Lecture24

Lecture24 - Chapter 19 The Kinetic Theory of Gases PHYS 2101 P.M.Shikhaliev LSU Fall 2010 1 19.2 Avogadros Number Avogadros Law All gases having

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Chapter 19 The Kinetic Theory of Gases 1 PHYS 2101, P.M.Shikhaliev LSU, Fall 2010
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19.2. Avogadro’s Number Avogadro’s number and “mole” quantity: Let us we have two gas samples: 1 st - N molecules of H 2 , and 2 nd - N molecules of O 2 The mass of the H 2 sample is M H = (N)x(2amu) = (N)x(2)x(1.66 x10 -24 g) The mass of the O 2 sample is N O = (N)x(32amu) = (N)x(32)x(1.66 x10 -24 g) If we select N = 6.02 x 10 23 , then (N)x(1.66 x10 -24 g) = 1 g, and M H = 2 g, and M O = 32 g The number N A = N = 6.02 x 10 23 is called Avogadro’s number By convention, Avogadro’s number is defined as number of atoms in 12 g Carbon. The amount of matter including N A atoms is called 1 mole of this matter All gases including N A atoms or molecules have same volume of V A = 22.4 L Molar mass M = N A x m , where m is the mass of the atom or molecule 2 PHYS 2101, P.M.Shikhaliev LSU, Fall 2010 Avogadro’s Law: All gases having same volume, same pressure, and same temperature contain same numbers of molecules.
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19.3. Ideal Gases Here p is the absolute pressure, n is the number of moles of gas present, and T is its temperature in Kelvin's. R is the gas constant that has the same value for all gases. 3
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This note was uploaded on 01/26/2011 for the course PHYS 2101 taught by Professor Grouptest during the Spring '07 term at LSU.

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Lecture24 - Chapter 19 The Kinetic Theory of Gases PHYS 2101 P.M.Shikhaliev LSU Fall 2010 1 19.2 Avogadros Number Avogadros Law All gases having

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