chapter-05

# chapter-05 - pV = nRT pV = nRT Density = g V =[p • MM[RT...

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1331 REVIEW CHAPTER 5 Gases : Take the shape and volume of their container Very compressible Three Parameters : VOLUME measured in liters TEMPERATURE measured in KELVIN [K] (K = ° C + 273) PRESSURE measured in ATMOSPHERES or mmHg [torr] (1 atm = 760 torr) or PASCALS (1 atm = 101,325 Pa) Atmospheric measured by BAROMETER Gas sample measured by MANOMETER Three Laws : BOYLE V 1 /P CHARLES V T GAY-LUSSAC P T Solve problems by setting up ratios For bigger ratio, bigger number on top; for smaller ratio, smaller on top AVOGADRO V n Ideal Gas Law pV = nRT R = 0.082 when liters, atm and Kelvin used Moles of A n A Moles of B n B Particles N A Particles N B grams of A g Volume of Solution, L Volume of Gas, V at Temp, T, and Pressure, P grams of B g Volume of Gas, V at Temp, T, and Pressure, P Volume of Solution, L n B = (b/a)n A M = n / L n = g / MM N = 6.02 x 10 23 n N = 6.02 x 10 23 n

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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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chapter-05 - pV = nRT pV = nRT Density = g V =[p • MM[RT...

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