Final answer:
The addition of O₂ to a system at equilibrium would shift the balance to form more NO, while increasing temperature favors the endothermic formation of NO. The concentration of all gases adjusts to reach a new equilibrium state.
Step-by-step explanation:
The question relates to reaching chemical equilibrium in a reaction between nitrogen (N₂) and oxygen (O₂) to produce nitric oxide (NO). When O₂ is added to the system at equilibrium, Le Chatelier's principle predicts that the system will adjust to counteract this change, favoring the production of NO and consuming some of the added O₂ and existing N₂ to re-establish equilibrium. Conversely, when the temperature is increased, the equilibrium shifts to favor the endothermic reaction, meaning the production of NO will increase. Therefore, in both cases, the equilibrium concentrations of the substances involved will adjust in attempts to reach a new equilibrium state.
Additionally, the student provided an equilibrium constant for a similar reaction involving N₂O and O₂ at 25°C (K = 1.7 × 10-13). If a system is initially at different partial pressures for N₂O, O₂, and NO, the system will adjust until the ratio of the concentrations of the products to the reactants raised to their stoichiometric coefficients equals the equilibrium constant (K). This adjustment involves a change in the partial pressures of the gases until equilibrium is reached.