Physical chemistry 0600-S1-O-CFIZ
The subject of physical chemistry is carried out for 75 hours. lecture, 90 hours laboratory and 45 hours accounting exercises.
The lecture covers the following content
1. Introduction (scope of the course, mathematical foundations)
2. States of matter
3. Gases
1) gas laws,
2) ideal gas equation of state;
3) real gas equations of state (van der Waals, viral);
3) the principle of states corresponding to each other;
4) liquefaction of gases;
5) kinetic theory of gases;
6) diffusion, effusion.
4. Thermodynamics, the first law of thermodynamics
1) basic concepts (system, heat, work, energy);
2) internal energy of the system;
3) First law of thermodynamics;
4) determination of internal energy changes (calorimetric bomb), heat capacity;
5) adiabate;
6) enthalpy;
7) determination of enthalpy changes (calorimeter), heat capacity;
8) interpretation of heat capacity at the molecular level;
9) enthalpy of physical changes;
10) standard condition;
11) enthalpy of chemical reactions;
12) Hess's law;
13) Kirchhoff equation.
5. Thermodynamics, the second law of thermodynamics
1) Carnot cycle;
2) entropy (direction of the spontaneous process; entropy and the second law of thermodynamics; entropy change);
3) calculation of entropy changes;
4) absolute entropies and the 3rd law of thermodynamics;
5) entropy and spontaneity of reactions;
6) consequences of the 2nd law of thermodynamics - free energy, free enthalpy, conditions of spontaneity of the process;
6. Thermodynamics, thermodynamic functions
1) relationship between thermodynamic functions;
2) extensive and intensive values;
3) partial molar sizes;
4) important thermodynamic equations (Gibbs-Duhem equation et al.).
7. Non-ideality of gases, gas mixtures, liquid solutions
1) the chemical potential of a component of the mixture;
2) volatility and volatility coefficients (gases);
3) activity et al. Activity;
4) the chemical potential of a non-ionic substance in solution;
5) the chemical potential of the electrolyte in solution;
6) electrochemical potential of ions in solution;
7) the chemical potential of the solvent.
8. Phase equilibria - one-component systems
1) phase transitions of the 1st and 2nd kind;
2) theoretical description of the 1st kind phase transition;
3) phase diagram and characteristic points;
4) thermal analysis;
5) Gibbs rule of phases;
6) examples of phase diagrams (water, sulfur, carbon dioxide, carbon, helium).
9. Phase equilibria - two-component systems
1) Gibbs rule of phases;
2) volatile liquid solutions (fractionated distillation, azeotropic solutions);
3) phase diagrams of liquid-liquid systems;
4) phase diagrams of liquid-solid systems;
5) thermal analysis;
6) phase diagrams of systems containing amphiphilic compounds.
10. Phase equilibria - three-component systems
1) Gibbs rule of phases;
2) Gibbs triangle;
3) examples of phase diagrams;
4) Nernst's law of distribution.
11. Solutions - colligative properties
1) lowering of the vapor pressure above the solution (Raoult's law, Henry's law);
2) increasing the boiling point, lowering the freezing point;
3) osmotic pressure, osmometry.
12. Solutions - solubility of substances
1) dissolving (influence of the molecular structure of a substance);
2) the product of solubility, the influence of various factors on the solubility of the substance;
3) solubility parameter.
13. Electrolyte solutions - equilibrium
1) methods of determining activity coefficients - discussion of the isopiestic method;
2) Debye-Hückel theory (ionic atmosphere, its thickness, Debye-Hückel limiting law);
3) equilibrium in electrolyte solutions (ionic product of water, Brønsted-Lowry theory of acids and bases, dissociation constants of acid, base);
4) ampholytes (ordinary, zwitterionic, isoelectric point);
5) acid-base titration (examples of titrations of polyprotonic acids, their mixtures, mixtures with salt and base);
6) buffers, buffer capacity;
7) acid-base indicators;
14. Electrolyte solutions - transport
1) ion transport equation (Nernst-Planck equation) and its components, diffusion coefficient, mobility;
2) basic quantities (current density, electrolytic conductivity, ion transfer number, electrolyte molar conductivity);
3) determination of electrolyte conductivity, conductometric probe constant;
4) dependence of electrolytic conductivity, molar conductivity on the concentration of electrolyte;
5) Debye-Hückel-Onsager theory of electrolyte conductivity;
6) Wien's effects;
7) measuring the number of ion transfers using the Hittorf method;
8) electrolyte diffusion (Fick's law I and II).
15. Chemical reactions - thermodynamics
1) free enthalpy of reaction;
2) spontaneous reaction;
3) coupled reactions;
4) chemical equilibrium constants;
5) influence of T, p on the equilibrium constants,
6) Le Chatelier-Braun's rule of defiance.
16. Chemical reactions - kinetics, part. 1
1) the speed of the chemical reaction;
2) kinetic laws;
3) order of reaction;
4) elemental reaction, molecularity;
5) irreversible reactions of the nth order, n = 0, 1, 2; differential and integral equations, half-life;
6) reversible reactions and equilibrium;
7) series reactions;
8) parallel reactions;
9) how to create differential equations for several related reactions;
10) determining the order of the reaction;
11) experimental techniques;
12) collision theory (Lewis 1918);
13) absolute speed theory of reaction;
14) diffusion-controlled reactions;
15) deriving kinetic equations;
16) equilibrium approximation;
17) Lindemann-Christiansen mechanism;
18) chain reactions;
19) radical polymerization;
20) kinetics of copolymerization;
21) branched chain reactions, explosions;
22) combustion;
16. Chemical reactions - kinetics, part. 2 catal
1) types of catalysis;
2) homogeneous catalysis;
3) enzymatic reactions;
4) competitive inhibition in enzymatic catalysis;
5) heterogeneous catalysis;
6) adsorption;
7) Langmuir-Hinshelwood kinetics;
8) catalyst deactivation;
9) comparison of heterogeneous and homogeneous catalysis.
17. Chemical reactions - kinetics, part. 3
1) kinetics of ionic reactions;
2) oscillatory reactions;
3) photochemical reactions.
18. Surface phenomena
1) interfacial layer;
2) surface and interfacial tension;
3) curved surfaces;
4) wetting;
5) surface films;
6) adsorption at the liquid-gas interface;
7) adsorption on the surface of solids.
19. Viscosity
1) definition of viscosity;
2) viscosity of solutions - related quantities;
3) viscosity average molecular weight;
4) flow in the capillary - Hagen-Poiseuille equation;
5) viscosity measurement;
6) the rheological behavior of materials.
20. Intermolecular interactions
1) interactions between ions;
2) interactions between permanent dipoles - Keesom energy;
3) interactions between induced dipoles - Debye energy;
4) interactions between electrically neutral molecules - dispersive energy (London energy),
5) atomic repulsive forces;
6) interparticle interactions
21. Electrochemistry - cells
1) Galvanic cells (partial reactions, half-cells).
2) Electrode reactions (cell, electrolyser).
3) Stockholm Convention.
4) Standard Hydrogen Electrode.
5) Cell and half-cell notation.
6) Reduction potentials (standard redox pair potential).
7) Reversible cells and half-cells (gas half-cells, second-type half-cells, redox half-cells).
8) Thermodynamic description of an electrochemical cell.
9) Electrochemical and Nernst potential.
22. Electrochemistry - current flow
1) Exchange current and Butler-Volmer equation.
2) Overvoltage in electrolysis.
3) Tafel's equations.
23. Electrochemistry - corrosion.
1) The concept of electrochemical corrosion.
2) The iron corrosion mechanism.
3) Thermodynamic and kinetic description of metal corrosion.
4) Evan diagram.
5) Pourbaix diagram.
The laboratory exercises include the following content:
1) Exercise 1: Determination of the calorimeter constant and the heat of dilution
2) Exercise 2: Determining the thermal effect of the neutralization reaction with a differential microcalorimeter
3) Exercise 4: Ebuliometric determination of: the molar mass of non-electrolytes or the osmotic ratio of strong electrolytes
4) Exercise 5: Determining the division factor. Nernst's law
5) Exercise 6: Determining the phase diagram of a condensed two-component system by thermal analysis
6) Exercise no. 7: Determining the isotherm of solubility in a three-liquid system; The Gibbs triangle
7) Exercise no. 8: The influence of surfactants on the surface tension; Gibbs adsorption isotherm
8) Exercise 9: Determining the isotherm of adsorption from a solution
9) Exercise 10: Solute refraction
10) Exercise 11: Dependence of liquid viscosity on temperature. Determination of liquid viscosity in an Ostwald viscometer
11) Exercise number 11a: Dependence of solution viscosity on concentration
12) Exercise no. 13: Measurement of the electromotive force of cells; Determination of half-cell potentials and solubility products of silver halides
13) Exercise no. 14: Determination of changes in thermodynamic functions of the generating reaction in cells
14) Exercise 15: Entropy of mixing solutions based on SEM measurements of concentration cells
15) Exercise No. 16: Determining the dissociation constant of a weak acid from SEM measurements of cells
16) Exercise No. 17: Dependence of electric conductivity of strong electrolytes on concentration
17) Exercise number 18: Conductivity of water and weak electrolytes. Determination of the dissociation constant Ka of weak electrolytes
18) Exercise 19: Determination of the oxygen permeation rate through the air-solution interface by voltammetry with a rotating platinum electrode
19) Exercise no.20: Mercury electrocapillary curve
20) Exercise no. 21: The kinetics of ester hydrolysis in an acid medium
21) Exercise no.22: Reaction kinetics with the kinetic equation of the first order - sucrose hydrolysis
22) Exercise number 23: Kinetics of the oxidation of iodide ions with persulfate ions
23) Exercise No. 24: Determining the rate constant of the decomposition of hydrogen peroxide on a carbon catalyst
24) Exercise number 25: Finding the Tafel equation constants
25) Exercise number 27: Determination of the diffusion coefficient of substances in a two-component system
26) Exercise no. 28: Determining the Joule-Thomson ratio of a real gas
The calculation exercises include the following content:
1. Calculations of work and heat in simple physical transformations, heat capacity,
2. The concept of the state function, calculations of changes in internal energy and enthalpy of physical changes, 1st law of thermodynamics,
3. Changes in internal energy and enthalpy in chemical reactions, heat of reaction, formation and combustion reactions, Hess's law,
3. Dependence of the heat of reaction on temperature - Kirchhoff's law
4. Second law of thermodynamics - entropy calculations of simple physical processes, entropy of reactions
5. Calculation of enthalpy and free energy of physical processes and chemical reactions.
6. The state of thermodynamic equilibrium - standard affinity and equilibrium constant - the law of mass action, the influence of temperature and pressure on the state of equilibrium - defiance rule.
7. Calculation of the constants Kp, Kx, Kc
8. Chemical kinetics - calculations of the rate constant and the progress of elementary reactions, parallel and subsequent reactions, dependence
reaction rate on temperature - Arrhenius equation
9. Electrochemistry - conductivity of electrolytes, Ostwald dilution law, emf of cells, Nernst equation, calculation of changes in thermodynamic functions from emf.
Term 2020/21:
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Term 2021/22:
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Term 2022/23:
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Term 2023/24:
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Total student workload
Learning outcomes - knowledge
Learning outcomes - skills
Learning outcomes - social competencies
Teaching methods
Expository teaching methods
Exploratory teaching methods
- seminar
- round table
Type of course
Prerequisites
Course coordinators
Term 2023/24: | Term 2022/23: | Term 2020/21: | Term 2021/22: |
Bibliography
1. P.W. Atkins, Chemia Fizyczna, PWN, Warszawa, 2001,
2. K. Pigoń, Z Ruziewicz, Chemia fizyczna, 1.Podstawy fenomenologiczne, PWN, Warszawa, 2005,
3. A.G. Whittaker, A.R. Mount, M.R. Heal, Krótkie wykłady, Chemia fizyczna, PWN, Warszawa, 2003,
4. P.W. Atkins, Podstawy chemii fizycznej, PWN, Warszawa, 1999,
5. Praca zbiorowa pod red. A. Bielańskiego i in., Chemia Fizyczna, PWN, Warszawa 1980,
6. F. Pruchnik, Kataliza homogeniczna, PWN, Warszawa, 1993.
7. Seria: Wykłady z chemii fizycznej, WNT, Warszawa:
H. Buchowski, W. Ufnalski, Fizykochemia gazĂłw i cieczy, 1998;
H. Buchowski, W. Ufnalski, Roztwory, 1995;
W. Ufnalski, Równowagi chemiczne, 1995;
H. Buchowski, W. Ufnalski, Podstawy termodynamiki, 1994,1998;
A. Molski, Wprowadzenie do kinetyki chemicznej, 2001,
A. Kisza, Elektrochemia I, Jonika, 2000,
A. Kisza, Elektrochemia II, Elektrodyka, 2001,
8. T. Engel, P. Reid, Physical Chemistry, Pearson, 3rd ed., 2013.
9. D.W. Ball, Physical Chemistry, Wadsworth, CENGAGE Learning, 2nd ed., 2015.
10. L. Sobczyk, A. Kisza, K. Gatner, A. Koll, Eksperymentalna chemia fizyczna, PWN, Warszawa 1982,
11. J. Demichowicz-Pigoniowa, Obliczenia fizykochemiczne, Oficyna Wydawnicza Politechniki Wrocławskiej, Wrocław 1997,
12. W. Ufnalski, Obliczenia fizykochemiczne, OWPW, Warszawa 1995,
13. A. Kisza, P. Freundlich, Ćwiczenia rachunkowe z chemii fizycznej, Wyd. Uniwersytetu Wrocławskiego, Wrocław, 2004.
Term 2020/21:
None |
Term 2021/22:
None |
Term 2022/23:
None |
Term 2023/24:
None |
Additional information
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