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Chapter 14: Gases

14.1 The Gas Laws
Kinetic theory
Boyle’s Law: P1V1= P2V2 (inversely proportional)
Charles's Law: V1/T1 = V2/T2
Gay-Lussac’s Law P1/T1 = P2/T2

14.2 The Combined Gas Law and Avogadro’s Principle
combined gas law
    (P1V1) / (n1T1) = (P2V2) / (n2T2)
molar volume means – 1mole of any gas at STP = 22.4 L

14.3 The Ideal Gas Law
PV = nRT the constant R depends on units of measure used for variables

Real vs ideal gases - For an ideal gas: (a) gas particles take up no space; (b) there are no intermolecular forces; follows the gas laws under all temp. and pressures conditions. There is no ideal gas, you can only get close. You get closest to ideal at VERY LOW pressures and HIGH temperatures.

Section 14.1 The Gas Laws
Section 14.2 The Combined Gas Law and Avogadro's Principle
Section 14.3 The Ideal Gas Law
Section 14.4 Gas Stiochiometry
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