Collisions of Gas Particles
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Transcript of Collisions of Gas Particles
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Collisions of Gas Particles
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Collisions of Gas Particles
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Kinetic Theory
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Kinetic Molecular TheoryPostulates of the Kinetic Molecular Theory of Gases
1. Gases consist of tiny particles (atoms or molecules)
2. These particles are so small, compared with the distances betweenthem, that the volume (size) of the individual particles can be assumedto be negligible (zero).
3. The particles are in constant random motion, colliding with the walls ofthe container. These collisions with the walls cause the pressure exertedby the gas.
4. The particles are assumed not to attract or to repel each other.
5. The average kinetic energy of the gas particles is directly proportionalto the Kelvin temperature of the gas
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Kinetic Molecular Theory (KMT)
1. …are so small that they are assumed to have zero volume
2.…are in constant, straight-line motion
3.…experience elastic collisions in which no energy is lost
4.…have no attractive or repulsive forces toward each other
5.…have an average kinetic energy (KE) that is proportional to the absolute temp. of gas (i.e., Kelvin temp.)
AS TEMP. , KE
explains why gases behave as they do
deals w/“ideal” gas particles…
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Elastic vs. Inelastic Collisions
8
3
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8
Elastic vs. Inelastic Collisions
8v1
elastic collision
inelastic collision
POW v2
v3 v4
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8
Elastic Collision
8v1
before
v2
after
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Model Gas Behavior
• All collisions must be elastic • Take one step per beat of the
metronome • Container
– Class stands outside tape box
• Higher temperature – Faster beats of metronome
• Decreased volume– Divide box in half
• More Moles – More students are inside box
Mark area of container with tape on ground.
Add only a few molecules of inert gas
Increase temperature Decrease volume Add more gas Effect of diffusion Effect of effusion
(opening size)
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Kinetic Molecular Theory
• Particles in an ideal gas…– have no volume.– have elastic collisions. – are in constant, random, straight-line motion.– don’t attract or repel each other.– have an avg. KE directly related to Kelvin temperature.
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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Molecular Velocities
speed
Fra
ctio
ns o
f pa
rtic
les
the Maxwell speed distribution
http://antoine.frostburg.edu/chem/senese/101/gases/slides/sld016.htm
molecules sorted by speed
many different molecular speeds
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Real Gases
• Particles in a REAL gas…– have their own volume– attract each other
• Gas behavior is most ideal…– at low pressures– at high temperatures– in nonpolar atoms/molecules
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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Characteristics of GasesGases expand to fill any container.
– random motion, no attraction
Gases are fluids (like liquids).– no attraction
Gases have very low densities.– no volume = lots of empty space
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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Characteristics of Gases• Gases can be compressed.
– no volume = lots of empty space
• Gases undergo diffusion & effusion.– random motion
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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Properties of Gases
V = volume of the gas (liters, L)
T = temperature (Kelvin, K)
P = pressure (atmospheres, atm)
n = amount (moles, mol)
Gas properties can be modeled using math.Model depends on:
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Pressure - Temperature - Volume Relationship
P T V P T V
Gay-Lussac’s P T
Charles V T
P T
V
P T
V P T V P T V
Boyle’s P 1V ___
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Pressure - Temperature - Volume Relationship
P T V P T V
Gay-Lussac’s P T
Charles V T
Boyle’s P 1V ___
P n V P n V
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Pressure and Balloons
A
B = pressure exerted ON balloonA = pressure exerted BY balloon
BWhen balloon is being filled:
PA > PB
When balloon is filled and tied:PA = PB
When balloon deflates:PA < PB
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When the balloons are untied,will the large balloon (A) inflatethe small balloon (B); will they end up the same size or will the small balloon inflate the large balloon?
Why?
Balloon Riddle
A
B
C
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Kinetic Theory and the Gas Laws
Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 323 (newer book)
original temperatureoriginal pressureoriginal volume
increased temperatureincreased pressureoriginal volume
increased temperatureoriginal pressureincreased volume
(a) (b) (c)
10 10 10
10