Consider this reaction at equilibrium: 2KClO3(s) ⇌ 2KCl(s) + 3O2(g). Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. a. O2 is removed from the reaction mixture. b. KCl is added to the reaction mixture. c. KClO3 is added to the reaction mixture. d. O2 is added to the reaction mixture.

Name: Chemistry: A Molecular Approach
Author: Tro
ISBN: 9780134112831

검증된 단계별 안내

Identify the principle governing the reaction shifts: Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.

For part (a), removing O2 decreases the concentration of a product. According to Le Chatelier's Principle, the equilibrium will shift to the right to produce more O2.

For part (b), adding KCl increases the concentration of a product. According to Le Chatelier's Principle, the equilibrium will shift to the left to reduce the concentration of KCl.

For part (c), adding KClO3 increases the concentration of a reactant. Since KClO3 is a solid, its concentration does not affect the equilibrium position, so the equilibrium remains unchanged.

For part (d), adding O2 increases the concentration of a product. According to Le Chatelier's Principle, the equilibrium will shift to the left to reduce the concentration of O2.

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. This means that if a reactant or product concentration is altered, the system will adjust to restore equilibrium, either by favoring the forward or reverse reaction.

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. Changes in concentration, pressure, or temperature can affect the value of K, influencing the direction in which the reaction will shift to re-establish equilibrium.

Reaction Quotient (Q)

The reaction quotient (Q) is a measure of the relative concentrations of products and reactants at any point in time, not just at equilibrium. By comparing Q to K, one can predict the direction in which the reaction will shift: if Q < K, the reaction shifts right to produce more products; if Q > K, it shifts left to produce more reactants.