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.
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.