651-2011/01 – Physical Chemistry I (FCHI)
| Gurantor department | Department of Chemistry and Physico-Chemical Processes | Credits | 5 |
| Subject guarantor | doc. Ing. Lenka Řeháčková, Ph.D. | Subject version guarantor | doc. Ing. Lenka Řeháčková, Ph.D. |
| Study level | undergraduate or graduate | Requirement | Compulsory |
| Year | 1 | Semester | summer |
| | Study language | Czech |
| Year of introduction | 2022/2023 | Year of cancellation | |
| Intended for the faculties | FMT | Intended for study types | Bachelor |
Subject aims expressed by acquired skills and competences
- 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.
Teaching methods
Lectures
Individual consultations
Tutorials
Experimental work in labs
Summary
The subject regards chemical thermodynamics - thermodynamic quantities and laws, chemical and physical equilibria, solutions and their properties.
Compulsory literature:
[1] Levine, I., Physical chemistry 6th Edition, McGraw-Hill, New York, 2008
Recommended literature:
[1] Levenspiel, O., Chemical Reaction Engineering 3rd Edition, John Wiley & Sons, USA, 1999
Way of continuous check of knowledge in the course of semester
Credit, oral and written exam
E-learning
Other requirements
Credit requirements:
- To pass subject credit requirements, students must complete two written tests and laboratory exercises.
- For two written tests, the highest score is 24 points (12 points for each test), a minimum score is 12 points (6 + 6). Each test can be repeated only once.
- Successful completion of laboratory exercises - max. 12 points, min. 6 points.
Credit points:
- min. 18 points
- max. 36 points
To obtain the credit, it is necessary to successfully pass both tests and submit all laboratory reports.
Exam points:
- written part of examination - max. 14 points, min. 7 points
- oral part of examination - max. 50 points, min. 26 points
The student must pass both parts of the exam and achieve at least a minimum number of points for their accomplishment.
The evaluation of the subject is obtained by the sum of points for the exercises and the exam. The final classification respects the Study and Examination Regulations of VŠB - TUO.
Prerequisities
Subject has no prerequisities.
Co-requisities
Subject has no co-requisities.
Subject syllabus:
- 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
Conditions for subject completion
Occurrence in study plans
Occurrence in special blocks
Assessment of instruction
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