Chapter 10b & 11a

Chapter 10b & 11a - Chapters 10B and 11A The Ideal...

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Chapters 10B and 11A 1 The Ideal Gas Law The ideal gas law relates the absolute pressure, volume, and absolute (Kelvin) temperature of a fixed amount of gas: PV = nRT n = number of moles of gas R = gas constant, 8.31 J/(mole K)
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Chapters 10B and 11A 2 Moles In this form of the ideal gas law the amount of gas is expressed in moles : 1 mole = 6.022 × 10 23 molecules (Avogadro’s number) One mole of any material has a mass, in grams, equal to its molecular mass, in atomic mass units (u).
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Chapters 10B and 11A 3 Molecular Masses Molecular mass = sum of atomic masses H 2 O: 2 hydrogen atoms @ 1 u: 2 u 1 oxygen atom @ 16 u: 16 u molecular mass for H 2 O: 18 u Mass of one mole of H 2 O: 18 grams
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Chapters 10B and 11A 4 The Ideal Gas Law The ideal gas law can also be expressed in terms of the number of molecules of gas: PV = Nk B T N = number of gas molecules = nN A k B = Boltzmann constant = R / N A k B = 1.38 × 10 -23 J/K
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Chapters 10B and 11A 5 Kinetic Theory of Gases Gas molecules are in constant motion, colliding with each other and with the walls of the container. The pressure and temperature of a gas relate to the
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Chapter 10b & 11a - Chapters 10B and 11A The Ideal...

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