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Unformatted text preview: Chapter 10 Gases A. Definitions B. Gas Laws C. Ideal Gas Equation D. Kinetic Theory of Gases E. Deviations from Ideal Behavior HW #P5 Covered on Quiz #3 and Exam #2 Chapter 10 Gases A. Definitions 1. Gas B molecules of a gas are not held together, expand to fill the space available and can be compressed. 2. Volume is the space occupied. 1 liter = 1 cubic decimeter 1 cc = 1 ml 1h = 1000 ml = 1000 cc 3. Temperature Scales hC = 5/9 (hF B 32h) K = hC + 273.15 absolute zero in temperature is 0 K or B 273.15hC 4. Pressure pressure is measured as a force acting on an area tires are pounds/in 2 We primarily use relative measures of pressure, since we are always surrounded by gases. A barometer at sea level will measure 760 mm of Hg. This is defined as 1 atm. 1 atm = 760 mm Hg also 1 mm Hg = 1 Torr STP (standard temperature and pressure) 1 atm (760 mm Hg) and 0hC (273 K) P = F A kg  meter/s 2 m 2 scientific is which is a Pascal (Pa) Example: Convert 0.605 atm into pressure in Torr. B. Gas Laws 1. Pressure and Volume Relations B Boyle = s Law Observation B for a given amount of air at constant temperature increasing pressure decreases the volume. 1 h at 1 atm 0.5 h at 2 atm Two Expressions PV = constant 2. Volume and Temperature Relations B Charles = Law Observation B demonstration for constant pressure V α T T is in Kelvin Charles = Law B At constant pressure the volume of a given quantity of gas is proportional to absolute temperature ....
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This note was uploaded on 09/28/2009 for the course CHE 101 taught by Professor Churchhill during the Fall '08 term at SUNY Buffalo.
 Fall '08
 Churchhill
 Chemistry, Mole

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