Lab 5 Discussion

Lab 5 Discussion - not totally balanced it correctly. In...

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In part one, we set up the apparatus as we were told. By following the procedure, we equlatized the pressure inside and ouside of the flasks. Then we spilled the catalyst into the peroxide solution contained in the flask. Then we placed this into water to equlibriate the temperature of the flasks. It turned out that heat was absorbed in this reaction. Then we were able to measure the amount of oxygen produced because it equaled the displacement of water. The balanced equation for part one is 2H2O(g) ->2H2O(l)+O2(g). Our results for the molar volume of O2 were 32.19L/m. This value was pretty close to the expected value. However, the minor difference may be accounted for because we had trouble in the beginning balancing the pressure inside and outside the flask and may have
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Unformatted text preview: not totally balanced it correctly. In the end, it all turned out to work out though. In part two we wanted to find the molar volume of Hydrogen. We followed to same steps as we did in part one, and eventually found out that H2 had a molar volume of 26.27L/m. The balanced equation for part two is Mg(s)+2HCl(aq)->MgCl2(aq)+H2(g). This value was also very close to our expected value, and since we had already gone through those steps, I felt we were able to do part two with much more efficiency and accuracy, even though there may have been minor errors such as in balancing the pressure and possibly skewing the temperature reading by not being very careful with the thermometer....
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This note was uploaded on 04/09/2008 for the course CHEM 1AL taught by Professor Hooker during the Fall '07 term at UCSB.

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