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:
For this problem, we need to do the following steps:
Step 1: Calculate ΔS˚rxn.
Step 2: Calculate T when ΔG˚
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?
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