Final answer:
A reaction with negative enthalpy and positive entropy will have a negative Gibbs Free Energy and be spontaneous at all temperatures, as both enthalpy and entropy favor product formation.
Step-by-step explanation:
If a reaction has a negative enthalpy (ΔH < 0) and a positive entropy (ΔS > 0), the sign of the Gibbs Free Energy (ΔG) will always be negative. According to the Gibbs Free Energy equation, ΔG = ΔH - TΔS, where T represents the temperature in Kelvin, which is always a positive value. Because the enthalpy is negative and entropy is positive, the product TΔS will be positive, resulting in a subtraction from a negative number (ΔH) that makes ΔG more negative. Therefore, the reaction will be spontaneous at all temperatures, indicating that the reaction can proceed without external energy input, and this is because both driving forces, enthalpy, and entropy, are in favor of product formation.