Consider the stepwise reduction of iron oxide: (1) kJ. (2) kJ. What is the enthalpy change for the target reaction: ?

Question

Consider the stepwise reduction of iron oxide: (1) $Fe_2O_3(s) + 3CO(g) \rightarrow 2Fe(s) + 3CO_2(g), \Delta H_1 = -26.8$ kJ. (2) $FeO(s) + CO(g) \rightarrow Fe(s) + CO_2(g), \Delta H_2 = -16.5$ kJ. What is the enthalpy change for the target reaction: $Fe_2O_3(s) + CO(g) \rightarrow 2FeO(s) + CO_2(g)$?

Prashant Kotian · Accepted Answer

Correct answer: A. Apply Hess's Law. Reverse equation 2 and multiply by 2: ( kJ). Add this to equation 1: . Net: . kJ.

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