Thermodynamics and Kinetics
Code: 100888Credits: 6
| Degree programme | Type | Course |
|---|---|---|
| Biochemistry | FB | 1 |
Contact lecturer
- Name :
- Vicenç Branchadell Gallo
- Email :
- vicenc.branchadell@uab.cat
Group languages
You can consult this information at the end of the document.
Prerequisites
the concepts included in Baccalaureate Chemistry.
Objectives
The general objective of the subject is to introduce the student, for the first time, to the theoretical study
of the chemical and biochemical phenomena, that is to say, to the contributions of Physical Chemistry to a life science like Biochemistry.
In the long run, the student has to become aware of the importance of Physical Chemistry as the theoretical basis of Biochemistry, and become familiar with its theoretical and experimental methodology.
The most general objective of the program is to help the student to understand the chemical and biochemical phenomena
of the macroscopic world. The basic concepts of Thermodynamics and Chemical Kinetics will be studied.
At the same time, we also want the student to be aware of the dual-theoretical-experimental character of the
Physical Chemistry. Another general objective is to give the student an interdisciplinary view of Biochemistry, in
particular, its close relationship with Chemistry, Physics, and Mathematics.
Specific objectives:
1) Understand the laws of Classical Thermodynamics and be able to apply them to the study of chemical and biological systems.
2) Know the basic foundations of the Chemical Kinetics and be able to apply them in the study of chemical and biochemical reactions.
3) Distinguish between phenomena governed by Thermodynamics and phenomena governed by Kinetics.
Learning outcomes
- KM02 (Identify the principles of thermodynamics, stereochemistry and chemical equilibrium, as well as the functional groups and reactivity of organic compounds present in biomolecules and metabolites.) Identify the principles of thermodynamics, stereochemistry and chemical equilibrium, as well as the functional groups and reactivity of organic compounds present in biomolecules and metabolites.
- SM01 (Apply the laws and principles of chemical equilibrium, thermodynamics and kinetics to biochemical processes.) Apply the laws and principles of chemical equilibrium, thermodynamics and kinetics to biochemical processes.
Contents
BLOCK 1. FUNDAMENTALS OF THERMODYNAMICS
1. Introduction to thermodynamics.
Introduction to thermodynamics. The ideal gas. Energy, heat and work. Types of systems. Expansion work. Reversible processes. Energy transfer in the form of heat. Principles of Thermodynamics.
2. Thermochemistry.
Enthalpy. Phase change enthalpies. Enthalpies of reaction. Calorimetry. Standard formation enthalpies. Enthalpy of bonding. Enthalpy of solution. Enthalpy of reaction and internal energy. Variation of the enthalpy of reaction with temperature. Thermodynamic properties of fuels.
3. Spontaneity and equilibrium.
Second principle. Variation in entropy in some processes. Reversible adiabatic expansion of an ideal gas. Molecular interpretation of entropy. Third principle. Absolute entropies and reaction entropy. Gibbs energy. Fundamental equations of a closed system. Gibbs energy and maximum work. Composition as a variable. Material equilibrium
BLOCK 2. MATERIAL EQUILIBRIUM
4. Phase equilibrium
Phase equilibrium in one-component systems. P-T phase diagram. Heating and cooling curves. Triple point and critical point. Clapeyron's equation. Clausius-Claperyron equation. Solid-solid phase equilibrium. The phase rule.
5. Dissolutions.
Partial molar properties. Chemical potential. Raoult's Law. Thermodynamics of mixtures. Ideal solution. Deviations from ideal behavior. Ideal diluted solution. Henry's Law. Colligative properties. Gibbs energy of mixing in a real solution.
6. Chemical equilibrium.
Introduction. Gibbs energy of reaction. Degree of reaction advance and Gibbs energy of reaction. Reaction quotient and equilibrium constant. Standard reaction Gibbs energy. Reactions in solution. Heterogeneous equilibria. Variation of the equilibrium constant with temperature.Displacement of equilibrium. Acid-base reactions.
BLOCK 3. KINETICS
7. Fundamentals of chemical kinetics.
Reaction speed. Speed equation. Reaction orders: differential method. Integration of velocity equations. Half-reaction time. Isolation method. Experimental techniques. Reaction speed and temperature. Microscopic interpretation of the speed of a reaction.
8. Reaction mechanisms.
Reaction mechanism. Reversible reactions. Parallel reactions. Consecutive reactions. Steady State approximation. Preequilibrium aproximation. Rate determining step. Reactions in solution. Catalysis. Acid-base catalysis. Enzymatic catalysis. Michaelis-Menten mechanism.
Learning activities and methodology
| Title | Hours | ECTS | Learning outcomes |
|---|---|---|---|
| Theory lectures | 30 | 1.2 | KM02, SM01 |
| Study and problem solving | 87 | 3.48 | SM01 |
| Team work | 10 | 0.4 | SM01 |
| Problem sessions | 15 | 0.6 | SM01 |
The subject will consist of three types of teaching activities:
1. Theoretical classes
The teacher will develop the contents of the program in-person or virtually, according to the instructions of the academic authorities. The contents of the theoretical classes will be available in advance on the Virtual Campus.
2. Problem classes
Several problems will be proposed for each topic, which will be solved by the students under the supervision of the teacher. Problem classes will be devoted to the discussion of the results of the problems in relation with the contents of the subject.
Assessment
Continuous assessment activities
| Title | Weight | Hours | ECTS | Learning outcomes |
|---|---|---|---|---|
| Parcial exam 1 | 30% | 2 | 0.08 | SM01 |
| Group evaluation | 20% | 3 | 0.12 | KM02, SM01 |
| Partial exam 2 | 50% | 3 | 0.12 | SM01 |
Written exams
Throughout the course there will be two partial exams. The weights of these exams in the final mark will be 30% and 50%, respectivelly, so that the whole of the two partial exams will represent 80% of the final mark.
The minimum mark of a partial exam that allows to calculate the average of the course is 4. If these minimum ones can not be reached, at the end of the course one or both partial exams can be retrieved. The mark obtained in the recovery will replace the mark obtained in the first attempt. It is also possible to come up with the recoveries to improve note. In this case, the last mark obtained in each partial exam is the one that prevails. In order to be entitled to a recovery, it is compulsory to have submitted to both partial exams.
Trace work
Throughout the course, a certain number of student tracking tests (problems solved individually or in groups, short classroom tests, etc.) will be collected. The average grade of these tests will represent 20% of the final mark
In each non-face-to-face assessment element, the grade obtained will be contrasted with an interview with the teacher. This will affect between 10 and 20% of the students in each evaluation element. The result of this interview will prevail over the grade initially obtained.
The performance of any irregularity in an assessment act (academic fraud, plagiarism or improper use of AI, unless such use is expressly authorized in the teaching guide), which may lead to a significant variation in the grade, means that this act will be graded with a 0. In the event that the teaching guide provides that in order to pass the subject it is an essential requirement to have obtained a minimum grade in this evaluation act or that there are several irregularities in the evaluation acts of the same subject, the final grade of this subject is 0. Apart from this, a disciplinary process may be initiated against the student who incurs in any of these irregularities.
The requirements to pass the subject are:
1. The mark of each partial exam must be equal to or greater than 4
2. The average mark of the subject must be equal or greater than 5
The subject will be considered non-evaluable if the weigth of the evaluation activities done represents less than 50% of the final mark for the subject. To qualify for the “Matrícula d’Honor\" qualification, the marks obtained in the partial exams will be taken into account preferably.
If in any of the midterm exams the minimum required grade is not reached but the overall grade calculated according to the weights of each evaluation element is equal to or greater than 5, the final grade of the subject will be 4.5.
Students who have opted for single assessment will have to take a final test that will consist of an examination of the entire syllabus of the subject to be carried out on the day on which the students of the continuous evaluation take the second partial exam. The student's grade will be the mark of this test.
If the final grade does not reach 5, the student has another opportunity to pass the subject through the recovery exam that will be held on the date set by the coordination of the degree.
Bibliography
1) I. N. Levine, Physical Chemistry, 6th Edition, McGraw Hill, 2009. (Translated edition: Principios de
fisicoquímica, 6ª edició, McGraw Hill, 2014).
2) P.W. Atkins, J. de Paula, Physical Chemistry for the Life Sciences, Oxford University Press, 2006.
3) R. Chang, Fisicoquímica para las ciencias químicas y biológicas, McGraw-Hill, 2008, 3a ed.
4) S.R. Logan, Fundamentos de Cinética Química, Addison Wesley iberoamericana, 2000.
5) R. Chang, Physical Chemistry for the Biosciences, University Science books, 2005.
Software
None.
Course groups and languages
The information provided is provisional until November 30. After this date, you will be able to consult the language of each group through this link. To access the information, you will need to enter the course CODE
| Type of teaching | Group | Language | Semester | Shift |
|---|---|---|---|---|
| (TE) Theory | 31 | Catalan | second semester | afternoon |
| (PAUL) Classroom practices | 311 | Catalan | second semester | afternoon |
| (PAUL) Classroom practices | 312 | Catalan | second semester | afternoon |