Gas Laws Review

# Gas Laws Review - Amonton/Charles’ Law: P1T1 = P2T2...

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Andrew Rosen Kinetic Molecular Theory of gasses 1) Gases are composed of tiny particles (molecules ) and they have attraction for each other 2) Molecules are small compared to the distance between them – Volume (exception: Ideal gases have no/neglible volume) 3) Move in a random straight line in motion 4) Collisions with each other transfers energy 5) Pressure is exerted with collisions with the container walls 6) Pressure = ForceArea Barometer: Measures atmospheric pressure Manometer: Used to measure pressure of a gas Ideal Gas: Have no attraction and no volume. High temp. and low pressure Real Gas: Have attraction and have volume. Low temp. and high pressure Boyle’s Law: P 1 V 1 = k = P 2 V 2 (Temp. constant) (Indirect and curved relationship) Charles’ Law: V1T1 = k = V2T2 (Pressure Constant) (Direct Relationship)
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Unformatted text preview: Amonton/Charles’ Law: P1T1 = P2T2 (Volume constant) (Direct relationship) Combined Gas Law: P1V1T1 = P2V2T2 (Direct relationship) Density of gases: Increase in D with; increase P, decrease in V and decrease in T Dalton’s Law of Partial Pressure: P total = P gas1 + P gas2 Collecting a gas over water: P total = P gas + P water vapor Graham’s Law of Diffusion: KE = ½ mV 2 Ke gas1 = Ke gas2 (T is constant) Vgas1Vgas2 = mgas1mgas2 Lussac’s Law of Combining Volumes of Gases: Relative volumes of gases and their products are in small whole number ratios 2 H 2 + 1 O 2 2 H 2 O 2 volumes of H 2 + 1 volume of O 2 2 volumes of H 2 O Avogadro: Equal volumes of gasses, same temp. and pressure, and same number of molecules...
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## This note was uploaded on 02/17/2011 for the course CHEM 101 taught by Professor Me during the Spring '11 term at Bellarmine.

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