Lecture 32 - Lecture 32 pls-32.1 Ideal Gas Law / Kinetic...

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Lecture 32 pls-32.1 Ideal Gas Law / Kinetic Theory Media: 1. VDF’s at several T’s 2. Thermal energy exchange videos 3. EDF’s at two different T’s. 1. Some Definitions and Relationships atomic mass unit : u = 1.6605 × 10 27 kg (= 1/12 mass of a C 12 atom) mole : 6.022 × 10 23 of any collection of objects (atoms, molecules, golf ball, etc. – let’s just refer to them generically as particles ) Avogadro’s number : N A = 6.022 × 10 23 mol 1 Boltzmann’s constant : k B = 1.3807 × 10 23 J/K gas constant : R = 8.31 J/(mol K) Relationship among these last three quantities: B A k N R = . Now consider the following: if N represent the number of particles of interest and n the number of moles of those particles, then A N n N = . Thus, R n k N n k N B A B = = . That is, B k N R n = This relationship is useful for re-expressing thermal quantities in terms of either B k or R .
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Lecture 32 pls-32.2 2. Ideal Gas Equations of State Equations of state are any equations for a system that relate the (macroscopic) thermodynamic variable. —ideal monatomic gas (IMG) T k N U B 2 3 = T k N PV B = or T R n U 2 3 = T R n PV = —ideal diatomic gas (IDG) T k N U B 2 7 = T k N PV B = or T R n U 2 7 = T R n PV = Clicker question 1 3. Kinetic Theory For any ideal gas (IMG, IDG, or other) the average CM kinetic energy
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Lecture 32 - Lecture 32 pls-32.1 Ideal Gas Law / Kinetic...

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