Chemical Reactions of Copper Compounds

Chemical Reaction of copper compounds

Introduction:

In this experiment, the objective was to conduct a series of chemical reactions that contain copper or copper compounds. That is to say that the products of each chemical reaction were used in the next reaction. The process starts with a solid copper wire dissolved in nitric acid and the end product is copper powder. The product which was used from the previous reaction is the limiting. In the initial step, the solid copper is the limiting reactant. For this experiment, the materials that will be used are copper wire, aluminum wire, six molar nitric acid, sodium hydroxide, six molar hydrochloric acid, a vacuum filtration apparatus, and ice.

Experimental Procedures:

1. First the copper wire that is twenty four gauge must be cut to approximately 40 cm. Take steel wool and scrape of all impurities off the wire to get pure copper, and weigh. Acquire a two hundred fifty milliliter beaker and put the copper wire in the beaker. Slowly add twenty milliliters of six molar nitric acid to the beaker. For best results cut the copper wire into tiny piece before adding the nitric acid. Place the beaker in fume hood for approximately twenty minutes. If the copper has not completely reacted with the nitric acid; heat the beaker to speed up the reaction. This reaction is represented by the equation: Cu (s) + 4 HNO3 (aq)  Cu(NO3)2+2NO2 (g) +2H2O (l) this reaction resulting in a blue liquid and brown gas that has the odor of chlorine.

2. For step two have a four hundred milliliter beaker filled with three hundred milliliters of ice water. Place the beaker from step one into the beaker with ice water. Twenty two milliliters of six molar sodium hydroxide will slowly be added to the first beaker which contains copper (II) nitrate and water. This reaction is represented by equation: Cu(NO3)2 (aq) + 2NaOH (aq) CuOH2(s) +2NaNo3 (aq). The copper (II) hydroxide is royal blue in color.

3. In the beaker from the previous step slowly add fifty milliliters of distilled water. After adding the water heat the beaker until the copper (II) hydroxide turns into copper (II) oxide. The presence of copper (II) oxide is determined if the reaction forms a black liquid.

4. Using the copper (II) oxide from the previous step add twenty five milliliters of six molar hydrochloric acid to form copper (II) chloride. By adding the hydrochloric acid the black liquid turns into an emerald green liquid.

5. Twist one hundred forty centimeters of aluminum wire into a coil then weigh. Add this to the copper(II) chloride formed from the previous step. This results in a violent reaction with the copper(II) chloride and the aluminum. This reaction forms copper powder and aluminum chloride. The copper powder is the reddish powder in the bottom of the beaker. When the reaction is done; drain of the liquid, and wash the solid with twenty five milliliters of distilled water. After the