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Unit 8
Gases
| Term | Definition |
|---|---|
| Pressure | The amount of force exerted per unit area of a surface |
| Newton | The 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 is applied (abbreviation, N) |
| 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 the force of 1 N exerted over an area of 1 m2 (abbreviation, Pa) |
| Partial Pressure | the pressure of each gas in a mixture |
| Dalton´s law of pressure | the law that states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases. |
| Boyle´s law | the law that states that a fixed amount of gas at a constant temperature, 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 temperature at which all molecular motion stops (0 K on the Kelvin scale or -273. 16 Celsius on the Celsius scale) |
| Charles law | the law that states that for a fixed amount of gas at a constant pressure, the volume of the gas increases as the temperature of the gas increases and the volume of the gas decreases as the temperature of the 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 temperature. |
| Combined gas law | the relationship between the pressure, volume, and temperature of a fixed amount of gas. |
| Avogrado´s law | the law that states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. |
| Standard molar volume of a gas | The volume occupied by one mole of a gas at STP. It has been found to be 22.414 10 L |
| Ideal gas law | the law that states that mathematical relationship of pressure (P), volume (V), temperature (T), the gas constant (R), and the number of moles of a gas (n); PV = nRT |
| Ideal gas constant | the proportionality constant that appears in the equation of state for 1 mol of an ideal gas; R = 0.082 057 84L x am/mol x K |
| Graham´s law of effusion | the law states that the rate of effusion of a gas is inversely proportional to the square root of the gas´s density. |
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