Question

At low temperatures, ΔH is larger than:

Option 1: ΔG.
Option 2: ΔS.
Option 3: ΔE.
Option 4: ΔT.

Answer 1

At low temperatures, the enthalpy change (ΔH) is larger than the Gibbs free energy change (ΔG), the entropy change (ΔS), the internal energy change (ΔE), and the temperature change (ΔT).

Step-by-step explanation:

At low temperatures, the enthalpy change (ΔH) is larger than the Gibbs free energy change (ΔG), the entropy change (ΔS), the internal energy change (ΔE), and the temperature change (ΔT).

The enthalpy change (ΔH) represents the heat absorbed or released during a process, while the Gibbs free energy change (ΔG) represents the maximum useful work that can be obtained from a system. At low temperatures, the enthalpy change is larger because it takes more energy to change the state of a substance and overcome the intermolecular forces holding it together.