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Unformatted text preview: 3 at 303K and 101.3 kPa: a. What would the samples volume be at 273.15K at constant pressure? b. What is the molar mass of the sample? 6. What are the mole fraction and partial pressure of each gas in a 2.50 L container into which 100.00g of nitrogen and 100.00g of carbon dioxide are added at 25 o C? What is the total pressure? 7. In an industrial process, nitrogen is heated to 500 K at a constant volume of 1.00 m 3 . The gas enters the container at 300 K and 100 atm. The mass of the gas is 92.4kg. Use the van der Waals equation to determine the approximate pressure of the gas at its working temperature of 500 K. for nitrogen, a = 1.352 L 2 atm mol-2 , b = 3.87 x10-2 Lmol-1 . 8. Compare the pressures predicted for 0.8 dm 3 of Cl 2 weighing 17.5g at 273.15K using: a. The ideal gas equation and b. The van der Waals equation....
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This note was uploaded on 01/31/2012 for the course CHEM ep103 taught by Professor Tukur during the Fall '11 term at UCSI.
- Fall '11