Chemical and Biological Engineering Thermodynamics
Objectives
Understanding the basic concepts of thermodynamics (laws of thermodynamics and relationships between the macroscopic equilibrium properties of a system), with an emphasis on phase equilibrium and reaction equilibrium.
General characterization
Code
12587
Credits
6.0
Responsible teacher
Ana Rita Cruz Duarte
Hours
Weekly - 4
Total - 56
Teaching language
Português
Prerequisites
None.
Bibliography
1. Physical Chemistry, I. Levine, 6ª ed., McGraw-Hill, 2009.
2. Termodinâmica Aplicada, E. Gomes de Azevedo, 4ª ed., Escolar Editora, 2018.
3. Principles and Problems in Physical Chemistry for Biochemists, 3ª ed., N.C. Price, R. A. Dwek, M. Wormald, R.G. Ratcliffe, Oxford University Press, 2001.
4. Physical Chemistry for the Life Sciences, 2ª ed., P. Atkins, J. de Paula, WH Freeman and Company, 2011.
Teaching method
Available soon
Evaluation method
Tests:
- 2 tests (70% of the final grade)
- First test > 9.5 values
Frequency > 9.5 values:
- Resolution 6 practical group exercises (4 students) in class (20% of the final grade)
- Resolution of a group mini-project in class (10% of the final grade)
Final grade: 70% test grade + 30% frequency
Subject matter
Thermodynamics os ideal gases. The second law of thermodynamics. The Carnot cycle. Entropy. Temperature scales. Helmholtz and Gibbs energies. Thermochemistry. Standard enthalpy and entropy. The third law of thermodynamics. Fundamental equations for a closed system in equilibrium. The Maxwell relations. The Gibbs-Helmholtz equation. Extension of the Gibbs equations to processes involving exchange of matter with the surroundings or irreversible composition changes. The chemical potential. One component phase equilibrium. The phase rule. The Clapeyron equation. Chemical potential of ideal and real gases. Fugacity. Solutions. Partial molar quantities. The Gibbs-Duhem equation. Ideal solutions. Colligative properties. Ideally dilute solutions. Nonideal solutions. Activity and activity coefficient. Excess functions. Liquid-liquid and solid-liquid equilibrium. Reaction equilibrium. Debye-Hückel theory of electrolyte solutions.