Fayetteville State University

College of Health, Science, and Technology (CHST)

Department of Chemistry, Physics, and Material Sciences

Syllabus

CHEM 313 – Physical Chemistry I

Fall 2021

I.   Locator Information

Instructor: Dr. Jairo Castillo-Chará

Course # and Name: CHEM 313-01                     Office Location: SciTech 313

Semester Credit Hours: 3                    Office hours: MW 8:00am-10:00am, TR 10:00am-12:00am

Day and Time Class Meets: TR 8:00 am- 9:15 am, SciTech338      Office Phone: (910) 672-2062

Total Hours for Class: 37.5 hours

Course Format (Face-to Face, Hybrid, Online): Face-to Face

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 about 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 will not assure 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

 

Covid-19 Statement

It is the policy of FSU for the Fall 2021 semester that all students are required to engage in safe behaviors to avoid the spread of COVID-19. Such behaviors specifically include the requirements that all students wear a mask while in classrooms or labs and in other instances where distancing is not possible, unless (a) a student is granted an accommodation from Disability Services, or (b) I otherwise explicitly grant permission to a student to remove their mask (such as while asking a question, participating in class discussion, or giving a presentation, all while at an appropriate physical distance from others). Students who do not have masks can obtain them from the building coordinator. Failure to comply with this policy in the classroom may result in dismissal from the current class session and charges under the Code of Student Responsibility. 

Stay Home and Self-Isolate under the following circumstances 

• If you are sick with COVID-19 symptoms https://www.cdc.gov/coronavirus/2019-ncov/symptoms-testing/symptoms.html 
• If you have tested positive for COVID-19 
• If you have been potentially exposed to someone with COVID-19 

Contact your supervisor regarding your absence from work 

Contact your healthcare provider for guidance regarding symptoms, testing, and potential exposure 

• Follow the guidance of your healthcare provider 
• You will need a note from your healthcare provider clearing you to return to work on campus 

Report positive COVID-19 test results to the Office of Human Resources (Kay Faircloth at 672-2461).  

• The University is required to report the total number of positive cases regularly.  
• Personally identifiable information (PII) is not reported.   

The FSU COVID-19 reporting dashboard can be accessed at https://www.uncfsu.edu/coronavirus-update 

II.     Course Description

CHEM 313 – 01: This is the first of a 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 the structure, properties, and transformations of matter, from macroscopic behavior to mechanisms that operate at the 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 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 introductory course in differential equations will be useful, however, provisions will be made during the course to satisfy this requirement.

III.    Services for Students with Disabilities

Under 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.

 

IV.      Title IX – Prohibited Sexual Conduct

Fayetteville State University (University) is committed to fostering a safe campus environment where sexual misconduct — including sexual harassment, domestic and dating violence, sexual assault, and stalking - is unacceptable and is not tolerated. The University encourages students who may have experienced sexual misconduct to speak with someone at the university so that the University can provide the support that is needed and respond appropriately. The Sexual Misconduct policy can be found at the following link: 

http://www.uncfsu.edu/Documents/Policy/students/SexualMisconduct.pdf

 

Consulting with a Health Care Professional - A student who wishes to confidentially speak about an incident of sexual misconduct should contact either of the following individuals who are required to maintain confidentiality: 

 

Ms. Pamela C. Fisher                                                    Ms.  Linda Melvin

            Licensed Professional Counselor                                   Director, Student Health Services

            Spaulding Building, Room 165                          Spaulding Building, Room 121

            (910) 672-387                                                              (910) 672-1454                                   

            psmith@uncfsu.edu                                          lmelvi10@uncfsu.edu

 

Reporting an Incident of Sexual Misconduct- The University encourages students to report incidents of sexual misconduct. A student who wishes to report sexual misconduct or has questions about University policies and procedures regarding sexual misconduct should contact the following individual: 

Ms. Jessica Tuttle

Title IX Coordinator

Barber Building, Room 242

(910) 672-1141

Unlike the Licensed Professional Counselor or the Director of Student Health Services, the Deputy Title IX Coordinator is legally obligated to investigate reports of sexual misconduct, and therefore cannot guarantee confidentiality, but a request for confidentiality will be considered and respected to the extent possible.

 

Students are also encouraged to report incidents of sexual misconduct to the University’s Police and Public Safety Department at (910) 672-1911.

V.     Textbook/Course Materials

1. Thomas Engel and Philip Reid, Physical Chemistry, 3rd Edition, Pearson, 2013.

VI.    Student Learning Outcomes

After completion of the first course in physical chemistry, students are expected:

1. To be able to learn and apply the basic language of thermodynamics to the study of chemical systems.
2. To demonstrate understanding of the laws of thermodynamics and know how to apply the laws to chemical systems.
3. 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.
4. 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.
5. To be able to use and apply tables of thermodynamic data to calculate thermodynamic functions and to sharpen graphing interpretation skills.
6. To be able to use and apply spreadsheet software to analyze, solve and visualize problems in physical chemistry and related areas.
7. To be prepared to take advanced, senior-level, and graduate courses in chemistry, biochemistry, and physics.

 

VII.   Course Requirements and Evaluation Criteria

1 Homework Policy

1.1 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.

1.2 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 deliver more professional work.

1.3 Each time that you submit the homework make sure that you write your name, date, and problem set number or chapter number.

1.4 Homework turned in late will be graded at a rate of 10 % per day late (you will lose 10 points per day late)

1.5 The problem sets will be graded according to the following scale: ”satisfactory effort” (100%), ”need improvement” (50%), and ”unsatisfactory effort” (0 %).

1.6 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 suits your schedule.

 

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.

The tests will be given through Canvas and require a computer with an Internet connection and

a webcam. Please, notify the instructor if these pieces of technology are no available to you

before any test takes place.

3       Disclaimer 

To accommodate emergent circumstances, the professor reserves the right to make reasonable changes in the syllabus while the course is in progress. Any understandings between a student and the professor including, but not limited to, changes, expectations, or modifications to course requirements or procedures must be in writing and must be signed by both parties. Any question of interpretation of course requirements or of understandings between a student and the professor will be at the discretion of the professor.

Inclement Weather Issues: If a particular lecture or lab session is not held due to inclement weather or other urgent reasons etc., instructions will be delivered via Canvas. In such cases of emergent issues stay tuned to Canvas and check for announcements and assignments.

 

4          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.

 

5          Due Date Assignments Policy:

The final due date for any assignment (homework, exams, or any other assignment) is 5:00 PM on the day of the final exam date. After this date, no assignments will be accepted.

 

6      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, the "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 on 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 online classes, did not interact with the 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 for them to take corrective action.

NEW FINAL GRADE: FN (FAILURE DUE TO NON-ATTENDANCE) Final grade for students who are on the class roster, but never attend the class. An FN grade is equivalent to an F grade in the calculation of the GPA.

 

7      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 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 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 concentration and distracts your peers.

 

8      Student Behavioral Expectations

8.1. Students are expected to arrive at class on time, remain in class until dismissed by the instructor, and refrain from preparing to leave class until it is dismissed.

8.2 Students should avoid passing notes or carrying on private conversations while class is being

conducted.

8.3 Students should avoid the use of profanity in the classroom.

8.4 Any form of cheating is considered academic dishonesty or misconduct and will be punished. For information about disciplinary measures and university policies for academic misconduct, read the Fayetteville State University Student Handbook.

8.5 Students should avoid the use of cell phones during exams and class time, this affects concentration and distracts their peers.

 

9      Consequences for Failing to Meet Behavioral Expectations

With a first-time violation of one of the rules above, he or she will be warned privately by the instructor after or before the 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]

VIII.     Academic Support Resources – 

Learning Center: 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 website (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/

Math Support Center- Provides one-on-one and group tutoring in 100 & 200 level math courses.

Writing Center- An essential component in the team effort to build writing skills for any course through individual writing conferences, writing-related resources, working with instructors and helping students help themselves.

IX.     Course Outline and Assignment Schedule

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 Thermodynamics 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 CP and 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 DGR for 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

 

1 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. 10^th****

The text book problems assigned above are identified by the key words below:

Q: discussions questions

P: problems

X.     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 PowerPoint 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, ask questions, and participate in class discussions.

XI.      Bibliography:

1. Peter Atkins and Julio de Paula, Physical Chemistry, 8th Ed., W. H. Freeman and Company,

2006.

2. Ira N. Levine, Physical Chemistry, McGraw-Hill, 2008.
3. David W. Ball, Physical Chemistry, Thomson Learning Inc, 2003.
4. Atkins, P.; de Paula, J. Explorations in Physical Chemistry: A Resource for Users of Mathcad;
5. H. Freeman: New York, 2002.
6. Noggle, J. H. Physical Chemistry, 3rd Ed, Harper Collins College Publishers, New York, NY., 1996.
7. Schwenz, R. W.; Moore, R. J. Physical Chemistry: Developing a Dynamic Curriculum;

American Chemical Society: Washington DC, 1993.

7. Gilbert Newton Lewis and Merle Randall (revised by Kenneth S. Pitzer and Leo Brewer) Thermodynamics, 2nd Ed. (Mc Graw-Hill 1961.)
8. Denbigh K. The principles of chemical equilibrium: with applications in chemistry

and chemical engineering, 2nd Ed. Cambridge U.P., 1966.

9. College of Basic and Applied Sciences Syllabus format, 2006.

XII.     Code of Student Conduct:

 https://www.uncfsu.edu/faculty-and-staff/divisions-departments-and-offices/division-of-student-affairs/student-conduct