ChE 312
Chemical Engineering Thermodynamics

Winter 2018

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

Instructors
Name email Office Hours
Lead Instructors Milo Koretsky (MK) milo.koretsky@oregonstate.edu  T 4-6 Gleeson 200
Natasha Mallette natasha.mallette@oregonstate.edu
Teaching Assistants Alyssa Saito saitoal@oregonstate.edu  T 4-6 Gleeson 200
Lynza Sprowl halbersl@oregonstate.edu  W 4-6 Gleeson 200
Jad Touma toumaj@oregonstate.edu  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

 


Announcements

  1. For text Problem 6.32, the triple point temperature is 225 K.
  2. Pre-quiz for Wed posted
  3. Week 1 lecture slides posted
  4. Homework #2 Posted.
  5. Pre-quiz for Fri posted
  6. Pre-quiz for Wed Posted
  7. Homework #1 Posted.
  8. Welcome to ChE 312 :)

Weekly Assignments

Week Topic Pre-Lecture
(Complete Quiz on Concept Warehouse)
Homework
(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
Mixtures
M: MLK Holiday
W: Textbook, pages: 321-329
F:  Textbook, pages: 334-344
HW#2 HW#2Sln Week 2

W:  Tie HW 1 as conceptual model in thermo 

       Gibbs for pure species; C and CC Eqns

F:    Looked at vacuum video Gs in terms of what changes deltag  -> arguing sv. Muddiest points
Week 3 Mixtures M: Textbook, pages: 344-347, 355
W: Textbook, pages: 357-359, 367-369
F: No reading!
HW#3 HW#3Sln Week 3

M:  Nomenclature developed wrt Studio 2

W:  Hypothetical paths: CW hw problem discussed emphasis of identifying phenomena and available data

F:     Entropy of mixing from a hypothetical path – CW question with a reversible                   path
Week 4 Chemical Potential
Fugacity
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:     Partial molar properties vs. pure species properties (vis Exam 1 Q1; relate to membrane separation)
 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
HW#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:  Textbook, pages: 467-483
HW#6
Problems 1-3
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: Exam 2
W: Textbook pages 467-484
F:  Textbook pages 484-486, 495-500
HW#6
Problem 4
HW#6 Sln
Problem 4
Week 8

W: 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

M: LLE (Prof. Mallette)

W: CW Phase diagram CW review

F: Chemical Reaction Equilibrium: Intro
Week 10 Chemical Reaction Equilibria M: Textbook pages 599-602
W:
F:
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.

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Old Exams

Old exams are avaiilable here for you to practice:

Exam 1 2016

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

ChE 312 had 3 exams  in 2016 - so the timing was different relative to content. Both exams 2 and 3 are posted below.

           
          Exam 2 2016

Exam 3 2016

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Lecture Handouts

Lecture handouts will be archived here in PDF format.

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Course Learning Objectives

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

  1. Describe the role of Gibbs energy in determining pure species phase equilibrium. Apply the Clapeyron equation to relate T and P for a pure species in phase equilibrium.
  2. Apply thermodynamics to mixtures by defining and finding values for pure species properties, total solution properties, partial molar properties, and property changes of mixing. Apply the Gibbs-Duhem equation to relate partial molar properties.
  3. Find the fugacity and fugacity coefficient of pure gases and gases in mixtures using tables, equations of state, and general correlations.
  4. For liquids and solids, identify Lewis/Randall and Henry’s Law reference states for ideal solutions. Correct the reference states for pressure. Solve for non-ideality by determining activity coefficients through models for excess Gibbs energy, gE.
  5. Solve phase equilibria problems for Vapor-Liquid equilibria (VLE) , Liquid-Liquid equilibria (LLE), vapor - liquid - liquid equilibria (VLLE) and Solid-Liquid equilibria (SLE). Identify and solve problems for systems containing azeotropes (VLE) and partially miscible solutions (LLE).
  6. 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 multiple chemical reactions.

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Studios

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

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Links

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