Problem: For the reaction, Fe2O3 (s) + 3 H2(g) &lt;=&gt; 2 Fe(s) + 3 H2O(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?

FREE Expert Solution

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

Fe2O3 (s) + 3 H2(g) ↔  2 Fe(s) + 3 H2O(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:

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

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

Step 1: Calculate ΔS˚rxn.

Step 2: Calculate T when ΔG˚

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Problem Details

For the reaction, Fe2O3 (s) + 3 H2(g) <=> 2 Fe(s) + 3 H2O(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?