1 chapter 12 : day 2 ideal gas lawideal gas law. 2 using kmt to understand gas laws recall that kmt...
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Chapter 12 : Day 2
•IDEAL GAS LAWIDEAL GAS LAW
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Using KMT to Understand Gas Using KMT to Understand Gas LawsLaws
Recall that KMT assumptions are
• Gases consist of molecules in constant, random motion.
• P arises from collisions with container walls.
• No attractive or repulsive forces between molecules. Collisions elastic.
• Volume of molecules is negligible.
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33Properties of Properties of GasesGases
Gas properties can be modeled using math. Model depends on—
• V = volume of the gas (L)
• T = temperature (K)
• n = amount (moles)
• P = pressure (atmospheres)
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IDEAL GAS LAW
Brings together gas Brings together gas properties.properties.
Can be derived from Can be derived from experiment and theory.experiment and theory.
P V = n R TP V = n R T
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55Using PV = nRTUsing PV = nRT
How much N2 is req’d to fill a small room with a volume of 27,000 L to P = 745 mm Hg at 25 oC?
R = 0.082057 L•atm/K•molSolution
1. Get all data into proper UNITS V = 27,000 L
T = 25 oC + 273 = 298 K
P = 745 mm Hg (1 atm/760 mm Hg) = 0.98 atm
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Using PV = nRTUsing PV = nRTR = 0.082057 L•atm/K•mol
Solution
2. Now calc. n = PV / RT
n = (0.98 atm)(2.7 x 10 4 L)
(0.0821 L • atm/K • mol)(298 K)n =
(0.98 atm)(2.7 x 10 4 L)
(0.0821 L • atm/K • mol)(298 K)
n = 1.1 x 10n = 1.1 x 1033 mol (or about 30 kg of gas) mol (or about 30 kg of gas)
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77Deviations from Deviations from Ideal Gas LawIdeal Gas Law
• Real molecules
have volume.
• There are intermolecular forces.
–Otherwise a gas could not become a liquid.
Fig. 12.20Fig. 12.20
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88Deviations from Ideal Gas Deviations from Ideal Gas LawLaw
Account for volume of molecules and Account for volume of molecules and intermolecular forces with intermolecular forces with VAN VAN DER WAAL’S EQUATIONDER WAAL’S EQUATION..
Measured V = V(ideal)Measured P
intermol. forcesvol. correction
J. van der Waals, J. van der Waals, 1837-1923, 1837-1923, Professor of Professor of Physics, Physics, Amsterdam. Amsterdam. Nobel Prize 1910.Nobel Prize 1910.
nRTV - nbV2
n2aP + ----- )(
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99Deviations from Ideal Gas Deviations from Ideal Gas LawLaw
Deviations from Ideal Gas Deviations from Ideal Gas LawLaw
ClCl22 gas has gas has aa = 6.49, = 6.49, bb = 0.0562 = 0.0562
For 8.0 mol ClFor 8.0 mol Cl22 in a 4.0 L tank at 27 in a 4.0 L tank at 27 ooC.C.
P (ideal) = nRT/V = 49.3 atmP (ideal) = nRT/V = 49.3 atm
P (van der Waals) = 29.5 atmP (van der Waals) = 29.5 atm
Measured V = V(ideal)Measured P
intermol. forces
vol. correction
nRTV - nbV2
n2aP + -----
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Gases are most ideal when:
1. higher temperatures = more motion
T2. lower pressures = fewer hits
P3 larger volumes = more space between
V4. less gas in space = fewer number
n
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IDEAL GAS LAWIDEAL GAS LAW
Brings together gas Brings together gas properties.properties.
Can be derived from Can be derived from experiment and theory.experiment and theory.
P V = n R TP V = n R T
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Chapter 12 : Day 3
GAS DENSITYGAS DENSITY
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GAS DENSITYGAS DENSITYGAS DENSITYGAS DENSITY
High High densitydensity
Low densitydensity = mass/ volume
d = g/V
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IDEAL GAS LAWIDEAL GAS LAW
Brings together gas properties.
Can be used to determine molar mass of a gas
or determine the density of a gas
P V = n R T
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Molar Conversions
moles = mass/ molar mass
n = g/
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1717GAS DENSITYGAS DENSITYPV = nRT
or PV = nRT
or
d and d and proportional proportional
n = P_V RT
g = P where g is the mass
V RT where is the molar mass
d = g = P V RT
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USING GAS DENSITYUSING GAS DENSITY
The density of air at 15 oC and 1.00 atm is 1.23
g/L. What is the molar mass of air?
1. Calc. moles of air.1. Calc. moles of air.
V = 1.00 LV = 1.00 L P = 1.00 atmP = 1.00 atm T = 288 KT = 288 K
n = PV/RT = 0.0423 moln = PV/RT = 0.0423 mol
2. 2. Calc. molar mass
mass/mol = 1.23 g/0.0423 mol = 29.1 g/mol