060708_-_ChE102_F10_Notes

060708_-_ChE102_F10_Notes - ChE102 Divisions 7, 9 & 10 Fall...

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Fall 2010 06 – Gases Petrucci et al., 10 th Edition: 6.1-6.3 Definition of Pressure When talking about gases, four properties are often used: amount (moles), temperature, Pressure is the force per unit area = force/area Force resulting from the collision of the gas molecules against the walls of the container Area of the walls of the container holding the gas Understanding Pressure Gas pressure is usually measured indirectly, by comparing it with liquid pressure Liquid pressure is directly proportional to the liquid density and the height of the liquid column P Hg = P air When the pressures are equal: Understanding Pressure (2) Open-ended Manometer 06-08 - Gases 1 A g m A F P air air air . = = g h A g A h A g V A g m A F P Hg Hg Hg Hg Hg Hg Hg . . . . . . . . ρ = = = = =
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Fall 2010 Petrucci Figure 6-5 06-08 - Gases 2
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Fall 2010 The Simple Gas Laws Boyle’s Law (1662): Petrucci Figure 6-6 “For a fixed amount of gas at a constant temperature, the gas volume is inversely proportional to the gas pressure” P is inversely proportional to V PV = constant for a given temperature and given amount of substance The Simple Gas Laws (2) Charles’ Law (1787): Petrucci Figure 6-8 “The volume of a fixed amount of gas at constant pressure is directly proportional to the Kelvin (absolute) temperature” V is directly proportional to T 06-08 - Gases 3 + = c C T V V o ) ( 1 0 V 0 : volume of the gas at 0ºC T : temperature in ºC c : a constant (for all gases at small pressures, c = 273.15)
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Fall 2010 Aside – Definition of Temperature from Charles’s Law Temperature is measured using the ratio of the volume of a gas at the measured temperature to the volume of the same gas at 0ºC (freezing point of water)
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This note was uploaded on 11/06/2010 for the course CHEM CHE102 taught by Professor Robinson during the Fall '10 term at Waterloo.

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060708_-_ChE102_F10_Notes - ChE102 Divisions 7, 9 & 10 Fall...

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