Consider this reaction at equilibrium: C(s) + H₂O(g) ⇌ CO(g) + H₂(g) Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. a. C is added to the reaction mixture. b. H₂O is condensed and removed from the reaction mixture. Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. c. CO is added to the reaction mixture. d. H₂ is removed from the reaction mixture.

Verified step by step guidance

1. Identify the reaction and the disturbance: The reaction given is C(s) + H2O(g) ⇌ CO(g) + H2(g), and the disturbance is the addition of solid carbon (C).
2. Understand the role of solid carbon in the reaction: Solid carbon (C) is a reactant in the given equilibrium reaction.
3. Apply Le Chatelier's Principle: According to Le Chatelier's Principle, if a reactant or product is added to a system at equilibrium, the system will shift in a direction that will use up the added substance.
4. Analyze the effect of adding more carbon: Adding more carbon (C) increases the concentration of one of the reactants.
5. Predict the direction of the shift: Since more reactant (C) is added, the reaction will shift to the right to form more products (CO and H2) and use up the added carbon.

Key Concepts

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. This principle helps predict the direction of the shift in equilibrium when a change is applied, such as concentration, pressure, or temperature.

Equilibrium Constant (K)

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It provides insight into the position of equilibrium; a larger K indicates a greater concentration of products, while a smaller K suggests a higher concentration of reactants.

Effect of Concentration Changes

When the concentration of a reactant or product in a chemical reaction at equilibrium is changed, the system will respond by shifting the equilibrium position to either the left (toward reactants) or the right (toward products). In this case, adding more solid carbon (C) does not affect the equilibrium position since solids do not appear in the equilibrium expression, thus the reaction remains unchanged.