text: free energy? ok, here is the problem... as shown in the equation below, nitrogen oxide, no, is common pollutant that is produced by the reaction of nitrogen and oxygen gases. since these gases are the major components of air, nitrogen oxideresults when air is heated in furnaces, motor engine cylinders, or other high temperature combustion areas.         n2 (g) + o2 (g)  2 no (g)  a. given that the standard enthalpy of formation for no2 (g) is 90.25 kj/mole and using the absolute entropies listed below, calculate the free energy change for this reaction at 25 degrees celcius. is this reaction product favores at 25 degrees celcius?                      absolute entropies n2 (g)  191.5 j/mol times k       o2 (g) 205.0 j/mole times k no (g)  210.7 j/mol times k  b. if the reaction is not product-favored at 25 degrees celcius, determine under what conditions it would be product favored.  show all work.  thanks for any help i can get! a.  free energy = δg  entropy change = δs°  δs° = δs products - δs reactants  δs° = 24.9  δg° = δh° - tδs° δg° = (90.25x1000) - (25+273.15)x24.9 δg° = 82.83 kj/mol  no this reaction will not work at 25 celcius  b.  a reaction becomes therodynamically favourable when δg ≥ 0  δg° = δh° - tδs° 0 = (90.25x1000) - t x 24.9 t= 3624.5k  only at very high tempratures does the reaction proceed.