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.
