Consider this reaction occurring at 298 K: N2O(g) + NO2(g) à 3 NO(g) DG0 f (N2O(g)) = 103.7 kJ, DG0 f (NO2(g)) = 51.3 kJ, and DG0 f (NO(g)) = 87.6 kJ a. Show that the reaction is not spontaneous under standard conditions by calculating DGo rxn. b. If a reaction mixture contains only N2O and NO2 at partial pressures of 1.0 atm each, the reaction will be spontaneous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous?c. Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, what temperature is required to make the reaction spontaneous under standard conditions?