$\mathbf{\Delta G}{\mathbf{\xb0}}_{\mathbf{rxn}}\mathbf{}\mathbf{=}\mathbf{}\mathbf{G}{\mathbf{\xb0}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{products}}\mathbf{}\mathbf{-}\mathbf{G}{\mathbf{\xb0}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{reactants}}\phantom{\rule{0ex}{0ex}}\mathbf{\Delta G}{\mathbf{\xb0}}_{\mathbf{rxn}}\mathbf{}\mathbf{=}[G{\xb0}_{f,\mathrm{Fe}\left(s\right)}+G{\xb0}_{f,{H}_{2}O\left(g\right)}]\mathbf{}\mathbf{-}\mathbf{}\mathbf{[}\mathbf{G}{\mathbf{\xb0}}_{\mathbf{f}\mathbf{,}\mathbf{}{\mathbf{Fe}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{3}}\mathbf{}\mathbf{\left(}\mathbf{s}\mathbf{\right)}}\mathbf{}\mathbf{+}\mathbf{}\mathbf{G}{\mathbf{\xb0}}_{\mathbf{f}\mathbf{,}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{}\mathbf{\left(}\mathbf{g}\mathbf{\right)}}\mathbf{]}\phantom{\rule{0ex}{0ex}}$

Consider the reaction

Fe_{2}O_{3} (s) + 3H_{2} (g) → 2Fe (s) + 3H_{2}O (g)

a. Use ΔG°_{f} values in Appendix 4 to calculate ΔG° for this reaction.

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