Chemistry_1031_day21_031809_actual

Chemistry_1031_day21_031809_actual - GENERAL CHEMISTRY I...

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GENERAL CHEMISTRY I CHE-1031 Dr. Jonathan M. Smith Wednesday, March 18
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Today ± Motion of molecules: kinetic theory of gases ± Collisions, diffusion, effusion ± Ideal gas and real gas deviations ± Energy ± Units ± Types ± Energy flow ± Re-Read Chapter 5 ± Begin Chapter 6 section 1-3 ± In class exam next Wednesday
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GASES Chapter 5
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Molecular Speed vs. Molar Mass ± in order to have the same average kinetic energy, heavier molecules must have a slower average speed
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Temperature and Molecular Velocities ± KE avg = ½NAmu 2 ± NA is Avogadro’s number ± KE avg = 1.5RT ± R is the gas constant in energy units, 8.314 J/mol·K ² 1 J = 1 kg·m 2 /s 2 ± equating and solving we get: ± NA·mass = molar mass in kg/mol 6 MM RT m N RT u A 3 3 rms = = as temperature increases, the average velocity increases
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Temperature vs. Molecular Speed ± as the absolute temperature increases, the average velocity increases ± the distribution function “spreads out,” resulting in more molecules with faster speeds
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() () m/s 482 10 32.00 K 298 314 . 8 3 MM 3RT mol kg 3 - K mol s m kg rms 2 2 = × = = u T(K) = t(°C) + 273.15, O 2 = 32.00 g/mol MM 3RT rms = u Ex 5.14 – Calculate the rms velocity of O 2 at 25°C O 2 , t = 25°C u rms Solution: Concept Plan: Relationship s: Given: Find: MM, T u rms MM 3RT rms = u K 298 T 273.15 25 T 273.15 C) t( T(K) = + = + ° =
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9 Mean Free Path ± molecules in a gas travel in straight lines until they collide with another molecule or the container ± the average distance a molecule travels between collisions is called the mean free path ± mean free path decreases as the pressure increases
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Chemistry_1031_day21_031809_actual - GENERAL CHEMISTRY I...

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