If _h = -60.0kj and _s = -0.200kj/k , the reaction is spontaneous below a certain temperature. calculate that temperature.

delta G = delta H - T delta S where T is the Kelvin temperature
delta G is the change in Gibbs Free Energy and must be negative for a spontaneous reaction. Set delta G = 0 (for equilibrium) and solve for T


0 = delta H - T delta S
T delta S = delta H
T(-0.200kJ/K) = -60.0kJ
T(-200J/K) = -60,000J
T = 300K

delta S is negative, so (-T delta S) is positive and G is more positive for higher temperatures
This reaction is spontaneous for temperatures less than 300K.