Question

Consider the reaction 2 NO₂(g) →N₂O₄(g) .

(a) Using ΔG_fN₂O₄(g) = 97.79 kJ/mol and ΔG_f NO₂(g) = 51.3 kJ/mol, calculate ΔG° at 298 K.
kJ

(b) Calculate ΔG at 298 K if the partial pressures of NO₂ and N₂O₄ are 0.25 atm and 1.30 atm, respectively.
kJ

Answer 1

DHwan = EDH formation of products - EDH formation of reactants A Gryn = {AG formation of Products - E AG formation of reactants DS ryn= EAS formation of Products - {As formation of reactants

Ahrya = A hyx = Daryo SG+ (N, o,) - 3 DG + (NO) 97.79 KJ - 2 (51.3) -4.8163 AG= Anorant RT lnk. R=8.314 Jo montar T is the temperature in kelvin K is equilibrium constant Oui Standard free energy. Dat hon standard free energy DG: -4.81 x3 + (8.314 7nofx") (7986) 19 ' (PNog) 2 1.30 AG= -4.81 kJ + (8-3145. mc (0.252 D G = -4.81 kJ + 7519.314J OG= -4.81K5 +7.519314 KJ OG 8.709314 kJ.