We’re being asked to determine the standard free energy change (ΔG) for the reaction of 2.33 mol Fe3O4. The given reaction is:
Fe3O4(s) + 4 H2(g) → 3 Fe(s) + 4 H2O(g); ΔH˚ = 151.2 kJ, ΔS˚ = 169.4 J/K
In the balanced chemical equation, 1 mole of Fe3O4 reacts. We can calculate for ΔG˚ of 1 mole of Fe3O4 using the following equation:
For the reaction
Fe3O4 (s) + 4H2 (g) → 3Fe (s) + 4H2O (g)
ΔH° = 151.2 kJ and ΔS° = 169.4 J/K
The standard free energy change for the reaction of 2.33 moles of Fe3O4(g) at 311 K, 1 atm would be ___________ kJ.
This reaction is (reactant, product) ____________ favored under standard conditions at 311 K.
Assume that ΔH° and ΔS° are independent of temperature.
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