3) The following “cycle of copper†experiment is performed insome general chemistry laboratories. The series of reactions startswith copper wire and ends with metallic copper. The steps are asfollows:
I. A piece of copper wire of known mass is allowed to react withconcentrated nitric acid, the products are copper(II) nitrate ,nitrogen dioxide, and water.
II. The copper(II) nitrate is treated with a sodium hydroxidesolution to form copper(II) hydroxide.
III. On heating, the copper(II) hydroxide decomposes to yieldcopper(II) oxide.
IV. The copper(II) oxide is combined with concentrated sulfuricacid to yield copper(II) sulfate.
V. Copper(II) sulfate is treated with excess solid zinc metal toform metallic copper.
VI. The remaining zinc metal is treated with hydrochloric acid,and metallic copper is filtered, dried, and weighed.
a. Write a balanced chemical equation for each step. Be sure topay attention to phase labels.
b. Classify each reaction as a precipitation, acid-base, orredox reaction.
c. Assuming that a student started with 65.6 g of copper,calculate the theoretical yield for each step
