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