* ΔH = 62.4 kJ/mol: This indicates that the reaction is endothermic. A positive enthalpy change means the reaction absorbs heat from its surroundings.

* ΔS = 0.145 kJ/mol K: This indicates that the reaction has a small increase in entropy. A positive entropy change means the reaction leads to a more disordered state.

Overall Analysis:

The reaction is endothermic (requires heat) and has a small increase in entropy. This means the reaction is not spontaneous under standard conditions.

Here's why:

* Spontaneity of a reaction is determined by the Gibbs free energy change (ΔG).

* ΔG = ΔH - TΔS

* For a spontaneous reaction, ΔG must be negative.

Since ΔH is positive (endothermic) and ΔS is small and positive, at standard temperatures (typically around 298 K), the value of ΔG will likely be positive. This indicates the reaction is non-spontaneous under standard conditions.

Important Note:

* Temperature plays a crucial role. Even though the reaction is non-spontaneous at standard conditions, it might become spontaneous at higher temperatures. This is because the TΔS term in the Gibbs free energy equation becomes larger as temperature increases.

In summary: Based on the provided information, the reaction is likely non-spontaneous under standard conditions. However, it might become spontaneous at higher temperatures.