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# Gas **

### Part 3

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

Earth's radius | 6370 Km |

Earth's barometric pressure | 760 mm Hg (density of Hg = 13.6 g/cm^3) |

Molecular mass of air | 29 g/mol |

partial pressure of a gas | the pressure exerted by a component of a mixture of gases |

mole fraction | n1/nt (partial pressure of one component of gas/total pressure) |

Equation for partial pressure involving mole fraction | (n1/nt)Pt = X1Pt |

The Kinetic-Molecular Theory (the theory of moving molecules by Calusius) | Gases consist of a lot of molecules (or atoms, in the case of the noble gases) that are in continuous random motion. Kinetic energy of the the molecules doesn't change w/time (as long as T is constant). |

Kinetic-Molecular Theory - what if you have two gas samples, both at the same temp. | then the kinetic energy for the collection of gas molecules in one sample is equal to the kinetic energy for the collection of gas molecules in the other sample. |

To to measure hardness of that the molecules hit the wall | V*M (velocity times mass of molecules) |

if the temp. of a gas is doubled, then the kinetic energy of its molecules is...? | doubled |

root mean square speed | = 1/2 mu^2 |

What happens when volume increases but the temp. is constant? | pressure will decrease |

What happens when temp. increase at a constant volume | increase in pressure. |

root mean square (rms) speed: | (sqrt(3RT/M) M is the molar mass |

effusion | rate of escape of a gas through a tiny or or pinhole in its container |

diffusion | the speed of one substance through space, or through a second substance (such as the atm) |

Which will effuse more rapidly, a lighter gas or a heavy gas | a lighter gas |

which will diffuse faster, lighter molecules or heavy ones | lighter ones |

Effusion rate equation | (sqrt(1/M)) |

mean free path | average distance traveled by a molecule |

The higher the density of gas, the (blank) the mean free path | smaller. (more likelyhood of a collision) |

The deviation from ideal gas behavior is (blank) at high pressure | large |

As temp. increases the deviation from ideal behavior (blank) | decreases |

characteristics of ideal gases | occupy no set volume, gas molecules have no attraction or repulsion for each other |

Is the ideal gas equation good at high pressures? | not really |

How are P and V related at constant P? | inversely proportional |

How are P and T related at constant V? | directly proportional |

P and n are related how at constant V? | directly proportional |

how are gas density related to molar mass and pressure? | density is proportional to molar mass and pressure |

how are gas density related to temperature? | density is inversely proportional to temperature |

Molar mass = | Density*R*T/P |

Created by:
Tiffastic