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ECTS Course Overview



Physical Chemistry

* Exchange students do not have to consider this information when selecting suitable courses for an exchange stay.

Course Unit Code651-2201/02
Number of ECTS Credits Allocated8 ECTS credits
Type of Course Unit *Optional
Level of Course Unit *First Cycle
Year of Study *
Semester when the Course Unit is deliveredWinter Semester
Mode of DeliveryFace-to-face
Language of InstructionEnglish
Prerequisites and Co-Requisites Course succeeds to compulsory courses of previous semester
Name of Lecturer(s)Personal IDName
DOB30prof. Ing. Jana Dobrovská, CSc.
DOC01Ing. Simona Zlá, Ph.D.
Summary
The topic of the subject is Chemical Thermodynamics (thermodynamical description of the systems and processes, chemical and phase equilibria) and Chemical Kinetics (rate analysis of homogeneous and heterogeneous reactions).
Learning Outcomes of the Course Unit
- to utilize the fundamental thermodynamic quantities (enthalpy, entropy, Gibbs energy) for the system behaviour describing;
- to describe the chemical equilibrium, to illustrate the influence of temperature and pressure;
- to describe the phase equilibrium, the Gibbs phase rule, phase equilibrium of pure substances;
- to define and to utilize basic terms of chemical kinetics - rate of chemical reaction, rate law and rate constants, reaction order. To illustrate the temperature dependence of reaction rates;
- to describe basic processes of heterogeneous reactions – diffusion, adsorption
- to determine the rate-limiting step for heterogeneous processes
- to apply obtained theoretical knowledge in tutorials and laboratory and on selected processes of chemical practice.
Course Contents
Lectures:
1. The subject introduction. Chemical thermodynamics – the First Law. Heat capacity and its temperature dependence. The conservation of energy. Internal energy and enthalpy. The standard enthalpy. Temperature dependence of enthalpy.
2. Chemical thermodynamics – application of the First Law. Chemical change: reaction enthalpies, enthalpies of combustion, standard enthalpies of formation, the variation od reaction enthalpy with temperature. Physical change: the enthalpy of phase transition.
3. Chemical thermodynamics – the Second Law: Entropy. Entropy and the Second Law. The direction of spontaneous change. The entropy accompanying heating, cooling and a phase transformation. The standard reaction entropy and the spontaneity of chemical reactions.
4. Chemical thermodynamics – the Second Law: the Gibbs energy. Properties of the Gibbs energy. Combination of the First and the Second Law. The variation of the Gibbs energy with pressure and temperature.
5. Chemical thermodynamics – application of the Second Law: the properties of mixture. Partial molar properties. Chemical potential and the equilibrium in heterogeneous systems.
6. Chemical thermodynamics – application of the Second Law: chemical equilibrium. The reaction Gibbs energy. Reactions in equilibrium – the equation of reaction isotherm. Equilibrium constants, expression for homogeneous and heterogeneous chemical reactions. The effect of temperature on chemical equilibrium.
7. Chemical thermodynamics – application of the Second Law: physical equilibria. The phase rule and its application for a one-component system. Phase diagram of pure substance, the triple point. Clapeyron and Clausius Clapeyron equation.
8. Chemical kinetics – reaction rates. The definition of rate, rate laws and constants. Reaction order. The determination of the rate law. First-order integrated rate laws, half-life.
9. Chemical kinetics – reaction mechanisms and the temperature dependence of reaction rates. Elementary reactions. Consecutive reactions. The formulation of rate laws. The rate-determining step. The Arrhenius equation, the Arrhenius parameters. The effect of catalyst.
10. Chemical kinetics – heterogeneous kinetics: diffusion. Physical and chemical steps of heterogeneous process. Diffusion, the Fick’s Laws. Diffusion coefficient, effect of temperature, effect of viscosity in fluids. The rate determining step – reaction control, diffusion control.
11. Chemical kinetics – heterogeneous kinetics: adsorption. Physisorption and chemisorption. Adsorption isotherms, the Freundlich and Langmuir isotherm.

Laboratory:
Laboratory 1: Determination of partial molar quantities.
Laboratory 2: Determination of calorimeter heat capacity.
Laboratory 3: Determination of temperature dependence of pressure of saturated vapours of the liquid and of its molar enthalpy of vaporization.
Laboratory 4: Thermal dissociation.

Recommended or Required Reading
Required Reading:
1. DOBROVSKA, J. Physical Chemistry (The Basics of Chemical Thermodynamics and Chemical Kinetics), VSB-Technical University of Ostrava, 2020.
2. ATKINS, P. W. a Julio DE PAULA. The elements of physical chemistry. 5th ed. Oxford: Oxford University Press, 2009. ISBN 978-0-19-922672-6.
1. Studijní opora: DOBROVSKÁ, Jana. Fyzikální chemie (základy chemické termodynamiky a kinetiky), VŠB-TUO, 2019, dostupné z https://www.vsb.cz/e-vyuka/
2. Studijní opora: PEŘINOVÁ, Kristina, Bedřich SMETANA, Simona ZLÁ a Gabriela KOSTIUKOVÁ. Teoretické základy fyzikální chemie v příkladech [online] 2008. Dostupné z: dostupné z https://www.vsb.cz/e-vyuka/
3. NOVÁK, Josef. Fyzikální chemie: bakalářský kurz. Praha: Vysoká škola chemicko-technologická [Praha], 2006. ISBN 80-7080-559-5.
4. ATKINS, P. W. a Julio DE PAULA. The elements of physical chemistry. 5th ed. Oxford: Oxford University Press, 2009. ISBN 978-0-19-922672-6.
Recommended Reading:
1. ATKINS, P. W. a Julio DE PAULA. Atkins' Physical chemistry. 10th ed. Oxford: Oxford University Press, c2014. ISBN 978-0-19-969740-3.
1. MOORE, Walter J. Fyzikální chemie. Praha: SNTL - Nakladatelství technické literatury, 1981.
2. KELLÖ, Vojtech a Alexander TKÁČ. Fyzikálna chémia. 3. upr. vyd. Bratislava: Alfa, 1977.
3. FISCHER, Oldřich. Fyzikální chemie: (termodynamika, elektrochemie, kinetika, koloidní soustavy). Praha: Státní pedagogické nakladatelství, 1984.
4. ADAMCOVÁ, Zdenka. Příklady a úlohy z fyzikální chemie. Praha: SNTL - Nakladatelství technické literatury, 1989. ISBN 80-03-00104-8.
5. NOVÁK, Josef. Fyzikální chemie: bakalářský a magisterský kurz. (První a druhý svazek). Praha: Vydavatelství VŠCHT, 2008. ISBN 978-80-7080-675-3. Dostupné též z: https://vydavatelstvi.vscht.cz/katalog/publikace?uid=uid_isbn978-80-7080-675-3
6. ATKINS, P. W. a Julio DE PAULA. Atkins' Physical chemistry. 10th ed. Oxford: Oxford University Press, c2014. ISBN 978-0-19-969740-3.
Planned learning activities and teaching methods
Lectures, Individual consultations, Tutorials, Experimental work in labs
Assesment methods and criteria
Tasks are not Defined