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Physical Chemistry I

Purpose of Course  showclose

This course will focus on the fundamentals of thermodynamics.  Thermodynamics is the study of energy and its transformations.  Energy is a physical property that can be converted from one form to another to perform work.  For example, a stone rolling down a hill is converting gravitational potential energy into kinetic energy of motion.

Thermodynamics can be applied to systems we use every day—from the operation of refrigerators to the thrusts of rockets.  An awareness of thermodynamics will help you learn other concepts involving chemical processes more quickly and will enable you to understand why many physical phenomena (such as automobile engines or chemical explosives) work the way they do, determine how much work they can put out, and know how to optimize their operation.

In this course, you will learn about the three laws of thermodynamics, thermodynamic principles, ideal and real gases, phases of matter, equations of state, and state changes.  We will also take a look at chemical kinetics—a branch of study concerned with the rates of reactions and other processes—as well as kinetic molecular theory and statistical mechanics, which relate the atomic-level motion of a large number of particles to the average thermodynamic behavior of the system as a whole.

In this course, we will concentrate on bulk properties of systems that can be described by classical mechanics.  However, there are many systems in which quantum mechanical effects influence or dominate.  These will be treated in CHEM106 (Physical Chemistry II).

Course Information  showclose

Welcome to CHEM105.  Below, please find general information on this course and its requirements. 
 
Course Designers: Edward Perry, Brian Dodson, and Karen Duca
 
Primary Resources: This course is built around a series of lectures delivered by Professor Moungi Bawendi and Professor Keith Nelson at MIT entitled “Thermodynamics and Kinetics.”  All the lecture notes and some PowerPoint slide shows on kinetics are available for bulk download at the OCW website.
 
In addition, there is one book recommended for your use throughout this course.  You will see suggested readings and problems from the following:
 
Mortimer, Robert G.  Physical Chemistry (3rd ed.).  Burlington, MA: Elsevier Academic Press, 2008.  Available here. 
 
(All suggested problems have answers in the back of the book so that you can check your work.)
 
Requirements for Completion: To complete this course, you mustwork through all the assigned resources (readings, interactives, lectures, and videos), complete seven assignments (Writing a Visual Description, Writing a Stylistic Description, Writing an Iconographic Analysis, Critical Summary of James Elkins’s “The Failed and the Inadvertent: Art History and the Concept of the Unconscious,” Critical Summary of Linda Nochlin’s “Why Have There Been No Great Women Artists?,” Short Answer Questions: Raymond Spiteri’s “A Farewell to Modernism? Re-Reading T. J. Clark,” and Critical Summary of Matthew Martin’s “Relics of Another Age: Art History, the ‘Decorative Arts,’ and the Museum”), and pass the Final Exam with a grade of 70% or more.  Your score on the exam will be tabulated as soon as you complete it.  If you do not pass the exam, you may take it again.
 
Time Commitment: This course should take you a total of 130 hours to complete.  Each unit includes a “time advisory” that lists the amount of time you are expected to spend on each subunit.  These should help you plan your time accordingly.  It may be useful to take a look at these time advisories to determine how much time you have over the next few weeks to complete each unit and then set goals for yourself.  For example, unit 1 should take you 17 hours.  Perhaps you can sit down with your calendar and decide to complete subunit 1.1 (a total of 4 hours) on Monday night, subunit 1.2 (a total of 5 hours) on Tuesday night, etc.
 
Tips/Suggestions: Although throughout the course every effort has been made to supply links to images and discussions of works that you may be unfamiliar with, you are encouraged to briefly research works discussed in the readings that you have not seen or do not know much about.  You should also note that many of these readings are theoretical and therefore very dense, so you may have to read over them, or at least sections of them, several times.

Learning Outcomes  showclose

Upon successful completion of this course, the student will be able to:
  • State and use laws of thermodynamics.
  • Perform calculations with ideal and real gases.
  • Design practical engines by using thermodynamic cycles.
  • Predict chemical equilibrium and spontaneity of reactions by using thermodynamic principles.
  • Describe the thermodynamic properties of ideal and real solutions.
  • Define the phases of matter, describe phase changes, and interpret/construct phase diagrams.
  • Relate macroscopic thermodynamic properties to microscopic states by using the principles of statistical thermodynamics.
  • Describe reaction rates and then do calculations to determine them.
  • Relate reaction kinetics to potential reaction mechanism.
  • Calculate the temperature dependence of rate constants and relate that to activation energy.
  • Describe a variety of complex reactions.
  • Describe catalysis.
  • Describe enzymatic catalysis.

Course Requirements  showclose

In order to take this course, you must:

√    Have a computer.

√    Have continuous broadband Internet access.

√    Have the ability/permission to install plug-ins or software (e.g., Adobe Reader or Flash).

√    Have the ability to download and save files and documents to a computer.

√    Have the ability to open Microsoft files and documents (.doc, .ppt., .xls, etc.).

√    Have competency in the English language.

√      Have read the Saylor Student Handbook.

√    Have completed at least two semesters of introductory chemistry, two semesters of introductory physics, and two semesters of calculus, including calculating and working with partial derivatives (see CHEM101, CHEM102, MA101, MA102, MA103, PHYS101, and PHYS102).

Preliminary Information

  • Course Materials

    This course is built around a series of lectures delivered by Professor Moungi Bawendi and Professor Keith Nelson at MIT entitled “Thermodynamics and Kinetics.”  All the lecture notes and some PowerPoint slide shows on kinetics are available for bulk download at the OCW website. 
     
    Books:
    There is one book recommended for your use throughout this course.  You will see suggested readings and problems from this book:
     
    Mortimer, Robert G.  (2008).  Physical Chemistry (3rd ed.).  Burlington, MA: Elsevier Academic Press.  Available here.
     
    All suggested problems have answers in the back of the book so that you can check your work.
     
    Terms of Use: Please respect the copyright and terms of use displayed on the webpages above.

Unit Outline show close


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  • Unit 1: Introduction to Thermodynamics  

    We begin by taking a look at the important thermodynamic concepts and terminology that you will use throughout this course.  Any thermodynamic system can be defined by the observer or experimenter and have particular properties.  For example, a system is called “isolated” if nothing—neither mass nor energy—can pass through the boundaries.  A “closed” system is one in which mass cannot pass through the boundary but energy can.  Finally, an “open” system has a completely permeable boundary; anything can pass in and out. 
     
    This unit will also define and examine thermodynamic properties and states and review common units, relationships, and conversions that you will need to recognize and use in this course.  For example, how do you define pressure?  How can we make conversions between SI (metric) and imperial (English) units?  You may be familiar with some or all of these; if this is the case, use this section as a refresher.  

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  • 1.1 Review of Units, Conversions, and Mathematics  
  • 1.1.1 SI and Non-SI Units  
  • 1.1.2 Units of Energy  
    • Reading: American Physical Society: “Energy Units”

      Link: American Physical Society: “Energy Units” (HTML)
       
      Instructions: Thermodynamics deals with energy calculations.  Please read the “Introduction” and “Basic Units” sections to review the basic units of energy that you will work with in this course. 
       
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  • 1.1.3 Unit Conversions  
    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)

      Instructions: Please read section 1.1 (pp. 4–11), which provides a brief review of the important units in chemistry and converting between different systems of units.  It also reviews the mathematical tools you will need to solve problems in physical chemistry.
       
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    • Reading: UC Davis ChemWiki: “Workshop: Unit Conversion & Dimensional Analysis”

      Link: UC Davis ChemWiki: “Workshop: Unit Conversion & Dimensional Analysis” (HTML or PDF)
       
      Instructions: Please read this entire webpage about unit conversion and the three-step method of dimensional analysis.  The NIST site above has links to online unit converters that can help you convert any unit from one system to another, and conversion factors are discussed in this section (HTML) of the Guide for the Use of the International System of Units (SI).  To access the PDF version, click on the ‘Make PDF’ link.
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           
       
      Instructions: Please complete problems 1.1, 1.3, 1.5, and 1.7 in Mortimer (beginning on p. 11).
       
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  • 1.2 Basic Thermodynamic Concepts and Definitions  
  • 1.2.1 History of the Field: An Empirical Discipline  
    • Reading: University of Waterloo: Richard Culham: “History of Thermodynamics”

      Link: University of Waterloo: Richard Culham: “History of Thermodynamics” (HTML)
       
      Instructions: Please read all seven biographies.  Note that thermodynamics as a field was formalized during the 19th century.  It developed as an empirical discipline that was originally concerned with heat energy and how it can be harnessed to do work.  Today, we apply it to a range of disciplines from surface and materials science to bioenergetics.  This site illustrates the history of the field with short biographies of some of its major contributors. 

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  • 1.2.2 Thermodynamic Systems: Open, Closed, or Isolated  
  • 1.2.3 Thermodynamic Properties: Intensive vs. Extensive Properties  
  • 1.2.4 Thermodynamic Equilibrium and the 0th Law  
  • 1.2.5 Thermodynamic Processes: Changes of State and Path Dependence  
    • Reading: UC Davis ChemWiki: “State Functions”

      Link: UC Davis ChemWiki: “State Functions” (HMTL or PDF)
       
      Instructions: Please read the “Introduction,” “Mathematics of State Functions,” and “State Functions vs. Path Functions” sections.  Thermodynamics deals primarily with state functions, which are independent of the path taken to reach them. To access the PDF version, click on the ‘Make PDF’ link.
       
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  • 1.3 Properties of Gases, Work, and Heat  
  • 1.3.1 Ideal Gases vs. Real Gases  
    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Links: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)
       
      Instructions: Please complete problems 1.9 and 1.11 in Mortimer (p. 12).
       
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    • Web Media: Dr. Michael Abraham (Oklahoma State University) and Dr. John Gelder (Ohio State University): “Gas Law Program”

      Link: Dr. Michael Abraham (Oklahoma State University) and Dr. John Gelder (Ohio State University): “Gas Law Program” (Java)
       
      Instructions: Please explore the relationships among P, V, T, and molecular velocity with this Java applet.  Change the number of moles of He and Ne as well as the T, P, and V values and then note how the other properties adjust to compensate the changes you make.
       
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  • 1.3.2 Work: Processes for Changing the Energy of a System  
    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)          
       
      Instructions: Please read section 2.1 (pp. 40–50) in Mortimer to learn about how systems change their states when work is done on them.
       
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    • Assignment: Please complete problems 2.1 and 2.3 in Mortimer (p. 50).

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)      
       
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  • 1.3.3 Heat: Energy Transfers Driven by Temperature Differences  
  • 1.3.4 Heat Capacity: Linking Heat to Temperature Changes  
    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please skim through pp. 50–53 to get a sense of what heat capacity is.  You will revisit this topic in more depth in unit 2.
       
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  • Unit 2: The First Law of Thermodynamics  

    The first law of thermodynamics simply states that energy is conserved.  While energy can be changed from one form to another—say, by converting chemical energy into heat by burning a candle and then converting the heat into mechanical work by heating a gas within a balloon—energy cannot be gained or lost once all transfers and conversions of energy are accounted for.

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  • 2.1 Internal Energy and Expansion Work  
    • Lecture: MIT: Professor Robert Field, Professor Moungi Bawendi, and Professor Keith Nelson: “Internal Energy, Expansion Work”

      Link: MIT: Professor Robert Field, Professor Moungi Bawendi, and Professor Keith Nelson: “Internal Energy, Expansion Work” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 52 minutes), where you will go deeper into the concept of heat capacity that was introduced in Unit 1, learn more about the first law, and discover how gases can do work under different conditions and how to maximize the work they do.  You will also learn about an important state function: U, the internal energy. You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please read chapter 2 (“Work, Heat, and Energy: The First Law of Thermodynamics—pp. 39–102), which covers all the topics included in unit 2.  You may prefer to watch the lectures first, read the material first, or go back and forth between the lectures and this reading.  Problems for this entire unit are given at the end of subunit 2.3. 

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  • 2.2 Enthalpy  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Enthalpy”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Enthalpy” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 55 minutes) to learn about the important state function enthalpy, H, which allows us to know the heat flow into or out of a system.  ΔH = Δ(U + PV) = qp.  You will also explore the dependence of the enthalpy on P and V as well as look at the Joule-Thompson experiment.  You can find the lecture notes for this video here (PDF).
       
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  • 2.3 Thermodynamics of Adiabatic Processes  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Adiabatic Changes” and “Thermochemistry”

      Links: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Adiabatic Changes” and “Thermochemistry” (Adobe Flash, Mp4, or iTunes)
       
      Also available in YouTube:
      Adiabatic Changes
      Thermochemistry
       
      Instructions: Please watch these videos (approximately 55 minutes and 52 minutes, respectively) to learn about state changes of ideal gases taking various paths, isothermal, isobaric, and adiabatic.  This leads us into the topic of thermodynamic cycles, which we can exploit to do work.  The topic of entropy is also introduced, and you will see your first application to nongas systems.  You can find the lecture notes for “Adiabatic Changes” here (PDF) and for “Thermochemistry” here (PDF).
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)
       
      Instructions: Work through the embedded exercises in chapter 2 as you read along.  Also, please complete problems 2.69 (p. 102), 2.71 (p. 103), and 2.73 (p. 103).  If you need more practice, please select other problems to work on your own.  This is the kind of material that is best learned through working problems and thinking through what is physically happening during the processes as they occur.  

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  • Unit 3: Applications of the First Law  

    In this unit, we are concerned with measuring thermodynamic properties for reactions and exploring the fundamentals of how heat engines operate.  Steam engines, internal combustion engines, diesel engines, jet engines, and rocket engines are all heat engines, as are refrigerators and heat pumps.  In ideal cycle analysis, the operations of these engines will be treated as thermodynamic cycles, and we will use the first law of thermodynamics to calculate their cycle efficiency and work output.  While such methods overlook effects that happen in nonideal systems, this basic approach can be adapted to treat more realistic engines.  Moreover, we can use thermodynamic cycles (Hess’s law) to arrive at values for thermodynamic state changes that we cannot easily measure by using the actual path the reaction takes, but we can compute by using cycles involving quantities we can measure along different paths.  

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  • 3.1 Calorimetry: Measuring the Enthalpy  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Calorimetry”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Calorimetry” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 55 minutes) to see how one uses calorimetry to obtain the enthalpy of formation of compounds and the enthalpy of reactions.  In fact, many thermochemical parameters can be measured in a calorimeter.  Also, if one cannot measure enthalpy directly, Hess’s law allows one to use a thermodynamic cycle (taking a different path) to find it.  You can find the lecture notes for this video here (PDF).
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)
       
      Instructions: Please complete these problems in Mortimer: 2.41 (p. 81), 2.43 (p. 84), 2.45 (p. 84), and 2.47 (p. 86).
       
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  • 3.2 Heat Engines  
    • Web Media: Georgia State University: Dr. Rod Nave: “Heat Engine Concepts”

      Link: Georgia State University: Dr. Rod Nave: “Heat Engine Concepts” (HTML)
       
      Instructions: Please look at this chart to explore the concept of heat engines.  We will use this site to see some practical engines based on thermodynamic cycles.  Just get a sense of these engines, and we will revisit them in more detail in Unit 4 and also do some calculations with them.
       
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  • 3.3 The Carnot Cycle  
    • Web Media: Georgia State University: Dr. Rod Nave: “Carnot Cycle”

      Link: Georgia State University: Dr. Rod Nave: “Carnot Cycle” (HTML)
       
      Instructions: Please read the “Carnot Cycle” section, which discusses the most efficient thermodynamic engine possible.  It is based on a cycle with two isothermal and two adiabatic paths.  You can input two temperatures to obtain the Carnot efficiency for that engine.  Are you surprised by what you see?
       
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  • 3.4 The Otto Cycle (Internal Combustion)  
  • 3.5 Refrigerators and Heat Pumps  
  • Unit 4: The Second Law of Thermodynamics  

    The second law of thermodynamics reflects the universal observation that moving things eventually stop and broken eggs never become whole.  It expresses this observation in terms of a new thermodynamic parameter known as entropy, which is a measure of the disorder in a system.  Renowned British physicist Sir Arthur Eddington believed that the second law is the most fundamental law of science and that, at its foundation, it is far broader than required by the narrow physical laws of our particular universe.  

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  • 4.1 The Second Law of Thermodynamics  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “The Second Law”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “The Second Law” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 50 minutes) on the second law of thermodynamics.  It starts off with a discussion of the relationship between enthalpies of formation and bond energies, following up the lectures on thermochemistry.  From there, you will learn about how the second law complements the first.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)

      Instructions: Read chapter 3.1 in Mortimer describing the Second Law.  Skim the rest of the chapter on applications of the Second Law (pp. 106–132).  You will return to see them in more detail later.
       
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  • 4.2 Entropy and the Clausius Inequality  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Entropy and the Clausius Inequality”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Entropy and the Clausius Inequality” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 50 minutes).  You will revisit some of the thermodynamic cycles with their corresponding engines that you saw in Unit 3 and learn about entropy around thermodynamic cycles where there are reversible and irreversible paths involved.  You can find the lecture notes for this video here (PDF).
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           
       
      Instructions: Please complete problems 3.1 and 3.3 in Mortimer (p. 113).
       
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  • 4.3 Entropy and Irreversibility  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Entropy and the Irreversibility”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Entropy and Irreversibility” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 53 minutes), which continues entropy calculations around cycles that involve reversible and irreversible processes, with particular emphasis on the direction of spontaneous change.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please skim section 3.2 and read section 3.3 (pp. 114–131), paying particular attention to the example problems.
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please complete problems 3.13, 3.19, and 3.23 in Mortimer (pp. 131–133).
       
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  • 4.4 Maxwell’s Demon  
    • Web Media: Albert Smith: “Maxwell’s Demon”

      Link:  Albert Smith: “Maxwell’s Demon” (Java)
       
      Instructions: Please explore this Java applet, which is based on a thought experiment that James Clerk Maxwell devised nearly 150 years ago to try to disprove the second law.  He did not succeed, but his idea raised interesting questions about the relationship between information and entropy.  Try to separate the fast from the slow molecules.  Are you violating the second law? No, because the amount of information needed to do this separation requires quite a large energy input!
       
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  • 4.5 Statistical Entropy: Microscopic vs. Macroscopic Viewpoints  
    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please read section 3.4 (pp. 133–138) to start getting a flavor of how microscopic states give rise to the bulk properties we measure in thermodynamics.
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please complete problems 3.27 and 3.29 in Mortimer (p. 138).
       
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  • Unit 5: The Third Law of Thermodynamics  

    The third law of thermodynamics is the odd man out, so to speak.  The zeroth law states that two bodies having the same temperature as a third have the same temperature as each other; the first law states that energy is conserved; and the second law states that heat cannot flow from a cold object to a hot object.  These seem reasonably clear, although not beyond dispute.  However, the third law is not as straightforward.  It states: “As a system approaches absolute zero, the entropy of the system approaches a minimum value.” However, despite the fact that the interpretation of the third law becomes rather confusing when quantum effects are included, there is no experimental example or reasonable theoretical result that violates the third law.

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  • 5.1 Fundamental Equation, Absolute Entropy, and the Third Law  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Fundamental Equation, Absolute S, Third Law”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Fundamental Equation, Absolute S, Third Law” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
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      Instructions: Please watch this entire video (approximately 52 minutes), which describes the third law and the definition of absolute entropy.  Although we can never reach absolute zero of temperature, it is an important reference point for us.  You will also learn about the entropy of mixing.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please read pages 139–144 about the third law and absolute entropy.
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           
       
      Instructions: Please complete problems 3.33 and 3.37 in Mortimer (p. 146).
       
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  • 5.2 Entropy of Mixing  
    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           
       
      Instructions: Please reread pages 130–131, paying particular attention to the example problems. 
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           
       
      Instructions: Please complete problem 3.31 in Mortimer (p. 138).
       
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  • Unit 6: Spontaneous Changes, Chemical Potential, and Equilibrium  

    A chemical system is in equilibrium when the activities and concentrations of the reactants and products do not change with time.  This usually comes about when the forward reaction rate and the reverse reaction rate are the same.  In this situation, known as dynamic equilibrium, chemical reactions are still in progress, and specific atoms move between molecules, but the total amount of the various chemical species remains the same.  As we will see, a chemical system in dynamic equilibrium tends to remain in equilibrium when disturbed by changing the conditions associated with the original equilibrium.  Equilibrium is associated with global minima in the appropriate free energy.  Metastability is associated with a local minimum in the appropriate free energy that is separated from the global minimum by an activation energy barrier.  Many chemical processes yield metastable conditions rather than equilibrium, however.  For example, a lump of carbon at equilibrium is a diamond, but we rarely see this happen.  Controlling and changing chemical equilibria is perhaps the most important skill that a chemist must develop.

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  • 6.1 Spontaneous Changes in Chemical Systems  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Criteria for Spontaneous Change”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Criteria for Spontaneous Change” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
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      Instructions: Please watch this entire video (approximately 48 minutes) to learn about how we judge whether a system is moving spontaneously toward an equilibrium state or is already there.  You will learn about the Gibbs and Helmholtz free energies, which are ways of predicting spontaneity under different conditions.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please read section 4.1 and skim sections 4.2 and 4.3 (pp. 152–172).  Spontaneity is a very important concept in reaction chemistry, and this reading will augment the video.
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please complete problems 4.1 and 4.3 in Mortimer (p. 158).
       
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  • 6.2 Gibbs Free Energy  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson” “Gibbs Free Energy”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Gibbs Free Energy” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
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      Instructions: Please watch this entire video (approximately 50 minutes) to learn about what is arguably the most important thermodynamic function in chemistry: the Gibbs free energy.  This function helps us determine the direction of spontaneity in any chemical reaction.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           
       
      Instructions: Please read section 4.4 (pp. 175–179) to see examples of how to apply and calculate DG in various situations.
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)          

      Instructions: Please complete problems 4.29 and 4.37 in Mortimer (pp. 180–181).
       
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  • 6.3 Multicomponent Systems and Chemical Potential  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Multicomponent Systems, Chemical Potential”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Multicomponent Systems, Chemical Potential” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
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      Instructions: Please watch this entire video (approximately 47 minutes) to learn about how to calculate the Gibbs free energy per mole of systems with multiple components.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please read sections 4.5 and 4.6 (pp. 182–194) to learn about chemical potential and augment the video lecture.
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please complete problems 4.41 (p. 188) and 4.47 (p. 194) in Mortimer.
       
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  • 6.4 Le Chatelier’s Principle  
  • 6.5 Chemical Equilibrium  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Chemical Equilibrium”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Chemical Equilibrium” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 51 minutes) to derive the relationship between Gibbs free energy, chemical potential, and equilibrium.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please read section 7.1 (pp. 304–310) to learn about the relationship between Gibbs free energy and the equilibrium constant.
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           
       
      Instructions: Please complete problem 7.1 in Mortimer (p. 310).
       
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  • 6.6 Effect of Temperature and Pressure on Chemical Equilibrium  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Temperature, Pressure and Kp”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Temperature, Pressure and Kp” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 52 minutes) to learn how to express the equilibrium constant in two ways, Kp, which is independent of total pressure and Kx, which does depend on the pressure.  You will see a more quantitative presentation of Le Chatelier’s principle as well as see how varying temperature, pressure, and volume affect the chemical potential and, thus, the equilibrium position.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           
                                                                     
      Instructions: Please read section 7.6 (pp. 335–339) to see how the equilibrium constant changes as a function of temperature.
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please complete problems 7.53 and 7.59 in Mortimer (p. 342).
       
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  • 6.7 Biological Applications of Equilibrium  
  • Unit 7: Phase Changes and Phase Equilibria  

    Phase changes deal with physical transformations of pure substances.  An important kind of equilibrium is one where the pure substance exists in two or more states of matter.  We exploit this property in many ways in all branches of science.  For example, we freeze cells in liquid nitrogen vapor, which is in equilibrium with its liquid in the storage tank.  In this unit, you will learn how to generate phase diagrams and perform calculations related to energy requirements for phase changes.

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  • 7.1 Review of Phase Changes  
  • 7.2 Phase Equilibria: One Component Systems  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Phase Equilibria – One Component”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Phase Equilibria – One Component” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Phase changes are little bit different from chemical reactions.  There are some different results and different equations that we use to describe them.  Please watch this entire video (approximately 51 minutes) to learn about phase changes—first in one component system and then in multiple component systems.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please read section 5.3 (pp. 205–213) to learn about the coexistence of phases of a pure substance and augment the video lecture.  Note that this reading will cover the material you need to know for subunits 7.3–7.4.
       
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  • 7.3 Clausius-Clapeyron Equation  

    Note: This subunit is covered by the reading assigned beneath subunit 7.2.

    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Clausius-Clapeyron Equation”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Clausius-Clapeyron Equation” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 50 minutes) on the Clausius-Clapeyron equation.  It helps us construct the phase diagram of a single component system with two phases.  Basically, one runs a Carnot engine, where the working fluid may be either a gas or liquid between two temperatures to define the vaporization curve.  You can find the lecture notes for this video here (PDF).
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please complete problems 5.9, 5.13, 5.15, and 5.17 in Mortimer (pp. 213–214).
       
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  • 7.4 Phase Equilibria: Two Component Systems  

    Note: This subunit is covered by the reading assigned beneath subunit 7.2.

  • Unit 8: Thermodynamic Properties of Solutions  

    A solution is a homogeneous mixture comprising two or more substances that are mutually miscible.  Common examples of solutions include the atmosphere, salt water, alcoholic beverages, and many metallic alloys.  Compound materials that are not solutions include milk, precipitate-hardened alloys, and carbon-fiber composites.  The special thermodynamic properties of solutions are generated by large entropic contributions from the atomic or molecular-level disorder that characterizes most homogeneous solutions.  These large entropy terms are associated with the complex thermodynamic properties of solutions.

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  • 8.1 Ideal Solutions  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Ideal Solutions”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Ideal Solutions” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 50 minutes) to learn about ideal solutions and their associated vapor pressures.  Raoult’s law and Henry’s law are also presented, and in certain situations, these ideal solutions do apply in the real world.  In the next section, you will learn about how most real solutions behave.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed) (HTML)  
       
      Instructions: Please read chapter 6 (pp. 237–299), but only skim section 6.4 on activities of nonvolatile solutes and section 6.6 on multicomponent phase diagrams.  Note that this reading will cover the material you need to know for subunits 8.2–8.3.
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please complete problems 6.7 (p. 197), 6.9 (p. 198), and 6.13 and 6.15 (p. 257) in Mortimer.
       
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  • 8.2 Nonideal Solutions  

    Note: This subunit is covered by the reading assigned beneath subunit 8.1.

    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Non-Ideal Solutions”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Non-Ideal Solutions” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
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      Instructions: Please watch this entire video (approximately 51 minutes) to learn more about how real solutions behave.  You can find the lecture notes for this video here (PDF).
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please complete problems 6.39 and 6.43 in Mortimer (pp. 280–281).
       
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  • 8.3 Colligative Properties  

    Note: This subunit is covered by the reading assigned beneath subunit 8.1.

    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Colligative Properties”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Colligative Properties” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 51 minutes).  Colligative properties of solutions are those that depend only on the number of dissolved solutes and not their chemical identity.  Examples of colligative properties are freezing point depression, boiling point elevation, and osmotic pressure.  You can find the lecture notes for this video here (PDF).
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please complete problems 6.63, 6.65, and 6.69 in Mortimer (p. 299).
       
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  • 8.4 Surface Properties of Solutions  
    • Web Media: Purdue University: “Surface Tension”

      Link: Purdue University: “Surface Tension” (HTML)
       
      Instructions: Surface tension is an important property of a solution.  It is defined as the amount of force needed to increase the surface of a solution by unit area.  Capillary action results from surface tension and the adhesive forces between the substance and the tube.  Please read the general definition of surface tension and look at the animation of the microscopic behavior at the liquid surface.
       
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    • Web Media: University of Florida: “Surface Tension”

      Link: University of Florida: “Surface Tension” (HTML)
       
      Instructions: This link has many interesting animations, videos, and pictures to help you get an intuitive grasp of surface tension and capillary action.  Explore the various parts of the site.  You will definitely want to watch the video of capillary action comparing two different substances in glass tubes.  After looking over the examples, try the three sample problems and the self-test at the bottom of the page.
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please read section 5.5 (pp. 222–229) to get a sense of the important physical properties at surfaces and interfaces.
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please complete problems 5.37 and 5.39 in Mortimer (p. 230).
       
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  • Unit 9: Statistical Thermodynamics – A Brief Overview  

    Thermodynamics describes the behavior of huge collections of microscopic particles through the use of such averaged properties as temperature, density, volume, entropy, energy, and so forth.  In doing so, thermodynamics avoids the extraordinarily difficult task of directly computing the behavior of such collections of particles by using Newton’s equations of motion.  The “dynamics” of thermodynamics has to do with changes in these averaged properties and not with the details of the microscopic configuration of the materials in the system. 
     
    On the other hand, statistical mechanics is based on one fundamental assumption: that all possible microscopic configurations that are consistent with the observed averaged thermodynamic properties are equally likely to occur.  This is an application of a philosophical position that has proven extremely useful in science: that we do not occupy a special place in the universe.  (This is often called the “mediocrity principle” and may have been originally introduced by Copernicus.)  If all possible microscopic configurations are equally likely, then the physics we measure are most likely to be that of the most common possible configurations.  This simple principle allows us to interpret the thermodynamic properties of materials in terms of their component particles and the interactions between them.  This leads to a more fundamental understanding of matter and why it behaves the way it does.

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  • 9.1 Introduction to Statistical Mechanics  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Introduction to Statistical Mechanics”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Introduction to Statistical Mechanics” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
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      Instructions: Please watch this entire video (approximately 52 minutes), which begins with a review of some topics in Unit 8 and then moves into a consideration of statistical mechanics.  Please pay particular attention to how one calculates the probability of finding a molecule in a particular energy state.  If we know the distribution of all the molecules of system in its various states, then we can arrive at the macroscopic thermodynamic functions for the system.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.)  (HTML)          

      Instructions: Please read Chapter 25 in Mortimer, “Equilibrium Statistical Mechanics. I. The Probability Distribution for Molecular States” beginning on p. 1039. Skim section 25.4 on molecular partition functions.  Skim Chapter 26, Sections 1-3 on the statistical thermodynamics of dilute gases.  IMPORTANT: As you are reading the material from Unit 9, try working the exercises embedded in the text to really make sure that you are understanding what the text and can work problems. Review problems covering the entire unit will be given at the end.
       
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  • 9.2 Partition Function (q): Large N Limit  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Partition Function (q) — Large N Limit”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Partition Function (q) — Large N Limit” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
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      Instructions: Please watch this entire video (approximately 51 minutes) to learn about partition functions and how we use them to determine what microstates are available to any given system.  Examples of a perfect crystal, a monoatomic gas, and a polymer in solution will help make these abstract ideas more concrete for you.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry 3rd ed.) (HTML)           
       
      Instructions: Please read Chapter 27 in Mortimer, “Equilibrium Statistical Mechanics. III.  Ensembles,” pp. 1121–1150.  Note that this reading will cover the material you need to know for subunits 9.3–9.5.
       
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  • 9.3 Partition Function (Q): Many Particles  

    Note: This subunit is covered by the reading assigned beneath subunit 9.2.

    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Partition Function (Q) — Many Particles”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Partition Function (Q) — Many Particles” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 51 minutes) to learn how we can use the partition functions to calculate the thermodynamic functions for the system, thereby relating the micro and macroscopic.  You can find the lecture notes for this video here (PDF), approximately corresponding to the first three pages of the file.
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)

      Instructions: Please review the following problems in Mortimer: 26.21 (p. 1105), 26.35 and 26.37 (p. 1119), 26.41 (p. 1120), 27.5 (p. 1128), 27.7, 27.9, and 27.11 (p. 1132), and 27.23 (p. 1151).
       
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  • 9.4 Statistical Mechanics and Discrete Energy Levels  

    Note: This subunit is covered by the reading assigned beneath subunit 9.2.

  • 9.5 Model Systems  

    Note: This subunit is covered by the reading assigned beneath subunit 9.2.

  • 9.6 Applications: Chemical and Phase Equilibria  
  • Unit 10: Chemical Kinetics  

    Chemical kinetics studies the rates of chemical reactions.  By studying chemical kinetics, we can construct mathematical models that describe the time-dependent properties of a chemical reaction and determine what mechanisms dominate the time-dependent behavior.  Rate laws link the reaction rate of a chemical process with the concentrations or pressures of the reactants, yielding a differential equation that can be solved to predict reaction rates.  There are numerous classes of rate law, each of which tells a chemist a good deal about the dominant reaction mechanisms and predicts the behavior of the chemical process prior to reaching chemical equilibrium.  Temperature and the presence of catalysts alter rate equations in characteristic directions and thus become tools in the chemist’s arsenal.  

    Time Advisory   show close
    Learning Outcomes   show close
  • 10.1 Introduction to Reaction Kinetics  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Introduction to Reaction Kinetics”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Introduction to Reaction Kinetics” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 51 minutes) to learn about basic principles of reaction kinetics. You will learn about reaction order and how to determine the order of reactions.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please read sections 11.1–11.5 (pp. 485–512) to learn about how to calculate rates of different kinds of reactions.  Note that this reading will cover the material you need to know for subunits 10.2–10.3.
       
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    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           
       
      Instructions: Please complete problems 11.1 (p. 488), 11.3, 11.5, 11.7, and 11.9 (p. 498), 11.15, 11.17, and 11.19 (p. 505), and 11.43 (p. 522) in Mortimer.
       
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  • 10.2 Complex Reactions and Mechanisms  

    Note: This subunit is covered by the reading assigned beneath subunit 10.1.

    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Complex Reactions and Mechanisms”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Complex Reactions and Mechanisms” (Adobe Flash, Mp4 or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 45 minutes) to learn about the various types of reaction mechanisms and how kinetics can help one infer a reaction mechanism.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Skim chapter 13, “Chemical Reaction Mechanisms II: Catalysis and Miscellaneous Topics.”  The goal is to familiarize yourself with the range of more complex reactions that can happen, such as oscillating reactions and reactions of polymers.
       
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  • 10.3 Steady-State and Equilibrium Approximations  

    Note: This subunit is covered by the reading assigned beneath subunit 10.1.

    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Steady-State and Equilibrium Approximations”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Steady-State and Equilibrium Approximations” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 51 minutes) to continue your study of complex reaction mechanisms. You will also learn about how reactions at equilibrium are actually in a steady-state which is dynamic, where products and reactants are constantly being made and consumed, but there is no net change.  You can find the lecture notes for this video here (PDF).
       
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    • Reading: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please read chapter 12, “Chemical Reaction Mechanisms I: Rate Laws and Mechanisms,” pp. 524–562.
       
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      The Saylor Foundation does not yet have materials for this portion of the course. If you are interested in contributing your content to fill this gap or aware of a resource that could be used here, please submit it here.

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  • 10.4 Chain Reactions  
    • Lecture: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Chain Reactions”

      Link: MIT: Professor Moungi Bawendi and Professor Keith Nelson: “Chain Reactions” (Adobe Flash, Mp4, or iTunes)
       
      Also available in:
      YouTube
       
      Instructions: Please watch this entire video (approximately 51 minutes) to finish up complex reactions and learn about an important category of reaction known as the chain reaction. These are very important in atmospheric chemistry and polymer formation. You can find the lecture notes for this video here (PDF).
       
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  • 10.5 Temperature Dependence, Activation Energy, and Catalysis  
  • 10.6 Enzyme Catalysis  
  • Kinetics Review Assignment  
    • Assignment: Robert G. Mortimer’s Physical Chemistry (3rd ed.)

      Link: Robert G. Mortimer’s Physical Chemistry (3rd ed.) (HTML)           

      Instructions: Please complete the following problems review kinetics: 11.43 (p. 22), 12.39 and 12.41 (p. 562), 12.43 (p. 563), and 13.41 (p. 615).
       
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  • Final Exam  
    • Final Exam: The Saylor Foundation's CHEM105 Final Exam

      Link: The Saylor Foundation's CHEM105 Final Exam

      Instructions: You must be logged into your Saylor Foundation School account in order to access this exam.  If you do not yet have an account, you will be able to create one, free of charge, after clicking the link.

      The Saylor Foundation does not yet have materials for this portion of the course. 

      The Saylor Foundation does not yet have materials for this portion of the course. If you are interested in contributing your content to fill this gap or aware of a resource that could be used here, please submit it here.

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