Lab Report #5

# Lab Report #5 - Determining an Empirical Formula(Lab#5...

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Determining an Empirical Formula (Lab #5) Jesse LaSalle TA: Jimmy Martin Experiment completed: October 18 th , 2007 Lab report submitted: October 25 th , 2007

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I) Purpose : The purpose of the experiment was to learn to determine the empirical formula of an unknown compound by combining weights. II) Procedure: Casey, J. and R. Tatz (2008). Determining an Empirical Formula. General Chemistry Laboratory Experiments , Hayden McNeil. Vol.1: 43-52. III) Data : (See attached Report Form) IV) Calculations : #4 Moles of copper in trial 1 = Moles of copper mass of copper samplemolar mass of copper = . . Mol Cu 1 1163g63 55g = . Mol Cu 0 01757 mol #7 Mass of Copper Sulfide product – Trial 1 = - Mass ofCopper Sulfide Avg mass of crucible and product Mass of crucible = . - . Copper Sulfide 17 0369g 15 6343g = . Copper Sulfide 1 4026g #8 Mass of sulfur in product – trial 1 = - Mass of sulfur Mass of copper sulfide mass of copper = . - . Sulfur 1 4026g 1 1163g = . Sulfur 0 2863g #9 Moles of sulfur in product –trial 1 = Moles of sulfur mass of sulfurmolar mass of sulfur = . . Mol S 0 2863g32 07g
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## This lab report was uploaded on 02/25/2008 for the course CHEM 121 taught by Professor Wyzlouzil during the Fall '07 term at Ohio State.

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Lab Report #5 - Determining an Empirical Formula(Lab#5...

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