Gases Outline

Gases Outline - and moles o Charles Law when temperature increases volume increases(constant pressure and moles o Gay-Lussac’s Law when

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CHEMISTRY 120 – CHAPTER 6 – REVIEW Gases Kinetic Molecular Theory (KMT): seeks to explain the behavior of gases. o Gases consist of small particles that: Are far apart. Move rapidly in straight lines. Move rapidly at higher temperatures. Do no interact with other gas particles. Have small particle volume compared to the volume a gas occupies. Pressure, P: Force exerted by a gas on the walls of the container. o Units: Atmosphere (atm), mmHg, Torr, Pascal. 1 atm = 760 mmHg (exact) = 760 torr o Atmospheric pressure: The pressure exerted by a column of air from the top of the atmosphere to the surface of the earth. Barometer: measures atmospheric pressure. o Boyle’s Law: when volume decreases, pressure increases. (constant temperature
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Unformatted text preview: and moles) o Charles Law: when temperature increases, volume increases (constant pressure and moles) o Gay-Lussac’s Law: when temperature increases, pressure increases (constant volume and moles). o Combined Gas Law: constant moles, P 1 V 1 /T 1 = P 2 V 2 /T 2 o Avogadro’s Law: gas volume is directly related the number of moles of gas. (constant T, P) • Partial Pressure: the pressure of a gas if it were the only gas in the container. o Total pressure: P T = P 1 + P 2 + P 3 …. o Gases in Blood: Oxygen flows into the tissues because the P oxygen is higher in the blood then the tissues. Carbon dioxide flows out of the tissues because its partial pressure is higher in the tissues and lower in the blood....
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This note was uploaded on 04/10/2008 for the course CHEM 231 taught by Professor Hanover during the Spring '08 term at Lansing.

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