Final answer:
At higher temperatures, TΔS can be larger than ΔG if the process is spontaneous. The relation ΔG = ΔH - TΔS indicates how temperature and entropy changes can affect the Gibbs free energy.
Step-by-step explanation:
The question essentially asks when TΔS (temperature times the change in entropy) is larger compared to other thermodynamic quantities such as ΔH (enthalpy change), ΔG (Gibbs free energy change), ΔE (internal energy change), and ΔT (temperature change). To answer this, we can consider the principles of thermodynamics, specifically the second law, which states that for spontaneous processes, ΔG must be negative (ΔG < 0). The equation ΔG = ΔH - TΔS gives us a direct way to relate these quantities. At sufficiently high temperatures, the TΔS term can become very large, which can make ΔG negative even if ΔH is positive. Therefore, at higher temperatures, TΔS can be larger than ΔG in cases where the process is spontaneous. Since the question is about when TΔS is larger, we are looking for a condition where a particular thermodynamic quantity is overtaken by the magnitude of TΔS, making Option 2: ΔG the most appropriate answer, as it links directly to the criterion for spontaneity and can be influenced by changes in TΔS.