Final answer:
The addition of carbon to a reaction at equilibrium does not change the concentrations of gaseous components; shifts in equilibrium are observed when gaseous reactants or products are altered or the temperature changes. Understanding these changes allows for prediction and determination of equilibrium concentrations.
Step-by-step explanation:
The problem presented involves chemical equilibrium and Le Chatelier's Principle in a reaction where carbon (C) is added to a system already at equilibrium. The reaction under consideration is C(s) + H₂O(g) ⇌ CO(g) + H₂(g). According to Le Chatelier's Principle, the addition of carbon, a solid reactant, does not change the concentrations of the gaseous components as the concentration of a pure solid is not included in the equilibrium constant expression. However, removing a product or reactant in gaseous form or altering the temperature would cause shifts in the concentrations of the other components in the system to re-establish equilibrium.
For example, if additional hydrogen gas (H₂) is added to the system, the equilibrium will shift to the right, increasing the concentration of carbon monoxide (CO) and decreasing the concentration of water vapor (H₂O). Conversely, if carbon monoxide is removed, the equilibrium will shift to the left, increasing the concentration of water vapor and hydrogen gas.
Understanding these concepts is essential in predicting how the system will respond to changes and determining the equilibrium concentrations of all components involved in the reaction.