In this experiment, copper (II) oxide is reacted with hydrochloric acid. Sulfuric acid can be used instead of hydrochloric acid. Write the balanced chemical equation, including states, for this reaction. In this experiment, copper chloride is reduced by zinc. Referring to the activity series of metals (see Appendix), all metals "above" copper in the series will reduce the copper chloride to copper. Aluminum is one of these metals. Write the balanced chemical equation, including states, for this reaction. In this experiment, the excess zinc is oxidized and made aqueous with the addition of hydrochloric acid. Other strong acids, such as cold sulfuric acid, may be used in this step, but warm nitric acid cannot be used. Why and what impact would this have on the percent recovery if warm nitric acid was used?
