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Thermodynamics and Chemical Dynamics 131C. Lecture 12. Entropy and The Second Law.

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Thermodynamics and Chemical Dynamics (Chem 131C) is part of OpenChem: video is part of a 27-lecture undergraduate-level course titled "Thermodynamics and Chemical Dynamics" taught at UC Irvine by Professor Reginald M. Penner.Recorded on April 30, 2012.Slide Information00:09 - Introduction01:02 - Announcements02:11 - where are we (chapter and timeline)?04:00 - 1st Law: Energy is conserved for an isolated system ΔU = 0.05:32 - Coin Experiment06:35 - experiment: conclusion (the most important one so far)06:51 - Boltzmann postulated that this parameter07:11 - We can readily apply this equation to this expansion of gas.08:11 - Now, what is the probability that...09:05 - Problem: Gas A and Gas B are located in two halves of a container13:07 - What if instead of the change in entropy...13:33 - Formula (S =)14:09 - Calculate the standard molar entropy of neon gas at (a) 200K, (b) 298.15K.15:53 - Sadi Carnot17:54 - match the scientist with his country18:44 - entropy19:28 - the Carnot Cycle21:00 - A heat engine extracts work from a temperature gradient21:41 - The Carnot Cycle (graph)23:31 - what do we know for sure? (graph continued from Carnot Cycle)24:18 - how efficient is a heat engine?25:10 - efficiency (slide at 24:18 continued)26:24 - how efficient is a Carnot Cycle?27:28 - let's prove this:27:52 - now, this pair of (T,V) data points lie on an adiabat:29:55 - Problem: A heat pump is used to maintain the temperature of a building at 18°C...32:03 - Problem: What is the entropy change, ΔS, for each of the four steps as a reversible Carnot cycle32:31 - Diagram: Since S is a state function, we can write:33:50 - so we represented in a Temperature-Entropy diagram...34:48 - Since S is a state function, we can write:For more information and access to courses, lectures, and teaching material, please visit the official UC Irvine OpenCourseWare website at:

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