546-0031/01 – Physical Chemistry II (FCHII)
| Gurantor department | Department of Environmental Engineering | Credits | 6 |
| Subject guarantor | doc. Mgr. Eva Pertile, Ph.D. | Subject version guarantor | doc. Mgr. Eva Pertile, Ph.D. |
| Study level | undergraduate or graduate | Requirement | Compulsory |
| Year | 2 | Semester | summer |
| | Study language | Czech |
| Year of introduction | 2015/2016 | Year of cancellation | 2019/2020 |
| Intended for the faculties | HGF | Intended for study types | Bachelor |
Subject aims expressed by acquired skills and competences
Physical chemistry occupies a central position among other chemical sectors, because it deals with the study of the laws that affect virtually all chemical disciplines and influence their development. The curriculum builds on the knowledge of Physical Chemistry I. The aim of the course is to acquaint students with the theoretical foundations of general practice different disciplines in an integrated form, based on fundamental physical principles and to deepen their knowledge of important conclusions and applications, including existing applications in science and technology. Another aim is also to gain knowledge about principles and laws of physical and chemical processes. After successful completion of the course, it is assumed that the listener will understand the problems of basic concepts of physical chemistry, their principles, relationships and patterns in the area of reaction kinetics, electrochemistry and colloidal chemistry and their significance in practice and will also be able to use the acquired knowledge of a general character as in other chemical subjects and in solving application problems.
Teaching methods
Lectures
Tutorials
Summary
Physical chemistry as a science discipline has close relationships with other sciences. It can therefore be used very well to understand environmental influences. The course covers elementary parts of physical chemistry, which are connected with topics of chemical reaction equilibrium, selected parts of the properties and behavior of systems containing electrolytes and description of velocity of chemical reactions (kinetics).
Compulsory literature:
ATKINS, Peter William - Julio de Paula. Physical chemistry for the Life Sciences. 1st ed. N.Y.: W. H. Freeman and Company, 2010, 699s. ISBN 0-1992-8065-9.
CHANG R.: Chemistry. 10th Edition. McGraw-Hill: New York, 2010. 1170 p. Dostupné z: https://archive.org/details/Chemistry_10th_Edition_Raymond_Chang.
Recommended literature:
RONIS David: Introductory Physical Chemistry I. McGill University.2015. Dostupné z: http://ronispc.chem.mcgill.ca/ronis/chem223/course_pac.pdf.
MALIJEVSKÝ A., et. al: Physical chemistry in brief. Institute of Chemical Technology, Prague, 2005. Dostupné z: http://old.vscht.cz/fch/en/tools/breviary-online.pdf.
Way of continuous check of knowledge in the course of semester
Student knowledge is verified in written form, emphasis is given to understanding the subject and applying theoretical knowledge to solving practical problems. The evaluation also includes collective evaluation and self-assessment.
E-learning
Other requirements
They are not defined. It is recommended that the successful discharge Physical Chemistry I.
Prerequisities
Co-requisities
Subject has no co-requisities.
Subject syllabus:
Electrochemistry homogenous systems: Electrolyte solutions. Equilibria in electrolyte solutions, characteristics of electrolytes, degree of dissociation, Arrhenius theory. Faraday's laws of electrolysis and its use. Conductivity of electrolyte solutions and its measurement. Molar conductivity and limiting molar conductivity of electrolytes and ions. Ion mobility and its measurement. Using conductivity measurement in chemistry. Activity and activity coefficient. Ionic strength. The dependence of the activity coefficient on the ionic strength. Debye-Hückel theory. Theory of acids and bases. Dissociation of strong and weak electrolytes. The degree of dissociation, and the dissociation constant. Arrhenius and Brönsted's theory of acids and bases. Autoprotolysis. pH and acidity scale (Hammett). Approximate calculations pH of acidic and basic solutions. PH measurement - practical pH scale. Hydrolysis of salts. Buffers - their description and practical implementation. Buffering capacity. Sparingly soluble salt. Ampholytes. Tautomeric equilibria of electrolyte solutions - acid-base indicators. Complex electrolytes. Lewis theory of acids and bases.
- Electrochemistry of heterogeneous systems: electrochemical potential. Electrode, galvanic cell. Equilibrium (electromotive) voltage and electrical work galvanic cell. The electrode potential. Nernst equation. Reversible electrodes - sorting and examples including the use in practice. Potential liquid interface. ISE - Ion Selective Electrode. Electric double layer. Kinetics of electrode processes. Polarization electrodes.
- Reaction kinetics: The isolated and simultaneous reactions. Reaction rate. Rate constant, reaction order, molecularity response. Reaction mechanism. Simple one-way reactions, 0, I and II. Regulations. Half-reaction, influence of temperature and other factors on the reaction rate. The reaction of higher order. Methods for determining the reaction order. Simultaneous reactions - reversible, parallel and consecutive, autocatalytic. Chain reactions. Catalysis - homogeneous, heterogeneous and enzymatic. Reaction in solution - the influence of ionic strength on the reaction rate. Photochemical processes.
- Colloidal Systems: Characteristics and basic properties of colloidal systems. Distribution of colloidal systems by phase arrangement, respectively. interactions at the interface. Lyophilic, lyophobic and association colloids, optical, kinetic and electrical properties of colloids, suspensions, interfacial properties, formation of a suspension, sedimentation, emulsion type emulsions, the theory of formation and stability of the liquid surface, the surface and interfacial tension, adsorption at the liquid interphase surface active agents, hydrophilic-lipophilic system, electric double layer, Nernst and zeta potential, the influence of electrolytes. Molecular and kinetic, optical and electrical properties of colloidal systems.
Physical properties of substances, photochemistry: The polarity of substances dipole moment, relative permittivity, absorption of electromagnetic radiation, Lambert-Beer law, atomic spectra of absorption and emission, absorption of light molecules in the UV, VIS, and IR regions of the electromagnetic radiation, nuclear magnetic resonance, mass spectrometry, emission molecular spectra (Raman phenomenon, fluorescence and phosphorescence), photochemical reactions.
Conditions for subject completion
Occurrence in study plans
Occurrence in special blocks
Assessment of instruction