Temperature and entropy effects (equation 7) play a critical role in this behavior. The Gibbs free energy equation, (Z), demonstrates that the system's spontaneity depends not only on the enthalpy change (ΔH) but also on the entropy change (ΔS), modulated by temperature (T). At elevated pressures, the system's entropy changes as the reaction involves gases like H2, which are sensitive to pressure-induced constraints on molecular motion. While higher pressures tend to favor negative enthalpy changes by increasing molecular interactions, they can also reduce entropy contributions, making ΔG less negative. This dynamic explains why, despite the generally favorable ΔG values at higher pressures, the reaction rate peaks at 0.26667 Pa, where entropy loss is minimized relative to the energy gained from enhanced interactions.