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# Gases

### Gases Yr 11 Chemistry

Term | Definition |
---|---|

Avogadro's Law | Equal volumes of any gas, measured at the same temperature and pressure, contain the same number of particles. V1/n1 = V2/n2 Direct |

Kinetic Theory of Gases | 1). Molecules move in continual random straight-line motion. 2). Average distance between molecules is very large. 3). Negligible intermolecular forces. 4). Perfectly elastic collisions between molecules - no net energy loss. 5). Pressure is due to collisions of the molecules with the walls of the container. 6). Temperature is the measure of the average kinetic energy of the molecules. |

Molar Volume formula | Number of moles of gas = volume of gas (at STP) / volume of one mole of gas (at STP) STP in this case is an example – the volumes must be measured at a consistent temperature and pressure, but it doesn’t need to be STP. |

STP | Standard Temperature and Pressure 0 C and 100 kPa |

SLC | Standard Laboratory Conditions 25 C and 100 kPa |

Molar Volume at STP | 22.71 L |

Molar Volume at SLC | 24.79 L |

Graham's Law | Rates of diffusion of gases at the same temperature and pressure are inversely proportional to the square roots of their molar masses. Rate A / Rate B = sqrt(Molar Mass B / Molar Mass A) |

Pressure formula | Pressure = force / area |

Dalton's Law | The total pressure of a mixture of gases is equal to the sum of the pressures of all the gases in the mixture. Ptotal = Px + Py + Pz Pgas = Ptotal x Moles of gas / Total moles |

Temperature is measured in | Kelvin (conversion from Celsius = C + 273) |

Boyle's Law | At a constant temperature, the volume of a fixed quantity of gas is inversely proportional to the applied pressure. P1V1 = P2V2 inverse relationship |

Charles' Law | At a constant pressure, the volume of a fixed quantity of gas is proportional to its absolute (kelvin) temperature. V1 / T1 = V2 / T2 direct |

Gay-Lussac's Law | If the volume of a container is held constant as the temperature of a gas increases, the pressure inside the container will also increase. P1 / T1 = P2 /V2 direct |

Combined Gas Law | P1V1 / T1 = P2V2 / T2 direct |

General Gas Equation (Ideal Gas Equation) | PV = nRT p = pressure, v = volume, n = number of moles, R = universal gas constant, T = temperature |

Created by:
MrMartyn1