Chapter 6 M

Chapter 6 M - CHAPTER 6 GASES CHM 25/Spring 2009 Prof. R.S....

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CHAPTER 6 – GASES CHM 25/Spring 2009 Prof. R.S. Miller
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Composition of Earth’s Atmosphere Compound %(Volume) Mole Fraction a Nitrogen 78.08 0.7808 Oxygen 20.95 0.2095 Argon 0.934 0.00934 Carbon dioxide 0.033 0.00033 Methane 2 x 10 -4 2 x 10 -6 ydrogen x10 - - Hydrogen 5 x 10 5 5 x 10 7 a. mole fraction = mol component/total mol in mixture.
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Properties of Gases ± Gases are highly compressible and occupy the full gy p p y volume of their containers. ± When a gas is subjected to pressure, its volume decreases. ± Gases always form homogeneous mixtures with other gases. ± Gases only occupy about 0.1 % of the volume of eir containers their containers.
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Measurement of Pressure
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evation and Atmospheric Pressure Elevation and Atmospheric Pressure
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Units for Expressing Pressure Unit Value Atmosphere 1 atm Pascal (Pa) 1 atm = 1.01325 x 10 5 Pa Kilopascal (kPa) 1 atm = 101.325 kPa mmHg 1 atm = 760 mmHg Torr 1 atm = 760 torr ar atm = 1 01325 bar Bar 1 atm 1.01325 bar mbar 1 atm = 1013.25 mbar si atm=147ps i psi 1 atm = 14.7 psi
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anometer Manometer
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Boyle’s Law (1627-1691) oyle’s Law: the volume of a fixed quantity of gas is inversely Boyle s Law: the volume of a fixed quantity of gas is inversely proportional to its pressure. Boyle (1627-1691) used a manometer to carry out the experiment.
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Charles’ Law (1746-1823) Charles’s Law: the volume of a fixed quantity of gas at constant pressure increases as the temperature increases
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Avogadro’s Law (1776-1856) The Quantity-Volume Relationship vogadro’s Law: the volume of gas at a given temperature and Avogadro s Law: the volume of gas at a given temperature and pressure is directly proportional to the number of moles of gas.
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Chapter 6 M - CHAPTER 6 GASES CHM 25/Spring 2009 Prof. R.S....

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