chapter 9 gases: their properties and behavior chemistry
TRANSCRIPT
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Chapter 9Gases: Their Properties and Behavior
C H E M I S T R Y
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Methanol (CH3OH) can be synthesized by the following reaction:
CO(g) + 2 H2(g) CH3OH(g)
What volume (in Liters) of hydrogen gas, measured at a temperature of 355K and a pressure of 738 mmHg, is required to synthesize 35.7 g of methanol?
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ExamplesConsider the reaction represented by the equation
P4(s) + 6 H2(g) 4H3(g)
What is the amount of P4 is required to react with 5.39 L of hydrogen gas at 27.0oC and 1.25 atm?
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Ptotal = P1 + P2 + … + PN
Mole Fraction (X) =
Dalton’s Law of Partial Pressures: The total pressure exerted by a mixture of gases in a container at constant V and T is equal to the sum of the pressures of each individual gas in the container.
Xi = Ptotal
PiXi =
ntotal
nior
Total moles in mixture
Moles of component
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ExamplesDetermine the mole fractions and partial pressures of
CO2, CH4, and He in a sample of gas that contains 0.250 mole of CO2, 1.29 moles of CH4, and 3.51 moles of He, and in which the total pressure is 5.78 atm
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ExampleA 1.00 L vessels contain 0.215 mole of N2 gas and 0.0118
mole of H2 gas at 25.5oC. Determine the partial pressure of each component and the total pressure
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1. A gas consists of tiny particles, either atoms or molecules, moving about at random.
2. The volume of the particles themselves is negligible compared with the total volume of the gas; most of the volume of a gas is empty space.
3. The gas particles act independently of one another; there are no attractive or repulsive forces between particles.
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The Kinetic-Molecular Theory of Gases
3. Collisions of the gas particles, either with other particles or with the walls of a container, are elastic (constant temperature).
4. The average kinetic energy of the gas particles is proportional to the Kelvin temperature of the sample.
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averagespeed
molarmass
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Diffusion: The mixing of different gases by molecular motion with frequent molecular collisions.
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Graham’s Law:
Effusion: The escape of a gas through a pinhole into a vacuum without molecular collisions.
Rate1
m
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Graham’s Law: Diffusion and Effusion of GasesIn comparing two gases at the same temperature and
pressure
√m2
√m1
Rate 1
Rate 2
=
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ExampleDetermine how much faster Helium atoms moves, on
average, than a carbon dioxide molecule at the same temperature
Determine the molar mass and identity of a gas that moves 4.67 times as fast as CO2
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The volume of a real gas is larger than predicted by the ideal gas law.
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Attractive forces between particles become more important at higher pressures.
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PV2
n2
= nRT+ V - n
van der Waals equation
ba
Correction for intermolecular attractions.
Correction for molecular volume.
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ExampleA sample of 3.50 moles of NH3 gas occupies 5.20 L at
47oC. Calculate the pressure of the gas (in atm) usingA) the ideal gas equationB) the van der Waals equation
a = 4.17 atm •L/mol2 b = 0.0371 L/mol