behavior of gases
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Behavior of Gases. Ch 12 – Prentice Hall. Kinetic Theory. Gases are composed of SMALL, SEPARATE particles called MOLECULES. Gas molecules are in CONSTANT MOTION All COLLISIONS between particles are PERFECTLY ELEASTIC - PowerPoint PPT PresentationTRANSCRIPT
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Behavior of GasesCh 12 – Prentice Hall
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Kinetic Theory• Gases are composed of SMALL,
SEPARATE particles called MOLECULES.
• Gas molecules are in CONSTANT MOTION
• All COLLISIONS between particles are PERFECTLY ELEASTIC
• The MOLECULES of a gas display no ATTRACTION or REPULSION for one another.
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Kinetic Theory
• The AVERAGE KINETIC ENERGY of the molecules is DIRECTLY PROPORTIONAL to the KELVIN temperature of the gas.
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Ideal Gas
• Gas whose BEHAVIOR conforms to the KINETIC THEORY -it is THEORETICAL.
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Gas Pressure:
Pressure = FORCE ÷ AREA = ____ atm
Atmospheric Pressure - the PRESSURE the earth’s ATMOSPHERE exerts due to its WEIGHT.
Barometer: Instrument used to measure �ATMOSPHERIC PRESSURE Invented by � TORRICALLI
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The Combined Gas Law
Combines the following laws and equations together:
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Charles law
Variation of gas volume with temperature while pressure is kept constant
V1/T1 = V2/T2
T (K) = t (0C) + 273.15
Temperature must bein Kelvin
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P1V1 = P2V2Boyle’s Law
Constant temperatureConstant amount of gas
Pressure and volume units can be any variant of pressure and volume
HOWEVER the units MUST agree for both pressures and both volumes!
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Combined Gas Law
• Expresses the relationship between the PRESSURE, VOLUME and TEMPERATURE of a FIXED amount of GAS.
Equation: P1V1 = P2V2
T1 T2
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STANDARD TEMPERATURE AND PRESSURE
• STP CONDITIONS
• 273 K
• 1 atm = 760 mmHg
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Combined Gas LawEx: A sample of gas has a volume of 201 L when its
temperature is 293 K and its pressure is 224 mmHg. What volume will the gas occupy at STP?
V1 = 201 L V2 = ?T1 = 293 K T2 = 273 KP1 = 224 mmHg P2 = 760 mmHg
(224) (201) = (760) x (293) (273)
(224) (201) (273) = (293) (760) x
X = 55 L
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Diffusion The � RAPID spreading of a GAS
Graham’s Law of Diffusion
Under the same conditions of �TEMPERATURE and PRESSURE, gases DIFFUSE at a rate INVERSLEY proportional to the SQUARE ROOT of their DENSITIES (or MOLAR MASS)
Equation:
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Ideal Gas Equation
Equation: PV = nRT • New variables:n = AMOUNT of gas in MOLES R = UNIVERSAL GAS CONSTANT* PROPORTIONALLY constant* value depends on UNITS used for
PRESSURE and VOLUME* value of R when using kPa and LR = 8.314 L . kPa / Mol . K
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Ex: The average lung capacity for a female student is 3.9 L. At normal body temperature, 37oC, and 110 kPa, how many moles of air could her lungs hold?
P = 110 kPa V = 3.9 L T = 310 K (273 + 37)
n = X R = 8.314 L . kPa / Mol . K
(110)(3.9) = x (310)(8.314)
(110)(3.9) = 0.17 mol(310)(8.314)
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Avogadro’s Law
• Equal VOLUMES of different GASES under the SAME conditions have the SAME number of PARTICLES.
• Conversely, if samples of DIFFERENT GASES at the same TEMPERATURE and PRESSURE contain the SAME number of PARTICLES, then the VOLUMES of all the SAMPLES must be EQUAL.
• At STP, one MOLE of any gas occupies a VOLUME of 22.4 L.
• 22.4 L is the MOLAR VOLUME of a gas.
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Dalton’s Law of Partial Pressures
• The PRESSURE of a gas MIXTURE is the SUM of the INDIVIDUAL PRESSURES of each gas ALONE.
Equation: PT = P1 + P2 + P3 …
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• Ex: Oxygen gas has been collected over water at a total pressure of 95.0 kPa and a temperature of 25oC. What is the pressure of the dry oxygen gas?
PT = 95 kPa P vapor = 3.17 kPa P oxygen = X
95 = 3.17 + x
91.83 kPa = x
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