Consider the reaction 4 NH₃(𝑔) + 5 O₂(𝑔) ⇌ 4 NO(𝑔) + 6 H₂O(𝑔), Δ𝐻 = −904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (f) increase temperature.

검증된 단계별 안내

Identify the type of reaction: The given reaction is exothermic, as indicated by the negative \( \Delta H = -904.4 \) kJ.

Apply Le Chatelier's Principle: In an exothermic reaction, increasing the temperature will shift the equilibrium position to favor the endothermic direction, which is the reverse reaction in this case.

Determine the effect on NO yield: Since the equilibrium shifts towards the reactants (reverse reaction), the yield of NO will decrease.

Consider the overall impact: Increasing temperature in an exothermic reaction generally decreases the yield of products formed in the forward reaction.

Conclude: Therefore, increasing the temperature will decrease the yield of NO at equilibrium.

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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 temperature changes, if the reaction is exothermic (releases heat), increasing the temperature will shift the equilibrium to favor the reactants, thereby decreasing the yield of products.

Exothermic Reactions

An exothermic reaction is one that releases energy in the form of heat. In the given reaction, the negative ΔH value indicates that it is exothermic. When the temperature is increased, the system will respond by favoring the endothermic direction (the reverse reaction) to absorb the added heat, which reduces the production of NO.

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 temperature can alter the value of K, affecting the position of equilibrium. For exothermic reactions, increasing temperature decreases K, leading to a lower concentration of products like NO at equilibrium.

Consider the reaction 4 NH3(𝑔) + 5 O2(𝑔) ⇌ 4 NO(𝑔) + 6 H2O(𝑔), Δ𝐻 = −904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (f) increase temperature.