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Chapter Outline
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10.1
10.2
10.3
10.4
10.5
10.6
10.7
10.8
10.9
10.10
10.11
10.12
The Properties of Gases
Effusion and the Kinetic Molecular Theory of Gases
Atmospheric Pressure
Relating P,T, and V: The Gas Laws
The Combined Gas Law
Ideal Gases and the Ideal Gas Law
Densities of Gases
Gases in Chemical Reactions
Mixtures of Gases
Solubilities of Gases and Henry’s Law
Gas Diffusion: Molecules Moving Rapidly
Real Gases
Ideal Gas Equation
Boyle’s law: V a 1 (at constant n and T)
P
Charles’ law: V a T (at constant n and P)
Avogadro’s law: V a n (at constant P and T)
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Standard Temperature and Pressure (STP).
Experiments show that at STP,
1 mole of an ideal gas
occupies 22.414 L.
PV = nRT
Sample Exercise 10.7:
Applying the Ideal Gas Law
Bottles of compressed O2 carried by climbers ascending Mt. Everest are
designed to hold one kilogram of the gas. What volume of O2 can one
bottle deliver to a climber at an altitude where the temperature is -38 oC
and the atmospheric pressure is 0.35 atm? Assume that each bottle
contains 1.00 kg of O2.
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Chapter Outline
10.1 The Properties of Gases
10.2 Effusion and the Kinetic Molecular Theory of Gases
10.3 Atmospheric Pressure
10.4 The Gas Laws
10.5 The Combined Gas Law
10.6 Ideal Gases and the Ideal Gas Law
10.7 Densities of Gases
10.8 Gases in Chemical Reactions
10.9 Mixtures of Gases
10.10 Solubility of Gases and Henry’s Law
10.11 Gas Diffusion: Molecules Moving Rapidly
10.12 Real Gases
Densities and Molecular Weights of
Gases Using PV = nRT
PV = nRT
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Sample Exercise 10.8:
Calculating the Density of a Gas
According to the U.S National Weather Service, the air temperature in Phoenix, AZ
reached 78 oF on January 1, 2012, when the atmospheric pressure was 1024 millibars.
What is the density of the air? Assume the average molar mass of air is 28.8 g/mol,
which is the weighted average of the molar masses of the various gases in dry air.
Example: Calculating the Molecular
Weight from PV = nRT
1.018 g of Freon-113 gas is trapped in a 145 mL container at
760 mmHg and 50.0°C. What is the molar mass of Freon-113?
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Chapter Outline
10.1 The Properties of Gases
10.2 Effusion and the Kinetic Molecular Theory of Gases
10.3 Atmospheric Pressure
10.4 The Gas Laws
10.5 The Combined Gas Law
10.6 Ideal Gases and the Ideal Gas Law
10.7 Densities of Gases
10.8 Gases in Chemical Reactions
10.9 Mixtures of Gases
10.10 Solubility of Gases and Henry’s Law
10.11 Gas Diffusion: Molecules Moving Rapidly
10.12 Real Gases
Gas Laws & Stoichiometry
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Example: Combining Stoichiometry and
the Ideal Gas Law
Chlorine gas can be prepared in the laboratory by the reaction of
manganese dioxide with hydrochloric acid:
MnO2(s) + 4 HCl(aq)  MnCl2(aq) + 2 H2O(l) + Cl2(g)
How many grams of MnO2 should be added to excess HCl to obtain 275
mL of chlorine gas at 5.0°C and 650 mmHg?
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