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Unformatted text preview: pV = nRT pV = nRT Density = g / V = [p • MM] / [RT] Molar Mass = gRT / pV STP 1 atm pressure, 273 K, 1 mole of ideal gas occupies 22.4 L Ideal Gas: 1. particles have negligible volume 2. particles do not interact with each other 3. all collisions are perfectly elastic 4. average kinetic energy T in K Dalton’s Law Gas in a mixture behave as if the only ones there Contribute PARTIAL PRESSURE Partial Pressure ∝ number of moles Partial Pressure = mole fraction x total pressure Graham’s Law Gases effuse or diffuse inversely proportional to √ mass Lighter move more quickly V 1 / V 2 = √ M 2 / M 1 Real Gases Van Der Waals Equation [VDW] Gases DO interact, so P bigger than measured (b in VDW) Gases DO have volume, so V smaller than measured (a in VDW) Gases more ideal at high V, high T, low n and low P....
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 Spring '08
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 pH, Kelvin, K Gas

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