Enthalpy and entropy changes of a reaction are 40.63 kJ mol-1 and 108.8 JK-1 mol-1 respectively. Predict the feasibility of the reaction at 27°C.
ΔH = 40.63 kJ mol-1 = 40630 Jmol-1 ΔS = 108.8 JK-1 mol-1 T = 27°C =27 + 273 = 300 K Now ΔG = ΔH – TΔS = 40630 – 3 × 108.8 = 7990 J mol-1 Since AG comes out to be positive (i.e., ΔG > 0), the reaction is not feasible at 27°C in the forward direction.
