Thermodynamics lectures

In lectures, thermodynamics lectures are often the seed or impetus behind the later development of important new theories and ideas. Various free-courseware thermodynamics lectures, from Strathcona-Tweedsmuir high school, MIT, Yale, etc., are posted below (a work in progress):

Famous lectures
A few famous examples of noted thermodynamics lectures include German physicist Rudolf Clausius’ 1865 reading of his paper “On Several Convenient Forms of the Fundamental Equations of the Mechanical Theory of Heat” to the Philosophical Society of Zurich on April 24th, in which the two famous enunciations of the laws of thermodynamics were first spoken, namely the energy of the universe is constant and the entropy of the universe tends to a maximum; English physiologist William Bayliss’ 1922 Twenty-fourth Robert Boyle Lecture “Life and the Laws of Thermodynamics”, delivered Before the Junior Scientific Club of the University of Oxford on 7th June; English astronomer Arthur Eddington’s 1927 Gifford Lectures delivered at the University of Edinburgh, January to March, resulting in the 1928 book The Nature of the Physical World, in which are found the shuffling card model of entropy and the notion of the entropy arrow of time; as well as Austrian physicist or Erwin Schrodinger’s 1943 lectures delivered at Trinity College, Dublin, in February 1943, resulting in the famous 1944 book What is Life?, in which are found the postulate that life feeds on negative entropy.
English physical chemist George Porter’s episode four "An Introduction to Chemical Change and Thermodynamics" of his 1965 BBC series of lectures entitled 'The Laws of Disorder: an Introduction to Chemical Change and Thermodynamics', wherein he discusses entropy, the arrow of time, and gives the following quote: “The second law has been quoted as the sine qua non of scientific enlightenment.” [6]

NIU | Human Chemical Thermodynamics | Spring 2013
The following is a 45-minute 16 Apr 2013 lecture entitled "Human Chemical Thermodynamics: Goethe's Elective Affinities to Human Free Energies" (see: lecture notes) by American electrochemical engineer Libb Thims given to the engineering students, primarily mechanical engineering thermodynamics students, and faculty of the Norther Illinois University—full lecture below left, condensed synopsis of experimental demonstrations below right:



MIT 5.111 Principles of Chemical Science | Fall 2005
The following are the main thermodynamics lectures from the 36-part lecture series of the Fall MIT course 5.111 Principles of Chemical Science: [1]




18. Thermodynamics and Spontaneous Change 23. Cell Potentials and Free Energy




Yale PHYS 200 Fundamentals of Physics | Fall 2006
The follow four lecture parts (20-23), by physicist Ramamurti Shankar, are devoted to thermodynamics: [2]


21. Thermodynamics22. Boltzmann constant and the first law of thermodynamics23. The second law of thermodynamics and Carnot's engine24. The second law of thermodynamics and entropy


AP Chem Thermodynamics (grade 12) | 2008
The following video set is by Rob Lederer a senior level / grade 12 chemistry teacher Strathcona-Tweedsmuir high school for over 26 years, who makes a DVD series on chemistry lessons (ChemGuy.com): [3]

Intro: Chemical energetics (introduction to energy)1. Entropy and spontaneous reactions2. Change in the entropy of the universe3. Gibbs free energy calculation 4. Free energy calculations: products – reactants = ΔG




5. Free energy, equilibrium constant; Nernst equation





MIT 5.60 Thermodynamics & Kinetics | Spring 2008
The following 36-part lecture series, delivered by chemists Moungi Bawendi (video one) and Keith Nelson (video three), based on the 2004 textbook Physical Chemistry by Robert Sibey, Robert Alberty, and Bawendi, deals primarily with equilibrium properties of macroscopic systems, basic thermodynamics, chemical equilibrium of reactions in gas and solution phase, and rates of chemical reactions. [4]


1. State of a system, 0th law, equation of state 2. Work, heat, first law 3. Internal energy, expansion work 4. Enthalpy 5. Adiabatic changes

6. Thermochemistry 7. Calorimetry 8. Second law 9. Entropy and the Clausius inequality 10. Entropy and irreversibility

11. Fundamental equation, absolute S, third law 12. Criteria for spontaneous change 13. Gibbs free energy 14. Multicomponent systems, chemical potential 15. Chemical equilibrium

16. Temperature, pressure and Kp 17. Equilibrium: application to drug design
18. Phase equilibria — one component 19. Clausius-Clapeyron equation 20. Phase equilibria — two components

21. Ideal solutions 22. Non-ideal solutions 23. Colligative properties24. Introduction to statistical mechanics25. Partition function (q) — large N limit

26. Partition function (Q) — many particles27. Statistical mechanics and discrete energy levels28. Model systems29. Applications: chemical and phase equilibria30. Introduction to reaction kinetics

31. Complex reactions and mechanisms32. Steady-state and equilibrium approximations33. Chain reactions34. Temperature dependence, Ea, catalysis35. Enzyme catalysis





36. Autocatalysis and oscillators






MIT 5.111 Principles of Chemical Science | Fall 2008
The following are the main thermodynamics lectures from the 36-part lecture series of the Fall MIT course 5.111 Principles of Chemical Science: [5]

16. Determining hybridization in complex molecules; thermochemistry and bond energies / bond enthalpies. 17. Entropy and disorder18. Free energy and control of spontaneity19. Chemical equilibrium20. Le Chatelier's principle (applied to blood-oxygen levels)



25. Electrochemical cells34. Temperature and kinetics




References
1. Video Lectures (1-36) – MIT 5.111 | Principles of Chemical Science | Fall 2005 – OCW.MIT.Edu.
2. Physics – Yale PHYS 200 | Fundamentals of Physics | Fall 2006 – Open Yale courses.
3. (a) BannanaIsCool – YouTube.com.
(b) Home – ChemGuy.com.
(c) Rob Lederer (about) – ChemGuy.com.
4. Video Lectures – MIT 5.60 | Thermodynamics & Kinetics | Spring 2008.
5. Video Lectures (1-36) – MIT 5.111 | Principles of Chemical Science | Fall 2008 – OCW.MIT.Edu.
6. (a) George Porter (collection) – NationalArchives.Gov.uk.
(b) Porter, George. (1972). Molecules to Men (quote, pg. 17). Heinemann Educational.

External videos
‚óŹ (a) Thermodynamics in a Nutshell: the Definition of Entropy in One Hour (1:49 hours) by Gian Beretta at the AIP 2008 - TechTV.mit.edu.
(b) Thermodynamics in a Nutshell (blackboard closeups) – Web.MIT.edu.

EoHT symbol


More pages