| Term | Definition |
|---|
| barometer | a device that measures atmospheric pressure |
| mm Hg | millimeters of mercury |
| torr | milimeters of mercury, in honor of Torricelli`standard |
| standard atmosphere | a unit of measurement for pressure equal to 760 mm Hg |
| pascal | the SI unit of measurement for pressure; equal to one newton per square meter |
| Boyle's Law | The volume of a given sample of gas at constant temperature varies inversely with the pressure |
| absolute zero | -273 C is the lowest point, when converted to Kelvin, is 0. cannot be lower than this on Kelvin scale |
| Charles's law | The volume of a given sample of gas at constant pressure is directly proportional to the temperature in kelvins |
| Avogadro's Law | Equal volumes of gases at the same temperature and pressure contain the same number of particles (atoms or molecules) |
| universal gas constant | The combined proportionality constant in the ideal gas law |
| ideal gas law | An equation relation the properties of an ideal gas, expressed as PV=nRT The equation expresses behavior closely approached by real gases at high temperature and/or low pressure |
| ideal gas | A hypothetical gas that exactly obeys the ideal gas law. A real gas approaches ideal behavior at high temperature and/or low pressure |
| combined gas law | P1V1/T1 = P2V2/T2. It holds when the amount of gas is held constant. |
| partial pressure | the independent pressures exerted by different gases in a mixture |
| Dalton's law of partial pressures | For a mixture og ases in a container, the total pressure exerted is the sum of the pressures that each gas would exert if it were alone |
| kinetic molecular theory | A model that assumes that an ideal gas is composed of tiny particles (molecules) in constant motion |
| molar volume | The volume of one mole of an ideal gas; equal to 22.42 liters at standard temperature and pressure |
| standard temperature and pressure | The condition 0 C and 1 atmosphere of pressure |
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