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Syllabus for Chemical Engineering 3853, Chemical Engineering
Thermodynamics
University of Utah Fall 2008
Professor: Geoff Silcox, Department of Chemical Engineering Phone: 581- FAX: 585- Office: 3290C MEB e-mail: geoff AT che.utah.edu web site: www.che.utah.edu/~geoff/ Office hours: When available or by appointment
Teaching assistant: Paula Buitrago Phone: 581- Office: EMRL 214 e-mail: p.buitrago AT utah.edu Office hours: TBA
Meetings: M W F, 10:45-11:35, WEB 112 Study Session: TBA Prerequisites: CH EN 2300 (Thermodynamics I) and CH EN 2800 (Fundamentals of Process Engineering), major standing. Co- requisite: CHEM 3060 (Physical Chemistry I). Required text: J. R. Elliott and C. T. Lira, Introductory Chemical Engineering Thermodynamics , Prentice Hall PTR (1999), ISBN
Suggested References
The Foundation Coalition (http://www.foundationcoalition.org) has developed a concise summary of the conservation and accounting framework that is central to chemical engineering and thermodynamics.
Noel de Nevers, Physical and Chemical Equilibrium for Chemical Engineers , John Wiley (2002), ISBN 0471071706.
H. C. Van Ness and M. M. Abbott, Schaum's Outline of Thermodynamics With Chemical Applications (Schaum's Outline Series), McGraw-Hill (1989). ISBN
Course Content and Objectives
Thermodynamics is the study of energy and its transformations. Chemical Engineering 3853 focus on physical and chemical equilibrium with applications in the chemical process industries. The course is divided into four sections: (1) Energy and Entropy Balances, (2) Generalized Analysis of Fluid Properties, (3)
Fluid Phase Equilibria in Mixtures, and (4) Energy Balances and Equilibrium in Reacting Systems. Learning objectives for each section follow. Many of these are directly quoted from the website of the author, Prof. Carl T. Lira (http://www.egr.msu.edu/~lira/thermtxt.htm).
General Objectives
By the end of this course you will be able to
- Practice effective approaches to solving homework problems and presenting their solutions, including the use of tools like Excel, Polymath, and MATLAB.
- Work effectively in a team and as an individual to solve problems and to produce a well written, technically clear report.
Objectives for Unit 1 - Energy and Entropy Balances
By the end of this section you will be able to
- Explain what is meant by internal energy from a molecular viewpoint.
- Explain why entropy increases when different species mix at constant temperature and pressure.
- Explain the connection between fluid flow in pipes, lost work, and the Fanning friction factor.
Objectives for Unit 2 - Generalized Analysis of Fluid Properties
By the end of this section you will be able to
- Find the relationship between any thermodynamic property (for example, U,
H, S, A, G) and measurable properties (for example, T, P, V, ρ, CP , CV ).
- Apply simple equations of state (for example, the virial and Peng-Robinson equations) to calculate properties (for example, enthalpy and entropy) of pure fluids using departure functions.
- Explain why the Gibbs energy is the key property that characterizes phase equilibria.
- Describe the relationship between the Gibbs departure function and the fugacity.
- Calculate the fugacity coefficient of a vapor using the virial correlation.
- Calculate the fugacity coefficient of a vapor or liquid given an expression for a cubic equation of state and the parameter values Z, A, B, and decide which root among multiple roots is most stable.
Objectives for Unit 3 - Fluid Phase Equilibria in Mixtures
By the end of this section you will be able to
- List the properties that are always equal in two phases at phase equilibrium.
- Calculate emissions for filling or charging, purging, heating, or depressurizing a tank containing a VOC or mixture.
- Choose between bubble, dew, flash calculations from a problem statement.
- Calculate equilibrium concentrations for processes involving multiple reactions.
- Extend the technique of direct minimization of Gibbs energy to include pressure effects.
Grading
Points for homework, the project, and exams are assigned as follows.
Two one-hour exams 25% each One final exam 30% Project 10% Homework 10%
Final grades will be based on the following table. The table represents grade guarantees. I reserve the right to lower the scale and to reevaluate the scores of students who just miss a grade. The high score in the class will be used to scale all other scores. For example, if the high score is 95%, all scores will be divided by 0.95.
Percentage Grade 95-100 A 90-95 A- 85-90 B+ 80-85 B 75-80 B- 70-75 C+ 65-70 C 60-65 C- 50-60 D < 50 E
Students with Disabilities
The University of Utah seeks to provide equal access to its programs, services and activities for people with disabilities. If you will need accommodations in the class, reasonable prior notice needs to be given to the Center for Disability Services (CDS), http://disability.utah.edu/, 162 Olpin Union Building, 581-5020. CDS will work with you and the instructor to make arrangements for accommodations. All written information in this course can be made available in alternative format with prior notification to the Center for Disability Services.
Examinations
All examinations are comprehensive. This means that you will have multiple chances to show me that you have learned the material. Useful tips on taking tests and information on reducing test anxiety are found at http://disability.utah.edu/test.htm.
All examinations are open book, notes, and homework. To receive full credit for your solutions, you must write out all equations that you use and you must state all values substituted in those equations. You must show all of your work to receive credit.
No make-up exams will be given except in exceptional circumstances. If you must miss an exam, please notify me before the exam.
Homework
Solutions to the homework are due Fridays before 16:00. Homework turned in after this time will be awarded a maximum of 50%. No homework will be accepted after the solutions have been posted.
The neatness, organization, and completeness of your homework are important. To receive full credit for your solutions, you must write out all equations that you use and you must state all values substituted in those equations. You must show all of your work to receive credit.
The solutions will be posted on the web. I encourage you to work with other students on the homework. You should be sure that you can set-up, solve, and understand all of the problems.
Using E-mail
I will be using the email system provided by the U to send you messages. Please be sure that you check your utah.edu mail.
W 10/8 VLE calculations by EOS 10.4-10. F 10/10 VLE calculations by EOS (cont) HW 7 10.4-10. M-F 10/13- 17
Semester Break
M 10/20 Activity Models. Excess properties. Modified Raoult’s law (MRL). Comparison with EOS methods.
W 10/22 Determining G E^ from experimental data 11. F 10/24 Regular solutions and van der Waals’s viewpoint
HW 8 11.4-11.
M 10/27 Local composition theory, Wilson’s equation 11. W 10/29 Local composition theory, UNIQUAC and UNIFAC. Fitting activity models to data.
F 10/31 Liquid-liquid phase equilibria (LLE). Onset of LL instability. Stability and G E^.
HW 9 12.1-12.
M 11/3 Plotting ternary LLE data. VLLE with immiscible components.
Unit IV Chemical Equilibrium Ch 14 W 11/5 Reacting systems. Reaction coordinate. Equilibrium constraint.
F 11/7 Reaction equilibria for ideal solutions HW 10 14. M 11/10 Review W 11/12 Exam 2 on Chapters 1- F 11/14 Temperature effects HW 11 14.4-14. M 11/17 Energy balances for reactions: Methods 1 and 2
W 11/19 Energy balances for reactions: adiabatic reactors
F 11/21 Pressure effects. Nonideal version of Example 14.
HW 12 14.6, 14.
M 11/24 Multi-reaction equilibria - simultaneous reactions
W 11/26 Multi-reaction equilibria - direct minimization of Gibbs energy
H-F 11/27-
Thanksgiving Holiday
M 12/1 Solid components in reactions 14. W 12/3 Simultaneous reaction and phase equilibrium 14. F 12/5 Reactions involving ions HW 13 M 12/8 Review W 12/10 Review F 12/12 Review HW 14 F 12/19 (^) Final Examination 10:30-12:
