The following equilibria were measured at 823 K: CoO(s) + H₂(g) ⇌ Co(s) + H₂O(g) K_c = 67 H₂(g) + CO₂(g) ⇌ CO(g) + H₂O(g) Kc = 0.14 (d) If the reaction vessel from part (c) is heated to 823 K and allowed to come to equilibrium, how much CoO(s) remains?

검증된 단계별 안내

Identify the relevant equilibrium reaction: CoO(s) + H2(g) ⇌ Co(s) + H2O(g).

Write down the expression for the equilibrium constant (Kc) for the reaction: Kc = [H2O]/([H2][CoO]). Note that solids like CoO and Co do not appear in the expression as their activity is considered to be 1.

Set up an ICE (Initial, Change, Equilibrium) table to track the concentrations of reactants and products. Assume initial moles of CoO and H2, and zero moles for Co and H2O. Define x as the amount of CoO that reacts.

Express the equilibrium concentrations in terms of x and substitute them into the Kc expression. Solve for x, which represents the amount of CoO that reacts at equilibrium.

Subtract the amount of CoO that reacted (x) from the initial amount of CoO to find the amount of CoO remaining at equilibrium.

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주요 개념

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Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In this state, the system is dynamic, meaning that reactions continue to occur, but there is no net change in the concentrations. Understanding equilibrium is crucial for predicting how changes in conditions, such as temperature or concentration, will affect the position of the equilibrium.

Equilibrium Constant (Kc)

The equilibrium constant (Kc) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. A larger Kc value indicates a greater concentration of products at equilibrium, while a smaller Kc suggests that reactants are favored. In the context of the question, the provided Kc values for the reactions will help determine the extent to which CoO remains after reaching equilibrium.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium. This principle is essential for predicting how the equilibrium position will shift in response to heating the reaction vessel, which can influence the amounts of CoO and other species present at equilibrium.

The following equilibria were measured at 823 K: CoO(s) + H2(g) ⇌ Co(s) + H2O(g) Kc = 67 H2(g) + CO2(g) ⇌ CO(g) + H2O(g) Kc = 0.14 (d) If the reaction vessel from part (c) is heated to 823 K and allowed to come to equilibrium, how much CoO(s) remains?