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# 092908 - y A sample of solid potassium chlorate was heated...

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Partial Pressures y What happens when two ideal gases are mixed in a container? y Dalton’s Law: The pressure exerted by a gas in a mixture is the same pressure that would have been exerted if the gas were alone in the container.

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Mole Fractions y The number of moles of a particular gas divided by the total number of moles of gas present
Partial Pressures y A gas mixture at 100 o C and 0.8 atm is made of: 50% He and 50% Xe by weight. What are the partial pressures of He and Xe?

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A mixture of gases contains 2.0 mol He, 3.0 mol Ne and 1.0 mol Ar, with a total pressure of 8.0 atm. What is the partial pressure of He? 4.0 atm 2.7 atm 1.3 atm 8.0 atm 9% 0% 5% 86% 1. 4.0 atm 2. 2.7 atm 3. 1.3 atm 4. 8.0 atm
Practice Problem y A container of unknown volume contains He at 25 o C and 1.960 atm. When a portion of the He is withdrawn and adjusted to 1.00 atm, it is found to have a volume of 1.75 mL. The gas remaining in the first container now has a pressure of 1.710 atm. Determine the volume of the container.

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Collecting a gas over water
Collecting a gas over water

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Unformatted text preview: y A sample of solid potassium chlorate was heated in a test tube and decomposed by the reaction that follows. The oxygen was collected by displacement of water at 22 o C at a total pressure of 754 torr. The volume of the gas collected was 0.650 L, and the vapor pressure of water at 22 o C is 21 torr. Calculate the mass of KClO 3 in the sample that decomposed. { KClO 3 (s) Æ KCl (s) + O 2 (g) Kinetic Molecular Theory y 1. Molecules are small and occupy little space in a gas. Therefore we assume they are only dimensionless points. Kinetic Molecular Theory y 2. Molecules move very rapidly in a gas and exert a force on the walls. Kinetic Molecular Theory y 3. Molecules have no forces between them. When they collide they undergo elastic collisions: the molecules do not absorb any energy. Kinetic Molecular Theory y 4. The average kinetic energy of a collection of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas....
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