If δh = -70.0 kj and δs = -0.500 kj/k , the reaction is spontaneous below a certain temperature. calculate that temperature. express your answer numerically in kelvins.
Answer is: temperature must be less than 140 K. Gibbs free energy
(G) determines if reaction will proceed spontaneously. If
the value of G is a negative, the reaction is spontaneous. ΔG = ΔH - T·ΔS. ΔH = -70.00 kJ. ΔS = -0.500 kJ/K. -70 kJ = T · (-0.5 kJ/K). T = -70.00 kJ ÷ (-0.500 kJ/K). T = 140 K.
