619-2001/03 – Physical Chemistry (FCH)
Gurantor department | Department of Physical Chemistry and Theory of Technological Processes | Credits | 8 |
Subject guarantor | prof. Ing. Jana Dobrovská, CSc. | Subject version guarantor | prof. Ing. Jana Dobrovská, CSc. |
Study level | undergraduate or graduate | Requirement | Compulsory |
Year | 2 | Semester | winter |
| | Study language | Czech |
Year of introduction | 2019/2020 | Year of cancellation | |
Intended for the faculties | FMT | Intended for study types | Bachelor |
Subject aims expressed by acquired skills and competences
- 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.
Teaching methods
Lectures
Individual consultations
Tutorials
Experimental work in labs
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).
Compulsory literature:
Recommended literature:
Way of continuous check of knowledge in the course of semester
FULL-TIME STUDY
List of conditions for obtaining of credit:
- required attendance at the exercises
- two written tests
- passing the required number of laboratory exercises, elaboration and defense
of laboratory protocols.
Points scoring for credit:
Min. number of points - 20
Max. number of points - 45
Points scoring for examination - combined examination.
The examination consists of two parts - written and oral examination.
Written examination (min. number of points - 5, max. number of points - 15)
Oral examination (min. number of points - 10, max. number of points - 40)
COMBINED STUDY
List of conditions for obtaining of credit:
- required attendance at the exercise
- elaboration of the specified calculation program
Points scoring for credit:
Min. number of points - 15
Max. number of points - 30
Points scoring for examination
Oral examination (min. number of points - 25, max. number of points - 70)
E-learning
Other requirements
No other activities are required.
Prerequisities
Subject has no prerequisities.
Co-requisities
Subject has no co-requisities.
Subject syllabus:
Lectures:
1. Introduction. Gases. Ideal gases, fundamental laws. Real gases,
compressibility factor, virial coefficients, critical state, Van der Waals
equation of state, theorem of corresponding states.
2. The chemical thermodynamics. Basic terms, thermodynamic system,
thermodynamic properties, thermodynamic process, thermodynamic state
functions. Heat capacities of substances, variation of heat capacities with
temperature, difference in the molar heat capacities between the products
and reactants. The First law of thermodynamics, definition, signification.
The work done by ideal gas. The heat at constant pressure and volume.
The fundamental thermodynamic function – enthalpy. The thermodynamic
definition of molar heat capacities.
3. The heating and cooling of substances. The heat of reaction. Laws of
thermochemistry, theoretical calculation of reaction heat. Kirchhoff’s law
- variation of the reaction enthalpy with temperature. The adiabatic
reaction temperature.
4. The Second law of thermodynamics – definition and signification. The heat
engine, Carnot heat engine. The fundamental thermodynamic function –
entropy (temperature and volume dependence for homogeneous system,
temperature and pressure dependence for a homogeneous system). The
statistical interpretation of entropy.
5. Thermodynamic potentials – Helmholtz and Gibbs free energy. Conditions of
thermodynamic equilibrium. Combined formulations of the first and second
laws of thermodynamics, Maxwell relations. The Gibbs and Helmholtz free
energy – temperature dependence, Gibbs-Helmholtz equations, significance
and application.
6. Partial molar quantities – definition, properties. The Gibbs-Duhem
equation. The chemical potential and its significance. Chemical
equilibrium. Conditions for chemical equilibrium. The van´t Hoff reaction
isotherm, thermodynamic equilibrium constant. Types of equilibrium constant
for homogeneous and heterogeneous chemical reactions.
7. The calculation of equilibrium composition and degree of conversion. The
effect of temperature on chemical equilibrium, van't Hoff reaction isochore
and isobar. The effect of pressure on chemical equilibrium. The Le
Chatelier’s principle.
8. The phase equilibrium. The Gibbs phase rule, phase, component, degree of
freedom. The phase diagram of a one-component system, triple point and
critical point. Phase equilibrium of pure substances, Clapeyron and
Clausius Clapeyron equation.
9. Two-component (binary) system. The third law of thermodynamics. Nernst's
theorem, Planck's postulate.
10. The chemical kinetics, significance. Homogeneous simple reactions. Basic
terms, rate of chemical reaction, order of reaction, molecularity, rate
constant, reaction mechanism. First-order reactions, reaction half-life,
second-order reactions, nth-order reactions.
11. The mechanism of simultaneous chemical reactions, reversible, parallel and
consecutive reactions, mathematic analysis.
12. The temperature dependence of the rate of a chemical reaction, Arrhenius
equation. The theory of chemical kinetics - collision theory and theory of
absolute reaction rates. The effect of pressure on reactions rate.
13. Kinetics of heterogeneous chemical reactions, elementary steps in
heterogenous reactions. The molecular diffusion, Fick’s laws of
diffusion,
consecutive and parallel diffusion, principles of analysis. The
convection diffusion.
14. The adsorption, physical adsorption and chemisorption. Adsorption from
gases on solids. Adsorption isotherms, Freundlich's and Langmuir´s
isotherms, BET model of adsorption isotherm.
Conditions for subject completion
Occurrence in study plans
Occurrence in special blocks
Assessment of instruction