A chemist went on a trip to Zambales to obtain a sample of chalcocite (copper (I) sulfide), one of the most important ores of copper. He tried to extract copper from the ore by performing these 2 steps: 1st step: After grinding, the chemist “roasted” (reacted with oxygen gas in the presence of heat) the powdered chalcocite sample to form a red cuprous oxide precipitate and gaseous sulfur dioxide. 2nd step: He then reacted the red precipitate with hydrogen gas inside a heated furnace to produce metallic copper and water vapor. 3rd step: Out of curiosity, the chemist tried to heat the metallic copper product in a hotplate. This yielded a different oxide of copper. Write the balanced chemical equation for this reaction (3rd step only) and identify the type of reaction.

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