Use the data shown below, to calculate ∆H°rxn, ∆S°rxn, and ∆G°rxn at 25°C for the following reaction: 3 H₂(g) + Fe₂O₃(s) → 2 Fe(s) + 3 H₂O(g) What is the value of ∆G°rxn at 25°C? Question 3 of 9Use the data shown below, to calculate AH°rxn, AS°rxn, andAG°xn at 25°C for the following reaction:3 H2(g) + FeżO3(s) → 2 Fe(s) + 3 H2O(g)What is the value of AG°rxn at 25°C?14SebstanceHOlg)-241.8Fels)*24.287.40130.727287.| +/-

The balanced reaction taking place is given as, => 3 H2 (g) + Fe2O3 (s) -------> 2 Fe (s) + 3 H2O (g) The enthalpy change for any reaction is given by, => ΔHo = sum of (ΔHof products X reaction coefficient of products) - sum of (ΔHof reactants X reaction coefficient of reactants) Hence for the above reaction, the ΔHo is given by, => ΔHo = ΔHof {Fe (s)} X 2 + ΔHof {H2O (g)} X 3 - [ ΔHof {Fe2O3 (s)} X 1 + ΔHof {H2 (g)} X 3 ] Hence substituting the values we get, => ΔHo = 0 X 2 + 3 X (-241.8) - [-824.2 X 1 + 0 X 3] = 98.8 KJ/mol = 98800 J/mol (since 1 KJ = 1000 J) Similarly, the entropy change for any reaction is given by, => ΔSo = sum of (Sof products X reaction coefficient of products) - sum of (Sof reactants X reaction coefficient of reactants) Hence for the above reaction, the ΔHo is given by, => ΔSo = Sof {Fe (s)} X 2 + Sof {H2O (g)} X 3 - [ Sof {Fe2O3 (s)} X 1 + Sof {H2 (g)} X 3 ]Hence substituting the values we get, => ΔSo = 27.28 X 2 + 3 X 188.8 - [87.4 X 1 + 130.7 X 3] = 141.46 J/mol.K Hence the Gibbs free energy change of the reaction is given by, => ΔGo = ΔHo - TΔSo T = temperature of reaction in K = 273 + 25 = 298 K Hence substituting the values we get, => ΔGo = 98800 - 298 X 141.46 = 56645 J/mol = 56.645 KJ/mol approx.