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Unformatted text preview: 1. Isotherms (Boyles law): T=const III. Ideal gases nRT PV RT m PV ) /( 31 . 8 K mol J R Equation of state n = m/ PV=const P 1 V 1 = P 2 V 2 T 1 T 2 > T 1 V P 2 2 2 1 1 1 T V P T V P const T PV n  number of moles m  total mass of gas =M  molar (atomic) mass (weight) 2. Isobars (Charless law): P=const V/T=const V 1 /T 1 = V 2 /T 2 P 1 P 2 > P 1 T(K) V 3. Isochors (GayLussaec ): V=const P/T=const P 1 /T 1 = P 2 /T 2 V 1 V 2 > V 1 T(K) P T(C) V273C Example 1: The temperature of an amount of an ideal gas has been increased twice, while the volume has been increased four times. What happened with the pressure? 1 1 1 2 2 2 T V P T V P T 2 = 2T 1 V 2 = 4V 1 P 2 /P 1 ? 2 1 2 4 1 1 2 2 1 1 2 T T V V P P 2 1 2 P P Example 2: What is the volume of 1 mole of an ideal gas at standard temperature and pressure? n = 1 mol T = 273 K (0 C) P = 1 atm = 1.013x10 5 Pa V  ?...
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This note was uploaded on 10/21/2010 for the course PHYS 221 taught by Professor Herrerasiklody during the Fall '08 term at Iowa State.
 Fall '08
 HerreraSiklody
 Physics, Mass

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