Final answer:
Chemical equilibrium can shift in reaction to the increase in concentration of reactants or products. Adding CO to the reaction will increase CO2 formation, lowering CO concentration, while adding CO2 will promote the recovery of CO and O2, lowering CO2 concentration.
Step-by-step explanation:
Understanding Chemical Equilibrium and Reaction Adjustments
When a chemical reaction is at equilibrium, adding a reactant or product can cause the system to adjust in order to reestablish equilibrium. This concept is clearly demonstrated with the reaction: 2CO(g) + O₂(g) ⇌ 2CO₂(g). If we increase the concentration of CO, the reaction will shift to the right, using up the added CO to produce more CO₂. Consequently, the concentration of CO will decrease (↓), and the concentration of CO₂ will increase (↑). Conversely, if we increase the concentration of CO₂, the reaction will shift to the left to produce more CO and O₂ by consuming the extra CO₂. This results in an increased concentration of CO (↑) and O₂ (↑), and a decreased concentration of CO₂ (↓).
The adjustment of the reaction is explained by Le Chatelier's Principle, which states that a change in concentration, pressure, or temperature of a system at equilibrium will cause an adjustment to partially counteract the change. This dynamic nature is essential in understanding chemical equilibria, as it enables the prediction of how a system will react to a given change.