For the reaction at 298 K, 2A +B ------> C
∆H = 400kJ/mol and ∆S =0.2 kJ/K/ mol. At what temperature will the reaction become spontaneous considering ∆H and ∆S to be constant over the temperature range?
Gibbs free energy,
∆G = ∆H-T∆S
0= 400 kJ/mol - T x 0.2 kJ/K/Mol
Temperature ,T = 400 / 0.2 = 2000K
Therefore, above 2000 K, the reaction will become spontaneous.