Updated 04/07 |

Updated 05/09 |

3. Explain the kinetic molecular theory with respect to gas phase and what the major gas parameters mean (T, P, V, and n). |

3. Explain the kinetic molecular theory (i.e. ideal gas condition) with respect to gas phase and what the major gas parameters mean (T, P, V, and n). Be able to tell the difference between the ideal gas condition and real gas condition. |

9. Describe the conditions under which a real gas deviates from ideal behavior. [6.4] |

*Each student will be able to:*

1. Eplain the differemce between compressible and incompressible and which phase of matter has each.

2. Explain what barometric pressure (including a barometer)is and be able to understand and calculate gas pressures from manometers.

3. Explain the kinetic molecular theory (i.e. ideal gas condition) with respect to gas phase and what the major gas parameters mean (T, P, V, and n). Be able to tell the difference between the ideal gas condition and real gas condition.

4. Using the kinetic molecular theory, explain the relationship (including doing calculations) between pressure and volume (Boyle's law), pressure and temperature (No-Name), volume and temperature (Charles' law), and the number of particles in a gas sample (Avogadro's hypothesis).**[6.1](6.1)**

5. Explain the relationship between temperature and average kinetic energy.**[6.2]**

6. Perform calculations using the ideal gas law including the gas constant, R. As part of this, understand the molar volume (i.e. volume of a mole of gas) is a constant for any gas at a specific temperature and pressure. Specifically for 273K and 1.0 atm (STP), the molar volume is 22.4L (experimentally determine this value). **[6.3](6.2)**

7. Use the combined gas law to determine changes in pressure, volume, or temperature.**[6.6](6.1)**

8. Explain the difference between diffusion and effusion including understand and calculating problems on Grahman's Law of Diffusion.