At constant pressure,the following reaction 2NO₂(g)$\to$ N₂O₄(g)is exothermic.The reaction (as written)is

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For an exothermic reaction at constant pressure, spontaneity depends on the sign and magnitude of the change in enthalpy (ΔH) and entropy (ΔS). Since the reaction is exothermic, ΔH is negative. According to the Gibbs free energy equation, ΔG = ΔH - TΔS, a negative ΔH favors spontaneity. However, if ΔS is negative (which is common in reactions where gases combine to form fewer gas molecules, suggesting a decrease in disorder), increasing temperature (T) makes the TΔS term more positive, potentially making ΔG positive at high temperatures, which means the reaction becomes non-spontaneous at high temperatures. Therefore, the reaction is spontaneous at low temperatures but not at high temperatures.

At Constant Pressure,the Following Reaction 2NO2(g) →\to→ N2O4(g)is Exothermic

At Constant Pressure,the Following Reaction 2NO₂(g) $\to$ N₂O₄(g)is Exothermic