- to define solutions - experience laws, thermodynamic quantities and models of
solutions
- to analyse phase diagrams of binary liquid mixtures
- to define and to utilize basic terms of chemical kinetics - homogeneous and
heterogeneous reaction, rate of chemical reaction, kinetic equation, order of
reaction, rate constant
- to monitor the dependence of the reaction rate on temperature
- to describe basic processes of heterogeneous reactions – diffusion, adsorption;
- to apply gained theoretical knowledge in routineto apply thermodynamic
quantities to electrolyte solutions
- to outline usage possibilities of electrochemical systems - electrodes,
electrolysis, galvanic cells
- to to describe properties of selected dispersion systems
- to apply gained theoretical knowledge in routine |
Chemical kinetics – classification of reactions, basic terms (reaction rate in homogeneous and heterogeneous systems, order of reaction, molecularity, rate constant, reaction mechanism). Integrated forms of the kinetic equation. The temperature dependence of the rate of a chemical reaction, Arrhenius equation. Kinetics of heterogeneous chemical reactions, elementary steps in heterogenous reactions.
Electrochemistry – electrolytes and theory of electrolytic dissociation. Strong electrolytes - activity and activitiy coefficient, Debye-Hückel limiting law. Solubility product. Equilibrium and dissociation in solutions of weak electrolytes - dissociation of week monobasic acids and bases, hydrolysis of salt, buffer solutions. Electrolysis, transport number, electric conductivity of electrolytes. Electrochemistry potentials, electrodes, galvanic cells.
Colloid chemistry - classification of dispersion systems, degree of dispersion. Selected kinetic, electrical and optical properties of colloid systems. Heterogeneous dispersion systems (lyophobic sols, emulsion, foam, aerosol).
|
Atkins,P.W., Physical Chemistry. Fourth Edition, Oxford: Oxford University
Press, 1993. 995 p.
Lupis,C.H.P.Chemical Thermodynamics of materials. New York, North-Holland,
1983. 581 p. |
Atkins,P.W., Fyzikálna chémia. Bratislava: STU,1999.
Adamcová,Z.a kol., Příklady a úlohy z fyzikální chemie. Praha: SNTL, 1989.
Bureš,M.,Černý,Č., Chuchvalec,P., Fyzikální chemie II. Praha: VŠCHT, 1994.
Fischer, O. a kol., Fyzikální chemie. Praha: SNTL, 1983. 333 s.
Holub,R. a kol., Fyzikální chemie I. Praha: VŠCHT, 1991. 243 s.
Kalousek.J.,Dobrovský, Ľ., Základy fyzikální chemie.Ostrava: ES VŠB,1985.155 s.
Kellö,V., Tkáč,A., Fyzikálna chemia. Bratislava: Alfa, 1977. 778 s.
Kopečný,M., Dobrovský,Ľ., Sbírka řešených příkladů z fyzikální chemie.
Ostrava: ES VŠB, 1991.
Linzer, E., Dorušková,M., Kalousek,J., Základy fyzikální chemie v příkladech.
Ostrava: ES VŠB 1994. 192 s.
Moore,W.J., Fyzikální chemie. Praha: SNTL, 1979. 974 s.
Novák,J.a kol.Fyzikální chemie:bakalářský kurs. Praha: VŠCHT, 2005. 216 s.
Elektronická verze: http://vydavatelstvi.vscht.cz/knihy/uid_isbn-80-7080-559-
5/pages-img/001.html
Peřinová, K. a kol., Sbírka příkladů z fyzikální chemie. elektronická verze
http://fmmi10.vsb.cz/619/login.php
Atkins,P.W., Physical Chemistry. Fourth Edition. Oxford: Oxford University
Press, 1993. 995 p. |