For the reaction:
3Fe(s)+2O2(g)→Fe3O4(s)3Fe_{(s)} + 2O_2{(g)} \rightarrow Fe_3O_4{(s)}3Fe(s)+2O2(g)→Fe3O4(s)
ΔH=−1650 kJ mol−1\Delta H = -1650\,\text{kJ mol}^{-1}ΔH=−1650kJ mol−1, ΔS=−600 J K−1mol−1\Delta S = -600\,\text{J K}^{-1} \text{mol}^{-1}ΔS=−600J K−1mol−1 at 300 K300\,\text{K}300K. What is the value of free energy change for the reaction at 300 K300\,\text{K}300K?