Entropy affects free energy through the relationship (equation 8), where H is enthalpy, T is absolute temperature, and S is entropy. As entropy increases, the -TS term reduces ΔG, promoting spontaneity (ΔG<0) . This aligns with the second law, as processes that increase the system's or universe's entropy often proceed spontaneously. At higher temperatures, the influence of entropy becomes more pronounced because T amplifies the contribution of -TS. For example, a reaction with a positive entropy change (ΔS>0) is more likely to be spontaneous at elevated temperatures, as the entropydriven reduction in GG offsets any unfavorable enthalpy change (H>0). Conversely, if entropy decreases (ΔS<0), the -TS term contributes positively to ΔG, opposing spontaneity unless balanced by a sufficiently negative enthalpy change (H<0). This highlights the temperature-dependent nature of entropy's effect on free energy, as higher temperatures exacerbate the penalty for reduced entropy. The second law thus explains how entropy drives systems toward thermodynamic equilibrium, shaping the conditions under which processes become energetically favorable. By linking entropy to Gibbs free energy, the second law provides a comprehensive framework for predicting the spontaneity of chemical and physical transformations.