Final answer:
In response to changes in reactant or product concentrations, the equilibrium of the chemical reaction 2CO(g) + O2(g) -> 2CO2(g) will shift according to Le Chatelier's Principle to counteract the introduced change, altering the concentrations accordingly.
Step-by-step explanation:
The question revolves around how the concentration of each species in a chemical equilibrium shifts when a change is made to the system. According to Le Chatelier's Principle, a system at equilibrium will adjust to counteract any changes made to it. If the concentration of a reactant or product is altered, the position of equilibrium will shift to reduce the impact of this change. Here's how the concentration of each species will change in reaction to adjustments to the system:
Increase CO concentration: The system will shift towards the products to reduce the additional CO, hence increasing CO2 and decreasing O2.
Decrease O2 concentration: The system will shift towards the reactants to restore the removed O2, leading to increased CO concentrations and decreased CO2.
Increase CO2 concentration: The equilibrium shifts towards the reactants to consume the additional CO2, increasing CO and O2 concentrations.
Decrease CO2 concentration: The system will shift towards the products to replace the CO2, reducing CO and O2 concentrations.