Data Analysis

1)

A. Due to the fact that CuO is not reactive with HCl, but copper is, adding 50 mL HCl to our beaker of 0.99 g of CuO showed us that unconverted Cu formed at the bottom of the beaker; therefore, the primary reaction was incomplete.

B. It is a possibility that by exposing more of the copper to oxygen, a better reaction would have happened and more copper oxide would have formed.

2)

A. Although we thought all 0.99 grams of powdered copper reacted when we heated it, retrieving the unconverted Cu, we discovered that in actuality, 0.33 g reacted.

B. 0.33/0.99 x 100% = 33%

33% of the total copper sample reacted when heated.

3)

A. Zn: + Cu^2+ → Zn^2+ + Cu:

B.

§  Zn was oxidized

§  II. Cu was reduced

§  III. Zn is the reducing agent

§  IV. Cu is the oxidizing agent

4)

A. The zinc became kind of brick color, and began to crust and crumble.

B. The reasoning behind this is because zinc is more reactive than copper; thus, the zinc caused copper to reduce as it oxidized.

C. When the color of the solution was fairly clear, it was an indication that the Cu2+ ions in the solution had reduced into solid Cu the zinc had oxidized.

5)

A. The resources used in the recovery process were Cu2+ and Zn.

B. Cu2+ reduced to Cu, and Zn oxidized to Zn2+ within the solution.