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Chapter 10 Gas Laws
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Air… The atmosphere is
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Diving Issues Nitrogen Narcosis
Nitrogen narcosis is a condition that occurs in divers breathing compressed air. When divers go below depths of approximately 100 ft, increase in the partial pressure of nitrogen produces an altered mental state similar to alcohol intoxication.
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The Bends Decompression sickness
nitrogen from the air will dissolve in the water in his or her body. If the diver were to swim quickly to the surface, it is just like uncorking a bottle of soda -- the gas is released. This can cause a very painful condition, and it is sometimes fatal.
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Increased pressure The pressure on divers increases by one atmosphere for every 33 feet of depth At 100 feet, some people say it is difficult to breathe
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Decompression If divers do not decompress as they surface, they can develop the bends. Stops at various intervals as they rise to the surface, sometimes for 15 to 20 minutes or more.
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Pressure Defined as the Equation: Psi, kg/m2, etc
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How is pressure measured?
Barometers Manometers p 123, fig 5.2 Units:
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Gas Properties Move The physical volume of the
Attractive/repulsive forces
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Gas Properties Energy is
Average kinetic energy is related to the absolute temperature
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The Gas Laws Boyle’s Charles’ Guy-Lussac’s Avogadro’s Combined Ideal
Molecular mass Dalton’s partial pressures
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Boyle’s Relates Equation: Temperature and number of molecules fixed
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Charles’ Relates Equation: Pressure and number of molecules fixed
If T increases, V increases Temperature must be in Kelvins – if the Celsius scale is used, the ratio is not constant
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Guy_Lussac’s Relates Equation Volume and number of molecules fixed
If T increases, P increases Temp in Kelvin, not C
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Avogadro’s Relates Equation Pressure and temp are fixed
Equal volumes of gases at the same P and T contain the same # molecules
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Combined Relates Equation Number of molecules is fixed
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Ideal Gas Law Combines all of the above Equation:
Use Standard Temperature and Pressure, 1.00 atm, 273 K P=Pressure, V=volume, n=number of moles, R=Gas law constant Latm/Kmol R was found by setting 1 mole of gas at 1.00 atm and 273 K and 22.4 L and solving using ideal gas law
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Molecular Mass Determine the molar mass of a gas n =
n=g/M n = PV/RT manipulate the gas law Also… in M = gRT/PV g/V is density in g/L
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Dalton and Partial Pressure
Ptotal = P1 + P2 + …
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