Editing revision 18 of Objectives Of Gases And Kinetic Molecular Theory - Revised 2015

ChemistryWiki | RecentChanges | Preferences

Editing old revision 18. Saving this page will replace the latest revision with this text.

<center>Gases and Kinetic Molecular Theory <nowiki>(KMT) - Revised 2015</nowiki></center>

Essential Questions (EQ4): Do and/or how do basic particles interact - Stay same?

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 and barometer. 2015-2016 Learner, NOT RESPONSIBLE FOR THIS CONCEPT.

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 (<nowiki>No-Name</nowiki>), volume and temperature (Charles' law), and the number of particles in a gas sample (Avogadro's hypothesis).[http://www.doe.mass.edu/frameworks/scitech/2001/standards/chem10_116.html 6.1](6.1) 
 
5. Explain the relationship between temperature and average kinetic energy. [http://www.doe.mass.edu/frameworks/scitech/2001/standards/chem10_116.html 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 (that is what <nowiki>STP</nowiki> stands for Standard Temperature and Pressure)), the molar volume is 22.4L (experimentally determine this value). [http://www.doe.mass.edu/frameworks/scitech/2001/standards/chem10_116.html 6.3](6.2)

7. Use the combined gas law to determine changes in pressure, volume, or temperature.[http://www.doe.mass.edu/frameworks/scitech/2001/standards/chem10_116.html 6.6](6.1)

8. Define Graham's Law of Diffusion/effusion and understand the difference between diffusion and effusion. 2015-2016 Learner, NOT RESPONSIBLE FOR THIS CONCEPT.

9. Calculate and understand Dalton's Law of Partial Pressure which defines how mixture of gas behave.2015-2016 Learner, NOT RESPONSIBLE FOR THIS CONCEPT. 
 
10. Be able to calculate gas generation problems where you are performing a chemical reaction and producing/consuming a gas in the reaction. Also, understand and be able to calculate the affect of collecting the gas over water (a liquid) or not (collecting the gas in a balloon without the presence of the liquid). 2015-2016 Learner, NOT RESPONSIBLE FOR THIS CONCEPT 
 
11. To perform, understand and calculate aspect of a Molar Volume of a Gas Lab. 2015-2016 Learner, NOT RESPONSIBLE FOR THIS CONCEPT

View other revisions
ChemistryWiki | RecentChanges | Preferences