Here's what I could understand from your question...
We start with a balanced chemical equation
#2NO_((g)) + O_(2(g)) -> 2NO_(2(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.
