Here's what I could understand from your question...
We start with a balanced chemical equation
2NO_((g)) + O_(2(g)) -> 2NO_(2(g))2NO(g)+O2(g)→2NO2(g)
The values given to you correspond to the standard enthalpy of formation (DeltaH_f^@, NOT DeltaH), the standard molar entropies (S^@, NOT DeltaS), and the standard Gibbs free energies of formation (DeltaG^@, NOT DeltaG). You can check all these values here:
http://en.wikipedia.org/wiki/List_of_standard_Gibbs_free_energies_of_formation
http://www.mrbigler.com/misc/energy-of-formation.PDF
This being said, the values for O_2's standard enthalpy of formation, standard molar entropy, and standard Gibbs free energy are:
DeltaH_f^@ = 0 (kJ)/(mol); S^@ = 205 J/(K * mol); DeltaG^@ = 0 (kJ)/(mol)
You could however calculate the values of DeltaH, DeltaS, and DeltaG for this reaction starting from these values.
