Physical Chemistry II
FACULTY | ENGINEERING | ||||
DEPARTMENT | CHEMICAL ENGINEERING | ||||
LEVEL OF STUDY | UNDERGRADUATE | ||||
SEMESTER OF STUDY | 4o | ||||
COURSE TITLE | Physical Chemistry II | ||||
| COURSEWORK BREAKDOWN | TEACHING WEEKLY HOURS | ECTS Credits | |||
| Lectures | 3 | ||||
| Laboratory | 2 | ||||
| Projects | 0 | ||||
TOTAL | 5 | ||||
| COURSE TYPE | General background | ||||
| PREREQUISITES | |||||
| LANGUAGE OF INSTRUCTION/EXAMS | Greek | ||||
| COURSE DELIVERED TO ERASMUS STUDENTS | Yes | ||||
MODULE WEB PAGE (URL) | https://eclass.uowm.gr/courses/CHEMENG194/ | ||||
2. LEARNING OUTCOMES
Learning Outcomes | |
| Upon successful completion of the course, students should acquire the following knowledge, abilities and skills: • They will encounter and understand the way of solving physicochemical problems and the physical chemistry methodology. • They will practice analytical thinking. • They will be able to solve complex problems in the classroom and elsewhere. • They will be able to connect the acquired knowledge with other disciplines - interdisciplinarity (physical chemistry requires skills of mathematics and physics). • They will be able to understand the physicochemical phenomena that take place in physical and chemical processes. • They will be able to carry out laboratory experiments as well as analyze the data of these experiments. | |
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| Acquisition and analysis of data and information, using the necessary tools. Adaptation to new situations. Decision making. Autonomous work. Teamwork. |
3. COURSE CONTENTS
| Theory: • Chemical kinetics (Part 1) • Electrochemistry (Part 2) • Colloidal systems (Part 3) Chemical kinetics (Part 1): • Rate of chemical reactions. • Measurements of reaction rate. • Dependence of reaction rate on concentration. • Reaction order. • Bidirectional and parallel reactions. • Complex reactions. • Mechanism of reactions. The importance of the rate determining steps • Complex reaction mechanisms. • Dependence of reaction rate on temperature. • Activation energy. • Frequency factor. • Theoretical calculation of reaction rate. • Collision theory. • Theory of the activated complex. • Enthalpy and entropy of activation. • Introduction to catalysis. Electrochemistry (Part 2): • Ionics: Liquid solutions. • Solvation of ions. • The standard thermodynamic functions during the formation of ions in solutions. • Theories of Arrhenius and Debye-Hückel. • The ionic strength. • Faradays laws and the electrochemical equivalent. • Coulometry. • Conductivity measurements. • Transport numbers and ion mobility. • Electrodes: Definition of potentials. • Galvanic elements. • Electromotive force (EMF) of a galvanic cell. • Free energy and equilibrium potential. • Entropy and enthalpy of electrochemical reactions. • Types of half cells (electrodes). • Standard electrode potentials. • Types of galvanic cells. • Electrochemical kinetics. • Polarization. • Overpotential. • Applied electrochemistry: Basic principles. Colloidal systems (Part 3): • Optical, kinetic and electrical properties of colloidal systems. • DLVO theory, stability of colloidal systems. • Emulsions, micro-emulsions, foams, gels. Laboratory courses: • Spectrophotometric monitoring of the kinetics of iodine oxidation by hydrogen peroxide. • Monitoring ester hydrolysis kinetics and the effect of temperature. • Pehametric determination of the acidity constant of acids. • Conductivity of electrolytic solutions. • Conductivity monitoring of reaction kinetics. • Determination of the standard potential of a redox half cell. • Effect of ionic strength on reaction rate. • Optical polosimetry to determine the kinetic constant of reactions. • Determination of metal ion activity coefficients. • Effect of temperature on salt solubility. • Electrochemical determination of iodine ions in water samples. • Electrolysis of a NaCl solution. |
4. TEACHING METHODS – ASSESSMENT
| MODE OF DELIVERY | Face-to-face | ||||||||||||||||||||||||
| USE OF INFORMATION AND COMMUNICATION TECHNOLOGY | Use of information and communication technology (ICT) during teaching and communication with students. | ||||||||||||||||||||||||
TEACHING METHODS |
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| ASSESSMENT METHODS | The overall grade of the course results from the grade of the Final Theory Examination (FTE), the Laboratory Exercises (LC), and the grade of the Final Laboratory Examination (FLE) and is given by the formula: 0.7*(FTE) + 0.15*(LC) + 0.15*(FLE) = FINAL GRADE |
5. RESOURCES
Suggested bibliography : |
| 1. P.W. Atkins, ATKINS PHYSICAL CHEMISTRY, 11E, 11th Edition (ISBN: 978-0198769866) 2. Ν.Α. Κατσάνου, ΦΥΣΙΚΟΧΗΜΕΙΑ - ΒΑΣΙΚΗ ΘΕΩΡΗΣΗ, Εκδόσεις Παπαζήση (ISBN: 960-02-0448-9) 3. Δ.Α. Γιαννακουδάκη, Π.Δ. Γιαννακουδάκη, ΕΠΙΤΟΜΗ ΦΥΣΙΚΟΧΗΜΕΙΑ, Εκδόσεις ΖΗΤΗ, (ISBN: 960-431-245-6) 4. Ν. Κουλουμπή, ΗΛΕΚΤΡΟΧΗΜΕΙΑ, Εκδόσεις ΣΥΜΕΩΝ (ISBN 960-7888-31-6) 5. Γ. Καραΐσκάκης, ΦΥΣΙΚΟΧΗΜΕΙΑ, Εκδόσεις Τραυλός (ISBN: 978-960-712-231-5) |
Related academic journals: |
| 1. The Journal of Physical Chemistry C 2. Electrochimica Acta 3. Physical Chemistry Chemical Physics (PCCP) |