Ch.5 - GasesSee all chapters

Sections | |||
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Pressure Units | 10 mins | 0 completed | Learn |

Manometer | 10 mins | 0 completed | Learn Summary |

Partial Pressure | 11 mins | 0 completed | Learn Summary |

The Ideal Gas Law | 47 mins | 0 completed | Learn Summary |

Standard Temperature and Pressure | 19 mins | 0 completed | Learn |

Effusion | 8 mins | 0 completed | Learn Summary |

Root Mean Square Speed | 11 mins | 0 completed | Learn Summary |

Kinetic Molecular Theory | 9 mins | 0 completed | Learn |

Van der Waals Equation | 22 mins | 0 completed | Learn |

Velocity Distribution | 7 mins | 0 completed | Learn |

End of Chapter Problems | 74 mins | 0 completed | Learn |

Additional Sections |
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Chemistry Gas Laws |

Ideal Gas Law Density |

Ideal Gas Law Molar Mass |

Gas Stoichiometry |

Collecting Gas Over Water |

Mean Free Path |

Real Gases & Intermolecular Forces |

Kinetic Energy of Gases |

Use the van der Waal's equation to calculate the pressure (in atm) exerted by 1.00 mol of chlorine gas confined to a volume of 2.00 L at 273K. The value of a = 6.49 L^{2} atm mol^{-2}, and that of b = 0.0562 L mol^{-1 }for chlorine gas.

a) no given answer is close

b) 9.9

c) 4.12

d) 1.54

e) 3.73

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