Group | Type | Day | Time | Classroom | Weeks | Comment |
---|---|---|---|---|---|---|
Common | I | Monday | 10-12 | U147 | 45, 47 | |
Common | I | Tuesday | 14-16 | U10 | 46, 48 | |
Common | I | Wednesday | 14-16 | U26 | 45-48 | |
Common | I | Thursday | 12-14 | U37 | 47-48 | |
S1 | TE | Monday | 08-10 | U147 | 47 | |
S1 | TL | Monday | 14-17 | 49-51 | ||
S1 | TE | Tuesday | 14-16 | U10 | 45 | |
S1 | TE | Tuesday | 16-18 | U148 | 46 | |
S1 | TL | Wednesday | 14-17 | 49-51 | ||
S1 | TE | Thursday | 10-12 | U148 | 48 | |
S1 | TE | Friday | 08-10 | U26 | 45-47 |
• display a broad insight to the concepts of classical physical chemistry including the established models and methods,
• explain energetic quantities and their combination in the fundamental theorems of thermodynamics,
• derive simple thermodynamic relations that follow directly from the relations derived in the textbook,
• explicate the terms chemical potential and equilibrium, and be capable to use them for the deriving of relations that interrelate the changes in pressure and temperature of pure phases (phase diagrams and vapour pressure equations),
• derive relations that relate phase equilibrium with concentrations of mixtures (freezing point depression, boiling point increase, osmotic pressure and solubility) and as well the relations describing the properties of liquid mixtures (vapour pressure, laws of Raoult and Henry),
• describe the deviations of real systems from ideal behaviour using quantities as compressibility, osmotic coefficients, and activity coefficients, and calculate them either from measured quantities or from tabled data as well as know the options to convert them for simple mixtures (Gibbs-Duhem equation)
• elucidate the term “amphiphile” using a property like surface activity and explain the effect of a surface active material,
• explicate the absorption of material onto surfaces and into interfaces (Langmuir isotherm) and be able to extract the adsorption coefficient from experimental data,
• define specific conductivities, limiting conductivities, ion mobilities and transport numbers. Students shall know Kohlrausch’s law and be able to calculate transport properties of strong electrolytes from tabled data as well as the degree of dissociation of weak electrolytes from conductivity measurements.
• apply Faraday’s law and set up mass and charge action equations for an electrolytic process,
• work quantitatively, considerate and routinely in a chemical laboratory and be able to judge the quality of experimental data,
• capable of planning and conducting, both autonomously and as well as member of a team, experimental studies on basic physical chemical problems including those systems that go beyond ideal behaviour.
Subject overview
non-ideal gases
basic thermodynamic quantities and processes based on the 1st and 2nd fundamental law of thermodynamics including heat engines
interfacial effects
transport properties, particularly conductivity and ion mobility
data treatment and experimental errors
Literature