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# Properties of Gases

### Properties of Gases and Gas Laws

Question | Answer |
---|---|

Definition of a gas | A gas is a substance that has no fixed shape or volume and diffuses to fill any container in which it is placed. |

Temperature used when measuring gases | Kelvin |

Brownian Motion | Random movement of particles in a gas |

Pressure of a gas (definition) | The pressure of a gas is the force it exerts per unit area. |

Units used to measure the pressure of a gas | N/m>2 or the pascal |

Atmospheric pressure in Pascals | 1x10>5 or 100,000Pa or 100kPa |

Units for measuring the volume of a gas | metres cubed |

How to convert cm cubed into meters cubed | divide by 1,000,000 |

STP | At STP 1 mole of ANY gas will occupy 22.4L |

Measurements for STP | Standard Temperature: 273K, 0 celcius. Standard Pressure: 1x10>5Pa/100kPa/1atm |

Boyle's Law | Boyle's Law states that at a constant temperature the volume of a fixed mass of gas is inversely proportional to its pressure. |

Relationship between Pressure and 1/Volume | Directly proportional |

Mathematical conclusion from Boyle's Law | pressure x volume = k |

Charles Law | Charles' Law states that at a constant pressure the volume of a fixed mass of gas is directly proportional to its temperature on the Kelvin scale |

Mathematical conclusion from Charles' Law | Volume/Temperature = k |

Guy Lussacs' Law of Combining VOlumes | Gases react in small whole number ratios provided that their volumes are measured at the same temperature and pressure |

Avogadro's Law | This states that equal volumes of gases contain equal numbers of molecules, under the same temperature and pressure |

4 rules of Kinetic Gas Theory | 1: Particles of a gas are in continuous random motion. 2: There is no attractive or repulsive forces between these molecules 3: There is no difference between the volume of a gas and the container it is in. 4: The collisions are perfectly elastic. |

Ideal Gas | An ideal gas is a gas that obeys all the assumptions of kinetic theory and all the gas laws at every temperature and pressure. |

Real Gases behave like Ideal Gases when: | Low pressure as the molecules are far apart. High temperature as the molecules are moving rapidly. |

Real Gases differ from Ideal gases when: | High pressure as the molecules are pushed close together. Low temperature as they begin to condense into liquids Most gases do exhibit some form of attractive of repulsive forces |

Ideal Gas Equation | Pv=nRT |

Volume of gases in the ideal gas equation | meters cubed |

Universal Gas Constant | 8.31 |

Created by:
cbschemistry