The catalytic decomposition of hydrogen peroxide, \(\text{H}_2\text{O}_2\text{(aq)}\), is represented by the following balanced equation:

\[ 2\text{ H}_2\text{O}_2\text{(aq)} \rightarrow 2\text{ H}_2\text{O(l)} + \text{O}_2\text{(g)} \]

For this reaction, the standard enthalpy change is negative (\(\Delta H^\circ < 0\)) and the standard entropy change is positive (\(\Delta S^\circ > 0\)). Which of the following statements best predicts the temperature conditions under which the reaction is thermodynamically favored, and provides the correct justification?