chap11[1] - Chapter 11 Gas Laws The Effect of Gas Pressure...

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Unformatted text preview: Chapter 11 Gas Laws The Effect of Gas Pressure the pressure exerted by a gas can cause some amazing and startling effects whenever there is a pressure difference, a gas will flow from area of high pressure to low pressure the bigger the difference in pressure, the stronger the flow of the gas if there is something in the gas path, the gas will try to push it along as the gas flows Soda Straws & Gas Pressure The pressure of the air inside the straw is the same as the pressure of the air outside the straw so liquid levels is the same on both sides. The pressure of the air inside the straw is lower than the pressure of the air outside the straw so liquid is pushed up the straw by the outside air. Air Pressure the atmosphere exerts a pressure on everything it contacts on average 14.7 psi the atmosphere goes up about 370 miles, but 80% is in the first 10 miles from the earths surface this is the same pressure that a column of water would exert if it were about 10.3 m high Common Units of Pressure Unit Average Air Pressure at Sea Level pascal (Pa) 101,325 kilopascal (kPa) 101.325 atmosphere (atm) 1 (exactly) millimeters of mercury (mmHg) 760 (exactly) inches of mercury (inHg) 29.92 torr (torr) 760 (exactly) pounds per square inch (psi, lbs./in 2 ) 14.7 Kinetic Molecular Theory the particles of the gas, (either atoms or molecules), are constantly moving the attraction between particles is negligible when the moving particles hit another particle or the container, they do not stick; but they bounce off and continue moving in another direction like billiard balls Kinetic Molecular Theory there is a lot of empty space between the particles compared to the size of the particles the average kinetic energy of the particles is directly proportional to the Kelvin temperature as you raise the temperature of the gas, the average speed of the particles increases but dont be fooled into thinking all the particles are moving at the same speed!! Kinetic Molecular Theory Boyles Law pressure of a gas is inversely proportional to its volume constant T and amount of gas graph P vs V is curve graph P vs 1/V is straight line as P increases, V decreases by the same factor Boyles Experiment added Hg to a J-tube with air trapped inside used length of air column as a measure of volume Length of Air in Column (in) Difference in Hg Levels (in) 48 0.0 44 2.8 40 6.2 36 10.1 32 15.1 28 21.2 24 29.7 22 35.0 Inverse Volum e vs Pressure of Air, Boyle's Expt.Inverse Volum e vs Pressure of Air, Boyle's Expt....
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This note was uploaded on 04/11/2008 for the course CHE 101 taught by Professor Churchhill during the Fall '08 term at SUNY Buffalo.

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chap11[1] - Chapter 11 Gas Laws The Effect of Gas Pressure...

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