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# Gas Laws

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

At a constant temperature the volume of a gas is inversely proportional to the pressure | Boyles Law |

At a constant Pressure and amount of moles, the volume of a gas sample is directly proportional to the temperature in Kelvin | Charles Law |

Equal volumes of gas, at the same temp and pressure, contain the same number of particles or molecules | Avogadro's Hypothesis |

The state of an amount of gas is determined by its pressure, volume, and temperature thus PV = nRT P= pressure, V= volume, n= number of moles, R= is the gas constant, T= temperature in kelvins | Ideal gas law |

Idea gas law is favored at _______ temperatures and _______ pressures | high and low |

This law states that the total pressure exerted by gaseous mixture is equaled to the sum of the partial pressures of each individual component in a gas mixture | Dalton's Law also called Dalton Law of partial pressures |

Boyle's Law equation | P1V1=P2V2 (n and T constant) |

Charle's Law equation | V1/T1=V2/T2 (n and P constant) |

Avogadro's Law equation | V1/n1=V2n2 (P and T constant) |

How does the kinetic theory model explain the properties of gases? | In gases, particles are spaced out and move around quickly, and so gases are compressible and expand to fill a container |

What is the temperature of a gas in terms of motion of particles? | The temperature of a gas is a measure of the average kinetic energy of the particles in the gas |

How does the Kinetic theory explain collisions between gas particles? | No energy is lost from the collision but it can be transferred from particle to particle |

What is the behavior of a gas in terms of motion of particles? | Gas particles move rapidly in random, straight-line motion until they collide with the sides of a container or eachother |

How do gases relate to the volume they occupy? | The actual volume of all the particles present in a sample of gas is much less than the total volume they occupy |

What Kinetic Theory assumption is made about the attractions between gas particles? | There are no attractive or repulsive forces between particles in a gas sample |

Combined Laws equation | P1V1/n1T1 = P2V2/n2T2 |

Ideal Gas Law | PV=nRT |

Definition of STP | At atmospheric pressure, the volume of 1 mole of gas at 0 degrees Celsius is 22.4L |

Definition of SLC | At atmospheric pressure, the volume of 1 mole of gas at 25 degrees Celsius is 24.5L |

Equation for total pressure of a mixture of gases | P(total) = n(total)RT/V |

According to the Ideal Gas Law how does the number of moles relate to the pressure of that gas? | The number of moles is directly proportional to the pressure of the gas |

How do Ideal Gases and Real Gases differentiate from each other? | Ideal Gases are assumed to have no attractions between particles, whereas Real Gases have attractions due to van der Waals forces. |

What is the mole fraction? | The mole fraction is defined by the moles of a component divided by the total moles present |

True or False, Water vapor is H2O in gaseous form and its pressure is taken into consideration when performing calculations | True |

Created by:
jezzmac93