Final answer:
Nitrogen and oxygen react at high temperatures to form nitrogen monoxide, and the reaction's equilibrium is unchanged by the addition of a catalyst. The equilibrium constant for this reaction can be calculated using the change in free energy (ΔGº).
Step-by-step explanation:
True, nitrogen and oxygen do indeed react at high temperatures. At equilibrium, if a catalyst is added, the reaction’s rate will increase, but the concentrations of N₂, O₂, and NO will remain unchanged. Catalysts do not affect equilibrium positions; they only speed up the rate at which equilibrium is reached.
A catalyzed reaction will typically have a lower energy hump on its reaction diagram compared to the uncatalyzed equivalent, indicating a lower activation energy.
Regarding the equilibrium constant (K), it can be calculated from the ΔGº of a reaction. For instance, the equilibrium constant for the formation of nitrogen monoxide can be calculated from its ΔGº value of 173.4 kJ/mol. The formation of nitrogen monoxide (NO) from nitrogen (N₂) and oxygen (O₂) gases is nonspontaneous at normal temperatures and pressures, being a highly endothermic reaction, however, it does occur at very high temperatures.