Experiment 6 - Experiment 6 Enthalpy of Vaporization of...

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Experiment 6: Enthalpy of Vaporization of Water Derek Ems Jon Pool TA: Rachel 11/14/07 1. Purpose The Purpose of this experiment is to determine experimentally the vapor pressure of water as a function of temperature and to determine the enthalpy of vaporization of water as a function of temperature by using the van t’Hoff equation. 2. Data Temperature (in degrees Celsius) Volume (in milliliters) 78.3 10.00 76.3 9.43 74.3 8.84 72.3 8.50 70.3 8.07 68.3 7.75 66.3 7.48 64.3 7.20 62.3 7.00 60.3 6.73 58.3 6.61 56.3 6.48 54.3 6.31 52.3 6.20 50.0 6.05
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800 ml of DI water in Beaker Pressure=761.1 MM Hg= 1.001 Atm Initial volume of air trapped=5.00 ml Actual volume of air trapped (in ml)=5.00-0.2=4.80 Volume of Air when chilled to 4.6 degrees Celsius=4.65 ml Actual volume of Air when chilled to 4.6 degrees Celsius=4.65-0.2=4.45 ml Literature Value of ∆H vap for water= + 40.7 KJ Mol -1 3. Graphs and Table of Results Temperature (in degrees Celsius) Actual volume in milliliters (volume-0.2 ml) 78.3 9.80 76.3 9.23 74.3 8.64 72.3 8.30 70.3 7.87 68.3 7.55 66.3 7.28 64.3 7.00 62.3 6.80 60.3 6.53 58.3 6.41 56.3 6.28 54.3 6.11 52.3 6.00
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50.0 5.85 P air p water 1/t lnPwater 0.600084566 0.399915 0.002847 -0.9165 0.633515533 0.366484 0.002863 -1.0038
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This note was uploaded on 04/16/2008 for the course CHEMISTRY 101 taught by Professor Pasternack during the Spring '08 term at Johns Hopkins.

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Experiment 6 - Experiment 6 Enthalpy of Vaporization of...

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