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Lab Experiment 1 9-11-07 - Ch 200-42 Experiment one Proving...

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9-7-07 Ch 200-42 Experiment one Proving Dalton’s Law of Proportions Experiment one:
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Purpose: The purpose is to validate Dalton’s law of proportions in part one and further back up our findings through experimentation in part two. Data and Calculations: 1. Mass of magnesium: .15g 2. Mass of magnesium oxide formed: .24g 3. Mass of oxygen from the air: .09g 4. Moles of Mg: .15g Mg /24.31g Mg = .006 Mol Mg. Moles of O: .09g O/16g O= .0056 Mol O. Closest whole number ratio is 1:1 5. Chemical Formula for Magnesium oxide is MgO 6. 2Mg+O 2 -- 2MgO Percent Error: ((.006-.0056)/.006)*100= 6.66% error Part II: 1. Mass of hydrated copper (II) sulfate: 5.53g 2. Mass of anhydrous copper (II) sulfate: 3.65g 3. Mass of lost water: 1.88g 4. Moles of CuSO 4 : 3.65g/159.62= .022 Mol. Moles of H 2 O: 1.88g/18.01= .104 Mol. 5. Moles of H 2 O per mole of CuSO 4 = 5 Formula for copper (II) sulfate hydrate: CuSO 4 *5H 2 O 6. CuSO 4 *5H 2 O CuSO 4 + 5 H 2 O Error:
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Possible sources of error come from random and systematic sources. Random sources include the inclusion of other particles while performing the experiment. Systematic may include
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