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CH. 12 Sections 1 and 2 from Week two of class

by: Melissa

CH. 12 Sections 1 and 2 from Week two of class PHYS 202

Marketplace > University of Oregon > Physics 2 > PHYS 202 > CH 12 Sections 1 and 2 from Week two of class
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About this Document

These are book notes
General Physics >4
Jenkins T
Class Notes
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This 2 page Class Notes was uploaded by Melissa on Sunday January 10, 2016. The Class Notes belongs to PHYS 202 at University of Oregon taught by Jenkins T in Fall 2015. Since its upload, it has received 19 views. For similar materials see General Physics >4 in Physics 2 at University of Oregon.

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Date Created: 01/10/16
Molecules bumping into each other creates pressure Molecules at a faster speed increase the temperature An increase in temperature increases the pressure which causes expansion because they are hitting the walls more frequently and with more force • 12.1 The atomic model of matter ⿞Phases ‣ Gas: system in which each particle moves freely through space until it collides with another particle or wall of its container ‣ Liquid: weak bonds permit motion while keeping the particles close together ‣ Solid: definite shape and can be compressed or deformed only slightly ⿞Atomic Mass and Atomic Mass Number ‣ Atomic mass number: sum of the protons and neutrons in the nucleus ‣ Molecular Mass: sum of the atomic masses of the atoms that form the molecule ⿞Definition of the Mole ‣ • Called Avogadro's number ‣ Molar mass: ‣ • Ex. 100g of oxygen and has molar mass of 32g/mol. How many moles are there? ⿞ ⿞Volume ‣ Characteristic of a macroscopic system • 12.2 The atomic model of an ideal gas ⿞Gases are compressible because their particles are so spread out whereas in liquids and solids, the particles are either fairly close to each other or are in direct contact ⿞Temperature of an ideal gas is directly proportional to the average kinetic energy per atom ‣ ‣ ‣ ‣ ‣ Thermal energy is proportional to change in temperature ⿞Molecular Speeds and Temperature ‣ RMS speed: • The speed of an atom with the average kinetic energy • Also related to the speed ⿞ • RMS speed is proportional to the square root of the temperature • Remember that changing x by a factor of c changes y by a factor of. ‣ Pressure • Collisions exert a force on wall they hit and net force causes gas to have a pressure • Area is proportional to the force exerted ⿞twice as big a circle means twice as many particles and thus double the force ⿞Pressure in a gas ‣ ⿞Be aware that pressure is not a force but a force creates the pressure ⿞Measured in pascals ‣ ‣ • A net pressure force is exerted only where there is a pressure difference between the two sides of a surface ⿞Ex. Force that holds the lid on a vacuum sealed jar where the pressure inside is less than the pressure outside ‣ To remove the lid, you have to exert a force greater than the force due to the pressure difference • Decreasing number of moles decreases the pressure ⿞From Collisions to Pressure and the Ideal Gas Law ‣


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