Syllabus for CHE0200 Chemical Engineering Thermodynamics Class 19309 Section 1030 Spring 2018 Lectures: M,W,F 8-9:50am, Room 309 BEH Recitations: Th 8-9:50am, Room 309 BEH Instructor: Prof. Karl Johnson Office: 904 BEH Phone: 412-624-5644 Email: karlj@pitt.edu Office hours: M 1:00-3:00pm and by appointment TA: Jon Ruffley Office: 1143D BEH Email: jpr54@pitt.edu Office hours: W, F, 2:00-4:00 pm TA: Nguyen Vo Office: 1143D BEH Email: miv22@pitt.edu Office hours: T, Th 1:00-3:00pm Required text: Engineering and Chemical Thermodynamics, 2 nd Edition, Milo D. Koretsky, Wiley Required software: TurningPoint from Turning Technologies for in class poll questions. Register through Courseweb. Cost: $17.99 per semester. Use Session ID KarlJohnson when polling. Recommended software: MATLAB Philosophy This course presents a detailed examination of chemical engineering thermodynamics at both a continuum and molecular level. The course covers the first and second laws of thermodynamics, equations of state and intermolecular interactions, the mathematical foundation and tools of thermodynamics, departure functions, partial molar properties, phase equilibria for pure materials and mixtures (vapor-liquid, liquid-liquid, vapor-liquid-liquid, solid-liquid, solid-solid), and chemical reaction equilibria. The course is roughly equivalent to a two-semester 3-credit series of courses in thermodynamics, which at some universities is divided into pure materials in the first semester and mixtures in the second semester. As such, most students find this to be a demanding course requiring significant time and effort to master. Audience This class is intended for chemical engineering undergraduate students in their sophomore year, having taken CHE0100 and the other prerequisites. Course Learning Objectives Learning objectives are stated at the beginning of each chapter of the text Engineering and Chemical Thermodynamics. The course objectives are aligned with the learning objectives for each chapter. A partial list of objectives is given here. At the end of this course, students should be able to: 1
Given two properties, identify the phases present on a PT or a Pv phase diagram, including solid, subcooled liquid, saturated liquid, saturated vapor, and superheated vapor and two-phase regions. Use the steam tables to identify the phase of a substance and find the value of desired thermodynamic properties with two independent properties specified, using linear interpolation if necessary. Write the integral and differential forms of the first law for (1) closed systems and (2) open systems under steady-state and transient (uniform-state) conditions. Convert these equations between intensive and extensive forms and between mass-based and molar forms. Given a physical problem, evaluate which terms in the equation are important and which terms are negligible or zero and determine whether the ideal gas model or property tables should be used to solve the problem. Apply the first law of thermodynamics to identify, formulate, and solve engineering problems for adiabatic and isothermal processes in the following types of systems: rigid tank, expansion/compression in a piston cylinder assembly, nozzle, diffuser, turbine, pump, heat exchanger, throttling device, filling or emptying of a tank, and Carnot power and refrigeration cycles. Create an appropriate hypothetical path to solve these problems with available data. Apply the second law of thermodynamics to identify, formulate, and solve engineering problems for isothermal and adiabatic processes in the following systems: rigid tank, expansion/compression in a piston cylinder assembly, nozzle, diffuser, turbine, pump, heat exchanger, throttling device, filling or emptying of a tank, and vapor compression power and refrigeration cycles. Develop a hypothetical reversible path to calculate the entropy change between any two states. Develop the expression for the entropy change of an ideal gas, a liquid, or a solid when the heat capacity is known. Calculate the entropy difference between two states if you are given either heat capacity data or property tables. Calculate entropy changes for species undergoing phase change or chemical reaction. State the molecular assumptions of an ideal gas. Describe how the terms in the van der Waals equation relax these assumptions. Identify how the general form of cubic equations of state accounts for attractive and repulsive interactions in a similar manner. State the principle of corresponding states on molecular and macroscopic levels. Apply this principle to develop expressions to solve for parameters in equations of state from the critical property data of a given species. Describe why the acentric factor was introduced and its role in constructing the generalized compressibility charts. Define a departure function. Use generalized enthalpy and entropy departure functions to solve first- and second-law problems for systems that exhibit nonideal behavior. Define a partial molar property and describe its role in determining the properties of mixtures. Calculate the value of a partial molar property for a species in a mixture from analytical and graphical methods. Apply the Gibbs Duhem equation to relate the partial molar properties of different species. Identify the role of the chemical potential that is, the partial molar Gibbs energy as the chemical criteria for equilibrium. 2
Calculate the pure species fugacity of a liquid or solid at high pressure using the Poynting correction. Identify how you correct a value of Henry s law for different pressures or temperatures. Define fugacity, fugacity coefficient, activity, activity coefficient, and excess Gibbs energy. State the criteria for chemical equilibrium in terms of fugacity. State why the excess Gibbs energy is useful for empirical models of activity coefficients. Identify when a binary mixture exhibits an azeotrope. Distinguish between maximum and minimum boiling azeotropes and explain this behavior in terms of intermolecular interactions. Use azeotropic data to determine activity coefficient model parameters. Use thermochemical data to determine the equilibrium constant for a chemical reaction at any given temperature. For a determined reaction stoichiometry and initial reactant composition, write the equilibrium constant in terms of the extent of reaction for gas- phase, liquid-phase, and heterogeneous reactions for ideal or nonideal systems. ABET Student Learning Outcomes This course addresses the following ABET Student Outcomes: (1) Ability to identify, formulate and solve complex engineering problems by applying principles of engineering, science and mathematics. This will be accomplished through lectures, in-class exercises, homework, and quizzes. (4) Ability to recognize ethical and professional responsibilities in engineering situations and make informed judgements, which must consider the impact of engineering solutions in global, economic, environmental and social contexts (5) Ability to function effectively on a team whose members together provide leadership, create a collaborative and inclusive environment, establish goals, plan tasks and meet objectives. This will be accomplished through a group design project. (7) Ability to acquire and apply new knowledge as needed, using appropriate learning strategies. This will be accomplished through quizzes on assigned reading material, in-class peer instruction exercises, and instruction on problem solving strategies. Grading Grades will be given on a modified straight scale. Grades will not be curved to artificially manipulate the number of As, Bs, etc. Grading on a curve discourages appropriate team work; learning to work in teams is an important part of engineering training. Points will be given for homework, a design project, quizzes, class participation, three midterm exams, and a final exam. Exam scores will be normalized as needed (e.g., if the exam is too hard). Extra credit points may be given for things like filling out surveys, etc. The weighting for each of these is given below. Homework 10% Design project 10% Quizzes 10% Class participation 5% Midterm exams (each) 15% Final Exam 20% 3
Class participation will be assessed through punctual attendance and participation with in-class interactive questions (through TurningPoint). The final grades will be based on the following scale: Weighted Score Grade 85% A- or higher 75 to < 85% B- to B+ 65 to < 75% C- to C+ 60 to < 65% D- to D+ <60% F Disability Statement If you have a disability for which you are or may be requesting an accommodation, you are encouraged to contact both your instructor and Disability Resources and Services, 140 William Pitt Union, 412-648- 7890 or 412-383-7355 (TTY) as early as possible in the term. DRS will verify your disability and determine reasonable accommodations for this course. Counseling The University Counseling Center's staff is dedicated to assisting students in their pursuit of personal and academic growth, to helping students gain a better understanding and appreciation of themselves, and to supporting students as they make important decisions about their lives. If you are in need of counseling services, please contact the University Counseling Center at 334 William Pitt Union (412) 648-7930. Refer to http://www.counseling.pitt.edu for details. Technology: Cellular Telephones, Recording Classes, etc. You may use devices (cell phone, tablets, laptops, etc.) to access polls that will be given in most every class. However, please make every effort to be here when you are here. Please do not check social media, engage in texting, or other use of your device that is not directly related to this class while you are in class. Please put your devices away (out of sight) when not used for the online polls. To ensure the free and open discussion of ideas, students may not record classroom lectures, discussion and/or activities without the advance written permission of the instructor, and any such recording properly approved in advance can be used solely for the student s own private use. Other use of such a recording is a violation of University policy and will be pursued through the appropriate University channels. Academic Integrity See http://www.as.pitt.edu/fac/policies/academic-integrity for the University Guidelines on Academic Integrity and http://www.engineering.pitt.edu/academic-integrity-guidelines/ for Swanson School of Engineering guidelines. Copying someone else's work or allowing someone else to copy your work is unacceptable and a clear violation of academic integrity. You should not borrow homework, homework solutions, exams, or other materials from students who took this or a similar course. You should not 4
copy homework solutions from any source whatsoever. Doing so only defeats the purpose of doing homework, which is to help you master the material and to teach you critical thinking and problem solving skills. Exams, whether in class or take home, must be strictly each student's individual effort. You must not discuss the exams with anyone but the instructor. Any violation of the Academic Integrity code will be prosecuted to the fullest extent possible. Homework You may work in groups of up to 3, but each person responsible for working each problem! Each group should turn in a single copy of the homework with names of all group members. If someone does not contribute, do NOT put their name on it. Homework will be due at the beginning of class and will be accepted up to 5 minutes after the start of class. It will be marked late if received after that. If received by 5:00 PM on the due date you will receive a 50% penalty and zero if turned in after that. Each problem will be scored as follows: Completely correct: 2 (MATLAB problems may count double) Partially correct: 1 Incorrect or no significant effort: 0 Design Project The purposes of the design project are to (1) help you lean to function effectively as a team; (2) develop the ability to acquire and apply new knowledge; (3) practice and improve your ability to write computer programs using a high-level language (e.g., MATLAB or Python); (4) develop a deep understanding of how cubic equations of state are used. More details about the project will be given later on, but the project will probably involve the following: 1. Write a computer code that will use the Peng-Robinson EOS to solve for P or V given T and V or P for any pure fluid for which parameters are available. 2. Incorporate the van der Waals mixing rules in the code to allow calculation of binary mixtures. 3. Compute fugacity coefficients for binary mixtures. 4. Test your code by comparing with output from ASPEN or ThermoSolver. 5
Schedule Date Topic Reading Assignment 1/8 Introduction, properties 1/10 States, equilibrium Preface, 1.1-1.4 1/12 Phase rule, phase surfaces, steam tables 1.5-1.8 1/15 No class MLK Holiday 1/17 First law, energy 2.1-2.2 1/19 First law, processes, efficiency 2.3-2.5 1/22 First law, open systems 2.6 1/24 First law, processes 2.7 1/26 First law, open-system energy balances 2.8 1/29 First law, thermodynamic cycles 2.9-2.10 1/31 First law, review 2.1-2.10 2/2 Midterm #1 Room G24 Cathedral of Learning 2/5 Second law, directionality of processes 3.1-3.2 2/7 Second law, entropy 3.3-3.4 2/8 (Th) Second law, open and closed systems 3.5-3.6 2/9 Second law, ideal gases, mechanical energy balances 3.7-3.8 2/12 Second law, Rankine cycle 3.9 2/14 Second law, Exergy 3.10 2/16 Second law, molecular view of entropy 3.11-3.12 2/19 Second law, review 3.1-3.12 2/21 Intermolecular forces 4.1-4.2 2/23 Equations of state, van der Waals, etc. 4.3 2/26 Generalized compressibility charts 4.4 2/28 Review 3/2 Midterm #2 Room G24 Cathedral of Learning 3/5-3/9 Spring Break for undergraduate students 3/12 Equations of state, mixtures 4.5-4.6 3/14 Thermodynamic web 5.1-5.3 3/16 Departure functions 5.4 3/19 Conditions for equilibrium, Clapeyron equation 6.1-6.2 3/21 Mixture properties, partial molar properties 6.3 3/23 Multicomponent phase equilibria, chemical potential 6.4-6.5 3/26 Fugacity 7.1-7.3 3/28 Activity coefficients 7.4 3/30 Models for activity coefficients, fugacity of solids 7.4-7.6 4/2 Phase equilibrium 8.1 4/4 Review 4/6 Midterm #3 Room G24 Cathedral of Learning 4/9 Liquid-liquid & solid-liquid equilibrium, colligative properties 8.2-8.6 4/11 Chemical reactions 9.1-9.3 4/12 (Th) Equilibrium constants 9.4-9.5 4/13 Calculating chemical reaction equilibrium 9.4-9.5 4/16 Electrochemical reactions, multiple reactions 9.6-9.7 4/18 Point defects in solids 9.8-9.9 4/20 Review 4/23 4:00 pm Final Exam G24 CL 6