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Copper has been used for thousands of years, either as a pure metal or in alloys....

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Chemistry

Copper has been used for thousands of years, either as a puremetal or in alloys. It is frequently used today in the productionof wires and cables. Copper can be obtained through smelting orrecycling. Determine the energy associated with each of theseprocesses in order to recycle 1.43 mol Cu. The smelting of copperoccurs 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 recyclingcopper is simplified to just the melting of the solid Cu startingat 25°C. The melting point of Cu is 1084.5°C with ΔH°fus = 13.0kJ/mol and a molar heat capacity, cP,Cu = 24.5 J/mol·°C. What isthe enthalpy change for the reaction recovering Cu from CuO?

Answer & Explanation Solved by verified expert
4.3 Ratings (746 Votes)

CuO(s)+CO(g) -----> Cu(s)+CO2​(g)

DHrxn = (1*DH0F,Cu(S) + 1*DH0F,CO2(g)) - (1*DH0F,CuO(s) + 1*DH0F,CO(g))

      = (1*0 + 1*-393.5)-(1*-155+1*-110.5)

      = -128 Kj/mol

heat required to melt(q) = n*Cp*DT + n*DHfus

                         = 1.43*24.5*(1084.5-25)+1.43*13*10^3

                         = 55.71 kj

total enthalpy change during the process (DH) = n*DHrxn + q

                                              = 1.43*-128 + 55.71

                                              = -127.33 kj
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