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Unit 8:
Gases
Term | Definition |
---|---|
Pressure | the amount of force exerted per unit of a surface |
Newton | th SI unit for force; the force that will increase the speed of a 1 Kg mass by 1 m/s each second that the force applied |
Barometer | an instrument that measures atmospheric pressure |
Millimeters of Mercury | a unit of pressure |
Atmosphere of Pressure | the pressure of earth's atmosphere at sea level; exactly equivalent to 760 mm Hg |
Pascal | the SI unit of pressure; equal to force of 1 N exerted over an area of 1 m2 |
Partial Pressure | the pressure of each gas in a mixture |
Dalton's law of partial pressure | the law that states that the total pressure of a mixture of gasses is equal to the sum of the partial pressures of the component gases |
Boyles Law | the law that states that for a fixed amount of gas at a constant temp, the volume of the gas increases as the pressure of the gas decreases and the volume of the gas decreases as the pressure of the gas increases |
Absolute Zero | the temp at which all molecular motion stops |
Charle's law | the law that states that for a fixed amount of gas at a constant pressure, the volume of the gas increases as the temp of the gas increases and the volume of the gas decreases as the temp of gas decreases |
Gay-Lussac's law | the law that states that the volume occupied by a gas at a constant pressure is directly proportional to the absolute temp |
Combined gas law | the relationship between the pressure, volume, and temp of a fixed amount of gas |
Avogadro's law | the law that states the equal volumes of gases at the same temp and pressure contain equal numbers of molecules |
Standard molar volume of a gas | the volume occupied by one mole of a gas at STP |
ideal gas law | the law that states that the mathematical relationship of pressure volume, temp, the gas constant, and number of moles of a gas |
ideal gas constant | the proportionality constant that appears in the equation of state for 1 mol of an ideal gas |
Graham's law of effusion | the law that states that the rate of effusion of a gas is inversely proportional to the square root of the gas's density |