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Ideal Gas Law

Ideal Gas Law. Date:. Ideal Gas Law. PV = nRT Pressure Volume in liters Number of moles R, ideal gas constant Temperature in Kelvin. Assumptions. Size of gas molecules does not matter No intermolecular forces between atoms Therefore, gases cannot condense into liquids.

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Ideal Gas Law

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  1. Ideal Gas Law Date:

  2. Ideal Gas Law • PV = nRT • Pressure • Volume in liters • Number of moles • R, ideal gas constant • Temperature in Kelvin

  3. Assumptions • Size of gas molecules does not matter • No intermolecular forces between atoms • Therefore, gases cannot condense into liquids. • We all know liquids exist, but the ideal gas law makes calculations easier and is accurate most of the time.

  4. Values of R • R depends on which unit pressure is measured in. • 8.31kPa*L/K*mol • 0.0821atm*L/K*mol • 62.4torr*L/K*mol torr and mmHg same

  5. Examples • What pressure, in atm is exerted by 1.5 mol of an ideal gas contained in a 1.5L vessel at 20.0oC? • PV = nRT • (P)(1.5L) = (1.5mol)(0.0821atmL/Kmol)(20+273K) • 1.5P = 36.08295 • P = 24 atm

  6. What volume will 15.0 mol of an ideal gas occupy at 25oC and 130. kPa? • PV = nRT • (130.kPa)(L) = (15.0mol)(8.31kPa/Kmol)(25+273K) • 130L = 37145.7 • 286 L

  7. If 88 g of CO2 gas are confined to a 25 L container at a temperature of 32oC, what pressure does the gas exert in kPa? • PV = nRT • P(25L) = (88/44 mol)(8.31kPaL/Kmol)(32+273) • 25P = 5069.1 • 2.0*102kPa 44 is the molar mass of CO2, divided by MM to get # mols

  8. What is the molar mass of a gas that has a pressure of 0.839 atm, a mass of 15.0 g, and a volume of 10.0L at a temperature of 27oC? PV = nRT (0.839atm)(10.0L) = n(0.0821atmL/Kmol)(27+273) 8.39 = 24.63n 0.340641494113 = n, the number of moles Molar mass is grams / mol 15.0g / 0.340641494113 44 g/mol Note: wait to round until the end of the problem.

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