Oxidation and Reduction Reactions: the Reactions of Copper
Week 10: Oxidation and Reduction Reactions: The Reactions of Copper
Data:
Part I: Preparing a solution of copper (II) nitrate Initial mass of copper wire: .520g Mass of copper wire after vigorously scouring: .518g Observations of Copper (II) ribbon mixed with HNO3: Solution turned green. Thick brown gas formed. Copper (II) bubbled vigorously. Cu (II) dissolved, solution appeared green/blue. After the addition of H2O a blue crusty precipitate formed.
Part II: Synthesis of solid copper (II) hydroxide Observations of Copper (II) nitrate when added to sodium hydroxide: a precipitate formed. The precipitate was cloudy and turned dark.
Part III: Formation of Copper oxide Observations of Copper (II) hydroxide when heated: Copper (II) hydroxide when heated turned very dark. It turned dark blue and had black specks floating around in the solution. After being heated for a time the aqueous solution turned gray and a black precipitate was formed.
Part IV: Formation of copper (II) sulfate Observations of copper (II) oxide when reacted with 6mL of 3 Moles of Sulfuric acid: the black precipitate disappeared. The resulting solution turned blue
Part V: Formation of copper metal Weight of Zn added: 1.107g *The professor also added some mossy Zinc. Weight unknown. Observations of copper (II) sulfate when 1.107g of Zinc was added: The solution turned from blue to cloudy dark blue-ish. With continued stirring it turned a dark red-brown. The reaction was not happening properly, so the professor added a small pinch of mossy Zinc.
Part VI: Recovery of copper metal Weight of dry casserole dish: 59.608g Weight of cooled casserole dish with dried copper metal: 60.645g Weight of Copper metal: 1.037g
Data Analysis: I: Balanced Chemical Reactions 1. Formation of copper nitrate from copper wire using concentrated nitric acid: Cu(s) + HNO3(aq) = Cu(NO3)2 + NO2 + H2O(l) + 2. Reaction of copper nitrate and sodium
Data:
Part I: Preparing a solution of copper (II) nitrate Initial mass of copper wire: .520g Mass of copper wire after vigorously scouring: .518g Observations of Copper (II) ribbon mixed with HNO3: Solution turned green. Thick brown gas formed. Copper (II) bubbled vigorously. Cu (II) dissolved, solution appeared green/blue. After the addition of H2O a blue crusty precipitate formed.
Part II: Synthesis of solid copper (II) hydroxide Observations of Copper (II) nitrate when added to sodium hydroxide: a precipitate formed. The precipitate was cloudy and turned dark.
Part III: Formation of Copper oxide Observations of Copper (II) hydroxide when heated: Copper (II) hydroxide when heated turned very dark. It turned dark blue and had black specks floating around in the solution. After being heated for a time the aqueous solution turned gray and a black precipitate was formed.
Part IV: Formation of copper (II) sulfate Observations of copper (II) oxide when reacted with 6mL of 3 Moles of Sulfuric acid: the black precipitate disappeared. The resulting solution turned blue
Part V: Formation of copper metal Weight of Zn added: 1.107g *The professor also added some mossy Zinc. Weight unknown. Observations of copper (II) sulfate when 1.107g of Zinc was added: The solution turned from blue to cloudy dark blue-ish. With continued stirring it turned a dark red-brown. The reaction was not happening properly, so the professor added a small pinch of mossy Zinc.
Part VI: Recovery of copper metal Weight of dry casserole dish: 59.608g Weight of cooled casserole dish with dried copper metal: 60.645g Weight of Copper metal: 1.037g
Data Analysis: I: Balanced Chemical Reactions 1. Formation of copper nitrate from copper wire using concentrated nitric acid: Cu(s) + HNO3(aq) = Cu(NO3)2 + NO2 + H2O(l) + 2. Reaction of copper nitrate and sodium