Lab 6 lab report - Matthew Mueller Sept. 28, 2007 CHEM...

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Matthew Mueller Sept. 28, 2007 CHEM 207-01A THE COPPER CYCLE Objective This experiment involved the stepwise conversion of copper solid into various copper compounds, and eventually back to a copper solid. Part A – Oxidation Reduction Reaction Cu (s) + 4HNO 3(aq) Cu(NO 3 ) 2(aq) + 2H 2 O (l) + 2NO 2(g) Compound Amount M.W. Moles Other Cu 1.003 g 63.55 gmol 1.578 × 10 -2 mol N/A HNO 3 15 mL (concentrated) 63.02 gmol corrosive Procedure Observations 1. Weigh out about one gram of copper wire (approx. 30 1-cm strips), record mass, and put the copper in a 250 mL Erlenmeyer flask. Mass of Cu (s) = 1.003 g 2. In the fume hood carefully add 15 mL of concentrated nitric acid (HNO 3 ). Place the flask on a hot plate and heat till the copper is dissolved. (Add more nitric acid if it evaporates before all the copper has dissolved. -Copper dissolves into an initially green and eventually blue solution. -A brown gas is given off from the solution as the copper dissolves. 3. Take the flask off the hot plate after all the copper had
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dissolved and cool. Part B – Precipitation Reaction Cu(NO 3 ) 2(aq) + 2NaOH (aq) Cu(OH) 2(s) + 2NaNO 3(aq) Compound Amount M.W. Moles Other NaOH 30 mL (6 M) 40.00 gmol 0.18 mol Cu(NO 3 ) 2 187.57 gmol Procedure Observations 1. Add 40 mL of DI water to the solution of copper (II) nitrate. 2.
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This lab report was uploaded on 04/08/2008 for the course CHEM 207 taught by Professor Richardson during the Fall '08 term at University of Louisville.

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Lab 6 lab report - Matthew Mueller Sept. 28, 2007 CHEM...

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