Physical Properties of Gases

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Presentation transcript:

Physical Properties of Gases Have mass Are compressible Fill their container Move through each other (diffusion) Exert pressure Pressure depends on temperature

Kinetic Molecular Theory (How gas molecules behave) Very small particles Distances between particles are large In constant, random motion Collisions are perfectly elastic Kinetic energy depends of temperature of gas Particles exert no force on each other

Pressure Pressure exerted by air = atmospheric pressure (air has mass and is attracted by Earth’s gravity) 1 atm = 101,325 Pascal (Pa) 101.325 kiloPascals (kPa) 760 mm Hg 14.7 psi 29.92 inches Hg

Gas Laws Boyle’s Law: P1V1=P2V2 Lussac’s Law: P1/T1 = P2/T2 Charles’ Law: V1/T1 = V2/T2 Dalton’s Law: Ptotal = P1 + P2 + … Ideal Gas Law: PV=nRT R=0.0821 atm*L/K*mol All Temperatures must be in Kelvin! (oC+273)