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9 Cards in this Set
- Front
- Back
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Pressure |
STP 1 atm = 101.3 kPa = 760 mmHg -Is the amount of force exerted on an area -Pressure at sealevel is 1 atm |
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Kinetic Theory |
-Base of all gas laws. Very essential -According to kinetic theory:g Gas composed of particles, considered small hard spheres with significant volume. no attractive/repulsive forces -In constant motion & gas fill container, unconstrained gas will diffuse -Average KE of collection of gas particles is directly proportional to kelvin temp of gas. |
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Variables that describe gas |
-Amount: pressure caused by collisions of particles within walls of container. Adding a gas increases number of particles, increases pressure. Directly proportional. -Volume: Pressure increased by reducing size of a container. Inversely proportional. -Temp: raising temp increases pressure. doubling kelvin, doubles pressure. |
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Boyles law |
-Constant temp, volume varies inversely with pressure: P1V1=P2V2 |
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Charles' law |
-Volume is directly proportional to kelvin temp. Pressure remains constant. - V1/T1=V2/T2 |
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Gay-Lussac's Law |
-Pressure is directly proportional to kelvin temp if volume is constant. - P1/T1=P2/T2 |
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Combined gas law |
Three gas laws above can be combined into a single gas law P1V1/T1=P2V2/T2 *Note temp must be kelvin and pressure and volume must be same units on both sides |
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Ideal gas law |
-Includes three variables (temp, pressure and volume). Adds another one- amount of gas in a system (expressed in moles) PV=nRT -Where R is a constant whose units change depending on the value used for pressure: -If you use kPa, R=8.315 kPa.L/mol -If you use atm, R= 0.0821 atm.L/mol -It you use mmHhg, R= 62.4 mmHg.l/mol |
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Ideal gas law + kinetic theory |
-KE assumes particles have no volume, therefore they don't exist -Ideal gas obeys all the gas laws at all conditions -Real gasses can be liquefied, ideal cannot. -Ideal can be compressed at 0k to be 0 volume (theoretically), real gasses cant- they have volume. They become liquids at low temp and high pressure |
