| Course Unit Code | 651-2011/01 |
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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 * | First Year |
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| Semester when the Course Unit is delivered | Summer 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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| R1E37 | doc. Ing. Lenka Řeháčková, Ph.D. |
| Summary |
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| The subject regards chemical thermodynamics - thermodynamic quantities and laws, chemical and physical equilibria, solutions and their properties. |
| Learning Outcomes of the Course Unit |
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- Acquire knowledge of basic principles of physical chemistry, define thermodynamic quantities (internal energy, enthalpy, entropy, Gibbs and Helmholtz energy), explain laws of thermodynamics,
- describe chemical equilibria and determine influencing factors (temperature, pressure, inert component, the concentration of reactants),
- characterize phase equilibria in single and multi-component systems,
- define solutions, their thermodynamic functions, properties and laws.
- verify the validity of selected physicochemical laws in laboratory exercises,
- apply the obtained knowledge and skills to practical cases.
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| Course Contents |
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- Gaseous state - general characteristics. Description of thermodynamics state of ideal and real gases using equations of state. Condensation of gases - definition, conditions, critical point, practical application of gas condensation. Joule-Thomson effect, Joule-Thomson coefficient and its dependence on temperature, inverse temperature, practical use.
- Definition of selected thermodynamic terms. Formulation and analysis of the first law of thermodynamics, its consequences, internal energy, enthalpy. Heat capacities - definitions, types, mutual differences, changes with temperature and during a chemical reaction. Pressure–volume work of ideal and real gas in isochoric, isobaric, isothermal and adiabatic processes.
- Thermodynamic definitions of molar heats, heating and cooling of substances including isothermal phase transformations. Thermochemistry - definitions of selected terms, thermochemical laws (Lavoisier and Laplace's law, Hess' law) and their practical use. Calculation of heat of reaction and its dependence on temperature - Kirchhoff's equations, practical applications. Calculation of maximum adiabatic temperature, enthalpy balance in dependence on a change of reaction conditions, practical use.
- Formulation and analysis of the second law of thermodynamics and its consequences. Thermal machines, Carnot heat engine, thermodynamic efficiency, Carnot cycle. General characteristics of equilibrium states - definition, types, description using appropriately chosen quantities. Entropy, its interpretation and dependence on thermodynamic state variables (adiabatic and isothermal process, entropy change with temperature, pressure and volume, during chemical reaction including isothermal phase transformations).
- Thermodynamic potentials - Gibbs, Helmholtz energy, relations between thermodynamic quantities. Dependence of Gibbs and Helmholtz energy on temperature – the Gibbs-Helmholtz equation, derivation, analysis, meaning, conditions of thermodynamic equilibrium. Maxwell's relations. Partial molar quantities, chemical potential, activity.
- Chemical equilibria, conditions for chemical equilibrium, physicochemical description of equilibrium states. Equilibrium constants - definition, types, meaning, use, their mutual conversion. Equations of reaction isotherm, application of equations to individual systems. Degree of dissociation.
- Factors that affect chemical equilibrium - the influence of temperature (equation of reaction isobar and isochore), pressure, inert component and concentration of reactants.
- Phase equilibria and their description. Gibbs phase rule, the phase diagram of a one-component system, Clapeyron and Clausius - Clapeyron equations.
- Phase equilibria in multicomponent systems. Solutions and their classification. Definition of solution composition, description of solutions using empirical laws, Raoult's and Henry's law.
- Real solutions, definition of component activity in terms of various standard states. Multicomponent systems, interaction coefficients in multicomponent systems. Thermodynamic functions of solutions, differential and integral thermodynamic quantities.
- Thermodynamic models of ideal, real, regular and athermal solutions. Gibbs - Duhem equation. Dependence of activity and activity coefficient on temperature. Colligative properties of solutions and their characterization, lowering of solvent vapor pressure above solution of non-volatile substance, ebullioscopic and cryoscopic effect, osmotic pressure.
- Phase diagrams of binary liquid systems – different miscibility of components, general characteristics of phase diagrams, phase diagrams of totally miscible liquids. Distillation - simple distillation, rectification, isothermal and isobaric distillation, practical use.
- Phase diagrams of partially miscible liquids, phase diagrams in binary systems with immiscible liquids, ternary systems (characterization). Distribution equilibria, material balance, the importance of extraction and its application. Phase diagrams for three-component systems. Basic properties of ternary phase diagrams for liquid systems.
The content of theoretical exercises will be in accordance with the syllabus.
A Lab exercise:
1. Laboratory task: Phase diagram of a three-component system
2. Laboratory task: Determination of partial molar volumes in binary liquid solutions
3. Laboratory task: Thermal decomposition of calcium carbonate
4. Laboratory task: Degree of association and equilibrium constant of electrolytic dissociation of benzoic acid
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| Recommended or Required Reading |
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| Required Reading: |
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[1] Levine, I., Physical chemistry 6th Edition, McGraw-Hill, New York, 2008
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[1] Moore, W. J., Fyzikální chemie: příručka pro vysoké školy chemickotechnologické, SNTL, Praha, 1981
[2] Kellö, V., Tkáč, A., Fyzikálna chémia: vysokoškolská učebnica, Alfa, Bratislava, 1977
[3] Novák, J. a kol. Fyzikální chemie: bakalářský a magisterský kurz. VŠCHT, Praha, 2008
[4] Peřinová, K., Smetana, B., Zlá, S., Kostiuková, G., Teoretické základy fyzikální chemie v příkladech, VŠB, Ostrava, 2018
[5] Atkins, P., de Paula, J., Physical Chemistry 9th Edition, Oxford University Press, New York, 2010
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| Recommended Reading: |
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| [1] Levenspiel, O., Chemical Reaction Engineering 3rd Edition, John Wiley & Sons, USA, 1999 |
[1] Brdička, R., Základy fysikální chemie: vysokoškolská učebnice 2. vyd., Academia, Praha, 1977
[2] Silbey, R. J., Alberty, R. A., Bawendi, M. G., Physical chemistry 4th Edition. Wiley, USA, 2004
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| Planned learning activities and teaching methods |
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| Lectures, Individual consultations, Tutorials, Experimental work in labs |
| 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 | 36 | 18 |
| Examination | Examination | 64 | 33 |