10-3 - Chapters 2 6 examined components Chapters 7 examine...

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Chapters 2 - 6:  examined components Chapters 7:  examine bulk properties Gases

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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 Section 7.1 Trapped gas is greater/less than 766 mm Hg? It’s pushing harder = 784 mm Hg +

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766 mm Hg H = 25 mm 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

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Ideal Gas Law PV = nRT PV = nRT Keep constant P i V i = P (8 atm) (4 atm)(4 L) = 16 atm•L V (2 L) 16 atm•L Inversely proportional Boyle’s Law Section 7.1 Demo: the belljar balloon And the Cartesian Diver
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

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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

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Keep constant VT TV P = nR V T Ideal Gas Law PV = nRT Section 7.1 P i T i
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10-3 - Chapters 2 6 examined components Chapters 7 examine...

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