The correct option is D 966K
ΔrH = HReactants−HProducts
ΔrH = -110.5 - (-266.3) = 155.8 kJ/mol
Similarly, ΔrS = SReactants−SProducts
ΔrS = (27.28 + 197.6) - (57.49 + 5.74) = 161.65 J/mol K
Now at ΔrG= 0, ΔrH = TΔrS
Therefore, T = ΔrH/ΔrS = 155.8 x 1000/ 161.65 = 964 K.
Thus, above 964 K the given reaction is spontaneous which implies at 966K the reaction is spontaneous (Correct Option: C)