Assuming that you could look up a table of standard molar enthalpies of formation and entropies of the reactants and products, and that the reactions are correct, you could calculate values of ΔH° and ΔS° for the reactions at standard conditions. Then you could calculate the temperature for which ΔG° is zero, meaning that the reaction will be at least at equilibrium. A negative value of ΔG° means that the reaction will proceed in the forward direction.
The formula relating ΔG° to ΔH° and ΔS° is: ΔG° = ΔH° - TΔS°, where T is temperature in Kelvin.