| Course Unit Code | 651-0402/02 |
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| Number of ECTS Credits Allocated | 5 ECTS credits |
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| Type of Course Unit * | Compulsory |
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| Level of Course Unit * | First Cycle |
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| Year of Study * | Second Year |
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| Semester when the Course Unit is delivered | Winter Semester |
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| Mode of Delivery | Face-to-face |
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| Language of Instruction | Czech |
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| Prerequisites and Co-Requisites | Course succeeds to compulsory courses of previous semester |
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| Name of Lecturer(s) | Personal ID | Name |
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| DOB30 | prof. Ing. Jana Dobrovská, CSc. |
| DOC01 | Ing. Simona Zlá, Ph.D. |
| ZAL041 | Ing. Monika Kawuloková, Ph.D. |
| Summary |
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The topic of the subject is chemical thermodynamics and chemical kinetics.
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| Learning Outcomes of the Course Unit |
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- to define thermodynamic quantities and thermodynamic laws
- to utilize the fundamental thermodynamic quantities (enthalpy, entropy, Gibbs
energy) for the system behaviour describing
- to describe the chemical equilibrium – to monitor the dependence of the
equilibrium constant on state variables (dependence on temperature, dependence
on pressure)
- to describe the phase equilibrium, Gibbs phase rule, phase equilibrium of pure
substances
- to define and to utilize basic terms of chemical kinetics - homogeneous and
heterogeneous reaction, rate of chemical reaction, kinetic equation, order of
reaction, rate constant
- to monitor the dependence of the reaction rate on temperature and on pressure
- to describe basic processes of heterogeneous reactions – diffusion, adsorption;
to determine the rate-limiting process for heterogeneous processes
- to apply gained theoretical knowledge in routine
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| Course Contents |
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Physical chemistry, signification, classification.
Chemical thermodynamics. Heat capacities, heating and cooling of substances. The first law of thermodynamics. Enthalpy, variation of the reaction enthalpy with temperature.
The second law of thermodynamics. Entropy and its interpretation. Helmholtz and Gibbs free energy. Chemical potential, activity.
Chemical equilibriums, equilibrium constant for homogeneous nad heterogeneous chemical reactions, Van´t Hoff reaction isotherm and isobare. The Le Chatelier’s principle.
Phase equilibrium - conditions of phase equilibrium. Gibbs phase rule, one-component system (Clapeyron and Clausius-Clapeyron equation), two-component (binary) system (ideal and real solutions, Raoult’s law and Henry’s law). Colligative properties of nonelectrolyte solutions - solutions with non-volatile solute. Phase diagram for two-component liquid mixtures (miscible liquids, partially miscible liquids, totally immiscible liquids). Distribution equilibrium.
The chemical kinetics - rate of chemical reaction, order of reaction, molecularity, rate constant, reaction mechanism. Integrated forms of the kinetic equation. The temperature dependence of the rate constant, Arrhenius equation. Kinetics of heterogeneous chemical reactions, elementary steps in heterogenous reactions.
Electrochemistry – electrolytes and theory of electrolytic dissociation. Strong electrolytes - activity and activitiy coefficient, Debye-Hückel limiting law. Solubility product. Equilibrium and dissociation in solutions of weak electrolytes - dissociation of week monobasic acids and bases, hydrolysis of salt, buffer solutions. Electrolysis, transport number, electric conductivity of electrolytes. Electrochemistry potentials, electrodes, galvanic cells.
Colloid chemistry - classification of dispersion systems, degree of dispersion. Selected kinetic, electrical and optical properties of colloid systems. Heterogeneous dispersion systems (lyophobic sols, emulsion, foam, aerosol).
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| Recommended or Required Reading |
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| Required Reading: |
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Atkins,P.W., Physical Chemistry. Fourth Edition, Oxford: Oxford University
Press, 1993. 995 p.
ATKINS,Peter; De Paula,Julio. Elements of Physical chemistry. Fifth Edition. Oxford: University of Oxford, 2009. 578s.
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DOBROVSKÁ, Jana. Fyzikální chemie - 1.část [online]. [s.l.] : [s.n.], 2008 [cit. 2010-08-15]. Dostupné z WWW: .
PEŘINOVÁ, Kristina; SMETANA, Bedřich; ZLÁ, Simona; KOSTIUKOVÁ, Gabriela. Teoretické základy fyzikální chemie v příkladech [online]. [s.l.] : [s.n.], 2008 [cit. 2010-08-15]. Dostupné z WWW: https://www.fmmi.vsb.cz/cs/katedry-a-pracoviste/619/vyukove-opory-katedry/index.html
Atkins,P.W., Fyzikálna chémia. Bratislava: STU,1999.
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| Recommended Reading: |
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Lupis,C.H.P.Chemical Thermodynamics of materials. New York, North-Holland,
1983. 581 p. |
MOORE,W.J., Fyzikální chemie. Praha: SNTL, 1979. 974 s.
KELLÖ,V., TKÁČ,A., Fyzikálna chemia. Bratislava: Alfa, 1977. 778 s.
ADAMCOVÁ,Z.a kol. Příklady a úlohy z fyzikální chemie. Praha: SNTL, 1989. 666 s.
Atkins,P. Čtyři zákony,které řídí vesmír. Praha: Academia, 2012. 99 s.
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| Planned learning activities and teaching methods |
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| Lectures, Individual consultations, Tutorials |
| Assesment methods and criteria |
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| Task Title | Task Type | Maximum Number of Points
(Act. for Subtasks) | Minimum Number of Points for Task Passing |
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| Credit and Examination | Credit and Examination | 100 (100) | 51 |
| Credit | Credit | 33 (33) | 17 |
| Písemka | Written test | 30 | 6 |
| Jiný typ úlohy | Other task type | 3 | 0 |
| Examination | Examination | 67 (67) | 18 |
| Písemná zkouška | Written examination | 16 | 5 |
| Ústní zkouška | Oral examination | 51 | 13 |