Butane Molar Mass Lab
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Introduction
Lab Partners Name Date November 8, 2009 Course Chemistry AP/IB Period 2 Butane's Molar Mass ABSTRACT Butane is a colorless gas with the molecular formula of C6H10 and is considered to be an Alkane. An Alkane is when the compound is formed by single bonds connecting the carbons and hydrogens. Butane was discovered by Dr. Walter Snellings in Pittsburg and he gas is used for cigarette lighters, heaters, stove fuels, and other heating appliances. The accepted value for the molar mass of butane is 58.124 g/mol. We tested the accepted value by calculating the molar mass of butane in a butane cigarette lighter. We took a beaker, and submerged it into water. Then we measured the mass of the cigarette lighter, and then slowly released butane gas bubbles into the beaker so that the bubbles collected at the top, where there was no air. We recorded the initial volume of water, then equalized the pressure inside and outside the beaker until the water levels inside and outside the beaker were the same. ...read more.
Middle
n = (0.976 atm)(0.0143 L) / (0.08206 Latm/molK)(295.65) n = 5.75e-4 n= PV/RT (Trial 3) n = (0.976 atm)(0.0158 L) / (0.08206 Latm/molK)(295.65) n = 6.356e-4 n= PV/RT (using averages) n = (0.976 atm)(0.0145 L) / (0.08206 Latm/molK)(295.65) n= 5.833e-4 Percent Error: The accepted value of the molar mass of butane is 58.124 g/mol. To calculate percent error: Trial 1: Difference between Calculated and Accepted values = 58.124 g/mol - 55.65 g/mol = 2.474 g/mol Trial 2: Difference between Calculated and Accepted values =58.124 g/mol - 69.53 g/mol = -11.406 g/mol Trial 3: Difference between Calculated and Accepted values = 58.124 g/mol - 47.20 g/mol = 10.924 g/mol Average: Difference between Calculated and Accepted values = 58.124g/mol - 56.57g/mol = 1.554g/mol CONCLUSION AND EVALUATIONS (CE) CONCLUDING - Determining the molar mass of butane through experimentation is possible with multiple trials. The more trials completed, the closer the average molar mass of butane is to the accepted value of the molar mass of butane. To determine the molar mass, take the mass of butane in the beaker and divide that by the number of moles of butane. ...read more.
Conclusion
Another systematic error that could have occurred is that the ambient room pressure was taken from a website dictating the pressure in the area, rather than directly in our room. The measurements in the lab are reliable taking into consideration the equipment windows of error and there are few to no flaws and weaknesses in the procedure itself. IMPROVING THE INVESTIGATION - The experiment could have been improved by measure the atmospheric pressure directly in the room, obtaining a more accurate room pressure to ensure that the pressure of butane was calculated correctly. Other improvements may include more accurate equipment such as a balance, beaker, and thermometer. Also, the butane used in the experiment could have been certified as pure butane, rather than butane from a common lighter. APPENDICES - "Cornellbiochem - Butane." Cornellbiochem - home. Web. 08 Nov. 2009. Brown, Theodore L., H. Eugene LeMay Jr., Bruce E. Bursten, and Catherine J. Murphy. Chemistry The Central Science; AP Edition. 10th ed. Upper Saddle River: Prentice Hall College Div, 2005. Print. ?? ?? ?? ?? 1 ...read more.
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