# Gas Laws - check it thoroughly because as our data will...

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Lauren Beauchamp Lab Partners: Jessica Tarver and Rachel Harp Gas Laws Due: April 13, 2010 1. The Procedure For this procedure we weighed out samples of the bicarbonate tablets to be under or at .17 grams, so that we would not create too much gas that we could not measure. We then assembled an apparatus that used flexible tubing to connect a reservoir, Buret, and an Erlenmeyer flask. The Buret was filled with water, and held level with the reservoir at all the times. Then using a piece of string we suspended the bicarbonate tablets in the Erlenmeyer flask that also had water in it. We suspended the tablet, because as soon as it made contact with the liquid it would begin the reaction. Then the carbon dioxide was measured using the buret. We did this reaction a total of three times. 2. Gas Leaks Gas leaks could be a disaster in this experiment. Each group should have made sure the top on the Erlenmeyer flask was firmly secured and that nothing could get out. However, my group did not

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Unformatted text preview: check it thoroughly because as our data will show, there was a small leak. 3. Experimental Results Trial One (mL of gas) 3.85 mL Trial Two (mL of gas) 1.94 mL Trial Three (mL of gas) 1.51 mL Average Percent Bicarbonate (using the formula PV=nRT) 4% Class Average Percent Bicarbonate 19.738% Standard Deviation of Class 13.67583 Group Standard Deviation 1.30512 Group Percent Error 79.73% 4. Wet Sample If the tablets had been in high humidity the measured carbon dioxide would be much less. This is because the bicarbonate reacts very quickly with water. If there was a lot of humidity in the air the reaction would have already part way occurred. 5. Partial Pressure of Water Because we used Dalton’s Law which states: P Total = P Water + P Carbon Dioxide If we had ignored the partial pressure of water then the answer would have decreased when we used P Total in the equation PV=nRT....
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