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4-7-2014 Unit 6 - Gas Laws (Silberberg Chpt 5) - student.pptx

4-7-2014 Unit 6 - Gas Laws (Silberberg Chpt 5) - student.pptx

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UNIT 6: Gas Behavior SPRING 2014 CHEM 104 General Chemistry II Drs. Baillie, Fajardo, & Wesolowski Fighting for change never goes out of style - Barack Obama
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Molar Volume What is the volume of 1 mole at room temperature? (RT = 25 C) 2
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Higher Density air Low density helium Gas Densities 3
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Densities of Gases Divide both sides of the ideal-gas equation by V and RT : n V P RT = is the mass of the gas in g M  is the molar mass of the gas Mass / volume = density So, P M RT m V = d = 4
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Molar Mass ( M ) of a Gaseous Substance We can manipulate the density equation to enable us to find the molecular mass of a gas: becomes P M RT d = dRT P M = d  is the density of the gas in g/L 5
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A 2.10-L vessel contains 4.65 g of a gas at 1.00 atm and 27.0  ˚ C.  What is the molar mass of the gas? 6
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Gas Stoichiometry What is the volume of CO 2  produced at 37  0 C and 1.00 atm when 5.60  g of glucose are used up in the reaction: C 6 H 12 O 6  ( s ) + 6O 2  ( g )           6CO 2  ( g ) + 6H 2 O ( l ) 7
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Dalton’s Law of Partial Pressures The total pressure of a mixture of gases equals the sum of the pressures that each would exert if it were present alone. In other words, P total = P 1 + P 2 + P 3 + … 8
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V  and  T  are  constant P 1 P 2 P total   =  P 1  +  P 2 Dalton’s Law of Partial Pressures 9
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