Worksheet 12 Key - Worksheet 12 CH 301, Dr. Sparks, Fall...

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Worksheet 12 CH 301, Dr. Sparks, Fall 2010 Gas Laws, Part 2 Note that the last question gives you five questions from your textbook to try. There are of course numerous others in your text if you feel the need for more practice problems! Material for questions 9 and 10 will be covered in class Thursday. 1. What do we assume about ideal gases? What is the ideal gas law? Give the units for each variable. Ideal gases can be thought of as infinitely small, hard spheres that do not interact with each other. They are essentially "blind" to other gas molecules and will bounce off of each other just as they would bounce of a wall. They exert no attractive or repulsive forces on each other and are very spread out compared to their size. The ideal gas law is PV = nRT. Common units for pressure, volume, n, and temperature are atmospheres, liters, moles, and Kelvin, respectively. R is a constant, which has a value of 0.08206 (L*atm)/(K*mol). 2. Assuming a constant molar quantity of gas, how could you produce the following effects?  a. decrease pressure  You could decrease the temperature or increase the volume.  b. decrease volume  You could decrease the temperature or increase the external pressure.  c. increase pressure  You could increase the temperature or decrease the volume.  d. increase volume  You could increase the temperature or decrease the external pressure. 3. What is the temperature of .75 moles of argon in an 18 L container with a pressure of 790 Torr? 4. n = .75 mole, V = 18 L, and P = 790 Torr (1 atm/760 Torr) = 1.04 atm 
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6. Rank the following in order of increasing density:  1 mole of CH 4  at 0.1 atm and 273 K  2 moles O 2  at 1 atm and 300 K  3 mol H 2  at 3 atm and 290 K  CH 4  < H 2  < O 2   CH 4 Density,  , is defined in this problem as grams per liter. So we need to use the Ideal Gas law to find the ρ   ratio of moles to volume, then I can use the molecular weight for each compound to convert from  moles/liter to grams/liter O 2   The same thing we did for CH 4  can be done using the formula shown below where MW is molecular  weight.  = PMW / RT 
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This note was uploaded on 09/19/2011 for the course CH 301 taught by Professor Fakhreddine/lyon during the Fall '07 term at University of Texas at Austin.

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Worksheet 12 Key - Worksheet 12 CH 301, Dr. Sparks, Fall...

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