1 the gaseous state. 2 gas laws in the first part of this chapter we will examine the quantitative...
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The Gaseous StateThe Gaseous State
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Gas LawsGas Laws
In the first part of this chapter we will In the first part of this chapter we will examine the quantitative relationships, or examine the quantitative relationships, or empirical lawsempirical laws, governing gases., governing gases.
• First, however, we need to understand the concept of pressure.
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PressurePressure
Force exerted per unit area of surface by Force exerted per unit area of surface by molecules in motion.molecules in motion.
– 1 atmosphere = 14.7 psi– 1 atmosphere = 760 mm Hg (See Fig. 5.2)– 1 atmosphere = 101,325 Pascals– 1 Pascal = 1 kg/m.s2
P = Force/unit area
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The Empirical Gas LawsThe Empirical Gas Laws
Boyle’s Law:Boyle’s Law: The volume of a sample of The volume of a sample of gas at a given temperature varies inversely gas at a given temperature varies inversely with the applied pressure. with the applied pressure. (See Figure 5.5 (See Figure 5.5 and and Animation: Boyle’s LawAnimation: Boyle’s Law))
V 1/P (constant moles and T)
or
iiff VPVP
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A Problem to ConsiderA Problem to Consider
A sample of chlorine gas has a volume of A sample of chlorine gas has a volume of 1.8 L at 1.0 atm. If the pressure increases to 1.8 L at 1.0 atm. If the pressure increases to 4.0 atm (at constant temperature), what 4.0 atm (at constant temperature), what would be the new volume?would be the new volume?
iiff VPVP using
)atm 0.4()L 8.1()atm 0.1(
PVP
Vf
iif
L 45.0Vf
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The Empirical Gas LawsThe Empirical Gas Laws
Charles’s Law:Charles’s Law: The volume occupied by any The volume occupied by any sample of gas at constant pressure is directly sample of gas at constant pressure is directly proportional to its absolute temperature.proportional to its absolute temperature.
(See Animation: Charle’s Law and Video: Liquid (See Animation: Charle’s Law and Video: Liquid Nitrogen and Balloons)Nitrogen and Balloons)
V Tabs (constant moles and P)
or
i
i
f
f
TV
TV
(See Animation: Microscopic Illustration of Charle’s Law)
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A Problem to ConsiderA Problem to Consider
A sample of methane gas that has a volume A sample of methane gas that has a volume of 3.8 L at 5.0of 3.8 L at 5.0°°C is heated to 86.0C is heated to 86.0°°C at C at constant pressure. Calculate its new constant pressure. Calculate its new volume.volume.
)K278()K359)(L8.3(
TTV
fi
fiV
L 9.4Vf
i
i
f
f
TV
TV
using
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The Empirical Gas LawsThe Empirical Gas Laws
Gay-Lussac’s Law:Gay-Lussac’s Law: The pressure exerted The pressure exerted by a gas at constant volume is directly by a gas at constant volume is directly proportional to its absolute temperature. proportional to its absolute temperature.
P Tabs (constant moles and V)
or
i
i
f
f
TP
TP
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A Problem to ConsiderA Problem to Consider
An aerosol can has a pressure of 1.4 atm An aerosol can has a pressure of 1.4 atm at 25at 25°°C. What pressure would it attain at C. What pressure would it attain at 12001200°°C, assuming the volume remained C, assuming the volume remained constant?constant?
i
i
f
f
TP
TP
using
)K298()K1473)(atm4.1(
TTP
fi
fiP
atm9.6Pf
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The Empirical Gas LawsThe Empirical Gas Laws
Combined Gas Law:Combined Gas Law: In the event that all In the event that all three parameters, P, V, and T, are three parameters, P, V, and T, are changing, their combined relationship is changing, their combined relationship is defined as follows: defined as follows:
f
ff
i
ii
TVP
TVP
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A Problem to ConsiderA Problem to Consider
A sample of carbon dioxide occupies 4.5 L A sample of carbon dioxide occupies 4.5 L at 30at 30°°C and 650 mm Hg. What volume C and 650 mm Hg. What volume would it occupy at 800 mm Hg and 200would it occupy at 800 mm Hg and 200°°C?C?
f
ff
i
iiTVP
TVP
using
)K 303)(Hg mm 800()K 473)(L 5.4)(Hg mm 650(
TPTVP
Vif
fiif
L7.5Vf
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• The volume of one mole of gas is called the molar gas volume, Vm. (See figure 5.12)
• Volumes of gases are often compared at standard temperature and pressure (STP), chosen to be 0 oC and 1 atm pressure.
The Empirical Gas LawsThe Empirical Gas Laws
Avogadro’s Law:Avogadro’s Law: Equal volumes of any two Equal volumes of any two gases at the same temperature and gases at the same temperature and pressure contain the same number of pressure contain the same number of molecules.molecules.
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– At STP, the molar volume, Vm, that is, the volume occupied by one mole of any gas, is 22.4 L/mol
– So, the volume of a sample of gas is directly proportional to the number of moles of gas, n.
The Empirical Gas LawsThe Empirical Gas Laws
Avogadro’s LawAvogadro’s Law
nV
(See Animation: Pressure and Concentration)
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A Problem to ConsiderA Problem to Consider
A sample of fluorine gas has a volume of A sample of fluorine gas has a volume of 5.80 L at 150.0 oC and 10.5 atm of 5.80 L at 150.0 oC and 10.5 atm of pressure. How many moles of fluorine gas pressure. How many moles of fluorine gas are present?are present?First, use the combined empirical gas law to determine the volume at STP.
)K423)(atm0.1()K273)(L80.5)(atm5.10(
TPTVP
Vistd
stdiiSTP
L3.39VSTP
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A Problem to ConsiderA Problem to Consider
Since Avogadro’s law states that at STP the Since Avogadro’s law states that at STP the molar volume is 22.4 L/mol, thenmolar volume is 22.4 L/mol, then
L/mol 22.4V
gas of moles STP
L/mol 22.4L 39.3
gas of moles
mol 1.75 gas of moles
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The Ideal Gas LawThe Ideal Gas Law
From the empirical gas laws, we See that From the empirical gas laws, we See that volume varies in proportion to pressure, volume varies in proportion to pressure, absolute temperature, and moles.absolute temperature, and moles.
Law sBoyle' 1/PV
Law sAvogadro' nV Law Charles' TV abs
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– Combining the three proportionalities, we can obtain the following relationship.
The Ideal Gas LawThe Ideal Gas Law
This implies that there must exist a This implies that there must exist a proportionality constant governing these proportionality constant governing these relationships.relationships.
)( PnTabs R""V
where “R” is the proportionality constant referred to as the ideal gas constant.
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The Ideal Gas LawThe Ideal Gas Law
The numerical value of The numerical value of RR can be derived can be derived using Avogadro’s law, which states that one using Avogadro’s law, which states that one mole of any gas at STP will occupy 22.4 mole of any gas at STP will occupy 22.4 liters.liters.
nTVP R
K) mol)(273 (1.00atm) L)(1.00 (22.4 R
KmolatmL 0.0821
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1919
The Ideal Gas LawThe Ideal Gas Law
Thus, the Thus, the ideal gas equationideal gas equation, is usually , is usually expressed in the following form:expressed in the following form:
nRT PV P is pressure (in atm)V is volume (in liters)n is number of atoms (in moles)R is universal gas constant 0.0821 L.atm/K.molT is temperature (in Kelvin)
(See Animation: The Ideal Gas Law PV=nRT)
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2020
A Problem to ConsiderA Problem to Consider
An experiment calls for 3.50 moles of An experiment calls for 3.50 moles of chlorine, Clchlorine, Cl22. What volume would this be . What volume would this be
if the gas volume is measured at 34if the gas volume is measured at 34°°C C and 2.45 atm?and 2.45 atm?
PnRT V since
atm 2.45K) )(307 1mol)(0.082 (3.50 Kmol
atmL
V then
L 36.0 V then
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Molecular Weight DeterminationMolecular Weight Determination
In Chapter 3 we showed the relationship In Chapter 3 we showed the relationship between moles and mass.between moles and mass.
mass molecular massmoles
or
mMmn
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Molecular Weight DeterminationMolecular Weight Determination
If we substitute this in the ideal gas If we substitute this in the ideal gas equation, we obtainequation, we obtain
RT)(PVmM
mIf we solve this equation for the molecular mass, we obtain
PVmRT Mm
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A Problem to ConsiderA Problem to Consider
A 15.5 gram sample of an unknown gas A 15.5 gram sample of an unknown gas occupied a volume of 5.75 L at 25occupied a volume of 5.75 L at 25°°C and a C and a pressure of 1.08 atm. Calculate its pressure of 1.08 atm. Calculate its molecular mass.molecular mass.
PVmRT M Since m
L) atm)(5.75 (1.08
K) )(298g)(0.0821 (15.5 M then Kmol
atmL
m
g/mol 61.1 Mm
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Density DeterminationDensity Determination
If we look again at our derivation of the If we look again at our derivation of the molecular mass equation,molecular mass equation,
RT)(PVmM
mwe can solve for m/V, which represents density.
RTPM
D Vm m
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2525
A Problem to ConsiderA Problem to Consider
Calculate the density of ozone, OCalculate the density of ozone, O33 (Mm = (Mm =
48.0g/mol), at 5048.0g/mol), at 50°°C and 1.75 atm of C and 1.75 atm of pressure.pressure.
RTPM
D Since m
K) )(323(0.0821g/mol) atm)(48.0 (1.75
D thenKmol
atmL
g/L 17.3 D
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Stoichiometry Problems Involving Stoichiometry Problems Involving Gas VolumesGas Volumes
Suppose you heat 0.0100 mol of Suppose you heat 0.0100 mol of potassium chlorate, KClOpotassium chlorate, KClO33, in a test tube. , in a test tube. How many liters of oxygen can you How many liters of oxygen can you produce at 298 K and 1.02 atm? produce at 298 K and 1.02 atm?
)g(O 3 KCl(s) 2 (s)KClO 2 23
• Consider the following reaction, which is often used to generate small quantities of oxygen.
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Stoichiometry Problems Stoichiometry Problems Involving Gas VolumesInvolving Gas Volumes
First we must determine the number of First we must determine the number of moles of oxygen produced by the reaction.moles of oxygen produced by the reaction.
3
23 KClO mol 2
O mol 3 KClO mol 0100.0
2O mol 5001.0
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Stoichiometry Problems Stoichiometry Problems Involving Gas VolumesInvolving Gas Volumes
Now we can use the ideal gas equation to Now we can use the ideal gas equation to calculate the volume of oxygen under the calculate the volume of oxygen under the conditions given.conditions given.
PnRT V
atm 02.1K) )(298 0821.0)(O mol (0.0150 Kmol
atmL2V
L 0.360 V
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Partial Pressures of Gas Partial Pressures of Gas MixturesMixtures
Dalton’s Law of Partial Pressures:Dalton’s Law of Partial Pressures: the the sum of all the pressures of all the different sum of all the pressures of all the different gases in a mixture equals the total pressure gases in a mixture equals the total pressure of the mixture. (Figure 5.19)of the mixture. (Figure 5.19)
....PPPP cbatot
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Partial Pressures of Gas Partial Pressures of Gas MixturesMixtures
The composition of a gas mixture is often The composition of a gas mixture is often described in terms of its mole fraction.described in terms of its mole fraction.
tot
A
tot
AA P
Pnn
Aof fraction Mole
– The mole fraction, , of a component gas is the fraction of moles of that component in the total moles of gas mixture.
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Partial Pressures of Gas Partial Pressures of Gas MixturesMixtures
The partial pressure of a component gas, The partial pressure of a component gas, “A”, is then defined as“A”, is then defined as
totAA P P – Applying this concept to the ideal gas equation,
we find that each gas can be treated independently.
RTn VP AA
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A Problem to ConsiderA Problem to Consider
Given a mixture of gases in the atmosphere Given a mixture of gases in the atmosphere at 760 torr, what is the partial pressure of Nat 760 torr, what is the partial pressure of N22
(( = 0 .7808) at 25 = 0 .7808) at 25°°C?C?
torr) (760 (0.7808) P then2N
torr 593 P2N
totNN P P since22
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Collecting Gases “Over Water”Collecting Gases “Over Water”
A useful application of partial pressures A useful application of partial pressures arises when you collect gases over water. arises when you collect gases over water. (See Figure 5.20)(See Figure 5.20)
– As gas bubbles through the water, the gas becomes saturated with water vapor.
– The partial pressure of the water in this “mixture” depends only on the temperature. (See Table 5.6)
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A Problem to ConsiderA Problem to Consider
Suppose a 156 mL sample of HSuppose a 156 mL sample of H22 gas was gas was
collected over water at 19collected over water at 19ooC and 769 mm C and 769 mm Hg. What is the mass of HHg. What is the mass of H22 collected? collected?
– First, we must find the partial pressure of the dry H2.
0HtotH 22P P P
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3535
A Problem to ConsiderA Problem to Consider
Suppose a 156 mL sample of HSuppose a 156 mL sample of H22 gas was gas was
collected over water at 19collected over water at 19ooC and 769 mm C and 769 mm Hg. What is the mass of HHg. What is the mass of H22 collected? collected?
– Table 5.6 lists the vapor pressure of water at 19oC as 16.5 mm Hg.
Hg mm 16.5 - Hg mm 697 P2H
Hg mm 527 P2H
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3636
A Problem to ConsiderA Problem to Consider
Now we can use the ideal gas equation, Now we can use the ideal gas equation, along with the partial pressure of the along with the partial pressure of the hydrogen, to determine its mass.hydrogen, to determine its mass.
atm 989.0 Hg mm 527 P Hg mm 760atm 1
H2
L 0.156 mL 156 V K 292 273) (19 T
? n
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A Problem to ConsiderA Problem to Consider
From the ideal gas law, PV = nRT, you From the ideal gas law, PV = nRT, you havehave
)K 292)( (0.0821L) atm)(0.156 (0.989
RTPV
nKmol
atmL
mol 0.00644 n – Next,convert moles of H2 to grams of H2.
22
22 H g 0.0130
H mol 1H g 2.02
H mol 0.00644
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Kinetic-Molecular TheoryKinetic-Molecular Theory A simple model based on the actions of A simple model based on the actions of
individual atoms individual atoms
Volume of particles is negligibleVolume of particles is negligible Particles are in constant motionParticles are in constant motion No inherent attractive or repulsive forcesNo inherent attractive or repulsive forces The average kinetic energy of a collection of The average kinetic energy of a collection of
particles is proportional to the temperature particles is proportional to the temperature (K)(K)
(See Animation: Kinetic Molecular Theory)
(See Animations: Visualizing Molecular Motion and Visualizing Molecular Motion [many Molecules])
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3939
Molecular Speeds; Diffusion and Molecular Speeds; Diffusion and EffusionEffusion
The root-mean-square (rms) molecular The root-mean-square (rms) molecular speed, u,speed, u, is a type of average molecular is a type of average molecular speed, equal to the speed of a molecule speed, equal to the speed of a molecule having the average molecular kinetic having the average molecular kinetic energy. It is given by the following formula:energy. It is given by the following formula:
mM3RT
u
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4040
Molecular Speeds; Diffusion and Molecular Speeds; Diffusion and EffusionEffusion
DiffusionDiffusion is the transfer of a gas through space is the transfer of a gas through space or another gas over time.or another gas over time. (See Animation: (See Animation: Diffusion of a Gas)Diffusion of a Gas)
EffusionEffusion is the transfer of a gas through a is the transfer of a gas through a membrane or orifice. (See Animation: Effusion of a membrane or orifice. (See Animation: Effusion of a Gas)Gas)– The equation for the rms velocity of gases
shows the following relationship between rate of effusion and molecular mass. (See Figure 5.22)
mM1
effusion of Rate
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4141
Molecular Speeds; Diffusion and Molecular Speeds; Diffusion and EffusionEffusion
According to According to Graham’s law,Graham’s law, the rate of the rate of effusion or diffusion is inversely proportional effusion or diffusion is inversely proportional to the square root of its molecular mass. to the square root of its molecular mass. (See Figures 5.28 and 5.29)(See Figures 5.28 and 5.29)
Agas of MB Gas of M
B"" gas of effusion of RateA"" gas of effusion of Rate
m
m
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4242
A Problem to ConsiderA Problem to Consider
How much faster would HHow much faster would H22 gas effuse gas effuse
through an opening than methane, CHthrough an opening than methane, CH44??
)(HM)(CHM
CH of RateH of Rate
2m
4m
4
2
8.2g/mol 2.0g/mol 16.0
CH of RateH of Rate
4
2
So hydrogen effuses 2.8 times faster than CH4
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Real GasesReal Gases
Real gases do not follow PV = nRT Real gases do not follow PV = nRT perfectly. The van der Waals equation perfectly. The van der Waals equation corrects for the nonideal nature of real corrects for the nonideal nature of real gases.gases.
a corrects for interaction between atoms.
b corrects for volume occupied by atoms.
nRT nb)-V)( P( 2
2
Van
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Real GasesReal Gases
In the van der Waals equation, In the van der Waals equation,
where “nb” represents the volume occupied by “n” moles of molecules. (See Figure 5.32)
nb)-V( becomesV
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Real GasesReal Gases
Also, in the van der Waals equation, Also, in the van der Waals equation,
where “n2a/V2” represents the effect on pressure to intermolecular attractions or repulsions. (See Figure 5.33)
)P( becomes P 2
2
Van
Table 5.7 gives values of van der Waals constants for various gases.
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A Problem to ConsiderA Problem to Consider
If sulfur dioxide were an “ideal” gas, the If sulfur dioxide were an “ideal” gas, the pressure at 0pressure at 0°°C exerted by 1.000 mol C exerted by 1.000 mol occupying 22.41 L would be 1.000 atm. Use occupying 22.41 L would be 1.000 atm. Use the van der Waals equation to estimate the the van der Waals equation to estimate the “real” pressure.“real” pressure.
Table 5.7 lists the following values for SO2
a = 6.865 L2.atm/mol2
b = 0.05679 L/mol
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A Problem to ConsiderA Problem to Consider
First, let’s rearrange the van der Waals First, let’s rearrange the van der Waals equation to solve for pressure.equation to solve for pressure.
2
2
V
an -
nb-VnRT
P
R= 0.0821 L. atm/mol. K
T = 273.2 K
V = 22.41 L
a = 6.865 L2.atm/mol2
b = 0.05679 L/mol
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A Problem to ConsiderA Problem to Consider
The “real” pressure exerted by 1.00 mol of The “real” pressure exerted by 1.00 mol of SOSO22 at STP is slightly less than the “ideal” at STP is slightly less than the “ideal” pressure.pressure.
2
2
V
an -
nb-VnRT
P
L/mol) 79mol)(0.056 (1.000 - L 22.41
)K2.273)( 06mol)(0.082 (1.000 P Kmol
atmL
2mol
atmL2
L) 41.22(
) (6.865mol) (1.000-
2
2
atm 0.989 P
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Operational SkillsOperational Skills Converting units of pressure.Converting units of pressure. Using the empirical gas laws.Using the empirical gas laws. Deriving empirical gas laws from the ideal gas law.Deriving empirical gas laws from the ideal gas law. Using the ideal gas law.Using the ideal gas law. Relating gas density and molecular weight.Relating gas density and molecular weight. Solving stoichiometry problems involving gases.Solving stoichiometry problems involving gases. Calculating partial pressures and mole fractions.Calculating partial pressures and mole fractions. Calculating the amount of gas collected over water.Calculating the amount of gas collected over water. Calculating the rms speed of gas molecules.Calculating the rms speed of gas molecules. Calculating the ratio of effusion rates of gases.Calculating the ratio of effusion rates of gases. Using the van der Waals equation.Using the van der Waals equation.
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Figure Figure 5.2: A 5.2: A mercury mercury barometbarometer. er.
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Figure Figure 5.5: 5.5: Boyle’s Boyle’s experimeexperiment. nt.
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Animation: Boyle’s LawAnimation: Boyle’s Law
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Animation: Charle’s LawAnimation: Charle’s Law
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Video: Liquid Nitrogen & Video: Liquid Nitrogen & BalloonsBalloons
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Animation: Microscopic Animation: Microscopic Illustration of Charle’s LawIllustration of Charle’s Law
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Figure 5.12: The molar volume of a Figure 5.12: The molar volume of a gas. gas.
Photo courtesy of James Scherer.Photo courtesy of James Scherer.
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Animation: Pressure and Animation: Pressure and Concentration of a GasConcentration of a Gas
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Animation: The Ideal Gas LawAnimation: The Ideal Gas Law
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Figure 5.19: An illustration of Figure 5.19: An illustration of Dalton’s law of partial pressures.Dalton’s law of partial pressures.
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Figure 5.20: Collection of gas Figure 5.20: Collection of gas over water.over water.
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6161Return to Slide 33
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Animation: Kinetic Molecular Animation: Kinetic Molecular TheoryTheory
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Animation: Visualizing Molecular Animation: Visualizing Molecular Motion [One Molecule]Motion [One Molecule]
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(Click here to open QuickTime animation)
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Animation: Visualizing Molecular Animation: Visualizing Molecular Motion [Many Molecules]Motion [Many Molecules]
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(Click here to open QuickTime animation)
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Animation: Diffusion of a GasAnimation: Diffusion of a Gas
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Animation: Effusion of a GasAnimation: Effusion of a Gas
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Figure 5.22: Elastic collision of steel balls: Figure 5.22: Elastic collision of steel balls: The ball is released and transmits energy to The ball is released and transmits energy to
the ball on the right. the ball on the right. Photo courtesy of Photo courtesy of American Color.American Color.
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Figure Figure 5.28:5.28:Gaseous Gaseous EffusionEffusion
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Figure Figure 5.29: 5.29: HydrogeHydrogen n FountainFountain
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Figure Figure 5.32: 5.32: Molecular Molecular VolumeVolume
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Figure 5.33: Figure 5.33: Intermolecular Intermolecular AttractionsAttractions
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