∆H = 30.56 kJ mol-1
∆H = 30560 J mol-1
∆S = 6.66 x 10-3 kJ K-1 mol-1
T = ? at which ∆G = 0
∆G = ∆H – T∆S
0 = ∆H – T∆S
T = ΔH / ΔS
![](https://www.sarthaks.com/?qa=blob&qa_blobid=14019417711267632882)
t = 4589 K
(i) At 4589K ; ∆G = 0, the reaction is in equilibrium.
(ii) At temperature below 4598 K, ∆H > T ∆ S ∆G = ∆H – T∆S > 0, the reaction in the forward direction, is non-spontaneous. In other words the reaction occurs in the backward direction.