Physical Chemistry 1200-1CHMCHFW4

The lecture is divided into three parts, covering topics in thermodynamics, kinetics, and electrochemistry.
Course content:
Thermodynamics
Subject of chemical thermodynamics, the concept of a physical system and surroundings, basic concepts of classical mechanics. Ideal gas, state parameters. Quantum model of an ideal gas. Internal energy. Number of microstates (thermodynamic probability), entropy. Boltzmann distribution, internal energy of an ideal gas, entropy of an ideal gas.
Sackur–Tetrode equation. Thermal equilibrium – thermodynamic definition of temperature; mechanical equilibrium – thermodynamic definition of pressure; equilibrium related to component exchange – thermodynamic definition of chemical potential. Concept of a total differential, total differential of entropy and internal energy.
First law of thermodynamics. Heat, work, volume work. Examples of reversible and irreversible processes. Second law of thermodynamics, entropy production.
Internal energy and process heat. System in contact with surroundings at constant pressure – enthalpy. Enthalpy and process heat. Thermodynamic functions of a chemical reaction. Relationship between reaction internal energy and reaction enthalpy.
System in contact with surroundings at constant temperature – Helmholtz free energy. System in contact with surroundings at constant temperature and pressure – Gibbs free energy. Free energy and spontaneity of processes. Gibbs free energy and spontaneity of processes. Legendre transformation. New thermodynamic functions as Legendre transforms of internal energy.
Partial derivatives of thermodynamic functions, Maxwell relations. Internal energy as a function of temperature and volume. Enthalpy as a function of temperature and pressure. Relationship between Cp and Cv. Entropy as a function of (T,V) and (T,p). Thermodynamic functions of an ideal gas. Calculation of reaction heat from thermodynamic data. Calorimetric measurements. Determination of substance entropy.
Chemical potential, molar chemical potential. Relationship between (molar) chemical potential and Gibbs free energy. Thermodynamic functions of an open system. Extensive and intensive quantities. Changes in Gibbs free energy during a chemical reaction. Condition of chemical equilibrium. Law of mass action, van’t Hoff equation.
Chemical kinetics
Reaction rate – definition, rate equations, rate constant, differential form of rate equations. Solutions of differential equations for 0th-, 1st-, 2nd-, and nth-order reactions, half-life.
Writing rate equations for complex reactions. Parallel, consecutive, and equilibrium (reversible) reactions.
Steady-state approximation (consecutive reaction, consecutive reaction with pre-equilibrium). Enzyme kinetics in the Michaelis–Menten model. Temperature dependence of the rate constant.
Electrochemistry
Ideal and real solutions. Ion–ion interactions in electrolyte solutions (elements of the Debye–Hückel theory). Ion–solvent interactions in electrolyte solutions (Born theory). Interactions of ions with an external electric field (Ohm’s law, specific and molar conductivity of electrolyte solutions, ionic mobility, dependence of specific and molar conductivity on electrolyte concentration).
Electron transfer processes in solution, electron transfer in the presence of a conducting phase (metal), electrode at equilibrium (electrode redox potential). Deviation of the electrode from equilibrium – kinetically and diffusion-controlled processes. Galvanic cells (cell diagram and notation rules, electromotive force, relationship between EMF and the thermodynamic functions of the cell reaction).

Type of course

obligatory courses

Mode

Classroom

Prerequisites (description)

The aim of the lecture is to familiarize students with selected areas of physical chemistry, such as thermodynamics, kinetics, and electrochemistry. The main emphasis is placed on the correct understanding of fundamental physicochemical concepts and laws, as well as the ability to explain, on their basis, selected phenomena observed in the surrounding world, including those related to biology and medicine. Total student workload: 3 × 30 = 90 hours Participation in classes: 30 hours Sectional tests: 4 hours Preparation for classes: 45 hours Consultations with the instructor: 11 hours

Course coordinators

Maciej Mazur

Learning outcomes

The student knows and understands:
- at an advanced level, the concepts and consequences of chemical transformations resulting from the laws of thermodynamics; knows and understands the fundamentals of physical chemistry in the areas of thermodynamics, thermochemistry, electrochemistry, interfacial phenomena, transport processes, and chemical kinetics, including the phenomena of catalysis and biocatalysis (K_W06)
- at an advanced level, the aspects of construction and operation of modern measuring instruments supporting scientific research in chemistry, biochemistry, and molecular biology (K_W18)
- at an advanced level, the principles of occupational health and safety sufficient for work in a chemical, biochemical, and molecular biology laboratory (K_W19)

The student is able to:
- solve theoretical problems as well as plan and carry out simple experimental studies in the field of chemical thermodynamics, thermochemistry, chemical kinetics, catalysis and biocatalysis, electrochemistry, interfacial phenomena, and transport processes (K_U06)
- plan and perform basic research, experiments, observations, and computer simulations in the fields of chemistry, biochemistry, and molecular biology, as well as critically evaluate their own results and discuss measurement errors (K_U15)
- design, assemble, and operate selected measuring instruments, perform measurements of selected physicochemical quantities, determine their values, and assess the reliability of the obtained results (K_U16)

Assessment criteria

Attending classes is compulsory. Two unexcused absences are allowed (in the case of more absences, a sick leave is required).

The lecture is divided into two blocks, which end with written partial tests. Partial tests are assessed as follows: I - 20 points, II - 20 points, so a total of 40 points can be obtained. A student who has obtained at least 38 points in the partial tests will be released from the exam with 5! grade. The rest of the participants take the entire material for the exam - the maximum number of points that can be obtained for the exam is 60. The score for the entire course is the sum of the points for the partial tests and the exam - a maximum of 40 + 60 = 100 points.

Points are converted into a grade as follows:
0 - 50.00 - N / A
50.01 –60.00 - 3
60.01 –70.00 - 3 +
70.01 –80.00 - 4
80.01 –90.00 - 4 +
90.01 –100.00 - 5

In the event of failure to complete the course, the student takes a written exam on the entire material (in the re-sit session). The maximum number of points in the re-sit examination is 100. Points are converted into the grade in the same way as above.

Practical placement

not applicable

Bibliography

1. Atkins, P.W., et al., Chemia fizyczna. 2016: Wydawnictwo Naukowe PWN SA.
2. Pigoń, K., Ruziewicz, Z., Chemia fizyczna: Podstawy fenomenologiczne. 1. 2007: Wydawnictwo Naukowe PWN.
3. Hołyst, R., A. Poniewierski, A. Ciach, Termodynamika dla chemików, fizyków i inżynierów. 2005: Wydawnictwo Uniwersytetu Kardynała Stefana Wyszyńskiego.
4. Shroeder D.V., An introduction to thermal physics. 2000: Addison Wesley Longman.
5. Jackowska, K., Repetytorium – Elektrochemia, 2017: Wydział Chemii UW, Zakład Dydaktyczny Chemii Fizycznej.

Additional information

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

Description of 1200-1CHMCHFW4 in USOSweb