text: A.\n\nfree energy = ΔG\n\nentropy change = ΔS°\n\nΔS° = ΔS products - ΔS reactants\n\nΔS° = 24.9\n\nΔG° = ΔH° - TΔS°\nΔG° = (90.25x1000) - (25+273.15)x24.9\nΔG° = 82.83 KJ/mol\n\nno this reaction will not work at 25 celcius\n\nB.\n\nA reaction becomes therodynamically favourable when ΔG ≥ 0\n\nΔG° = ΔH° - TΔS°\n0 = (90.25x1000) - T x 24.9\nT= 3624.5K\n\nonly at very high tempratures does the reaction proceed.