We’re being asked to determine the **equilibrium constant (K)** at **298 K** for the given reaction:

Fe_{2}O_{3} _{(s)} + 3 H_{2}_{(g)} ↔ 2 Fe_{(s) }+ 3 H_{2}O_{(g)}

We’re given the **ΔH˚ and ΔG˚** of each reactant and product:

**ΔH˚ = 100 kJ**

** ΔG**˚ = 63 kJ

We can use the following equation to solve for ** ΔG˚_{rxn}**:

$\overline{){\mathbf{\Delta G}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{\Delta H}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{-}}{\mathbf{T\Delta S}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}}$

For this problem, we need to do the following steps:

*Step 1:* Calculate ΔS˚_{rxn}.

*Step 2:* Calculate T when **ΔG**˚

For the reaction, Fe_{2}O_{3} (s) + 3 H_{2}(g) <=> 2 Fe(s) + 3 H_{2}O(g), ΔG° = 63 kJ at 25 °C and ΔH° = 100 kJ. Which of the following is completely true about the relationship between ΔG and T for this reaction?

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