Physical Chemistry 1200-1ENCHFIZW3
Thematic scope:
Thermodynamics:
The concept of the system and its surroundings. States of matter. Perfect and real gases, ideal gas equation. Parameters of state: temperature, pressure, volume, quantity. Basic concepts of classical mechanics: vector, velocity, acceleration, momentum, work, kinetic energy, Newton's laws of dynamics, conservation of energy and momentum, elastic collisions. Internal energy, entropy, heat, work. Laws of thermodynamics (zero, first, second, third). Complete differential. Legendre transformation of functions of one and multiple variables. Thermodynamic functions: enthalpy, Helmholtz free energy, Gibbs free energy. Heat of a process at constant volume and pressure. Heat capacity at constant volume and constant pressure. Entropy production and spontaneity criteria under the conditions of an isolated system, constant volume and constant pressure. Calculating changes of thermodynamic functions, including those for an ideal gas. Chemical potential, homogeneity of thermodynamic functions (Euler's theorem), condition of thermodynamic equilibrium (law of mass action).
Chemical kinetics:
Chemical reaction rate, kinetic equation: reaction rate constant, reaction order, reaction molecularity. Kinetic equations of the 1st and 2nd order (determination of the reaction rate constant). Complex reactions (parallel, sequential, equilibrium, sequential with initial equilibrium). Steady state approximation. Determining the reaction order. Dependence of reaction rate constant with temperature (Arrhenius equation). Collision theory, transition state theory. Enzymatic catalysis.
Electrochemistry
Ideal and real solutions, ion activity and electrolyte activity. Assumptions of the Debye-Hückel theory. Ohm's law. Specific and molar conductivity of electrolyte solutions. The concept of ion mobility. Dependence of the specific conductivity of strong electrolytes on the concentration of the electrolyte, charge, ion mobility and on the physicochemical parameters of the solvent. Relaxation and electrophoretic effect. Solvation (Born's theory).
Nernst equation, standard potential. Class I and II electrodes, gas electrodes: diagrams, half-reactions - Stockholm convention. Standard hydrogen electrode. Electrochemical cells - diagrams. Galvanic and electrolytic cells. Electromotive force of a galvanic cell. Relationship of electromotive force with thermodynamic functions of the reaction taking place in the cell. Application of EMF measurements to determine thermodynamic parameters of reactions. Kinetic and diffusion control of electrode processes (Butler-Volmer equation, Tafel equation).
Main fields of studies for MISMaP
Type of course
Mode
Remote learning
Prerequisites (description)
Learning outcomes
After the course the student:
- knows the basic terms and how to use them in thermodynamics, thermochemistry, chemical kinetics, electrochemistry,
- knows the main relationships in Physical Chemistry and how to use them,
- knows the basis of fundamental physicochemical processes,
- is able a direction of physicochemical processes after the change of various parameters, like temperature, pressure, concentration, potential,
- knows which experimental methods one can use in the studies of physicochemical processes,
is able to determine the fundamental physicochemical parameters from experimental data
- is able to interpret experimental data and infer appropriate conclusions.
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 35 points in the partial tests will be released from the exam with 5 grade (however, he / she can write the exam to obtain a grade of 5!). The rest of the participants take the entire material for the exam, but 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 –98.00 - 5
98.01 –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., Physical Chemistry. 2018: Oxford University Press; 11th Edition.
2. Pigoń, K., Ruziewicz, Z., Chemia fizyczna: Podstawy fenomenologiczne. 1. 2007: Wydawnictwo Naukowe PWN.
3. Hołyst, R., A. Poniewierski, Thermodynamics for Chemists, Physicists and Engineers. 2012: Springer Netherlands.
4. Jackowska, K., Repetytorium – Elektrochemia, 2017: Wydział Chemii UW, Zakład Dydaktyczny Chemii Fizycznej.
Additional information
Information on level of this course, year of study and semester when the course unit is delivered, types and amount of class hours - can be found in course structure diagrams of apropriate study programmes. This course is related to the following study programmes:
- Nuclear Power Engineering and Nuclear Chemistry, full time 3 year programme leading to B. Sc. Degree
Additional information (registration calendar, class conductors, localization and schedules of classes), might be available in the USOSweb system: