Textbook Question
Consider the following equilibrium: Ag+ (aq) + Cl-(aq) → AgCl(s) Use Le Châtelier's principle to predict how the amount of solid silver chloride will change when the equilibrium is disturbed by: (a) Adding NaCl (b) Adding AgNO3
Ch.15 - Chemical Equilibrium
Chapter 15, Problem 118d
Consider the following equilibrium: Ag+(aq) + Cl-(aq) ⇌ AgCl(s) Use Le Châtelier's principle to predict how the amount of solid silver chloride will change when the equilibrium is disturbed by: (d) Removing Cl-; also account for the change using the reaction quotient Qc
Verified step by step guidance1
Identify the initial equilibrium condition for the reaction: Ag^+(aq) + Cl^-(aq) ⇌ AgCl(s).
Understand that removing Cl^- from the system will disturb the equilibrium.
Apply Le Châtelier's principle: The system will shift to counteract the disturbance, which means it will shift to the right to produce more Cl^- ions.
Recognize that as the equilibrium shifts to the right, more AgCl(s) will form, increasing the amount of solid silver chloride.
Use the reaction quotient Q_c to confirm the shift: Q_c = [Ag^+][Cl^-]. Removing Cl^- decreases Q_c, making it less than K_c, thus the reaction shifts right to restore equilibrium.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Le Châtelier's Principle
Le Châtelier'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 can involve changes in concentration, pressure, or temperature. In the context of the given equilibrium, removing Cl<sup>-</sup> ions will shift the equilibrium to the left, favoring the formation of more reactants to compensate for the loss.
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Le Chatelier's Principle
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. For the reaction Ag<sup>+</sup>(aq) + Cl<sup>-</sup>(aq) ⇌ AgCl(s), K is defined in terms of the concentrations of Ag<sup>+</sup> and Cl<sup>-</sup>. Changes in concentration of reactants or products will affect the position of equilibrium but not the value of K itself.
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Reaction Quotient (Q<sub>c</sub>)
The reaction quotient (Q<sub>c</sub>) is calculated using the same formula as the equilibrium constant but with the current concentrations of the reactants and products, regardless of whether the system is at equilibrium. By comparing Q<sub>c</sub> to K, one can determine the direction in which the reaction will shift to reach equilibrium. If Q<sub>c</sub> is less than K, the reaction will shift to the right, while if Q<sub>c</sub> is greater than K, it will shift to the left.
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Related Practice
Textbook Question
Consider the following equilibrium: Ag+ (aq) + Cl-(aq) → AgCl(s) Use Le Châtelier's principle to predict how the amount of solid silver chloride will change when the equilibrium is disturbed by: (c) Adding NO3, which reacts with Ag+ to form the complex ion Ag(NH3)2+
Textbook Question
For the water–gas shift reaction CO1g2 + H2O1g2 ∆ CO21g2 + H21g2, ΔH° = - 41.2 kJ does the amount of H2 in an equilibrium mixture increase or decrease when the temperature is increased? How does Kc change when the temperature is decreased? Justify your answers using Le Châtelier's principle.