Final answer:
For a chemical reaction with ∆H < 0 and ∆S > 0, statement III is true, meaning the reaction is spontaneous at any temperature. Statement II is also true, as the reaction becomes more spontaneous with increasing temperature. Statement I is false, as the reaction is not limited to being spontaneous at low temperature only.
Step-by-step explanation:
Given that ∆H < 0 and ∆S > 0, we need to determine the statements that are true based on this information:
I) The reaction is spontaneous at low temperature only.
II) As temperature increases, the reaction becomes more spontaneous.
III) The reaction is spontaneous at any temperature.
To answer this question, we need to consider the equation AG = AH - TAS. If ∆H < 0 and ∆S > 0, then the term -TAS will dominate, making the reaction spontaneous at all temperatures. Therefore, statement III is true. However, as temperature increases, the magnitude of the -TAS term increases, leading to a larger negative value for AG. As a result, the reaction becomes more spontaneous with increasing temperature. Therefore, statement II is also true. Statement I is false because the reaction is spontaneous at any temperature, not just low temperature.