Editing revision 19 of Objectives Of Gases And Kinetic Molecular Theory
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<center><b>Gases and Kinetic Molecular Theory <nowiki>(KMT)</nowiki></b></center> <center><b>Updated 04/07</center></b><br> <i><b>Essential Question: Do you believe that? (theory explains observations)</b></i> <i>Each student will be able to:</i><br> 1. Eplain the differemce between compressible and incompressible and which phase of matter has each.<br> 2. Explain what barometric pressure (including a barometer)is and be able to understand and calculate gas pressures from manometers.<br> 3. Explain the kinetic molecular theory with respect to gas phase and what the major gas parameters mean (T, P, V, and n).<br> 4. Using the kinetic molecular theory, explain the relationship (including doing calculations) between pressure and volume (Boyle's law), pressure and temperature (<nowiki>No-Name</nowiki>), volume and temperature (Charles' law), and the number of particles in a gas sample (Avogadro's hypothesis).<b>[http://www.doe.mass.edu/frameworks/scitech/2001/standards/chem10_116.html 6.1](6.1)</b><br> 5. Explain the relationship between temperature and average kinetic energy.<b>[http://www.doe.mass.edu/frameworks/scitech/2001/standards/chem10_116.html 6.2]</b><br> 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 (<nowiki>STP</nowiki>), the molar volume is 22.4L (experimentally determine this value). <b>[http://www.doe.mass.edu/frameworks/scitech/2001/standards/chem10_116.html 6.3](6.2)</b><br> 7. Use the combined gas law to determine changes in pressure, volume, or temperature.<b>[http://www.doe.mass.edu/frameworks/scitech/2001/standards/chem10_116.html 6.6](6.1)</b><br> 8. Explain the difference between diffusion and effusion including understand and calculating problems on Grahman's Law of Diffusion.<br> 9. Describe the conditions under which a real gas deviates from ideal behavior.<b>[http://www.doe.mass.edu/frameworks/scitech/2001/standards/chem10_116.html 6.4]</b><br>
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