The decomposition of calcium carbonate is represented by the equation CaCO3(s) → CaO(s) + CO2(g). Given the standard Gibbs free energies of formation ΔG°f[CaCO3(s)] = -1128.8 kJ/mol, ΔG°f[CaO(s)] = -604.0 kJ/mol, and ΔG°f[CO2(g)] = -394.4 kJ/mol, at what temperature does this reaction become spontaneous if ΔH° = 178.3 kJ/mol and ΔS° = 160.5 J/(mol·K)? Assume that the values of ΔH° and ΔS° are constant with temperature.