Form of studyWay of compl.Extent
Full-time Credit and Examination 3+3

Subject aims expressed by acquired skills and competences

- to observe and describe thermodynamic conditions of phase equilibrium in multiphase and multicomponent systems - to define solutions - experience laws, thermodynamic quantities and models of solutions - to determine partial molar quantities - to analyse phase diagrams of binary liquid mixtures - to apply thermodynamic quantities to electrolyte solutions - to outline usage possibilities of electrochemical systems - description of electrochemical systems, electrodes, electrolysis, galvanic cells - to apply obtained theoretical knowledge in tutorials and laboratory and on selected processes of chemical practice

Teaching methods

Individual consultations
Experimental work in labs


Thermodynamics of solution – non-electrolyte solutions (empirical laws, ideal, dilute and real solutions, partial molar quantities, thermodynamics functions and models) colligative properties, phase diagrams - binary liquid miscible and immiscible mixtures. Properties of electrolytes (acid, base, salt, buffer) and electrochemical heterogeneous systems (electrodes, galvanic cells). Description and application of electrochemical methods. Thermodynamics of real gas mixtures.

Compulsory literature:

[1] ATKINS,P.W. Physical Chemistry. Fourth Edition, Oxford: Oxford University Press, 1993. 995 p.

Recommended literature:

[1] ATKINS,Peter; De Paula,Julio. Elements of Physical chemistry. Fifth Edition. Oxford: University of Oxford, 2009. 578s. [2] BAGOTSKY, V. S. Fundamentals of Electrochemistry, Second Edition. Hoboken, N.J: John Wiley, 2006. 722 p. Elektronická verze: http://onlinelibrary.wiley.com/book/10.1002/047174199X

Way of continuous check of knowledge in the course of semester

Podmínky pro získání zápočtu: - 100 % účast na teoretických cvičeních - 2 body - účast na teoretických cvičeních menší než 86% (více než 1 neúčast) poskytuje možnost neudělení zápočtu - úspěšné absolvování dvou samostatných výpočtových písemek – hodnocení (14 + 14) = max. 28 bodů - oprava písemky – lze opravit maximálně jednu písemku maximálně jedenkrát. - absolvování 5 laboratorních cvičení, odevzdání a obhájení protokolů – max. 15 bodů (toto bodové ohodnocení představuje hodnocení jak vlastní teoretické přípravy na zadanou laboratorní úlohu, tak hodnocení práce v laboratoři a hodnocení obsahové a formální stránky laboratorního protokolu včetně jeho obhajoby) Bodové hodnocení zápočtu: - zápočet min. bodů 20 - zápočet max. bodů 45 V celkovém zisku bodového ohodnocení zápočtu musí být obsaženo nenulové hodnocení obou výpočtových písemek (min. 5 bodů za 1 písemku) a laboratorního cvičení (min. 8 bodů), tzn. student musí absolvovat obě výpočtové písemky a splnit podmínky laboratorního cvičení (musí absolvovat 5 laboratorních úloh). Bodové hodnocení zkoušky: zkouška kombinovaná - písemná část zkoušky - max. 15 bodů - teoretická část zkoušky - max. 40 bodů V celkovém zisku bodového ohodnocení zkoušky musí být obsaženo jak nenulové hodnocení výpočtové zkouškové písemky (min. 5 bodů) tak nenulové hodnocení vlastní ústní zkoušky, tzn. student musí absolvovat obě části zkoušky. Bodové hodnocení předmětu se získá součtem bodů za cvičení a za absolvování zkoušky, výsledná klasifikace je dána podmínkami ve Studijním a zkušebním řádu VŠB TUO.


Other requirements

No other activities are required.


Subject has no prerequisities.


Subject has no co-requisities.

Subject syllabus:

1. Solutions and their classification. Nonelectrolyte solutions, ideal and real solutions. Experience laws - Raoult´s and Henry´s laws. Non-ideal solutions, definition of the standard states for component in binary solutions, deviation from Raoult´s and Henry´s law, activity and activity coefficient. Multicomponents systems, activities and interaction coefficients. 2. Thermodynamic functions of solutions. Partial molar quantities. Differential and integral quantities. Mixing and excess quantities. Determination of partial molar quantities. Thermodynamic models of solutions – ideal, real, regular and athermal solution. The Gibbs-Duhem equation, applications. The dependence of the activity and the activity coefficient on temperature. 3. Colligative properties of nonelectrolyte solutions. Vapor pressure lowering (decrease in the boiling pressure at constant temperature), boiling point elevation (ebullioscopy), freezing point depression (cryoscopy), osmotic pressure. Phase diagrams of two-component liquid mixtures (isothermal diagram, isobaric diagram, y-x diagram, miscible liquids, partially miscible liquids, totally immiscible liquids). 4. Distillation, simple distillation, rectification, azeotropic points, azeotropic mixtures, explaining the deviations. Phase diagram of the liquid ternary systems. Three-component system containing two liquid phases, Nernst’s distribution law, extraction. Electrochemistry, basic terms. Electrolytes and ions, strong electrolyte, weak electrolyte, ion charge number, theory of electrolytic dissociation, dissociation constant, degree of dissociation. 5. Electrolysis and its significance, Faraday’s laws, reactions occurring during electrolysis, concentration changes during electrolysis. Coulometers. Cation and anion transport numbers, cation and anion mobility, Hittorf method of determining transport numbers. 6. Electric conductivity of electrolytes. Specific and molar electric conductivity, concentration dependence Molar conductivity at infinite dilution, theory of ionic conductivity, Kohlrausch’s law of independent migration of ions. Conductivity measurement and its utilization - Ostwald´s dilution law, determination of solubility product, conductometric titrations. 7. Strong electrolyte. Deviation from ideal state. Osmotic coefficient. Mean molality, concentration, activity and activity of electrolyte. Ionic strength of a solution, Debye-Hückel limiting law, activity coefficients at higher concentrations. Conduction coefficient, electrophoretic effect, relaxation effect. Solubility of sparingly soluble salts, solubility product. 8. Equilibrium and dissociation in solutions of weak electrolytes. Ionic product of water. Theory of acids and bases (Brönsted´s, Arrhenius and Lewis theory). Classification of solvents. Determination of pH, acidobasic indicators. Dissociation of week monobasic acids and bases. Hydrolysis of the salt. Buffer solutions, Henderson–Hasselbalch equation, buffer capacity, signification. 9. Electrodes. Electrochemistry potentials - electrode and redox potentials, liquid junction and membrane potentials. Classification of half-cells, description, function, utilization of electrodes - first-type electrodes, second-type electrodes, reduction-oxidation electrodes, ion-selective electrodes. 10. Galvanic cells, classification, electromotive force of the cell and its measurement. Chemical cells (cells with transference, cells without transference), electrode and electrolyte and concentration cells (cells with transference, cells without transference). Electromotive force and thermodynamic quantities. 11. Theory of liquid junction potential. Electromotive force of galvanic cells with liquid junction potential. Significance of galvanic cells. Electrochemistry power sources. 12. Potentiometry. Direct potentiometry – pH determination, determination of solubility product, activity coefficients and dissociation constants. Potentiometric titrations, equivalence point. 13. Electrode processes. Electrode polarization. Chemical and concentration polarization, elimination, significance. Decomposition voltage, overvoltage. Hydrogen overvoltage, Tafel equation, Butler–Volmer equation, mechanism of hydrogen deposition. Oxygen overvoltage. Basic aspects of polarography and electrochemical corrosion. 14. Real gases. Equations of state, theorem of corresponding states, compressibility factor, compressibility diagram. Thermodynamics of liquids.

Conditions for subject completion

Full-time form (validity from: 2015/2016 Winter semester, validity until: 2019/2020 Summer semester)
Task nameType of taskMax. number of points
(act. for subtasks)
Min. number of points
Credit and Examination Credit and Examination 100 (100) 51
        Credit Credit 45 (45) 20
                Laboratorní práce Laboratory work 15  0
                Písemka Written test 28  0
                Jiný typ úlohy Other task type 2  0
        Examination Examination 55 (55) 15
                Písemná zkouška Written examination 15  5
                Ústní zkouška Oral examination 40  10
Mandatory attendence parzicipation:

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Occurrence in study plans

Academic yearProgrammeField of studySpec.ZaměřeníFormStudy language Tut. centreYearWSType of duty
2019/2020 (N3909) Process Engineering (2805T019) Chemical and environmental engineering P Czech Ostrava 1 Compulsory study plan
2018/2019 (N3909) Process Engineering (2805T019) Chemical and environmental engineering P Czech Ostrava 1 Compulsory study plan
2017/2018 (N3909) Process Engineering (2805T019) Chemical and environmental engineering P Czech Ostrava 1 Compulsory study plan
2016/2017 (N3909) Process Engineering (2805T019) Chemical and environmental engineering P Czech Ostrava 1 Compulsory study plan
2015/2016 (N3909) Process Engineering (2805T019) Chemical and environmental engineering P Czech Ostrava 1 Compulsory study plan

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