Flask Volume 100.0 + 100.0 + 79.6 mL = 279.6 mL Mass of Flask + Cap 143.85 g Mass of Flask + Condensed Liquid 144.95 g Mass of Condensed Liquid 1.10 g Temperature of Water Bath (oC) 84.1 oC Barometric Pressure (atm) 0.985 atm What is the molar mass of the unknown? What will its temperature be when the pressure is 1.20 atm and the volume is 250.0 mL?
Flask Volume 100.0 + 100.0 + 79.6 mL = 279.6 mL Mass of Flask + Cap 143.85 g Mass of Flask + Condensed Liquid 144.95 g Mass of Condensed Liquid 1.10 g Temperature of Water Bath (oC) 84.1 oC Barometric Pressure (atm) 0.985 atm What is the molar mass of the unknown? What will its temperature be when the pressure is 1.20 atm and the volume is 250.0 mL?
Chapter24: Introduction To Spectrochemical Methods
Section: Chapter Questions
Problem 24.4QAP
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Question
In the Dumas method for determining the molar mass of an unknown volatile liquid, a sample of a volatile liquid that boils below 100oC is vaporized in a boiling water bath and the mass of the vapor required to fill the flask is determined. The following data was collected:
Flask Volume |
100.0 + 100.0 + 79.6 mL = 279.6 mL |
Mass of Flask + Cap |
143.85 g |
Mass of Flask + Condensed Liquid |
144.95 g |
Mass of Condensed Liquid |
1.10 g |
Temperature of Water Bath (oC) |
84.1 oC |
Barometric Pressure (atm) |
0.985 atm |
- What is the molar mass of the unknown?
- What will its temperature be when the pressure is 1.20 atm and the volume is 250.0 mL?
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