ChE 312
Chemical Engineering Thermodynamics

Winter 2018

Lecture: MWF 10-10:50  210 LINC
Studio: R Afternoon; BXL 102 or 103

Name email Office Hours
Lead Instructors Milo Koretsky (MK)  T 4-6 Gleeson 200
Natasha Mallette
Teaching Assistants Alyssa Saito  T 4-6 Gleeson 200
Lynza Sprowl  W 4-6 Gleeson 200
Jad Touma  W 4-6 Gleeson 200
Learning Assistants Ayman Alabdullatif
Ryan Cashen
Connor Haynes

AIChE Concept Warehouse

The general syllabus for course is available here.


Page Contents



  1. Some Practice Problems to prepare for the Final Exam:
    Examples 8.1, 8.2, 8.3, 8.5, 8.7, 8.12, 8.19
    Problems 8.1, 8.2, 8.3, 8.6, 8.10, 8.29, 8.30, 8.44, 8.73
    Examples 9.1, 9.2, 9.3, [9.4 (a), (b) part (i)], 9.5, 9.6, [9.7 part (a)], 9.8, 9.9, 9.10, 9.11
    Problems 9.1, 9.7, 9.10, 9.20, 9.21, 9.23, 9.24, 9.29, 9.32, 9.33
  2. Lecture slides and HW solutions for the entire term are posted.
  3. Pre-quiz for Friday posted
  4. Spreadsheat for Studio 10
  5. Pre-quiz for Wed posted
  6. HW 7 solutions and Week 8/9 slides posted
  7. Pre-quiz for Mon posted
  8. Homework 7 due date has been changed to the start of class on March 9.
  9. Please bring a laptop to Week 9 Studio
  10. Class exampe for Week 9 Wednesday here
  11. Pre-quiz for Wed posted
  12. No pre-quiz for Monday
  13. Pre-quiz for Fri posted
  14. HW 7 Posted
  15. HW 6 solution posted
  16. Office Hours Week 8 Changed:
    M 5-7 PM (200 Gleeson)
    Tu 3-4 (306 Gleeson)
    Tu 4-6 (200 Gleeson)
    MK will be available M 5:15-6 and Tu (3-4:30)Old Exam 2s have been posted.
  17. Course Learning Objectives have been updated.
  18. Week 3 lecture slides have been posted
  19. No pre-quiz Monday or Wednesday
  20. Due to the P-Chem exam, there is no reading or reading quiz for Friday
  21. HW #6 Due date has been extended to 2/26
  22. Pre-quiz for Wed posted
  23. No pre-quiz for Monday
  24. HW 4 and 5 solutions and Lecture slides through Week 6 are posted
  25. Pre-quiz for Fri posted
  26. HW 6 posted
  27. Pre-quiz for Wed posted
  28. Week 5 muddiest and surprising responses are available here
  29. Pre-quiz for Mon posted
  30. No pre-quiz for Fruday
  31. Pre-quiz for Wed posted
  32. Pre-quiz for Mon posted
  33. Pre-quiz for Fri posted
  34. HW 4 and 5 are posted
  35. Course Learning Objectives have been updated.
  36. Exam 1 is on January 31.
    It is closed book and closed notes.
    You may have one 8.5" x 11" sheet of paper with only your own hand writing (both sides is ok), a calculator, and something to write with.
    There will be opportunity in Studio 4 to work with your group for extra credit towards your exam score
  37. Exam 1 from 2016 and 2017 have been posted
  38. Week 3 lecture slides have been posted
  39. No pre-quiz for Monday or Wednesday
  40. Pre-quiz for Fri posted
  41. For HW #3, you do not need to complete problem 6.46 part b
  42. Pre-quiz for Wed posted
  43. Week 2 lecture slides posted
  44. Pre-quiz for Mon posted
  45. HW 1 and HW 2 solutions posted
  46. Approach (model) 3 described in class with sign corrected is provided here
  47. HW 3 posted
  48. Week 1 muddiest and surprising responses are available here
  49. Pre-quiz for Fri posted
  50. For text Problem 6.32, the triple point temperature is 225 K.
  51. Pre-quiz for Wed posted
  52. Week 1 lecture slides posted
  53. Homework #2 Posted.
  54. Pre-quiz for Fri posted
  55. Pre-quiz for Wed Posted
  56. Homework #1 Posted.
  57. Welcome to ChE 312 :)

Weekly Assignments

Week Topic Pre-Lecture
(Complete Quiz on Concept Warehouse)
(Due in Studio)
HW Solution Lecture Slides Topics Covered
Week 1 Review
Pure Species Equilibrium
Before W lecture: Textbook, pages 16-17, 20-24
Before F lecture: Textbook, pages 315-321
HW#1 HW#1Sln Week 1

M:    Introduction; Psat vs. T for a pure substance

W:   intensive vs. extensive properties hv, vv. (CW prob)

         Vacuum video (what causes the ICE?)

F:   Gibbs energy as combined 1st and 2nd

      Gibbs for pure species; C and CC Eqns
Week 2 Pure Species Equilibrium
M: MLK Holiday
W: Textbook, pages: 321-329
F:  Textbook, pages: 334-344
HW#2 HW#2Sln Week 2

W:   Gibbs for pure species; C and CC Eqns

        Looked at vacuum video Gs in terms of what changes deltag  -> arguing sv. F:    Nomenclature developed wrt Studio 2;  Muddiest & Surprising points
Week 3 Mixtures M: Textbook, pages: 334-344
W: Textbook, pages: 344-347, 355
F: Textbook, pages: 357-359, 367-36
HW#3 HW#3Sln Week 3

M:  Discussion of Gibbs ("has units of")  energy; introduction  to multicomponent equilibrium and mixtures; property  definitions and Studio 2

W:  Mixture studio: Would EtOH and H2O separate? Is there a chemical reaction. Pure species Gibbs energy vs. partial molar Gibbs energy as a criteria

F:     Entropy of mixing from a hypothetical path (Studio 3); CW enthalpy of mixing question   
Week 4 Chemical Potential
M: Review Chapter 6
W: Exam 1
F: Textbook, pages: 391-402 
No HW Week 4

M:   Partial molar Gibbs energy and chemical potential; criteria for chemical equilibrium;  volume properties of an ideal gas

F:    Fugacity definition; emphasis on the reference state; criteria for chemical equilibrium
 Week 5 Fugacity in the vapor M: Muddiest / Surprised reflection
W: Work through Examples 7.1, 7.2, 7.3
F:  Graphic text on fugacity p 1-4
Elby Paper
HW#4 Sln Week 5

M:  Fugacity definition; emphasis on the reference state; criteria for chemical equilibrium

W:  Fugacity for a pure vapor; steam tables, vdW equation.

F:    Fugacity from EOS and gen corr.
Week 6 Fugacity in  vapor mixtures
Fugacity in the liquid
M: Textbook, pages: 403-414, Example 7.4
W: Textbook, pages: 414-418
F:  Textbook, pages: 425-436
HW#5 HW#5 Sln Week 6

M: Fugacity of mixtures from EOS; Lewis fugacity rule.

W: Fugacity of mixtures from EOS

F:    Fugacity of liquids: Ideal solutions, Lewis Randall and  Henry's reference states; activity coeff.
Week 7 Fugacity in the liquid, solid M: Textbook, pages: 419-420, 436-441, 449
W: Textbook pages 450-452; Graphic text on             fugacity p 5-8
F:  No Reading
HW#6 Sln Week 7

M:   Models for gE. Two-suffix Margules equation.

W:   Assymetric models for gE. calculation of pure liquid fugacity

F:     Work with phase diagrams and three-suffix Margules  building on Studio 7
Week 8 Phase Equilibria: VLE M: Textbook pages 467-484
W: Exam 2 
F:  Textbook pages 484-486, 495-500
No HW Week 8

M: Phase diagrams, Raoult's law, lever rule

F:    Deviations from RL; Azeotropes; Studio 8 analysis
Week 9 Phase Equilibria: LLE and SLE
Chemical Reaction Equilibria
M: Textbook pages 511-515, 523-531
W: Textbook pages 563-568
F:  Textbook pages 579-580, 586
HW#7 HW#7 Sln Week 9


W: CW Phase diagram CW review

F: Chemical Reaction Equilibrium: Intro
Week 10 Chemical Reaction Equilibria M: Textbook pages 599-602
HW#8 HW#8 Sln Week 10

M: Chemical Reaction Equilibrium: K, extent, and fugacity

W: Chemical Reaction Equilibrium: K from thermochemical data

F:     Review and Final details

Homework assignments are to be turned in at the beginning of class on the due date.


Old Exams

Old exams are avaiilable here for you to practice: 

Exams 1 and 2 from 2016 and 2017 are  available on the link above.  One point of note.  The emphasis on which content we are covering is different this year, so the exam emphasis will also change.

Also ChE 312 had 3 exams  in 2016 - so the timing was different relative to content.

Exam 1

Exam 1 2016

Exam 1 2017

Exam 2

Exam 2 2016

Exam 2 2017


Lecture Handouts

Lecture handouts will be archived here in PDF format.


Course Learning Objectives

By the end of this course, you will be able to:

  1. Pure species phase equilibrium:
    Describe the role of Gibbs energy in determining pure species phase equilibrium.  
    Apply the Clapeyron equation to relate T and P between two states of a pure species in phase equilibrium. State when you can simplify the Clapeyron equation to the Clausius-Clapeyron equation.
    [CBEE 211 & ChE 311] Apply the first law to systems which undergo a phase change.
  2. Thermodynamics of mixtures:
    Apply thermodynamics to mixtures by defining and finding values for pure species properties, total solution properties, partial molar properties, and property changes of mixing.
    Explain enthalpy and entropy of mixing in physical terms.
  3. Fugacity
    Explain how fugacity relates to partial molar Gibbs energy (chemical potential) and why we use it.
    Define fugacity. Explain the role of the reference state (and that T0=T)
  4. Fugacity in the vapor phase: 
    Calculate fugacity and fugacity coefficient for a pure species i using tables, EOS, and generalized correlations.  Identify appropriate data and reference state
    Calculate fugacity and fugacity coefficient for a species i in a mixture using EOS
    Describe the Lewis and ideal gas approximations for fugacity of i in a mixture. Provide physical explanations for the fugacity coefficient
  5. Fugacity in the liquid phase:
    Explain why we choose the ideal solution as a reference state for a liquid. Explain the molecular origin and calculate reference fugacities based on the Lewis/Randall and Henry’s reference states. Identify the "shift" in curves of ln(gamma,i).
    Identify when like or unlike interactions are stronger. Know when the Lewis/Randall reference state equals the saturation pressure and how to correct when it does not.
    Define gE and explain why we use it. Given a model for gE determing an expression for gamma,i. Calculate gamma,i.
  6. Phase Equilibrium:
    Solve phase equilibria problems for Vapor-Liquid equilibria (VLE), Liquid-Liquid equilibria (LLE).
    Identify and solve problems for systems containing azeotropes (VLE) and partially miscible solutions (LLE). Explain what causes each.
    Describe how phase diagrams are constructed. When given any phase diagram, an overall composition, and T or P determine what phase or phases are present. When two phases are present determine their composition and how many total moles are in each phase.
  7. Chemical Reaction Equilibrium:
    Distinguish between reaction rate and reaction equilibrium in a chemically reacting system
    Use thermochemical data to determine the equilibrium composition for a chemical reaction. Calculate the equilibrium constant at different temperatures.
    Determine the equilibrium composition for a system with a single reaction or multiple chemical reactions in a single phase or for heterogeneous reactions



Studio 1
Studio 1 Simulation
Studio 10
Sec Day/Time/Date Location Curr Instructor
1 MWF 1000-1050 LINC 210 139 Milo Koretsky
11 R 1300-1350 BEXL 102 24 Alyssa Saito
Ryan Cashen
12 R 1300-1350 BEXL 103 24 Jad Touma
Connor Haynes
13 R 1400-1450 BEXL 102 23 Allysa Saito
Ryan Cashen
14 R 1400-1450 BEXL 103 22 Lynza Sprowl
Ayman Alabdullatif
15 R 1500-1550 BEXL 102 23 Jad Touma
Connor Haynes
16 R 1500-1550 BEXL 103 23 Lynza Sprowl
Ayman Alabdullatif