CH104chpt7.pdf CH 104
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This 2 page Class Notes was uploaded by Regan Dougherty on Thursday November 5, 2015. The Class Notes belongs to CH 104 at University of Alabama - Tuscaloosa taught by Stephen Woski in Summer 2015. Since its upload, it has received 11 views. For similar materials see Introductory Chemistry in Chemistry at University of Alabama - Tuscaloosa.
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Date Created: 11/05/15
Thursday November 5 2015 CH 104 Chapter 7 Gases Liquids and Solids The Three States of Matter Solid Liquid Gas Existing as a gas liquid or solid depends on the balance between the kinetic energy of its particles the strength of the interactions between the particles intermolecular forces Gases Measurable properties of gases volume liters number of particles moles temperature kelvins Kelvins MUST be used in calculations Increasing temperature increases kinetic energy pressure atmospheres is the force exerted per unit area as gas particles collide with the walls of a container 1atm 760 mm Hg 760 torr 147 psi pounds per square inch 101325 Pa pascals know mm Hg and torr Thursday November 5 2015 Gas Laws Boyle s Law As P increases V decreases for constant T and n Charles s Law As T increases V increases for constant P and n GayLussac s Law As T increases P increases for constant V and n Combined Gas Law shows the relationship of P V and T when two quantities are changed and the number of moles is constant combines all 3 gas laws see Table 72 for equations P pressure the units do not matter as long as they are consistent V volume the units do not matter as long as they are consistent T temperature MUST be in Kelvins n moles Molar Volume At STP standard temperature and pressure 298 K 1 atm1 mol of any gas occupies 224 L ldeal Gas Law PV nRT R gas constant we will be given this All units in the equation must be the same as the units in the constant moles Kelvin atm L Dalton s Law of Partial Pressure The total pressure of a mixture of gas is the sum of all of the pressures of the gases
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