Gases
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25 terms
Terms | Definitions |
|---|---|
 Millimeters Mercury | The common unit of pressure, symbolized mm Hg |
| Atmosphere | a unit of pressure: the pressure that will support a column of mercury 760 mm high at sea level and 0 degrees centigrade |
| bar | a unit of pressure that is nearly, but not quite equal to an atmosphere; 1.013bar = 1atm = 760mm Hg |
| Ideal Gas Law | Volume is directly proportional to amount. Volume is directly proportional to absolute temperature.Volume is inversly proportional to pressure. |
| Ideal Gas Equation | PV=nRT |
| R | Gas constant; 0.0821 (L atm/ mol K), 8.31 (J/ mol K), 8.31x10³ (g m²/ s² mol K) |
| STP | standard temperature and pressure; EX: At STP, one mole of gas occupies 22.4 L. |
| Vapor Pressure | the pressure exerted by a vapor over a liquid |
| Mole Fraction | The ratio of the moles of the substance to the total moles. |
| Partial Pressure | the pressure of each gas in a mixture |
| Effusion | passage of a gas through a small hole |
| Combined Gas Law | P₁V₁/ T₁ = P₂V₂/ T₂ |
| Boyle | held temperature constant; Equation: P₁V₁ = P₂V₂ (Chickens Go Bawk) |
| Charles | held pressure constant; Equation: V₁/ T₁ = V₂/ T₂ (Chickens Go Bawk) |
| Gay-Lussac | held volume constant; Equation: P₁/ T₁ = P₂/ V₂ (Chickens Go Bawk) |
| Avogadro's Law | Equal volumes of gases at the same temperature and pressure contain the same number of particles. |
| Diffusion | the spreading of a gas through a room. |
| Dalton's Law | the total pressure is equal to the sum of its parts. |
| Graham's Law | velocity of gas varies inversley with mass. |
| Kinetic Theory | the theory that gases are made up of a large sum of small particles. |
| Vapor | the gaseous form of any substance |
| Velocity | the distance traveled per unit time |
| Manometer | a pressure gauge for comparing pressures of a gas |
| Barometer | an instrument that measures atmospheric pressure |
| Kinetic Molecular Theory | -KE is directly proportional to the absolute temperature. -The volume of s gas particle is negligible relative to the volume in which the gas is contained. -Attractive and repulsive forces between gas molecules are negligible. -Gases consist of atoms or molecules in constant, random motion. -At a given temperature, all gases will have the same average KE. -Collisions between gas particles and their container are elastic. |
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