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A reaction with a negative ΔS can still be spontaneous if the ΔG (change in Gibbs free energy) is negative, which can occur if the enthalpy change (ΔH) is sufficiently negative and/or the temperature (T) is high enough. Exothermic reactions are not always spontaneous because spontaneity also depends on entropy changes and temperature. Free energy is dependent on temperature, as shown in the Gibbs free energy equation ΔG = ΔH - TΔS. A decrease in free energy does not ensure an increase in the system's entropy; it indicates the process is spontaneous under constant pressure and temperature, but the entropy change could be in the surroundings or the system.

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