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Chapter 11

# Chapter 11 - Chapter 11 Properties of Gases Pressure =...

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Chapter 11 Properties of Gases Pressure = force/area Units of force lbs/in 2 SI unit = Pascal (Pa) = N/m 2 Standard atmosphere = 101,325 Pa 1 atm = 101 kPa 1 atm = 760 torr see figure 11.3 for definition of a torr Pressure/Volume/Temperature relationships for a fixed amount of a gas Boyles Law 1 V α ------ at constant Temperature and mass P or PV = C where C is a constant see figure 11.5 Charles Law V α T at constant pressure and mass Or V/T = C But! T must be in Kelvin (K) See figure 11.6 and video demonstration of ballon Chem 111 Lecture notes By Alan Zombeck page 1

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Chapter 11 Gay-Lussac’s Law P α T Or P = C x T The combined Gas Law We can write PV/T = constant (for a fixed amount of a gas) We can then write P 1 V 1 ------ = C T 1 And P 2 V 2 ------ = C T 2 We arrive at the combined gas law by P 1 V 1 P 2 V 2 ------ = ------- T 1 T 2 Example 11.2 A sample of argon is trapped in a gas bulb at a pressure of 760 torr when the volume is 100 mL and the temperature is 35’C. What must its temperature be if its pressure becomes 720 torr and its volume 200 mL? Chem 111 Lecture notes By Alan Zombeck page 2
Chapter 11 The Ideal Gas Law Relationship of gas volumes in gas phase reactions Example Hydrogen + chlorine hydrogen chloride 1 vol 1 vol 2 vol The reacting volumes, measured under identical temperatures and pressures, given beneath the names, are in ratios of simple whole numbers. Avogadro’s principle when measured at the same temperature and pressure, equal volumes of gases contain equal numbers of moles Stated otherwise

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