Course Syllabus
FAYETTEVILLE STATE UNIVERSITY
DEPARTMENT OF CHEMISTRY AND PHYSICS
COLLEGE OF ARTS AND SCIENCES
Syllabus
CHEM 313 - 01
PHYSICAL CHEMISTRY I
Fall 2018
1 LOCATOR INFORMATION
Lecture schedule: MWF 11:00 - 11:50 AM, LSA130
Lecturer: Dr. Jairo Castillo-Chará
Office: ST 313
Telephone: (910) 672-2062
Office Hours: M 9:00 - 11:00 am, T 11:00am -1:00pm, R 2:00 - 4:00pm, F 12:00 - 2:00pmand by appointment
e-mail: jcastill@uncfsu.edu
Website: http://faculty.uncfsu.edu/jcastill/
FSU Policy on Electronic Mail: Fayetteville State University provides to each student, free of charge, an electronic mail account (username@uncfsu.edu) that is easily accessible via the Internet. The university has established FSU email as the primary mode of correspondence between university officials and enrolled students. Inquiries and requests from students pertaining to academic records, grades, bills, financial aid, and other matters of a confidential nature must be submitted via FSU email. Inquiries or requests from personal email accounts are not assured a response. The university maintains open-use computer laboratories throughout the campus that can be used to access electronic mail.
Rules and regulations governing the use of FSU email may be found at
http://www.uncfsu.edu/PDFs/EmailPolicyFinal.pdf
2 COURSE DESCRIPTION
CHEM 313 – 01:This is the first of two-semester sequence course to present the fundamentals of physical chemistry from the macroscopic point of view. Without losing rigorousness, the essential ideas of physical chemistry will be introduced hopefully in a way that would be interesting, comprehensible and enjoyable to students with a background of one year of college calculus and physics. The lectures in this class will cover thermodynamics, kinetics and chemical change.
2.1 Motivation
The main objective of physical chemistry is the understanding of structure, properties and transformations of matter, from macroscopic behavior to mechanisms that operate at molecular level. Physical chemists collect, select and analyze experimental data from all areas of chemistry and use this information to construct models capable of predicting new phenomena. Physical chemistry permeates much of the modern science and constitutes a driving force promoting scientific advances in a wide range of fields. Based on concepts from chemistry, physics and mathematics, physical chemistry contributes to many areas of science as diverse as medicine, molecular biology, molecular engineering, chemical engineering, materials and earth sciences.
2.2 Course Prerequisites:
This course assumes that the students have taken college calculus (MATH 241-2), physics (PHYS 121) and chemistry (CHEM 210). An introduction course in differential equations will be useful, however provisions will be made during the course to satisfy this requirement.
3 DISABLED STUDENT SERVICES:
In accordance with Section 504 of the 1973 Rehabilitation Act and the Americans with Disabilities
Act (ACA) of 1990, if you have a disability or think you have a disability to please contact the Center for Personal Development in the Spaulding Building, Room 155 (1st Floor); 910-672-1203.
4 TEXTBOOK
- Thomas Engel and Philip Reid, Physical Chemistry, 3rd Edition, Pearson, 2013.
5 CHEM 313 GOALS:
- The most important goal in CHEM313 is the understanding of the three laws of thermodynamics and how to apply the laws to chemical systems.
- The understanding of the thermodynamic basis of chemical equilibrium.
- And finally to understand how the physical laws enable us to understand the fundamental principles of chemistry in an abstract way.
6 STUDENT LEARNING OUTCOMES:
After completion of the first course in physical chemistry, students are expected:
- To be able to learn and apply the basic language of thermodynamics to the study of chemical systems.
- To become familiar with the applications of thermodynamics in different areas of chemistry.
- To be able to solve physical chemistry problems based on critical analysis of the available data and by the appropriated use of concepts and mathematical tools.
- To relate the principles, methods, theories and models of physical chemistry to other areas of chemistry and other areas of science such as biology, physics, earth sciences, and engineering.
- To increase their familiarity with the use of tables of thermodynamic data to calculate thermodynamic functions and to sharpen their graphing interpretation skills.
- To be familiar with spread sheet software to analyze, solve and visualize problems in physical chemistry and related areas.
- To be prepared to take advanced, senior-level and graduate courses in chemistry, biochemistry and physics.
7 COURSE REQUIREMENTS AND EVALUATION CRITERIA
7.1 Homework Policy
- Homework will be given during Friday class and should be completed in approximately two weeks and submitted on Friday by 5:00 PM. You can turn in your homework during class or bring it to my office.
- Homework problems should be neatly written to make sure that the instructor understands your solutions (not credit will be given for confusing, unreadable work). I advise you to work out your solution first, then do all the necessary editing as you do when you write a paper. This process will allow you to eliminate any errors and to deliver a more professional work.
- Each time that you submit the homework make sure that you write your name, date and problem set number or chapter number.
- Homework turned in late will be graded at a rate of 10 % per day late (you will lost 10 points per day late)
- The problem sets will be graded according to the following scale: ”satisfactory effort” (100%), ”need improvement” (50%) and ”unsatisfactory effort” (0 %).
- Questions about homework or questions related to grading will be discussed during office hours. If you cannot see the instructor at the office hours cited above, you can email or call to make an appointment that suit your schedule.
7.2 Grading
This course will be graded on a maximum of 100 points distributed as follows:
|
Section |
% |
|
|
Three hour Exams |
45 |
|
|
Final Exam + ACS Test |
25 |
|
|
Homework |
30 |
|
|
Total |
100 Points |
|
|
Percentile Points |
Letter Grade |
|
|
92 - 100% |
A |
|
|
83 - 91% |
B |
|
|
73 - 82% |
C |
|
|
64 - 72% |
D |
|
|
63 or less % |
F |
|
Your course grade will be determined using the total number of points that you have accumulated during the semester.
7.3 Make up Examination Policy:
There will be no make-up examinations except in the case of serious illness or accident (properly documented), family emergency, or participation in University official activities (class field trips, etc.). For the latter case, make up-examination arrangements must be made in advance.
7.4 Due Date Assignments Policy:
The final due date for any assignment (homework, exams, or any other assignment) is by 5:00 PM of the day of the final exam date, Dec. 10thof 2018.After this date no assignments will be accepted.
7.5 REVISION OF GRADES - STUDENTS RESPONSIBILITIES
Absences from class will be handled following strictly the University policy. Absences of more than 10 % of the total contact hours the course meets during the semester, which is approximately seven (7) total hours of unexcused absences will fall in the category of ’EXCESSIVE ABSENCES-EA’. As indicated in the new guidelines, ’WN’ grade has been eliminated and it is the STUDENT’S RESPONSIBILITY TO WITHDRAW HIMSELF OR HERSELF FROM THE CLASS. Please, check the ’Revision of Grades-Student Responsibilities’ at:
www.uncfsu.edu/fsuretension/policiesprocedures.htm. A copy of the Revision of Grades-Student Responsibilities has been provided in the last page of this document.
X GRADE (NO SHOW): will be assigned to any student on the roster that did not attend during the first week of classes or, in on line classes, did not interact with class website during the first week of classes. Since X grade is not a final grade, it can be removed if the student begins attending class.
EA GRADE (EXCESSIVE ABSENCES): will be assigned to students whose absences exceed 10 % of class contact hours. After the grade has been assigned the student will be warranted in order for them to take the corrective action.
NEW FINAL GRADE: FN (FAILURE DUE TO NON-ATTENDANCE) Final grade for students who are on class roster, but never attend the class. An FN grades is equivalent to an F grade in the calculation of the GPA.
7.6 Academic Integrity Statement
One of the fundamental pillars of the university is the academic and personal integrity of all its members. You must be truthful and honest at all times and must be aware of what kind of situations and activities constitute ethical violations. In this class the following activities or situations will be considered violations of the ethical code and will be punished accordingly: cheating on exams, plagiarism (misrepresentation of materials obtained from the Internet or from other sources), lying, helping someone else to cheat, reuse of assignments, unauthorized collaboration, alteration of graded assignments, forgery, falsification and unfair competition. Please, report any violation to the instructor. Unauthorized cheating is not limited only to those enumerated above, for a more complete list you are advised to consult the Fayetteville State University Student Handbook. Any form of cheating is considered as an academic dishonesty. Cheating in this class will be punished with an F for the exam or for any other assignment where the cheating is discovered.
The use of programmable calculators is strictly forbidden during exams and quizzes, try to bring a simple no programmable calculator if you need one during the exam. Avoid the use of cell phones during the exam and class time, this affects the concentration and distract your peers.
7.7 Student Behavioral Expectations
- Students are expected to arrive to class on time, remain in class until dismissed by the instructor, and refrain from preparing to leave class until it is dismissed.
- Students should avoid passing notes or carrying on private conversations while class is being conducted.
- Students should avoid the use profanity in the classroom.
- Any form of cheating is considered an academic dishonesty or misconduct and will bepunished. For information about disciplinary measures and university policies for academic misconduct, read the Fayetteville State University Student Handbook.
- Students should avoid the use of cell phones during exams and class time, this affects the concentration and distract your peers.
7.8 Consequences For Failing to Meet Behavioral Expectations
With first time violation of one of the rules above, he or she will be warn privately by the instructor after or before next class. Second time violations will be punished by deducting as many as twenty points from the student’s next exam grade. With third time violations, the student will be reported to the Dean of Students for disciplinary action according to the FSU Code of Student Conduct.[8]
8 ACADEMIC SUPPORT RESOURCES
The instructor will try to make available any additional material that will be required for the proper instruction of students, through the canvas website (https://adfs3.uncfsu.edu/), and the instructor web site (http://faculty.uncfsu.edu/jcastill/).
Other off campus resources are available at: NIST Chemistry WebBook, NIST Standard Reference
Database Number 69: http://webbook.nist.gov/chemistry/
Topics in Thermodynamics: http://www.le.ac.uk/chemistry/thermodynamics/
9 COURSE OUTLINE
Chapter/Section Topic page
1 Fundamental Concepts of Thermodynamics 1
1.1 What Is Thermodynamics and Why Is It Useful? 1
1.2 The Macroscopic Variables Volume, Pressure, and Temperature 2
1.3 Basic Definitions Needed to Describe Thermodynamic Systems 6
1.4 Equations of State and the Ideal Gas Law 7
1.5 A Brief Introduction to Real Gases 10
2 Heat, Work, Internal Energy, Enthalpy, and the First Law of Thermodynamics 17
2.1 The Internal Energy and the First Law of Thermodynamic 17
2.2 Work 18
2.3 Heat 21
2.4 Doing Work on the System and Changing the System Energy from a Molecular Level Perspective 23
2.5 Heat Capacity 25
2.6 State Functions and Path Functions 28
2.7 Equilibrium, Change, and Reversibility 30
2.8 Comparing Work for Reversible and Irreversible Processes 31
2.9 Determining U and Introducing Enthalpy, a New State Function 34
2.10 Calculating q, w, U, and H for Processes Involving Ideal Gases 35
2.11 The Reversible Adiabatic Expansion and Compression of an Ideal Gas 39
3 The Importance of State Functions: Internal Energy and Enthalpy 45
3.1 The Mathematical Properties of State Functions 45
3.2 The Dependence of U on V and T 50
3.3 Does the Internal Energy Depend More Strongly on V or T ? 52
3.4 The Variation of Enthalpy with Temperature at Constant Pressure 55
3.5 How Are CPand CV Related? 57
3.6 The Variation of Enthalpy with Pressure at Constant Temperature 58
3.7 The Joule-Thomson Experiment 60
3.8 Liquefying Gases Using an Isenthalpic Expansion 63
4 Thermochemistry 67
4.1 Energy Stored in Chemical Bonds Is Released or Taken Up in Chemical Reactions 67
4.2 Internal Energy and Enthalpy Changes Associated with Chemical Reactions 68
4.3 Hess’s Law Is Based on Enthalpy Being a State Function 71
4.4 The Temperature Dependence of Reaction Enthalpies 73
4.5 The Experimental Determination of U and H for Chemical Reactions 75
4.6 (Supplemental) Differential Scanning Calorimetry 77
5 Entropy and the Second and Third Laws of Thermodynamics 85
5.1 The Universe Has a Natural Direction of Change 85
5.2 Heat Engines and the Second Law of Thermodynamics 86
5.3 Introducing Entropy 90
5.4 Calculating Changes in Entropy 91
5.5 Using Entropy to Calculate the Natural Direction of a Process in an Isolated System 96
5.6 The Clausius Inequality 97
5.7 The Change of Entropy in the Surroundings 98
5.8 Absolute Entropies and the Third Law of Thermodynamics 101
5.9 Standard States in Entropy Calculations 104
5.10 Entropy Changes in Chemical Reactions 105
5.11 (Supplemental) Energy Efficiency: Heat Pumps, Refrigerators, and Real Engines 106
5.12 Using the Fact that S Is a State Function to Determine the Dependence of S on V and T 115
5.13 The Dependence of S on T and P 117
5.14 The Thermodynamic Temperature Scale 118
6 Chemical Equilibrium 125
6.1 The Gibbs Energy and the Helmholtz Energy 125
6.2 The Differential Forms of U , H , A, and G 130
6.3 The Dependence of the Gibbs and Helmholtz Energies on P, V, and T 132
6.4 The Gibbs Energy of a Reaction Mixture 134
6.5 The Gibbs Energy of a Gas in a Mixture 135
6.6 Calculating the Gibbs Energy of Mixing for Ideal Gases 136
6.7 Calculating DGRfor a Chemical Reaction 138
6.8 Introducing the Equilibrium Constant for a Mixture of Ideal Gases 139
6.9 Calculating the Equilibrium Partial Pressures in a Mixture of Ideal Gases 141
6.10 The Variation of KP with Temperature 142
6.11 Equilibria Involving Ideal Gases and Solid or Liquid Phases 145
6.12 Expressing the Equilibrium Constant in Terms of Mole Fraction or Molarity 146
6.13 The Dependence of the Extent of Reaction on T and P 147
6.14 (Supplemental) A Case Study: The Synthesis of Ammonia 148
6.15 (Supplemental) Expressing U and H and Heat Capacities Solely in Terms of Measurable Quantities 153
6.16 (Supplemental) Measuring for the Unfolding of Single RNA Molecules 157
6.17 (Supplemental) The Role of Mixing in Determining Equilibrium in a Chemical Reaction 158
7 The Properties of Real Gases 165
7.1 Real Gases and Ideal Gases 165
7.2 Equations of State for Real Gases and Their Range of Applicability 166
7.3 The Compression Factor 170
7.4 The Law of Corresponding States 173
7.5 Fugacity and the Equilibrium Constant for Real Gases 175
8 Phase Diagrams and the Relative Stability of Solids, Liquids, and Gases 181
8.1 What Determines the Relative Stability of the Solid, Liquid, and Gas Phases? 181
8.2 The Pressure–Temperature Phase Diagram 184
8.3 The Phase Rule 190
8.4 The Pressure–Volume and Pressure–Volume–Temperature Phase Diagrams 191
8.5 Providing a Theoretical Basis for the P–T Phase Diagram 193
8.6 Using the Clausius–Clapeyron Equation to Calculate Vapor Pressure as a Function of T 194
8.7 The Vapor Pressure of a Pure Substance Depends on the Applied Pressure 196
8.8 Surface Tension 197
8.9 (Supplemental) Chemistry in Supercritical Fluids 201
8.10 (Supplemental) Liquid Crystal Displays 202
9 Ideal and Real Solutions 209
9.1 Defining the Ideal Solution 209
9.2 The Chemical Potential of a Component in the Gas and Solution Phases 211
9.3 Applying the Ideal Solution Model to Binary Solutions 212
9.4 The Temperature–Composition Diagram and Fractional Distillation 216
9.5 The Gibbs–Duhem Equation 218
9.6 Colligative Properties 219
9.7 The Freezing Point Depression and Boiling Point Elevation 220
9.8 The Osmotic Pressure 222
9.9 Real Solutions Exhibit Deviations from Raoult’s Law 224
9.10 The Ideal Dilute Solution 227
9.11 Activities Are Defined with Respect to Standard State 229
9.12 Henry’s Law and the Solubility of Gases in a Solvent 232
9.13 Chemical Equilibrium in Solutions 233
9.14 Solutions Formed from Partially Miscible Liquids 237
9.15 The Solid-Solution Equilibrium 238
10 HOMEWORK ASSIGNMENT
|
TOPIC |
CHAP. |
ASSIGNED PROBLEMS |
|
|
Fundamental Concepts |
1 |
Q1.6, Q1.8, Q1.10, P1.2, P1.7, P1.10, P1.11, P1.16, P1.18, P1.20, P1.28 |
|
|
The Properties of Real Gases |
7 |
Q7.4, Q7.5, Q7.8, Q7.11, Q7.18, P7.2, P7.5, P7.11, P7.19, P7.21 |
|
|
Heat, Work and Internal Energy ***EXAM I Sept. 3rd week **** |
2 |
Q2.2, Q2.5, P2.14, P2.19, P2.31,P2.33, P2.34, P2.44 |
|
|
Internal Energy and Enthalpy |
3 |
Q3.7, Q3.11, Q3.12, Q3.14, Q3.20, P3.3, P3.4, P3.9, P3.12, P3.20, P3.26, P3.27, P3.31, P3.32 |
|
|
Thermochemistry ***EXAM II Oct. 3rd week **** |
4 |
Q4.2, Q4.3, Q4.4, Q4.6, Q4.7, 4.10, Q4.12, Q4.14, Q4.15, Q4.16, P4.1, P4.4, P.4.6, P4.14, P4.18, P4.19, P4.22, P4.31 |
|
|
Entropy, the Second and Third Law |
5 |
Q5.1,Q5.3, Q5.6, Q5.9, Q5.11, Q5.12, P5.1, P5.6, P5.7, P5.16, P5.22, P5.27, P5.39 |
|
|
Chemical Equilibrium ***EXAM III Nov. Last week**** |
6 |
Q6.3, Q6.5, Q6.7, Q6.9, P6.2, P6.5, P6.15, P6.18, P6.23, P6.24, P6.29, P6.35 |
|
|
Phase Diagrams |
8 |
Q8.1, Q8.2, P8.18, P8.24, P8.35 |
|
|
Ideal and Real Solutions |
9 |
Q9.2, Q9.5, Q9.6, Q9.7, Q9.8, Q9.10, P9.8, P9.30, P9.34, P9.36 |
|
****Final Exam Dec. 10th****
The text book problems assigned above are identified by the key words below:
Q: discussions questions
P: problems
11 TEACHING STRATEGIES
For this course, the basic concepts will be discussed and illustrated with examples and demonstrations whenever possible. Lectures will be delivered using standard blackboard and power point presentations. I strongly encourage students to read the checklist of key ideas at the end of each chapter in the textbook each time that a new chapter will be starting. Students are also encouraged to take notes, to ask questions and to participate in class discussions.
12 BIBLIOGRAPHY
- Peter Atkins and Julio de Paula, Physical Chemistry, 8th Ed., W. H. Freeman and Company,
2006.
- Ira N. Levine, Physical Chemistry, McGraw-Hill, 2008.
- David W. Ball, Physical Chemistry, Thomson Learning Inc, 2003.
- Atkins, P.; dePaula, J. Explorations in Physical Chemistry: A Resource for Users of Mathcad;
- H. Freeman: New York, 2002.
- Noggle, J. H. Physical Chemistry, 3rd Ed, Harpper Collins College Publishers, New York, NY., 1996.
- Schwenz, R. W.; Moore, R. J. Physical Chemistry: Developing a Dynamic Curriculum;
American Chemical Society: Washington DC, 1993.
- Gilbert Newton Lewis and Merle Randall (revised by Kenneth S. Pitzer and Leo Brewer) Thermodynamics, 2nd Ed. (Mc Graw-Hill 1961.)
- Denbigh K. The principles of chemical equilibrium: with applications in chemistry
and chemical engineering, 2nd Ed. Cambridge U.P., 1966.
- College of Basic and Applied Sciences Syllabus format, 2006.
Course Summary:
| Date | Details | Due |
|---|---|---|