Problem: Copper has been used for thousands of years, either as a pure metal or in alloys. It is frequently used today in the production of wires and cables. Copper can be obtained through smelting or recycling. Determine the energy associated with each of these processes in order to recycle 1.23 mol Cu. The smelting of copper occurs by the balanced chemical equation:CuO(s) + CO(g) ---> Cu(s) + CO2(g)where ΔH°f,CuO is = –155 kJ/mol. Assume the process of recycling copper is simplified to just the melting of the solid Cu starting at 25°C. The melting point of Cu is 1084.5°C with ΔH°fus = 13.0 kJ/mol and a molar heat capacity, cP,Cu = 24.5 J/mol·°C.Enthalpy change for the reaction recovering Cu from CuO(in kJ)Energy for recycling Cu (in kJ)

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We are being asked to determine the energy associated with each of these processes in order to recycle 1.23 mol Cu


Recall that ΔH˚rxn can be calculated from the enthalpy of formation (ΔH˚f) of the reactants and products involved:

 ΔH°rxn = ΔH°product - ΔH°reactant



Part A. Smelting of copper


The reaction for the smelting of copper:

CuO(s) + CO(g) ---> Cu(s) + CO2(g)


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Problem Details

Copper has been used for thousands of years, either as a pure metal or in alloys. It is frequently used today in the production of wires and cables. Copper can be obtained through smelting or recycling. Determine the energy associated with each of these processes in order to recycle 1.23 mol Cu. The smelting of copper occurs by the balanced chemical equation:

CuO(s) + CO(g) ---> Cu(s) + CO2(g)

where Δf,CuO is = –155 kJ/mol. Assume the process of recycling copper is simplified to just the melting of the solid Cu starting at 25°C. The melting point of Cu is 1084.5°C with ΔH°fus = 13.0 kJ/mol and a molar heat capacity, cP,Cu = 24.5 J/mol·°C.

Enthalpy change for the reaction recovering Cu from CuO(in kJ)

Energy for recycling Cu (in kJ)

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