Determining the Molar Volume of Carbon Dioxide PDF

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Determining the Molar Volume of Carbon Dioxide

Purpose of the lab: To determine the molar volume of an ideal gas, by sublimating a sample of dry ice and measuring the carbon dioxide collected. Fundamental principle or theory behind the experiment: According to Avogadro’s law we know that one mole of any gas should have the same volume at STP, 22.4 L/mol. The brief procedure(s) or method(s) to reach the goal of the experiment: First we took two empty flasks, plugged them with stoppers and weight them in order to get their mass. We then took two pieces of dry ice and put one in each flask. Next we waited until the entire piece of dry ice sublimated in the flask. We then promptly plugged the flasks with their respective stoppers, and took the mass of each flask once again (this time the flasks were filled with CO₂). Using those two masses we calculated the volume of the CO₂ at STP in L/mol, and then took the average of those two measurements which gave us an average volume of 25.2 L/mol. We then found the percent error of our findings to the excepted volume of an ideal gas of 22.4 L/mol. Our error was 12.5%, not as good of a result as could be hoped for. Please see attached Data Sheet for any findings and measurements. Discussion regarding possible experimental errors: There are a few errors that could have occurred:  

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Since the stoppers do not weight the same, it was important not to switch which stopper went with which flask, that could cause a huge error in our end measurements. While doing the experiment it was important not to close the flask with the stopper until the entire piece of dry ice had vaporized completely. If the stopper was plugged earlier than that, the flask would weight more than it should since we would have more sample of dry ice and carbon dioxide in it. Also, we are comparing our results with the ideal results of a gas at STP. There is a possibility that the pressure might have been slightly lower on the day of our experiment. Since pressure and volume are inversely proportional, this might explain why our volume was slightly higher that the excepted amount.

Conclusion: Although our results were not as good as I would have liked them to be, I believe this was due to the slight variation of our variables (temperature and pressure), since we were

very careful and diligent when doing the experiment. I would have liked to have known the exact temperature and pressure of the room in order to make the best calculations possible. Overall, if all the information for the experiment is correct, I think this is a very good way to determine the molar volume of an ideal gas....