Download M12 L2 Dalton`s Law of Partial Pressure

M12 L2 Dalton's Law of Partial Pressure Sunday, March 01, 2009 9:24 AM VOICETHREAD http://voicethread.com/share/66693/ Cmap http://cmapspublic2.ihmc.us/rid=1210805180212_1334086090_36923/Apologia,%20ed%201,%20Module%2012%20Concept%20Map.cmap Periodic Table Yes Chart of water
See course page, just under the exam link, to get the chart needed. Vapor Pressure Slides Notes Overview of the module: Everything comes back to moles. Point out the pv=nrt If everything else is the same when you compare two gases and the only difference is it being a different molecule, it won't matter when
it comes to pressure. If it is H2 it will have the same pressure as O2 for the same volume, temperature, and number of moles. Notice that you can solve for the mole fraction starting out with the moles of each component or the atm of each component. Why would
the moles and the atm end up being so 'interchangeable'? How is this like finding what percentage of the total gas mixture is from a specific component? There are a few more laws that apply to ideal gases. 5 + 5 + 10 = 20 Two containers. If you move all the air of one container to the other, just add them together to get the final. Liquid to a gas phase - evaporation Kinetic theory - molecules are in motion. With enough speed, the molecules break through the surface. This gas will often sit right above the surface making a vapor. This has
pressure = vapor pressure. Vapor pressure will be greater as you have greater temperature. Use the chart on pg 413. The problem has an error. It should be 26 not 25 degrees. Water's vapor pressure at 26 degrees Celsius is 25.2 Torr. Convert: 25.2 Torr to atm units because the chart is in one unit and the problem has pressure in another unit. x=0.0332 atm PT = Phydrogen + Pwater vapor 1.115 atm = Phydrogen + 0.0332 1.082 atm Hydrogen Use chart on pg 413. Water's vapor pressure at 22 degrees is 19.8 Torr. 961 = 19.8 + Pcarbon dioxide = 941 torr M12, L2 Quiz: STUDENTS WILL NEED THE CHART FOR SOME OF THESE. VT: None have walk throughs http://voicethread.com/share/1813172/ Review Question 12.8: Two steel containers of equal volume contain two different gases at the
same temperature. The first container holds 1.3 moles of N2 gas and the
second contains 1.3 moles of SO3 gas. Compare the pressures of the two
containers. http://voicethread.com/#q.b1813172.i9526967 They both have the same pressure because Dalton's Law tells us
that the pressure of an ideal gas is independent of its identity. Mole fraction is really just finding what percentage of the total moles of gas you have of a particular gas. Review Question 12.9: A liquid's temperature is lowered from 50 degrees Celsius to 10 degrees
Celsius. What happened to the liquid's vapor pressure during this time? http://voicethread.com/#q.b1813172.i9526965 Temperature and vapor pressure are directly proportional, so
when the temperature is lowered the vapor pressure will lower
too. Review Question 12.10: The mole fraction of nitrogen gas in compressed air is 0.80. If you have
1,000 molecules of compressed air, how many will be nitrogen molecules? http://voicethread.com/#q.b1813172.i9526966 In words, you are asking what is 80% of 1000. Mathematically,
thing of the of as always indicating multiplication. So 0.80 x 1000 = 800 Practice Problem 12.4: http://voicethread.com/#q.b1813172.i9526968 In an experiment similar to experiment 6.1, a chemist collects carbon
dioxide over water at 27 degrees Celsius. If the gas in the collection vessel
has a pressure of 787 torr, what pressure of carbon dioxide is in the vessel?
(You will need the table provided just below the exam link to answer this
question) PT = Pcarbon dioxide + Pwater vapor 787 torr = Pcarbon dioxide + 26.7 7.6 x 10^2 torr Practice Problem 12.5: As part of an environmental experiment, the mixture of gasses released
from a smokestack is collected in a balloon. If the mixture is analyzed and
found to contain 15.0 g if SO2, 12.1 g of NO gas, and 2.5 g of SO3 gas,
what is the mole fraction of each? http://voicethread.com/#q.b1813172.i9526969 SO2 is 0.350 NO is 0.603 SO3 is 0.046 Practice Problem 12.7: http://voicethread.com/#q.b1813172.i9526972 A steel container is filled with 5.00 atms of nitrogen, 2.00 atms of oxygen,
and 0.50 atms of argon. What is the total pressure in the vessel and what is
the mole fraction of each component? The total pressure is 7.50 atms The mole fractions are … Nitrogen: 0.667 Oxygen: 0.267 Argon: 0.067 Review Question 12.10: ADDED IN SO THE STUDENT HAVE WHAT THEY NEED FOR A QUIZ QUESTION: The mole fraction of oxygen gas in compressed air is 0.60. If you have 1,000 molecules of compressed air, how many will be nitrogen molecules? In words, you are asking what is 60% of 1000. Mathematically, thing of the of as always indicating multiplication. So 0.60 x 1000 = 600.0