Oct_01 - Chapter 4 - Gases Suggested Problems Chapter 4 -...

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Chapter 4 - Gases Suggested Problems Chapter 4 - 21, 29, 31, 43, 49, 53, 55, 57, 67, 77
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Pressure SI: (Pa) = 1 N m -2 1 bar = 100,000 Pa 1 atm = 760 mmHg = 760 torr = 101,325 Pa = 14.7 lb in -2 Pressure = Force Area
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Pressure Measurements P gas = d fluid hg “absolute pressure” P gas = P atm + d fluid hg “gauge pressure” NIST: P a = x psi NIST: P g = x psi
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Boyle's Law P 1/V or PV = constant ( for constant n and T) Common zero intercept for plots of P vs. 1/V over a range of temperatures
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Charles's Law V T at constant n and P T = absolute temperature in Kelvin (K) The common intercept is -273.15 ºC or a bsolute zero for the Kelvin temperature scale 0 K = -273.15 ºC
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Avogadro's Law “Equal volumes of gas under the same conditions of pressure and temperature contain the same number of molecules.” V n (at constant T and P)
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Combined Gas Law If you combine all three of the laws you get: V nT P Ideal Gas Law PV = nRT R = gas constant = 8.3145 J mol -1 K -1 = 0.08206 L atm mol -1 K -1 S tandard T emperature and P ressure (STP): P = 1 atm T = 273 K (~ 0 ºC)
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This note was uploaded on 01/20/2011 for the course CHEM 154 CHEM 154 taught by Professor Yang during the Spring '10 term at The University of British Columbia.

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Oct_01 - Chapter 4 - Gases Suggested Problems Chapter 4 -...

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