DEGREE REGULATIONS & PROGRAMMES OF STUDY 2015/2016

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DRPS : Course Catalogue : School of Engineering : Chemical

Undergraduate Course: Chemical Engineering Thermodynamics 3 (CHEE09011)

 School School of Engineering College College of Science and Engineering Credit level (Normal year taken) SCQF Level 9 (Year 3 Undergraduate) Availability Available to all students SCQF Credits 10 ECTS Credits 5 Summary Thermodynamics covers the concepts of Gibbs Free Energy and chemical potential and their relationship to both phase equilibrium and chemical reaction equilibrium in heterogeneous systems and multiple simultaneous reactions. Mixing rules for Equations of State (EoS) are introduced as well as calculation of vapour pressure from EoS. Course description This course comprises 20 hours of lectures and 10 tutorials assessed by written examination. Lectures The course is delivered in two hour lectures. Lecture 1 Statement of the VLE problem. The Gibbs phase rule. Definition of the Chemical Potential - m. Extensive vs intensive thermodynamic properties. Euler's theorem of homogeneous functions. Partial molar quantities. . Lecture 2 Clausius-Clapeyron equation. V-L curve. V-S curve. L-S curve. Interpolation of vapour pressure data. Prediction of vapour and sublimation pressures from C-C equation. Chemical potential of a mixture. Fugacity and fugacity coefficients. Composition dependence of the chemical potential. Ideal mixtures. Activity and activity coefficients. Lecture 3 Fugacity of a component in a liquid mixture. Pressure dependence of the chemical potential. Poynting correction factor. Fundamental VLE equation: g-f and f-f approach. Simplified versions of the g-f approach. Vapour pressure equations. Excess Gibbs energy and activity coefficients. T vs x,y and P vs x,y diagrams - positive and negative deviations. Lecture 4 Dew point and bubble point calculation. Calculation of binary T vs x,y, P vs x,y and y vs x plots. Example VLE with azeotrope. Isothermal flash calculation. Example of a binary flash. Gibbs-Duhem equation. Thermodynamic consistency of VLE data. Partial pressures from total pressure data. Example of ethanol-water isothermal data. Gas-liquid equilibrium. Relationship between symmetric and a-symmetric activity coefficients. Liquid-liquid equilibrium. Solid-liquid equilibrium. Lecture 5 Sources of thermodynamic data. Two and three parameter law of corresponding states. Prediction of critical constants and acentric factor: Joback and Ambrose methods. Prediction of vapour pressure. Lecture 6 Equations of State (EOS). Cubic equations of state (EOS). Parameters from critical constants. Helmholtz free energy (A). Calculation of vapour pressures from EOS. Residual functions and thermodynamic properties from A. Lee and Kesler EOS and tables. Example of L-K and SRK. Lecture 7 Mixing rules for EOS. Michelsen-Kistenmacher syndrome. Fugacity coefficients from EOS. Advanced mixing rules for cubic EOS. Properties of EOS at infinite pressure. Sample calculation of VLE using EOS. Lecture 8 Thermodynamic models in Aspen/UniSim. Things to watch for in using computer codes Styrene-ethylbenzene example. Thermoworkbench examples. GCEOS. Lecture 9 Chemical reaction equilibria. Extent of reaction. Heat of reaction. Equilibrium constant and its temperature dependence. Reference states in common applications. Multiple chemical reactions - reactors in series and Lagrange multipliers. Lecture 10 Review and open discussion. Tutorials Each lecture has a corresponding tutorial plus one tutorial on Unisim.
 Pre-requisites Students MUST have passed: Thermodynamics (Chemical) 2 (CHEE08009) Co-requisites Prohibited Combinations Other requirements None
 Pre-requisites None High Demand Course? Yes
 Academic year 2015/16, Not available to visiting students (SS1) Quota:  1 Course Start Semester 2 Timetable Timetable Learning and Teaching activities (Further Info) Total Hours: 100 ( Lecture Hours 20, Formative Assessment Hours 1, Summative Assessment Hours 1.5, Programme Level Learning and Teaching Hours 2, Directed Learning and Independent Learning Hours 75 ) Assessment (Further Info) Written Exam 100 %, Coursework 0 %, Practical Exam 0 % Additional Information (Assessment) One 2 hour degree examination in December One 2 hour degree resit examination in August Feedback Not entered No Exam Information Academic year 2015/16, Available to all students (SV1) Quota:  None Course Start Semester 1 Timetable Timetable Learning and Teaching activities (Further Info) Total Hours: 100 ( Lecture Hours 20, Formative Assessment Hours 1, Summative Assessment Hours 1.5, Programme Level Learning and Teaching Hours 2, Directed Learning and Independent Learning Hours 75 ) Assessment (Further Info) Written Exam 100 %, Coursework 0 %, Practical Exam 0 % Additional Information (Assessment) One 2 hour degree examination in December One 2 hour degree resit examination in August Feedback Not entered Exam Information Exam Diet Paper Name Hours & Minutes Main Exam Diet S2 (April/May) 2:00
 Students should be able to: - apply the phase rule to determine degrees of freedom and show how these may be satisfied - describe the significance of Chemical Potential in mixtures and understand phase equilibria formulations. - use Standard heats and free energies of formation to evaluate equilibrium constants, and hence determine equilibrium - concentrations in reacting mixtures
 1. Smith J.M., Van Ness H.C. & Abbott M.M., Introduction to Chem. Eng. Thermodynamics, McGraw-Hill. 5th Ed., 1996. 2. Prausnitz J.M., Lichtenthaler R.N. & de Azevedo E.G., Molecular Thermodynamics of Fluid-Phase Equilibria, 3rd Ed., 1999. Prentice-Hall. 3. Poling B., Prausnitz J.M. & O'Connell J.P., The Properties of Gases and Liquids, 5th Ed., 2000. McGraw-Hill. 4. Perry R.H. and Green D.W., Perry's Chemical Engineers' Handbook. 7th Ed., 1997. McGraw-Hill.
 Graduate Attributes and Skills Not entered Keywords Not entered
 Course organiser Prof Stefano Brandani Tel: Email: S.Brandani@ed.ac.uk Course secretary Mrs Lynn Hughieson Tel: (0131 6)50 5687 Email: eto@eng.ed.ac.uk
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