Dinitrogen and dioxygen the main constituents of air do not react with each other in atmosphere to form oxides of…

Strategy: Consider the thermodynamics and activation energy for the reaction between $\ce{N2}$ and $\ce{O2}$.

Step 1: Nitrogen Inertness Nitrogen $(\ce{N2})$ has an extremely high bond dissociation enthalpy $(\approx 941 \text{ kJ/mol})$ due to the triple bond $(\ce{N\equiv N})$, making it virtually inert at room temperature.

Step 2: Endothermic Nature The reaction $\ce{N2(g) + O2(g) \rightleftharpoons 2NO(g)}$ is highly endothermic. It requires very high temperatures (like in lightning or internal combustion engines) to proceed significanty.

$\boxed{\text{Answer: (Option) [d] The reaction is endothermic and require very high temperature}}$