ChE 312
Chemical Engineering Thermodynamics

Winter 2019

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

Name email Office Hours
Lead Instructors Milo Koretsky (MK) Gleeson 200 Tu 4-6 PM
Kostas Goulas  Gleeson 200 W 2-4 PM
Teaching Assistants Fuqiong Lei Gleeson 200 Tu 4-6 PM
Marjan Khorshidi Zadeh Gleeson 200 W 2-4 PM
Teaching/Learning Assistant Ryan Cashen
Learning Assistant Mark Li

AIChE Concept Warehouse

The general syllabus for course is available here.


Page Contents



  1. HW 3 posted (01/18)
  2. HW 2 Solutions posted (1/17)
  3. Week 1 Muddiest / Suprised points are here.
  4. Please bring your laptop to Studio in Week 2 (1/14)
  5. Week 1 Lecture Notes posted (1/11)
  6. Homework #2 Posted (1/11)
  7. Jamil found another vacuum video here
  8. HW 1 Solutions posted (1/11)
  9. You can find your GTA here (1/8).
  10. You should now have access to Gradescope. Please use the School Credentials tab to log on (1/8).
  11.  Homework #1 Posted. (12/31)
  12. Welcome to ChE 312 :)

Weekly Assignments

Week Topic Pre-Lecture
(Complete Quiz on Concept Warehouse)
(Due Thursday by 1 PM)
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:    Scientific reasoning; Vacuum  video

F:      Models and modeling: Vacuum; home heating; outdoor pizza oven

Week 2 Pure Species Equilibrium
W: Textbook, pages: 321-329
F:  Textbook, pages: 334-344
HW#2 HW#2Sln Week 2

M:    Gibbs Energy as combined first and second laws; criteria for chemical equilibrium of a pure specties; Muddiest/Surprised Points

W:   Clayperon and Clausius Clayperon equations

Week 3 Mixtures M: MLK Holiday
W: Textbook, pages: 344-347, 355
F: Textbook, pages: 357-359, 367-36
HW#3 HW#3Sln Week 3

M: Martin Luther King Jr. Day


Week 4 Chemical Potential
M: Review Chapter 6
W: Exam 1
F: Textbook, pages: 391-402 
No HW Week 4


W:   Exam 1 (individual)

 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



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



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



Week 8 Phase Equilibria: VLE M: Textbook pages 467-484
W: Exam 2 
F:  Textbook pages 484-486, 495-500
No HW Week 8


W:   Exam 2 (individual)

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



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




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 2017 and 2018 are  available on the links below.  One point of note.  The emphasis on which content we are covering is different this year, so the exam emphasis will also change.

Exam 1

Exam 1 2017

Exam 1 2018

Exam 2

Exam 2 2017

Exam 2 2018


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



Sec Day/Time/Date Location Curr Instructor
1 MWF 1000-1050 LINC 210 103 Milo Koretsky
Kostas Goulas
11 R 1300-1350 BEXL 102 21 Fuqiong Lei
Ryan Cashen
12 R 1300-1350 BEXL 103 21 Marjan Khorshidi Zadeh
Mark Li
13 R 1400-1450 BEXL 102 21 Fuqiong Lei
Ryan Cashen
14 R 1400-1450 BEXL 103 21 Marjan Khorshidi Zadeh
Mark Li
15 R 1500-1550 BEXL 102 19 Ryan Cashen
Mark Li