CH7 - Chapters 2 - 6: examined components Chapters 7:...

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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 L•atm 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
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766 mm Hg H = + 18 mm P gas = P atm + H = 766 18 Section 7.1 Pressure of 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 P gas = P atm + H = 766 25 Section 7.1 Pressure ofgas is greater/less than 766 mm Hg? It’s not Pushing as hard = 741 mm Hg -
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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 7.1 778 mm 778 mm (1 atm/760 mm)= 1.02 atm
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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
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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
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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
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PV = nRT Keep constant VT TV P = nR V T Ideal Gas Law PV = nRT Section 7.1 P i T i Directly proportional 4 atm 0.02 atm/K 20 K P f 8 atm 0.02 atm/K = T f = 40 K Gay-Lussac’s Law
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_______ liters A 22L balloon with 28 grams of air at 298 K is in a room at 1 atmosphere. The pressure in the room is increased to 2 atmospheres. What will the new volume of the balloon be? (Just use ratios to work it out, not R) Pressure and volume are __________ proportional. Section 7.1
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What is the pressure in mm Hg inside a 7.20-L container filled with 13 grams of CO 2 at 35 o Celcius? PV = nRT P = nRT V 13 g CO 2 * mole CO 2 44.01 g CO 2 0.0821 atm* L K*mol (35 + 273.15) K 7.2 L 13 g CO 2 * mole CO 2 44.01 g CO 2 0.0821 atm* L K*mol P = * (35 + 273.15) K * 7.2 L P = 1.038 atm * 760 mm Hg atm = 789 mm Hg Section 7.1
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PV = nRT V V Ideal Gas Law PV = nRT P = n V RT Gas Concentration mol / L = molarity = M Expressed as [gas] V a RT = V b RT + n a n b P mixture = P a + P b Dalton’s Law or Law of Partial Pressures Section 7.1
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2.126 g He and 19.038 g F 2 are placed in a 14.2-L container at 75 o C. What are the molar concentrations and partial pressures of the gases? Section 7.1
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CH7 - Chapters 2 - 6: examined components Chapters 7:...

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