Question

During his or her lifetime, the average American uses approximately 795 kg of Cu in the form of coins, plumbing pipes, and electrical wiring. Most of this copper is obtained from sulfide ores, such as chalcocite, Cu2S. To obtain the copper metal, the chalcocite is first roasted (heated in the presence of oxygen), forming a copper oxide, Cu2O. The balanced reaction for this process is Cu2S + O2 → Cu2O + SO2 How many moles of O2 are needed to roast 10.0 mol of Cu2S? How many grams of SO2 are formed when roasting 10.0 mol of Cu2S? How many kilograms of O2 are required to form 2.68 kg Cu2S?

          During his or her lifetime, the average American uses
approximately 795 kg of Cu in the form of coins, plumbing pipes,
and electrical wiring. Most of this copper is obtained from sulfide
ores, such as chalcocite, Cu2S. To obtain the copper
metal, the chalcocite is first roasted (heated in the presence of
oxygen), forming a copper oxide, Cu2O. The balanced
reaction for this process is
                                                                                                                                     
Cu2S + O2 → Cu2O + SO2

How many moles of O2 are needed to roast 10.0 mol of Cu2S? How many grams of SO2 are formed when roasting 10.0 mol of Cu2S? How many kilograms of O2 are required to form 2.68 kg Cu2S?

Added by Chad A.

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