Final answer:
Adding O₂ to the equilibrium of N₂(g) + O₂(g) = 2NO(g) shifts the equilibrium to the right, increasing the production of NO and reducing the excess O₂. The reaction is influenced by Le Châtelier's Principle and has a low equilibrium constant, suggesting little NO production under normal conditions.
Step-by-step explanation:
When O₂ is added to the equilibrium mixture of the reaction N₂(g) + O₂(g) = 2NO(g), the reaction will shift according to Le Châtelier's Principle. Adding more O₂ increases its concentration, and as a response, the equilibrium will shift to the right to consume the excess O₂. This results in an increase in the production of NO and a decrease in the concentration of O₂. Conversely, the concentration of N₂ will only change if the reaction shifts significantly to the right, which would depend on the kinetics and equilibrium constant (Keq) of the reaction.
The equilibrium constant for the reaction N₂(g) + O₂(g) = 2NO(g) is very low (Keq = 1.0 × 10⁻²⁵), indicating that under normal conditions, very little NO is produced, and the reactants N₂ and O₂ do not react readily. However, in circumstances where temperature is high, such as in lightning strikes or internal combustion engines, the reaction rate can increase, and more NO can be formed.