Final answer:
The question mixes two different reactions but focuses on the Haber process. The equilibrium constant expression (Kp) for the reaction of nitrogen and hydrogen to form ammonia is Kp = (P₂NH₃) / (P₂N₂ (PH₂)³). Temperature influences Kp and thus the favorability of the reaction.
Step-by-step explanation:
The student appears to be confused about the reaction they are describing. The question initially mentions nitrogen monoxide and water reacting to form ammonia and oxygen, which is not a standard reaction. Instead, the reaction of nitrogen and hydrogen to form ammonia (3 H₂(g) + N₂(g) = 2 NH₃(g)) is a well-known equilibrium, often referred to as the Haber process. The pressure equilibrium constant (Kp) for this reaction would be written as:
Kp = (P₂NH₃) / (P₂N₂ (PH₂)³)
where PNH₃ is the partial pressure of ammonia, PN₂ is the partial pressure of nitrogen, and PH₂ is the partial pressure of hydrogen, raised to the power of their respective stoichiometric coefficients. The Kp values provided at various temperatures can give insights into the reaction conditions, such as temperature, that will favor the production of ammonia. For example, at 25°C, Kp is significantly larger, indicating a much greater extent of reaction than at 327°C.