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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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- Spring '10
- Erlenmeyer flask, Average Percent Bicarbonate