Ch 8.1 gas laws - Chapter 8 Gases Georgia Tech Chem 1310J...

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Chapter 8 1 Chapter 8 Gases Georgia Tech Chem 1310J Fall 2009
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Chapter 8 2 Pressure The Pressure of a gas is the force exerted by the gas molecules as they strike the surfaces around them. – Depends on several factors. • The concentration of the molecules (moles/volume) • The kinetic energy of the molecules.
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Chapter 8 3 Atmospheric Pressure and Common Units barometer “standard pressure” 760 mm Hg = 760 torr = 1 atm = 101.325 kPa
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Chapter 8 4 Physical Properties of Gases A sample of gas has four basic physical properties: These properties are interrelated in very specific ways: – Pressure / volume – Volume / temperature – Volume /moles – etc An Ideal Gas:
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Chapter 8 5 Boyle’s Law: Relationship between P and V
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Chapter 8 6 Charle’s Law: V and T Jacques Charles ascended over Paris in a hydrogen-filled balloon December 1, 1783.
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Chapter 8 7 Absolute Zero and Kelvin Temperature Scale
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Avogadro’s Law Chapter 8 8 Avogadro’s law (1811) V = a n n= number of moles of gas a = proportionality constant For a gas at constant temperature and pressure the volume is directly proportional to the number of moles of gas.
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Chapter 8 9 V 1 / V 2 = T 1 / T 2 (at a fixed pressure) P 1 V 1 = P 2 V 2 (at a fixed temperature) Boyle’s Law Charles’ Law V = k P -1 V = b T V = an (at a fixed pressure and temperature) Avogadro V α n TP -1 1662 1787 1811 n = number of moles an empirical law
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This note was uploaded on 03/08/2010 for the course CHEMISTRY 1310 taught by Professor Williams during the Spring '10 term at Georgia Tech.

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Ch 8.1 gas laws - Chapter 8 Gases Georgia Tech Chem 1310J...

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