Consider the following equilibrium, for which Δ𝐻<0
2 SO₂(𝑔) + O₂(𝑔) ⇌ 2 SO₃(𝑔)
(f) How will each of the following changes affect an equilibrium mixture of the three gases: SO₃(𝑔) is removed from the system?

검증된 단계별 안내

insert step 1> Identify the type of reaction and the effect of removing a product on the equilibrium. This is an exothermic reaction (Δ𝐻 < 0), and removing a product will shift the equilibrium to the right according to Le Chatelier's Principle.

insert step 2> Apply Le Chatelier's Principle: When a product (SO₃) is removed, the system will try to counteract this change by producing more SO₃.

insert step 3> Predict the shift in equilibrium: The equilibrium will shift to the right, favoring the formation of more SO₃ from SO₂ and O₂.

insert step 4> Consider the effect on concentrations: As the equilibrium shifts to the right, the concentration of SO₂ and O₂ will decrease, while the concentration of SO₃ will increase.

insert step 5> Conclude the effect on the system: The removal of SO₃ results in the system adjusting to restore equilibrium by producing more SO₃, thus shifting the equilibrium to the right.

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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 position of equilibrium shifts to counteract the change. In the context of the given reaction, removing SO₃ will decrease its concentration, prompting the equilibrium to shift to the right to produce more SO₃, thereby restoring balance.

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. For the reaction provided, K is determined by the concentrations of SO₃, SO₂, and O₂. Changes in concentration, such as the removal of SO₃, can affect the system's ability to reach a new equilibrium state.

Endothermic vs. Exothermic Reactions

Reactions are classified as endothermic or exothermic based on the heat exchange with the surroundings. The given reaction is exothermic (ΔH < 0), meaning it releases heat. Understanding this helps predict how temperature changes might affect the equilibrium; for instance, removing a product like SO₃ can shift the equilibrium to the right, potentially releasing heat and favoring the formation of more products.

Consider the following equilibrium, for which Δ𝐻<02 SO2(𝑔) + O2(𝑔) ⇌ 2 SO3(𝑔)(f) How will each of the following changes affect an equilibrium mixture of the three gases: SO3(𝑔) is removed from the system?