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Chem 222; Chapter 5 Notes

by: Haley Notetaker

Chem 222; Chapter 5 Notes Chem 222

Marketplace > Portland State University > Chemistry > Chem 222 > Chem 222 Chapter 5 Notes
Haley Notetaker
GPA 3.2

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About this Document

Basics of what was covered with Gasses
General Chemistry
Dr. Eric Sheagley
Class Notes
25 ?




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This 3 page Class Notes was uploaded by Haley Notetaker on Wednesday January 20, 2016. The Class Notes belongs to Chem 222 at Portland State University taught by Dr. Eric Sheagley in Winter 2016. Since its upload, it has received 16 views. For similar materials see General Chemistry in Chemistry at Portland State University.


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Date Created: 01/20/16
Chapter 5: Gasses Tuesday, January 19, 2016 11:24 PM NOTE: When dealing with gasses, Temperature needs to be in Kelvin!  Pressure is created through the force of collision of particles with a surface.  Pressure= Force/Area  As temp increases so does the pressure PV=nRT  o R= ideal gas constant  0.08206 L*atm/mol*K  8.3145 J/mol*K  62.364 L*torr/mol*K  Combined Gas Law o P1V1/n1T1= P 2 2n 2 2  Standard pressure is equal to exactly one atmosphere Standard Temperature is 273 K or 0 ̊C  Kinetic Molecular Theory  Gas is always moving  Energy is imparted through collisions of other particles  There is a lot of empty space between particles o Average Kinetic Energy of a particle proportional to its temp in Kelvin  As temp rises the energy increases  KE= 1/2mv 2  Mass units= kilograms (kg)  Not all particles move at the same speed. Molecular Velocity  The speeds at which the particles travel will follow a Boltzmann distribution  o Found with using the average velocity of the particles traveling o KE= 3/2RT  Average Kinetic Energy of a gas depends on the mass and average velocity  KE=1/2mv = 1/2m<v>= 3/2RT  With different masses, in order to have the same Kinetic Energy they need to have different velocities  Speed vs. Mass o At constant temp, in order to have the same average kinetic energy, 2 heavier molecules must have a slower average speed. KE = ½mv  Diffusion= spread of particles from an area of high concentration to an area of low concentration  Effusion= collection of molecules that escape through a small hole to a vacuum Graham's Law of Effusion  for two different gases at the same temperature, the ratio of their rates of effusion is given by the following equation:


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