lecture8 - Fri. Sept. 19, 2003 Todays Lecture Gases 5.1-5.3...

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Fri. Sept. 19, 2003 Today’s Lecture Gases • 5.1-5.3 Gas Laws • 5.4 Gas Stoichiometry • 5.5 Partial pressure
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h = 760mm Hg for standard atmosphere Vacuum • Pressure: – units of pressure: • mm Hg = Torr • atmosphere (atm) • Pascal (Pa): Pressure – unit factors: 1 atm = 1.01325 x10 5 N/m 2 101.3 Kpa = 1 atm = 760 mm Hg = 760 Torr = 14.7 psi IUPAC units: 1bar = 10 5 Pa Pa m N area force 2 = = = Fig. 5.2
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• Gas Laws: – Boyle (1627-1691): PV = k P = pressure V = volume k = constant at a specific temperature same as the equation describing a straight line: y = mx + b slope intercept P 1 k P k V = = Fig. 5.3
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• Therefore, a plot of V vs 1/P should give a straight line of slope k . V is inversely proportional to pressure P (in Hg) 0 20 40 60 50 100 P P 2 V 2 V 0 0 1/ P (in Hg) 0.01 0.02 0.03 20 40 slope = k V (in 3 ) Fig. 5.4
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• Ideal gas: a gas that strictly obeys Boyle’s law. – i.e., an increase in P generates the same PV value. – Since k is constant: P 1 V 1 = P 2 V 2 05_51 PV (L • atm) 0 22.25 P (atm) 1.00 0.75 0.50 0.25 22.30 22.35 22.40 22.45 Ne O 2 CO 2 Ideal Fig. 5.5
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Balloon in Liquid N 2
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• Volume increases linearly with temperature, at constant pressure for a fixed amount of gas. V = bT
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lecture8 - Fri. Sept. 19, 2003 Todays Lecture Gases 5.1-5.3...

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