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.