i need help for the three questions

Use the References to access important values if needed for this question. A student determines the value of the equilibrium constant to be 1.10106 for the following reaction. 3Fe2O3(s)+H2(g)2Fe3O4(s)+H2O(g) Based on this value of Keq : G for this reaction is expected to be than zero. Calculate the free energy change for the reaction of 2.17 moles of Fe2O3(s) at standard conditions at 298K. Grxn= A student determines the value of the equilibrium constant to be 7.901037 for the following reaction. H2S(g)+2H2O(l)3H2(g)+SO2(g) Based on this value of Keq : G for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 2.23 moles of H2S(g) at standard conditions at 298K. Grxn0=kJ A student determines the value of the equilibrium constant to be 2.011018 for the following reaction. N2(g)+2O2(g)2NO2(g) Based on this value of Keq : G for this reaction is expected to be (greater,less) than zero. Calculate the free energy change for the reaction of 2.11 moles of N2(g) at standard conditions at 298K. Gxn=