Consider the following equilibrium, for which Δ𝐻<0
2 SO₂(𝑔) + O₂(𝑔) ⇌ 2 SO₃(𝑔)
(e) the total pressure of the system is increased by adding a noble gas

검증된 단계별 안내

Identify the equilibrium reaction: 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g). Note that ΔH < 0 indicates the reaction is exothermic.

Understand the effect of adding a noble gas: Adding a noble gas at constant volume increases the total pressure but does not change the partial pressures of the reactants and products.

Apply Le Chatelier's Principle: Since the partial pressures remain unchanged, the position of equilibrium is not affected by the addition of a noble gas at constant volume.

Consider the effect of pressure changes: If the pressure change were due to a change in volume, the equilibrium would shift towards the side with fewer moles of gas. However, in this case, the addition of a noble gas does not affect the equilibrium position.

Conclude the analysis: The addition of a noble gas at constant volume does not shift the equilibrium position of the reaction 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g).

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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 system will adjust to counteract the change and restore a new equilibrium. In the context of the given reaction, increasing the total pressure by adding a noble gas does not shift the equilibrium position because the noble gas does not react with the components of the equilibrium.

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 provided, K is determined by the concentrations of SO3 and the reactants SO2 and O2. Changes in pressure or concentration can affect the position of equilibrium but not the value of K unless temperature changes.

Effect of Inert Gases on Equilibrium

Inert gases, such as noble gases, do not participate in chemical reactions and do not affect the concentrations of the reactants or products in a chemical equilibrium. When an inert gas is added to a system at constant volume, it increases the total pressure but does not change the partial pressures of the reacting gases, thus having no effect on the position of equilibrium.

Consider the following equilibrium, for which Δ𝐻<02 SO2(𝑔) + O2(𝑔) ⇌ 2 SO3(𝑔)(e) the total pressure of the system is increased by adding a noble gas