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A Brief Introduction to Thermodynamics Professor Yu Qiao University of California, San Diego 9500 Gilman Dr. MC 0085, La Jolla, CA 92093-0085 Phone: 858-534-3388 Email: yqiao@ucsd.edu Outline History of Thermodynamics: From


  1. A Brief Introduction to Thermodynamics Professor Yu Qiao University of California, San Diego 9500 Gilman Dr. MC 0085, La Jolla, CA 92093-0085 Phone: 858-534-3388  Email: yqiao@ucsd.edu Outline • History of Thermodynamics: From Metaphysics to Science • Basic Concept: Energy Conservation and Entropy • System Behaviors: Most Energetically Favorable Configurations 1

  2. History Anaximander (610 BC – 546 BC): Apeiron (w/o limit) The Milesian Group: The world is The world is made of made of Water A Single, Key Substance: Water, Fire, Air (Ether), or Thales of Miletus (624 BC - 564 BC): The first philosopher and scientist Soil… Tsou Yen: Taoism Democritus (305 BC – 240 BC) Leucippus Ajivika & Carvaka (460 BC – 370 BC) (5 th Century BC) schools in ancient Anaxagoras India (6 th Century BC) (500 BC - 428 BC) Pluralism Atomism Empedocles (490 BC - 430 BC) History What was Thales really trying to look for? Why a single key substance? Was he simply wrong? Thermodynamics : Why and How does Energy! energy dominate matters (17 th to 18 th Century) Roger Boskovic John Dalton (1745) (1808) Metaphysics: Beyond Physics – The fundamental principles of the universe Issac Newton Science & (1643-1727) Engineering Dmitri Mendeleev Aristotle Antoine (1865) (384 BC - 322 BC) Leibniz (1714): Monad Lavoisier (1777) 2

  3. Basic Concept Zero-th Law: If two systems are each in thermal equilibrium with a third, they are also in thermal equilibrium with each other. First Law: A change in the internal energy of a closed thermodynamic system is equal to the difference between the heat supplied to the system and the amount of work done by the system on its surroundings.  Energy Conservation!  Energy flows (wordpress.com) Basic Concept • Second Law: Heat cannot spontaneously flow from a colder location to a hotter location.  Energy flow is one-way, irreversible (so does time!)  Always along the direction to maximize entropy  Perpetual motion machines do not exist • Third Law: As a system approaches absolute zero, all processes cease and the entropy of the system approaches a minimum value. UC Davis: Chemiwiki http://silenced.co 3

  4. Basic Concept • The probability for a system/material to increase entropy is always higher than to decrease entropy • For example, consider a number of hard beads being shaken in a box: Scenario A: all the beads distribute uniformly Scenario B: the beads only distribute in one side of the box, leaving the other half empty Both Scenarios A & B have the same internal energy, but A has a higher entropy (the number of possible arrangements of the beads is larger). Thus, the system configuration tends to leave B and stay at A. • The beads are analogues to the air molecules in a room. Marek Straszak DonnaBellas.com AlexB17 System Variables A number of variables are used to characterize a system/material: • Temperature ( T ) There are other variables, such as voltage and charges, that can also be taken into • Pressure ( P ) consideration according to necessity. • Volume ( V ) • Internal energy ( U ): Heat – the total thermal energy • Entropy ( S ) – Measure of uncertainty of the system/material configuration       S k ln S k P ln P B B i i  i 1 For an isolated system in For an isolated system in equilibrium, where P i = 1/  equilibrium, where P i = 1/  k B = Boltzmann Constant = 1.38  10 -23 J/K P i = The probability of the i -th configuration of the system/material  = The total number of the possible configurations 4

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