Copper Cycle Essay

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The Copper Cycle Chem 111-62 Jamie Kichler w/ Clara Lenhart and Anna F Purpose: The purpose of this experiment is to help us become more comfortable in the lab with dangerous solutions and practice safety precautions. It is also to help us identify and make the connection between the reactions we see and the reactions we write on paper. Procedure: Please refer to pages 33-35 in our laboratory manual. No modifications were made. Experimental results: Reaction 1: Metallic Copper with Nitric Acid Cu(s) + 4HNO3(aq) Cu(NO3)2(aq) +2NO2(g) + 2H2O(l) Net ionic: Cu(s) + 4H+(aq) + 2NO3- (aq) 2NO2 (g) + Cu2+ (aq) + 2H2O(l) Type of Reaction: Redox Reaction: Copper loses electrons and is oxidized to copper (II) ion. Nitrogen gains electrons from the copper ion, and is reduced to nitrogen dioxide gas. Nitric acid is an oxidizing agent. Copper is the reducing agent. Observations: * Solution turns green and bubbles * Warm to the touch * Brown gas produced * Copper Dissolves Reaction 2: Copper (II) Nitrate with Sodium Hydroxide Cu(NO3)2(aq) + 2NaOH(aq) Cu(OH)2(s) + 2NaNO3(aq) Net ionic: Cu2+(aq) + 2OH-(aq) Cu(OH)2(s) Type of Reaction: Precipitate Reaction Observations: * With addition of water, the solution becomes blue, thick, and slime-like * When added to litmus paper, paper turns dark blue * Dark blue shows that the solution is basic Reaction 3: Heating Copper Cu(OH)2(s) CuO(s) + H2O(l) Net ionic: Cu(OH)2(s) CuO(s) + H2O(g) Type of Reaction: Redox Reaction: Cu is oxidized from 2- to 2+. The reducing agent is Cu(OH)3 Observations: * While heating and stirring, solution turns greyish blue, then becomes black * Cool water mixes, solution settles to the bottom * *NOT ALL WATER WAS POURED OFF Reaction 4: Copper (II) Oxide with Sulfuric Acid CuO(s) + H2SO4(aq) CuSO4(aq) +

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