| Course Unit Code | 651-2201/02 |
|---|
| Number of ECTS Credits Allocated | 8 ECTS credits |
|---|
| Type of Course Unit * | Optional |
|---|
| Level of Course Unit * | First Cycle |
|---|
| Year of Study * | |
|---|
| Semester when the Course Unit is delivered | Winter Semester |
|---|
| Mode of Delivery | Face-to-face |
|---|
| Language of Instruction | English |
|---|
| Prerequisites and Co-Requisites | Course succeeds to compulsory courses of previous semester |
|---|
| Name of Lecturer(s) | Personal ID | Name |
|---|
| DOB30 | prof. Ing. Jana Dobrovská, CSc. |
| DOC01 | Ing. 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 |