651-2201/01 – Physical Chemistry (FCH)
| Gurantor department | Department of Chemistry and Physico-Chemical 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 | 2022/2023 | 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:
Additional study materials
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 - 5 points
- elaboration of the specified calculation program - 25 points
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 to the subject. Gaseous state. Ideal gas, basic laws. Behavior of real gases, compressibility factor, critical gas state, van der Waals equation. Heat capacities of substances, calculation, changes with temperature and during chemical reactions.
2. Chemical thermodynamics. Basic concepts. I. thermodynamic theorem, formulation and significance. Ideal gas work. Heat at constant pressure and volume, thermodynamic state function of enthalpy. Thermodynamic definition of molar heats. Calculation of heating and cooling of substances. Heat of reaction. Thermochemical laws, calculation of reaction heats.
3. Dependence of heat of reaction on temperature, Kirchhoff's laws and their use. Theoretical reaction temperature. II. thermodynamic theorem – formulation and significance. Heat engine, Carnot cycle. Entropy in terms of chemical thermodynamics. Entropy from the point of view of statistical thermodynamics.
4. Calculation of entropy changes under different conditions. Absolute entropy. Nernst's thermal theorem. Thermodynamic potentials – Helmholtz and Gibbs energy. Conditions for the spontaneity of processes and their balance. Affinity.
5. Relations between thermodynamic state functions, Maxwell's equations. Gibbs–Helmholtz equations and their application. Partial molar quantities - definition, properties. Gibbs–Duhem equation. Chemical potential and its meaning.
6. Chemical balances. Reaction isotherm equation. Expression of equilibrium constants for homogeneous and heterogeneous chemical reactions. Calculation of equilibrium composition, degree of conversion. The effect of temperature on the equilibrium of a chemical reaction. The effect of pressure on the equilibrium of a chemical reaction. The Le Chaterier–Braun principle.
7. Thermodynamics and mechanism of basic technological reactions: Thermal dissociation of compounds, dissociation temperature and tension. Indirect reduction of metals. Direct reduction of metals, Boudouard reaction. Topochemical reactions.
8. Phase equilibria. Gibbs phase law, phase, state, component, degree of freedom. One-component system, phase diagram, triple point. Equilibrium of a single-component two-phase system, Clapeyron and Clausius Clapeyron equations. Equilibrium of a two-component system.
9. Solutions. Classification of solutions. Solutions of non-electrolytes, ideal and real solutions. Empirical laws describing solutions – Raoult's law and Henry's law. Real solutions, choice of standard state for solution components, deviations with respect to Raoult's and Henry's law, different concepts of activity, activity coefficient. Activities and activity coefficients in multicomponent systems.
10. Thermodynamic functions of solutions. Partial molar quantities. Differential and integral quantities. Mixing and additive quantities. Thermodynamic functions and solution models – ideal, real, regular, athermal solution model. Gibbs-Duhem equation and its applications. Solubility of gases in metals.
11. Colligative properties of solutions – reduction of vapor pressure above a solution of a non-volatile substance, ebulioscopic effect, cryoscopic effect, osmotic pressure. Phase diagrams of binary liquid mixtures at different miscibility of components. Principle of distillation, rectification. Distribution equilibria, Nernst distribution law, extraction.
12. Thermodynamic conditions for the formation of nuclei of a new phase, homogeneous and heterogeneous nucleation. Crystallization from melts, driving force of crystallization.
Conditions for subject completion
Occurrence in study plans
Occurrence in special blocks
Assessment of instruction