The reaction Fe 3+ (aq) + Cl - (aq) ⇌ FeCl 2+ (aq) is endothermic. How will the equilibrium concentration of FeCl 2+ change when b. Cl - is precipitated by addition of AgNO 3 ?

Hello everyone today. We have the following problem. The following reaction is eggs are thermic. Will the concentration of scandia hydroxide increase decrease or remain unchanged when titanium nitrate is added to the solution, precipitating hydroxide. Well, if we look at this reaction, hydroxide is a reaction. So if we remove this, so if removed, the equilibrium will shift to produce more of it so it's going to shift to the left. This is known as long as principal, so shift to the left to produce more. So we can say that our scan diem two plus hydroxide will be consumed in order to produce more hydroxide ions. So this concentration will decrease and with that we have our final answer overall. I hope this helped ahead until next time.

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7. Energy, Rate and Equilibrium

Le Chatelier's Principle

GOB Chemistry

7. Energy, Rate and Equilibrium

Le Chatelier's Principle

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Problem 66b

Textbook Question

The reaction Fe³⁺(aq) + Cl^-(aq) ⇌ FeCl²⁺(aq) is endothermic. How will the equilibrium concentration of FeCl²⁺ change when
b. Cl^- is precipitated by addition of AgNO₃?

Verified step by step guidance

Identify the key components of the reaction: The reaction is Fe³⁺(aq) + Cl⁻(aq) ⇌ FeCl²⁺(aq), and it is endothermic. The equilibrium depends on the concentrations of Fe³⁺, Cl⁻, and FeCl²⁺.

Understand the effect of adding AgNO₃: Ag⁺ ions from AgNO₃ will react with Cl⁻ ions to form a precipitate of AgCl (Ag⁺(aq) + Cl⁻(aq) → AgCl(s)). This reduces the concentration of Cl⁻ in the solution.

Apply Le Châtelier's Principle: When the concentration of Cl⁻ decreases, the equilibrium will shift to counteract this change by producing more Cl⁻. This means the reaction will shift to the left (toward the reactants).

Determine the effect on FeCl²⁺: As the equilibrium shifts to the left, the concentration of FeCl²⁺ will decrease because it is being converted back into Fe³⁺ and Cl⁻.

Summarize the result: The equilibrium concentration of FeCl²⁺ will decrease when Cl⁻ is precipitated by the addition of AgNO₃.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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. In this case, adding AgNO3 causes Cl- ions to precipitate, which reduces their concentration in the solution. According to Le Chatelier's Principle, the equilibrium will shift to the right to produce more Cl- ions, thereby increasing the concentration of FeCl2+.

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 Fe3+ + Cl- ⇌ FeCl2+, the equilibrium constant can help predict how changes in concentration will affect the system. If Cl- is removed from the solution, the equilibrium constant remains unchanged, but the concentrations of the species will adjust to restore equilibrium.

Endothermic Reactions

An endothermic reaction is one that absorbs heat from its surroundings, resulting in a decrease in temperature of the environment. In the context of the given reaction, the endothermic nature implies that increasing temperature will favor the formation of products. However, in this scenario, the focus is on the concentration changes due to the precipitation of Cl-, which will influence the equilibrium position without directly altering the temperature.

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The reaction CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g) has ∆H = -9.8 kcal/mol (-41 kJ/mol). Does the amount of H₂ in an equilibrium mixture increase or decrease when the temperature is decreased?

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The reaction H₂(g) + I₂(g) ⇌ 2 HI(g) has ∆H = -2.2 kcal/mol (-9.2 kJ/mol). Will the equilibrium concentration of HI increase or decrease when

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