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2-Variable Gas Laws
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Kinetic-Molecular
Theory1. Gas particles do not attract or repel each other
2. Gas particles are much smaller than the distances between them
3. Gas particles are in constant, random motion
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Kinetic-Molecular
Theory
5. All gases have the same average kinetic energy at a given temperature
4. No kinetic energy is lost when gas particles collide with each other or with the walls of their container
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Boyle’s LawVolume and pressure are inversely related in gases at a constant temperature.
P1V1 = P2V2
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Boyle’s Law PracticeA sample of helium gas in a
balloon is compressed from 4.0 L to 2.5 L at a constant temperature. If the pressure of the gas in the 4.0 L volume is 210 kPa, what will the pressure be at 2.5 L?
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Temperature ConversionSince temperature relates
directly to the kinetic energy of a sample, we must use an absolute scale when doing gas law calculations.
Always convert to Kelvins before solving gas law calculations.
K = °C + 273
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Charles’s LawVolume and temperature (K) of a gas are directly proportional at constant pressure.
V1 = V2
T1 T2
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Charles’s Law PracticeA gas sample at 40.0℃ occupies a
volume of 2.32 L. If the temperature is raised to 75℃, what will the volume be, assuming the pressure remains constant?
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Gay-Lussac’s LawPressure is directly
proportional to the temperature (K) of a gas when volume is constant
P1 = P2
T1 T2
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Gay-Lussac’s Law PracticeThe pressure of a gas in a tank is
3.20 atm at 22.0 ℃. If the pressure falls to 1.55 atm, what will be the Celsius temperature of the gas in the tank?