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Gases• KMT = particles
constant motion• AKE, temperature,
pressure, volume, amount of a gas are all related
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Pressure & Force• D/t collisions of
molecules on surfaces
• P = defined as the force per unit area on a surface = force/area
• Force unit = newton (N)
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The Barometer
• Pressure depends on area of contact; smaller area, greater pressure
Ex.: high heels; ballerina• Atmosphere exerts
pressure - total of individual gas pressures (mostly N, then O)
• Measured using barometers
• Units(ie. 1 torr = 1 mm Hg)
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Dalton’s Law of Partial Pressures
• Partial pressures are exerted by individual gases
• Law states that total pressure of a gas mixture is the sum of the component pressures
• PT = P1+P2+P3…
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Boyle’s Law• Inversely relates
pressure and volume
• Examples?• P1V1=P2V2
• What is the constant?
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MUST KNOW
• Use the temperature in Kelvins when solving these gas problems.
• K = ºC + 273• STP means standard temperature (0ºC)
pressure (1 atm).• 1 atm = 101.3 kPa = 760 torr = 760 mm Hg
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Charles’s Law• Directly relates
volume and temperature
• V1/T1 = V2/T2
• What is the constant?
• K = degrees C + 273
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Gay-Lussac’s Law• Directly relates
pressure and temperature
• P1/T1=P2/T2
• Constant?
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Combined Gas Law
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Avogadro’s Law• Equal volumes of gases
at the same temperature and pressure contain equal numbers of molecules.
• Example: At the same temperature and pressure, balloons of equal volume have equal numbers of molecules, regardless of which gas they contain.
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Molar Volume of a Gas
• 22.4 L at STP• STP = 1 atm and
0 degrees C (273 K)
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Ideal Gas Law• Solve for moles within a gas PV = nRT
R is a constant (0.0821 Lxatm/molxK). This is used when the volume is in liters, the pressure is in atmospheres, and the temperature is in Kelvins.
n is the number of moles
Use a table for values of R when other units for n, P, V, and T are used.
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Comparison of Diffusion with Effusion
• Effusion is the process by which gas molecules under pressure pass through a tiny opening.
• Diffusion is the mixing of two gases by random molecular motion.
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Graham’s Law of Effusion• Rates of effusion of
gases at the same temperature and pressure is inversely proportional to the square roots of their molar masses
• Square root of Molar Mass B/Square root of Molar Mass A