A | B |

Boyle's Law | PV = PV |

Charles's Law | V/T = V/T |

inverse | relationship between pressure and volume |

direct | relationship between volume and temperature |

ideal gas law | takes into account pressure, volume, temperature, and moles present |

Dalton's law | deals with partial pressures |

partial pressure | amount of pressure exerted by a gas in a mixture of gases |

Avogadro's hypothesis | equal volumes of a gas at the same temp. and pressure contain equal numbers of particles |

22.4 Liters | volume a gas occupies at STP |

STP | standard temperature and pressure |

1 atmosphere | = 760 mm Hg |

2 atmospheres | = 202.6 kPa |

1 mm Hg | = 1 torr |

ideal gas constant | 8.31 L*kPa/K*mol |

diffusion | the tendency of molecules to move from areas of higher concentration to areas of lower concentration |

effusion | the process of a gas escaping through a small opening |

temperature | measure of the average kinetic energy of gas particles |

Kelvin temperature | degrees celsius + 273 |

absolute zero | where volume of a gas is zero |

combined gas law | PV/T = PV/T |

ideal gas | gas whose particles have no volume and no attraction to one another |

kinetic molecular theory | based on the concept that particles of all forms of matter are in constant motion |