| Course Unit Code | 619-0809/03 |
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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 * | Second Cycle |
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| Year of Study * | First 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 | |
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| Prerequisities | Course Unit Code | Course Unit Title |
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| 619-0403 | Physical Chemistry Fundamentals of Combustion and Explosion Processes |
| Name of Lecturer(s) | Personal ID | Name |
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| DOB30 | prof. Ing. Jana Dobrovská, CSc. |
| DUD32 | doc. Ing. Rostislav Dudek, Ph.D. |
| SME06 | prof. Ing. Bedřich Smetana, Ph.D. |
| Summary |
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Application of the physico-chemical laws on the processes of combustion,
explosion and extiguishing. |
| Learning Outcomes of the Course Unit |
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- to define the thermodynamic quantities and thermodynamic laws
- to describe the chemical equilibrium – to monitor the dependence of the equilibrium
constant on state variables (dependence on temperature, dependence on pressure) –
to utilize Le Chatelier’s principle (effect of initial composition, pressure and inert
component on the equilibrium composition)
- to describe the phase equilibrium - Gibbs phase rule, phase equilibria of pure
substances and liquid-vapour equilibrium in mixtures
- to define and apply basic principles of chemical kinetics - rate of chemical reaction,
kinetic equation, order of reaction, rate constant, the theory of reaction rates
- to describe basic steps of heterogeneous process - physical processes limiting
kinetics of heterogeneous processes, diffusion, the Fick's first and second law,
adsorption, adsorption isotherms
- to apply the chemical thermodynamics a kinetics on the processes of combustion,
explosion and extinguishing
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| Course Contents |
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Gases, ideal gas, equation of state of an ideal gas, special cases, real gases, Van der Waals equation of state, Abel equation.
Heat capacities of substances – definition, variation of heat capacities with temperature, difference in the molar heat capacities between the products and reactants.
The First law of thermodynamics, definition, signification, constant pressure heat, constant volume heat, enthalpy. Heating and cooling of substances.
Heats of reaction. Thermochemistry laws, theoretical calculation of reaction heats. Heats of combustion. Heat of explosion.
Variation of the reaction heat with temperature - Kirchhoff’s equations and their utilization. Adiabatic reaction temperature.
The second law of thermodynamics, entropy. Thermodynamic potentials – Helmholtz and Gibbs free energy, significance and application.
Chemical equilibriums, types of equilibrium constants for homogeneous nad heterogeneous chemical reactions. Van´t Hoff reaction isotherm. Degree of conversion. Effect of temperature on chemical equilibrium.
Phase equilibrium. Evaporation of pure liquid. Clausius-Clapeyron equation.
Solutions, Raoult’s law.
Chemical kinetics, basic terms - rate of chemical reaction, law of mass action, (Guldberg-Waage law), molecularity, order of reaction, reaction mechanism.
Kinetics of first-order reactions, reaction half-life.
Temperature and pressure dependence of the rate of a chemical reaction. Effect of concentration on reaction rates.
Kinetics of heterogeneous chemical reactions - elementary reaction steps in heterogenous process, diffusion, laws of diffusion.
Adsorption, adsorption of gases on solid surfaces, Freundlich adsorption isotherm.
Mechanism of burning reaction, theory of chain reactions, theory of thermal spontaneous ignition.
Ignition limit, first, second and third pressure ignition limit.
Heterogeneous and homogeneous combustion. Kinetic and diffusion combustion.
Adiabatic (theoretical) flame temperature.
Combustible composition and burning products. Specific combustion heat and specific caloric power.
Combustion of fuels. Amount of oxygen and air for combustion. Mechanism of explosive transformations.
Explosive hazards. Theory of extinguishing.
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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.
Warnatz,J., Maas,U., Dibble,R.W., Combustion. Physical and Chemical
Fundamentals, Modelling and Simulation, Experiments, Pollutant Formation.
Springer-Verlag Berlin Heidelberg New Uork. 1996. 265 p.
|
Kalousek,J.:Základy fyzikální chemie hoření, výbuchu a hašení. Edice SPBI
Spektrum, Ostrava, 2000 (II. vydání)
Kalousek.J. – Dobrovský, Ľ. : Základy fyzikální chemie. Ostrava, VŠB 1985. 155 s.
Atkins,P.W., Physical Chemistry. Fourth Edition, Oxford: Oxford University Press, 1993. 995 p.
|
| Recommended Reading: |
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Warren Strahle C., An Introduction to Combustion. Gordon and Breach Science
Publishers. Combustion Science and Technology Book Series.Volume 1. 1993. 166p.
|
Warnatz,J., Maas,U., Dibble,R.W., Combustion. Physical and Chemical
Fundamentals, Modelling and Simulation, Experiments, Pollutant Formation.
Springer-Verlag Berlin Heidelberg New Uork. 1996. 265 p.
Warren Strahle C., An Introduction to Combustion. Gordon and Breach Science
Publishers. Combustion Science and Technology Book Series.Volume 1. 1993. 166p.
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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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| Exercises evaluation and Examination | Credit and Examination | 100 (100) | 51 |
| Exercises evaluation | Credit | 38 (38) | 12 |
| Written exam | Written test | 36 | 0 |
| Other task type | Other task type | 2 | 0 |
| Examination | Examination | 62 (62) | 16 |
| Written examination | Written examination | 12 | 4 |
| Oral | Oral examination | 50 | 12 |