Final answer:
The question focuses on chemical equilibrium within a reaction involving CO(g) and H₂O(g) forming CO₂(g) and H₂(g). A calculation of the moles of CO₂ at equilibrium is required, along with an analysis of how system changes affect the equilibrium mixture.
Step-by-step explanation:
The question is about chemical equilibrium, where a mixture of gases CO(g) and H₂O(g) reacts to form CO₂(g) and H₂(g). It involves calculating the number of moles of CO₂ present in the equilibrium mixture starting with initial conditions of 6.0 moles each of CO(g) and H₂O(g) in a 2.0 L container.
We use the provided equilibrium concentrations to find out how the system changes under different conditions. This requires an understanding of equilibrium concepts including the reaction quotient and Le Chatelier's principle.
To solve the problem, we apply stoichiometry and the balanced chemical equation CO(g) + H₂O(g) = CO₂(g) + H₂(g). Comparison between different equilibrium states shows how changes in the amount of reactants or products can shift the equilibrium position.
This also demonstrates the dynamic nature of chemical equilibrium and how the system responds to maintain balance.
For instance, when the concentration of H₂ increases and H₂O decreases, the discussion around why the water vapor concentration at equilibrium remains the same despite the change in the system is a key part of understanding chemical reactions in a dynamic equilibrium.