Fundamentals of physical chemistry 0600-S1-ChK-ChF

Basics of equilibrium thermodynamics: principles of thermodynamics, criteria of system behavior. Chemical potential of the component. States of matter. Balance of chemical reaction. Equilibrium of phase transitions. Properties of gases, liquids and solids. Chemical kinetics: basic concepts, mechanisms and kinetic equations of reaction. Catalysis. Surface phenomena and dispersion systems. Conductivity of electrolytes. Galvanic cells, half-cells. Electrochemical corrosion.

Laboratory content:
Experimental determination of selected physicochemical quantities and interpretation of the obtained results. Experimental determination of thermodynamic quantities - changes in process enthalpy. Characteristics of the liquid phase (viscosity). Phase equilibria (Gibbs triangle, Nernst law). Experimental determination of reaction rate constants in the presence of a homo- and heterogeneous catalysts. Determination of adsorption isotherms. Measurement of conductivity of electrolyte solutions. Half-cells and galvanic cells, solubility product of sparingly soluble salts.

Program content of calculus exercises
1. Calculations of work and heat in simple physical transformations, heat capacity,
2. The concept of state functions, calculations of changes in internal energy and enthalpies of physical transformations, 1st law of thermodynamics,
3. Changes in internal energy and enthalpy in chemical reactions, heat of reaction, formation and combustion reactions, Hess's law,
4. Dependence of the heat of reaction on temperature - Kirchhoff's law
5. Chemical kinetics - calculations of the rate constant and progress of elementary reactions, parallel and successive reactions, dependence of the reaction rate on temperature - Arrhenius equation
6. Electrochemistry - conductivity of electrolytes, Ostwald's dilution law, emf of cells, Nernst equation, calculation of changes in thermodynamic functions based on emf of cells.

Total student workload

1. 30 h lecture, 60 h laboratory, 15 h exercises, 25 h consultations, total 130 contact hours, 2. 35 h individual work, 3. 60 hours of time required for preparation in the assessment process, 4. the total student workload is 225 hours.

Learning outcomes - knowledge

W1. Knows the basics of physical chemistry (W01) W2. Knows the basics of mathematical analysis and statistics necessary to describe and model chemical phenomena (W02) W3. Knows the role of experiment in chemical processes (W03)

Learning outcomes - skills

U1. Uses concepts from the field of physical chemistry (U01) U2. Has the ability to describe chemical phenomena (U02) U3. Has the ability to perform measurements of basic chemical quantities and is able to develop the results of chemical experiments (U03)

Learning outcomes - social competencies

K1. Analytical thinking: works independently and effectively with large amounts of information, notices relationships and correctly draws conclusions using the principles of logic (K01) K2. Creativity: thinks creatively to improve existing or create new solutions (K02) K3. Conscientiousness and accuracy: is focused on completing the task as best as possible; cares about detail; is systematic (K03) K4. Striving for development: is focused on constantly acquiring new knowledge, skills and experiences; sees the need for continuous improvement and improvement of professional competences; knows the limitations of his own knowledge and understands the need for further education (K05) K5. Teamwork: Establishes and maintains long-term and effective cooperation with others; strives to achieve team goals by appropriately planning and organizing the work of oneself and others; motivates co-workers to increase their effort in order to achieve the set goals (K09)

Teaching methods

Lecture Lecture supported by PP presentations Laboratory: Physicochemical experiments performed by 2 people, under the guidance of the teacher, physicochemical calculations, discussion of the results.

Expository teaching methods

- informative (conventional) lecture

Exploratory teaching methods

- practical
- seminar
- laboratory
- round table

Type of course

compulsory course

Prerequisites

Basic knowledge of general chemistry, analytical chemistry, mathematics and computer science.

Course coordinators

Term 2022/23Z:

Piotr Adamczak
Wojciech Kujawski

Term 2024/25Z:

Piotr Adamczak
Stanisław Koter

Term 2023/24Z:

Piotr Adamczak
Stanisław Koter

Term 2021/22Z:

Piotr Adamczak
Wojciech Kujawski

Assessment criteria

Lecture: written exam – W1, W2, U1, U2
Laboratory: assessment based on completed laboratory exercises and studies, mid-semester tests - W1, W3, U1, U2, U3, continuous student assessment during classes - K1, K2, K3, K4, K5.

Exam topics:
1. Features of gas, liquid and solid. Description of the states of matter (pressure, temperature, amount of substance). Ideal and real gases. Kinetic theory of gases. Equations of state of an ideal and real gas. Liquids: surface tension and viscosity of liquids.
2. Basic concepts in thermodynamics: system, surroundings, work and heat, thermodynamic functions, first law of thermodynamics, internal energy and enthalpy, enthalpy of chemical reactions, Hess's law, second law of thermodynamics, process entropy, reaction entropy and spontaneous reaction, free enthalpy of the process , free enthalpy of reaction and spontaneous reaction, standard free enthalpy, molar partial quantities, chemical potential, fugacity, activity.
3. Gibbs phase rule, phase diagrams of typical substances (water, carbon dioxide, carbon and helium), phase diagrams of two- and three-component systems, properties of non-electrolyte solutions (ideal and real solutions, colligative properties of solutions, activity coefficient, osmotic coefficient).
4. The concept of the ratio and constant of chemical equilibrium, description of the influence of external conditions on the state of equilibrium.
5. Basic concepts in kinetics (reaction rate, reaction rate constant, reaction order, molecularity, kinetic equation). Reaction kinetic equations. Differential and integral kinetic equations. Kinetics of simple reactions. Kinetics of reactions involving a catalyst. Enzymatic reactions, Michaelis-Menten mechanism.
6. Conductivity of electrolyte solutions, strong and weak electrolytes. The influence of electrolyte concentration on its conductivity. Galvanic cells (types of half-cells and cells, rules for writing a half-cell diagram, half-cell potential, electromotive force of the cell and its measurement). Partial reactions in a half-cell, the cell reaction. Electrochemical corrosion (corrosion protection).
7. The concept of physical and chemical adsorption, Freundlich and Langmuir adsorption isotherms. Surface-active substances (basic structural features, influence on surface tension, excess Gibbs isotherm).

Practical placement

not applicable

Bibliography

Literature:
Basic reference materials:
P. W. Atkins, Fundamentals of Physical Chemistry, Scientific Publishing House, Warsaw 1999, 2002, 2009; in Polish, in English also available.
2. P. W. Atkins, Physical Chemistry, PWN Publishing House, Warsaw 2001, 2003, 2007, 2012; in Polish, in English also available.
K. Pigoń, Z Ruziewicz, Physical Chemistry, 1. Phenomenological Foundations, Wydawnictwo Naukowe PWN, Warszawa 2005, 2007; in Polish.
4. A. G. Whittaker, A. R. Mount, M. R. Heal, Physical Chemistry. Short lectures, Wydawnictwo Naukowe PWN, Warszawa 2004; in Polish, in English also available.
5. L. Sobczyk, A. Kisza, Physical Chemistry for Naturalists, PWN, Warsaw 1981; in Polish.
6. T.W. Hermann (ed.), Physical Chemistry: A Handbook for Pharmacy Students and Medical Analyzes, Medical Publishing House, Warsaw 2007; in Polish.
7. K. Sobner, A. Kisza, K. Gatner, A. Koll, Experimental Physical Chemistry, PWN, Warsaw 1982; in Polish.
8. J. Ceynowa, M. Litowska, R. Nowakowski, J. Ostrowska-Czubenko, Handbook for laboratory exercises with physical chemistry, Wydawnictwo UMK, Toruń 2006; in Polish.
9. J. Demichowicz-Pigoniowa, A. Olszowski, Physical Chemistry. T.3. Physicochemical calculations, Scientific Publishing House, Warsaw, 2010; in Polish.
10. Komorowski, A. Olszowski, Physical Chemistry. T.4. Laboratory of Physicochemistry, Scientific Publishing House, Warsaw, Poland; in Polish.
11. A. Kisza, P. Freundlich, Ćwiczenia rachunkowe z chemii fizycznej, Wyd. Uniwersytetu Wrocławskiego, Wrocław, 2004

Additional literature:

1. W. Ufnalski, Physicochemical calculations on your PC, WNT, Warsaw 1997; in Polish.
2. K.-H. Lautenschläger, W. Schröter, A. Wanninger, Modern Compendium of Chemistry, Wydawnictwo Naukowe PWN, Warszawa 2007; in Polish.
3. Series: Lectures on Physical Chemistry, WNT, Warsaw (in Polish):
a. H. Buchowski, W. Ufnalski, Physicochemistry of gases and liquids, 1998.
b. H. Buchowski, W. Ufnalski, Solutions, 1995.
c. W. Ufnalski, Chemical equilibrium, 1995.
d. H. Buchowski, W. Ufnalski, Basics of Thermodynamics, 1998.
e. A. Molski, Introduction to chemical kinetics, 2009.
f. A. Kisza, Electrochemistry I, Jonika, 2000.
g. A. Kisza, Electrochemistry II, Electrodes, 2001.
4. F. Pruchnik, Kataliza homogeniczna, PWN, Warszawa, 1993.
5. T. Engel, P. Reid, Physical Chemistry, Pearson, 3rd ed., 2013.
6. D.W. Ball, Physical Chemistry, Wadsworth, CENGAGE Learning, 2nd ed., 2015.

Additional information

Additional information (registration calendar, class conductors, localization and schedules of classes), might be available in the USOSweb system:

Description of 0600-S1-ChK-ChF in USOSweb