Consider the reduction of copper and iron from their respective ores. By definit

Question

Consider the reduction of copper and iron from their respective ores. By definition, the enthalpies of these processes equal the negative of their enthalpies of formation. Calculate the enthalpy of the reaction in which 1.00 g of the pure metals are formed from their respective ores. Given your result, would you expect the price that recycling operators are willing to pay for scrap iron per kilogram to be greater or less than that for scrap copper? deltaH^degree_f(CuFeS_2)=-173^kJ/mol deltaHdegree_f(Fe_2O_3)=-824^kJ/mol

Explanation / Answer

enthalpy of reaction of CuFeS2 = -173/183.5 = -0.943 KJ/g

enthalpy of reaction of Fe2O3 = -824/160 = -5.15 kJ/g

Since energy required for the extraction of of Cu is greater than that of Fe, recycling Fe is cheaper than recycling Cu.

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