Question | Answer |

diffusion | spontaneous mixing of the particles of two substances caused by their random motion |

effusion | a process by which gas particles pass through a tiny opening |

elastic collision | a collision between gas particles and between gas particles and container walls in which there is no net loss of kinetic energy |

fluid | a substance that can flow and therefore take the shape of its container, a liquid or a gas |

ideal gas | an imaginary gas that perfectly fits all the assumptions of the kinetic molecular theory |

kinetic-molecular theory | a theory based on the idea that particles of matter are always in motion |

real gas | a gas that does not behave completely according to the assumption os the kinetic molecular theory |

atmosphere of pressure (atm) | exactly equivalent to 760 mm Hg |

barometer | a device used to measure atmospheric pressure |

millimeter of mercury (mm of Hg) | a common use of pressure |

newton | the SI unit for force, the force that will increase the speed of a one kilogram mass by one meter per second each second it is applied |

pascal | the pressure exerted by a force of one newton acting on an are of one square meter |

kilopascal | equal to 1.013 x 10 ^5 |

pressure | the force per unit area on a surface |

standard temperature and pressure (STP) | the agreed upon standard conditions of exactly 1 atm pressure and 0 degrees cecius |

standard ambient temperature and pressure (SATP) | equal to one bar |

torr | equal to 1 mm Hg |

absolute zero | the temperature -273.15 degree Celsius given a value of 0 in the kelvin scale |

Kelvin | the temperature at which all thermal motion ceases |

Boyle’s Law | the volume of a fixed mass of gas varies inversely with pressure at constant temperature |

Charles’s Law | the volume of a fixed mass of gas at constant pressure varies directly with the kelvin temperature |

Combined gas law | the relationship between the pressure, volume, and temperature of a fixed amount of gas |

Dalton’s Law of partial pressure | the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases |

Gay-Lusscac’s Law | the pressure of a fixed mass of gas at constant volume varies directly with the kelvin temperature |

Ideal gas law | the mathmatical relationship of pressure volume temperature and the number of moles of a gas |

Partial pressure | the pressure of each gas in a mixture |

Avogadro’s Law | equal volumes of gases at the same temperature and pressure contain equal numbers of molecules |

van der Waals equation | equation that relates the behavior of real gases to those of ideal gases |

bar | |

Gas Constant | |