If \( \Delta \mathrm{G}=-177 \mathrm{kcal} \) for (I) \( 2 \mathrm{Fe}(\mathrm{s})+\frac{3}{2} \...

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If \( \Delta \mathrm{G}=-177 \mathrm{kcal} \) for
(I) \( 2 \mathrm{Fe}(\mathrm{s})+\frac{3}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}(\mathrm{~s}) \)
and \( \Delta \mathrm{G}=-19 \mathrm{kcal} \)
- (II) \( 4 \mathrm{Fe}_{2} \mathrm{O}_{3} \) (s) \( +\mathrm{Fe} \) (s) \( \longrightarrow 3 \mathrm{Fe}_{3} \mathrm{O}_{4} \) (s)
-What is the Gibbs free energy of formation of \( \mathrm{Fe}_{3} \mathrm{O}_{4}(\mathrm{~s}) \) ?
(a) \( +229.6 \mathrm{kcal} / \mathrm{mol} \)
(b) \( -242.3 \mathrm{kcal} / \mathrm{mol} \)
(c) \( -727 \mathrm{kcal} / \mathrm{mol} \)
(d) \( -229.6 \mathrm{kcal} / \mathrm{mol} \)
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