We are asked to calculate the value of ΔH˚ for 4 FeO(s) + O_{2}(g) → 2 Fe_{2}O_{3}(s)

$\overline{){\mathbf{\Delta H}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{\Delta H}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{product}}{\mathbf{-}}{\mathbf{\Delta H}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{reactant}}}$

Note that we need to *multiply each ΔH˚ by the stoichiometric coefficient* since ΔH˚ is in kJ/mol.

Balanced reaction : 4 FeO(s) + O_{2}(g) → 2 Fe_{2}O_{3}(s)

You may want to reference (Pages 187 - 190) Section 5.7 while completing this problem.

Using values from Appendix C, calculate the value of ΔH˚ for each of the following reactions.

4 FeO(s) + O_{2}(g) → 2 Fe_{2}O_{3}(s)

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