Gas Station

# Gas Station - 2 PV = nRT • P V T are measurable • P...

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Gas Station How do molecules move around? How do the properties of a gas interrelate? o Text: 7.0-7.2 A. States of Matter     1. Gas: Random motion throughout container   molecules apart 2. Liquid: random motion throughout volume   molecules touching 3. Solid: oscillation around fixed positions   “molecules” touching B. Kinetic Molecular Theory     1. Molecules move with a: Distribution of speeds Distribution of kinetic energies 2. KE = ½ m v^2 KE = avg. KE, m = mass, v^2 = avg. speed 3. Ave KE  α  T (Ave KE = Thermal E) Two Gasses at same T o Same as ave KE!! C. Ideal Gas Law     1. “Ideal Gas” Particles are few and far between Particles don’t interact

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Unformatted text preview: 2. PV = nRT • P, V, T are measurable • P: pressure (measure with barometer) • V: volume of container • T: absolute temp. (In Kelvin) • n: # of moles of gas • R: PV/nT = .0821 L-atm/mol-K o “Ideal gas constant” o 1 atm = 760mm Hg = 760 torr 3. PV = nRT allows predictions • P vs. V • P vs. T • V vs. T 4. Some mathematical corrections • For “real gases” o Ex. Van der Waals eq. o (P + a [n/V]^2) (V-bn) = nRT o a and b are constants Goals • Describe molec. Motion in g, 1, s • Compare KE’s, speeds of gases • Make predictions using PV = nRT...
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Gas Station - 2 PV = nRT • P V T are measurable • P...

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