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Thermodynamics: Four Laws That Move the Universe

Thermodynamics: Four Laws That Move the Universe

Professor Jeffrey C. Grossman, Ph.D.
Massachusetts Institute of Technology

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Thermodynamics: Four Laws That Move the Universe

Course No. 1291
Professor Jeffrey C. Grossman, Ph.D.
Massachusetts Institute of Technology
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4.3 out of 5
68 Reviews
79% of reviewers would recommend this series
Course No. 1291
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Course Overview

What is heat? What is temperature? What is energy? What is time? When we look beneath the surface of these everyday terms to learn how scientists understand them, we encounter a realm of fundamental processes that rule the universe.

This is the domain of thermodynamics, the branch of science that deals with the movement of heat. Nothing seems simpler, but nothing is more subtle and wide-ranging in its effects. And nothing has had a more profound impact on the development of modern civilization.

Thermodynamic processes are at the heart of everything that involves heat, energy, and work, making an understanding of the subject indispensable for careers in engineering, physical science, biology, meteorology, and even nutrition and culinary arts. Consider these applications of the laws of thermodynamics:

  • The second law of thermodynamics leads to the concept of entropy, which explains the arrow of time and the unidirectionality of all processes—including the evolution of the universe.
  • In daily life, thermodynamics explains why salt melts ice, why cars are so inefficient, and why the cheese on a hot slice of pizza burns the roof of your mouth, but the crust at the same temperature doesn’t.
  • New advances in alternative energy, materials science, and a host of other fields are in the works as thermodynamic processes are being applied at scales as small as the quantum realm.

Thermodynamics: Four Laws That Move the Universe gives you an in-depth tour of this vital and fascinating science in 24 enthralling lectures that are suitable for everyone from science novices to experts who wish to review elementary concepts and formulas. Your teacher is Professor Jeffrey C. Grossman of the Massachusetts Institute of Technology, a scientist at the forefront of research on new materials.

Four Far-Reaching Laws

The four laws of thermodynamics describe how energy moves, why it changes from one form to another, and how matter is affected during these transformations. With these laws as a launching point, you learn foundational concepts that are critical pillars of science and engineering—ideas such as entropy, chemical potential, Gibbs free energy, enthalpy, osmotic pressure, heat capacity, eutectic melting, and the Carnot cycle. These and other ideas shed light on many phenomena in the natural world, and they are the analytical tools that engineers use to create new devices and technologies.

Thermodynamics is illustrated with scores of informative diagrams, animations, and simple equations that add depth and clarity to the presentation. And in nearly every lecture, Professor Grossman puts on his lab coat and goggles and smashes, breaks, ignites, or otherwise converts energy from one form into another—showing thermodynamics in action in demonstrations such as these:

  • Work = heat: See how a piece of cotton can be set afire by striking a piston with a hammer, illustrating the first law of thermodynamics, which relates heat to mechanical motion.
  • When 1+1 doesn’t equal 2: Combine 50 milliliters of water with an equal volume of ethanol and you get 97—not 100—milliliters of solution. The thermodynamic concept of partial molar volume explains why.
  • Potato battery: Insert a copper wire and a zinc wire into a potato. Connect the wires to an LED. Voila: light! Discover the role of the potato in this demonstration of electrochemical energy.

At the end of Thermodynamics, Professor Grossman discusses his own pioneering research on clean energy and water. Having come this far in the course, you will truly appreciate his excitement over innovative solar thermal fuels and desalination membranes, both based on thermodynamic principles. Best of all, you will understand how and why they work!

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24 lectures
 |  31 minutes each
  • 1
    Thermodynamics—What’s under the Hood
    Starting with the example of cooked food, see how thermodynamics governs all processes that use energy to transform materials—whether the product is a pan of brownies or a cell phone. Preview the course by imagining what it would take to build modern technological civilization from scratch. x
  • 2
    Variables and the Flow of Energy
    Chart the key historical milestones in the development of thermodynamics. Then compare macroscopic and microscopic views of the world, and consider how the relationship between a material’s properties, structure, performance, and processing can be represented by the four corners of a tetrahedron. x
  • 3
    Temperature—Thermodynamics’ First Force
    Analyze the most central idea of thermodynamics: temperature. Investigate the origin of different temperature scales and the various methods for measuring temperature. See how the concept of temperature is a consequence of the zeroth law of thermodynamics, which deals with the nature of thermal equilibrium. x
  • 4
    Salt, Soup, Energy, and Entropy
    Explore other basic concepts that are critical to thermodynamics. These include the idea of a system, boundary conditions, processes that occur within systems, the meaning of the state of a system, the definition of equilibrium, and a much-misunderstood quantity called entropy. x
  • 5
    The Ideal Gas Law and a Piston
    Understand how pressure, volume, and temperature are state functions related by a formula known as the ideal gas law. Contrast these variables with work and heat, learning why they are not state functions. See how the ideal gas law can be used to calculate the work done by a piston. x
  • 6
    Energy Transferred and Conserved
    Discover that the values for work and heat in a given system depend on the path taken to get to a particular state. But note that the sum of work and heat does not depend on the path; it is a constant. This remarkable fact is the foundation of the first law of thermodynamics. x
  • 7
    Work-Heat Equivalence
    Witness examples of energy transforming from one type to another—from mechanical to heat. First, see how the ideal gas law can be used to ignite a piece of cotton. Then, witness how soup can be made piping hot by rapid mixing. Also, probe the concepts of reversibility and irreversibility x
  • 8
    Entropy—The Arrow of Time
    Probe the connection between entropy and the second law of thermodynamics, which states that all real processes tend to increase the entropy of the universe. Explore some important consequences of the law, including the fact that time flows in only one direction. x
  • 9
    The Chemical Potential
    Study molar and partial molar quantities, which are indispensable for describing what happens when materials are combined. Focus on the case of water mixed with ethanol, which adds up to a surprising volume. These ideas lead to one of the most important variables in thermodynamics: chemical potential. x
  • 10
    Enthalpy, Free Energy, and Equilibrium
    Define the Gibbs free energy, which is closely related to entropy and allows the determination of equilibrium for systems under realistic experimental conditions. Then encounter a related variable, enthalpy, which is useful when discussing constant pressure processes. x
  • 11
    Mixing and Osmotic Pressure
    Marvel at the power of osmosis by investigating the thermodynamic force that drives a liquid to flow from one side of a barrier to another. This force is called the chemical potential gradient, and it has wide application in performing work, from desalinating water to generating electricity. x
  • 12
    How Materials Hold Heat
    Learn how different materials vary in their ability to absorb heat. This factor is called heat capacity, and it provides a crucial way to correlate energy flow with temperature. Study the heat capacity of various materials, and see how quantum effects reduce heat capacity at very low temperatures x
  • 13
    How Materials Respond to Heat
    Turn to the problem of thermal energy flow and volume. This phenomenon causes materials to expand when heated and contract when cooled. Analyze these events at the atomic scale, and study the unusual behavior of water when it freezes—an attribute that is essential to life as we know it. x
  • 14
    Phases of Matter—Gas, Liquid, Solid
    Investigate the properties of different materials as they change phase from solid to liquid to gas. Witness the surprising behavior of supercooled water, and discover that phase diagrams are an important tool for predicting how temperature and pressure determine when phase transitions occur. x
  • 15
    Phase Diagrams—Ultimate Materials Maps
    Why does ice melt above 0°C? Why does water boil above 100°C? What quantity governs the equilibrium between liquid and gaseous phases? Use phase diagrams to probe these and other questions. Also watch a stunning demonstration of the triple point, where freezing and boiling occur simultaneously! x
  • 16
    Properties of Phases
    Dig deeper into the properties of phases and phase diagrams. First, see how a flask of water can be made to boil by cooling it. Then, explore why a curve in a phase diagram has a certain slope. Close with a multicomponent phase diagram that explains why salt causes ice to melt. x
  • 17
    To Mix, or Not to Mix?
    Explore the phenomenon of mixing—a crucial process for any situation where the product is composed of more than one material. Focus on the case of oil and water, which are notoriously unmixable, and discover what keeps them separate at the molecular level. x
  • 18
    Melting and Freezing of Mixtures
    Apply phase diagrams to the analysis of phase transitions of mixtures. Find that a mixture of two different components often has surprising properties. Learn why solder and other eutectic materials melt at a dramatically lower temperature than do their constituent substances. x
  • 19
    The Carnot Engine and Limits of Efficiency
    Study heat engines and their design limits for converting heat into work. The maximum possible efficiency in a heat engine is defined by the Carnot engine, an unattainable ideal whose properties illustrate the second law of thermodynamics. x
  • 20
    More Engines—Materials at Work
    Evaluate four other approaches to generating work from thermodynamic forces: magnetism, phase change, entropy, and surface tension. These unusual engines demonstrate the many different ways to produce mechanical energy from the unique properties of materials. x
  • 21
    The Electrochemical Potential
    Use a classic science fair project—the potato battery—to trace the source of the electron flow that makes batteries so indispensable to modern life. In the process, learn about the electrochemical potential, which describes the underlying thermodynamics of any system in which chemical reactions are occurring together with charged particles. x
  • 22
    Chemical Reactions—Getting to Equilibrium
    Chemical reactions are fundamentally part of everything we do. Learn how the concepts of thermodynamics reveal when a reaction will occur, and when it will not. Focus on the famous Haber process, which transformed agriculture by allowing nitrogen to be easily extracted from the atmosphere. x
  • 23
    The Chemical Reaction Quotient
    Continue your study of chemical reactions by contrasting two different types of reactions, shedding light on a crucial factor called the reaction quotient. In the first reaction, study pure compounds reacting together. Then look at dissolved compounds reacting. Learn how to compute the reaction quotient at any concentration. x
  • 24
    The Greatest Processes in the World
    Review the major concepts covered in the course. Then look ahead at innovative technologies that may help solve the world’s urgent energy and fresh water needs. These promising processes rely on the design of new materials, which can only be achieved through a deep understanding of thermodynamics. x

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Your professor

Jeffrey C. Grossman

About Your Professor

Jeffrey C. Grossman, Ph.D.
Massachusetts Institute of Technology
Dr. Jeffrey C. Grossman is Professor in the Department of Materials Science and Engineering at the Massachusetts Institute of Technology (MIT). He earned his B.A. in Physics from Johns Hopkins University and his M.S. in Physics and his Ph.D. in Theoretical Physics from the University of Illinois at Urbana-Champaign. Before joining MIT, Professor Grossman founded and headed the Computational Nanoscience research group at the...
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Reviews

Thermodynamics: Four Laws That Move the Universe is rated 4.3 out of 5 by 68.
Rated 5 out of 5 by from Excellent course! Excellent content balance of lecture, demos, graphics, and math/equations.
Date published: 2017-09-13
Rated 5 out of 5 by from Interesting... to say the least. I'm not a scientist, and do not have the math skills to understand the complexities of thermodynamics, but this course is presented in an easy to understand format, each lesson building on the proceeding, with added humor that really makes me look forward to the next lesson. It answers a lot of questions I've always had.
Date published: 2017-07-17
Rated 2 out of 5 by from Disappointing I was very excited to get this course and finally have thermodynamics explained to me. The instructor starts out ok and next thing you know he is just reading the formula like that is the explanation. Yes, the formula is an explanation but if I was at the level that the formula was all I needed to understand it I wouldn't have bought this course, I would have just looked up the formula on the internet. I was really expecting to be talked through these formulas and maybe given a bit of insight from a knowledgeable source.
Date published: 2017-06-25
Rated 2 out of 5 by from Couldn't finish. I was not able to finish this course. I don't think the material is that impossibly difficult--after all, I passed Thermo in college. But the inability to ask questions (*) means that anything I didn't understand (even after repeated viewing) leaves a gap that inhibits understanding of material in later lectures that depends on it. (*) I have e-mailed questions to The Great Courses on several occasions, for forwarding to the instructor, and never got a response back.
Date published: 2017-05-18
Rated 5 out of 5 by from Kid gloves approach I'm nearly through the course and have to admit I learned more about Thermo than I did in my college physical chemistry class. Great teacher who jokes about how "exciting" the material is.
Date published: 2017-03-30
Rated 5 out of 5 by from I Was Moved to Watch this in a Warmer Room Although I was neither a physicist nor a mathematician, my academic background (over 50 years ago) was in both. But I never took a specific course in thermodynamics, considering it a subject for engineering students. I ordered this course in the hope that it would fill a hole in my knowledge, and in the belief (according to quite a few reviews) that it would not be too basic. Both my hopes and beliefs were fulfilled, as Professor Grossman does not shy away from difficult concepts nor some of the easier math underlying those concepts. For me this is about a 300-level college course for engineers and science majors, minus the problem assignments and tests. This means that Dr. Grossman assumes (for the most part) a working knowledge of both differential and integral calculus, a couple of semesters of chemistry and a few more of physics. Viewers of the course without this background would still (IMO) get quite a bit of some basic concepts, but would have difficulty with concepts like Gibbs free energy. On the other hand Professor Grossman presents a clear explanation of entropy that I think could be understood by most without a science and math background. To be fair, the material, some a bit difficult is presented in fairly rapid sequence and probably needs a bit more time for reflection than is possible in 30 minutes. At least I had to hit pause and rewind in several places in order to get the points being made clear. Further I needed re-watch a couple of lectures in order to properly understand the issues. In the real world, one would go back and work out several problems outside of the classroom in order to really understand the math behind the equations, and in fact Professor Grossman in several cases mentions things that we could work out on our own. The graphics are quite good, especially those that focus on the molecular level and the multicolor phase diagrams especially by the time we got to the last couple were equally helpful. I loved the set, although it really did not contribute to the learning experience. And as for the presentation, I found the delivery almost flawless, leaving aside the few times that I could not keep up with the delivery (me, not him). It was clear that Professor Grossman loved his subject and equally loved getting students to feel the same way. A be of boyish humor (as others have noted) helped leaven what could be a dry subject and most of all I Dr. Grossman frequently referred to concepts that he liked as “cool”. His last lecture, where he discussed alternative energy sources, working in his own research just capped of the course. Professor Grossman, you are pretty cool and so is your subject. Great job.
Date published: 2017-03-06
Rated 3 out of 5 by from Gibbs "Free" Energy More examples would have helped. Do the instructors ever listen to themselves for clarity? Also, researched discussed did not cover the energy IN required to MAKE new materials could be more than energy OUT. Gibbs energy may not be "free" if there is a metaphorical power cord plugged in.
Date published: 2017-02-14
Rated 4 out of 5 by from title is apt I just started the course but find the professor interesting and the material easy to understand. I took thermodynamics in college and had a hard time with entropy etc. This seems much easier to understand or maybe I'm just deluding myself.
Date published: 2017-02-11
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