Performing calculations on gas mixture systems
Undertaking thermodynamic calculations using data from Thermochemical Tables
Calculating equilibrium compositions, thermodynamic functions and reaction equilibrium conditions
Constructing partial pressure-composition diagrams in binary liquid/gas systems as well as solving problems in cryoscopic, zeseoscopic and osmotic systems
The students are expected to have a good command of differential equations and integrals as well as basic knowledge of chemistry.
Partial molar properties. Gibbs-Duhem equation. Ideal and real gas mixtures. Lewis-Randall rule. Equilibria of reactions involving gases. Stoichiometry. Direction and extent of reaction. General condition of equilibrium. Equilibrium constant. Standard Gibbs free energy of reaction. Van’t Hoff relation. Enthalpy of reaction. General relations for the temperature dependence of Κp and ΔG. Other forms of the equilibrium constant. Standard thermodynamic functions (G, H, S) of formation. Hess’ Law. Reaction equilibria involving gases with immiscible liquids and solids. Number of independent reactions. Maximum attainable yield. Le Chatelier’s principle. Gibbs’ Phase Rule. Degrees of freedom. Effect of inert gas on the vapor pressure of a component. General properties of solution. Partial pressure – composition relations. Raoult’s and Henry’s Law. Deviations. Duhem-Margules equation. Solubility. Ideal solutions. The chemical potential model for ideal solutions. Thermodynamic properties of mixing in ideal solutions. Tand P dependence of the Henry’s law constant. Equilibrium between ideal solution and pure crystalline component. Freezing point depression. Boiling point elevation. Osmotic pressure. Non ideal solutions and the chemical potential model. Activity coefficients. Gibbs – Duhem equation in representation of activity coefficients. Activity coefficients of solutes. Activity. Excess properties.
LECTURES: 4 h/w
RECITATION: 1 h/w
Total Module Workload (ECTS Standards):
1) The student can take two (2) tests on volunteer basis (6th and 13th week of the semester).
2) Undertaking of case studies/projects by small (3,4) student groups, on volunteer basis.
3) Final exam. The average of the exams (1) – if greater than 5.0 – is considered together with the (optional) project (2) for improving the final module grade.
1. P. Atkins, J. de Paula, “Physical Chemistry”, 9th Edition, Oxford University Press, 2014
2. Υ.Α. Cengel, M. A. Boles, «ThermodynamicsQ An Engineering Approach» 8th Edition (in Greek), A. Tziola & Sons Ed., 2016