CH 101 notes 10-3

CH 101 notes 10-3 - Chapters 2 - 6: examined components...

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Chapters 2 - 6: examined components Chapters 7: examine bulk properties Gases Gas Laws variable: amount (n) unit: mole (mol) Ideal Gas Law Constant: R R = 0.0821 atm•L K•mol Variables of state and their units: variable: pressure (P) unit: atmosphere (atm) variable: volume (V) unit: liter (L) conversion factors: variable: temperature (T) unit: Kelvin (K) conversion factor: K = o C+273 1 atm 760 mm Hg 1 atm 760 torr Section 7.1 766 mm Hg H = + 18 mm P gas = P atm + H = 766 18 Section 7.1 Trapped gas is greater/less than 766 mm Hg? It’s pushing harder = 784 mm Hg + 766 mm Hg H = 25 mm P gas = P atm + H = 766 25 Section 7.1 Trapped gas is greater/less than 766 mm Hg? It’s not Pushing as hard = 741 mm Hg - 766 mm Hg H = 12 mm What is the pressure of the gas in the bulb? How do I get that pressure from mm Hg to atmospheres? Section 7.1 Ideal Gas Law PV = nRT PV = nRT Keep constant P i V i = P f (8 atm) (4 atm)(4 L) = 16 atm•L V f (2 L) 16 atm•L Inversely proportional Boyle’s Law Section 7.1 Demo: the belljar balloon And the Cartesian Diver
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Directly proportional Charles’ Law V i T i 4 L 1 L/K 4 K V f 8 L 1 L/K = 8 K = T f Ideal Gas Law PT PT V = nR P T PV = nRT Keep constant PV = nRT Section 7.1 Demo: balloon and N 2 Absolute Temperature The temperature at which any number of moles of gas has a volume of ZERO is O Kelvin (Otherwise known as –273.15 C) Section 7.1 Directly proportional V x n x 11.2 L 22.4 L/mol 0.5 mol V z 22.4 L 22.4 L/mol = 1 mol = n z Avagadro’s Law Ideal Gas Law Pn Pn V = RT P n PV = nRT Keep constant PV = nRT Section 7.1 Demo: blowing a balloon up PV = nRT Keep constant VT TV P = nR V T
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This note was uploaded on 06/08/2008 for the course CH 101 taught by Professor Bigham during the Fall '08 term at N.C. State.

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CH 101 notes 10-3 - Chapters 2 - 6: examined components...

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