determination of chemical formula

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Date Performed: 2/25/2010 Name: Joe Staba Date Submitted: 3/4/2010 Name: Alyssa S. Instructor: Zhibing Xu Determination of a Chemical Formula Objective To determine the percentage composition and simplest formula for an oxide of copper by its reduction with methane gas (CH4) at approximately 500°C. This experiment is a study of stoichiometry. Experimental Data Mass of Test Tube = 20.002 ± .01g Mass of Test Tube + Copper Oxide = 22.258 ± .01g Mass of Copper Oxide = 2.256 ± .01g Sample Calculations Mass of Copper Oxide 22.258 ± .01g – 20.002 ± .01g = 2.256 ± .01g Uncertainty = √((.01)^2 + (.01)^2) = .01g Mass of Copper 21.805 ± .01g – 20.002 ± .01g = 1.803 ± .01g Uncertainty = √((.01)^2 + (.01)^2) = .01g Mass % Copper 1.803g Copper / 2.256g Copper Oxide (100) = 79.9% Copper Uncertainty = (Sr/.799)^2 = (.01/1.803)^2 + (.01/2.256)^2 = .006 Mass of Oxygen 2.256 ± .01g – 1.803 ± .01g = .453 ± .01g Uncertainty = √((.01)^2 + (.01)^2) = .01 Mass % Oxygen .453g Oxygen / 2.256g Copper Oxide (100) = 20.1% Uncertainty = (Sr/.201)^2 = (.01/.453)^2 + (.01/2.256)^2 = .005
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Moles of Copper 1.803g Copper / 63.55 g/mol Copper (molar mass) = .0284 mol Copper Uncertainty = (Sr/.0284)^2 = (.01/1.803)^2 + (.01/63.55)^2 = .0002 Moles of Oxygen .453g Oxygen / 16.0 g/mol Oxygen (molar mass) = .0283 mol Oxygen Uncertainty = (Sr/.0283)^2 = (.01/.453)^2 + (.01/16.0)^2 = .0006
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