At 373 K, 𝐾𝑝 = 0.416 for the equilibrium 2 NOBr(𝑔) ⇌ 2 NO(𝑔) + Br2(𝑔) If the pressures of NOBr(𝑔) and NO(𝑔) are equal, what is the equilibrium pressure of Br2(𝑔)?

Ch.15 - Chemical Equilibrium

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Brown 14th Edition

Ch.15 - Chemical Equilibrium

문제 53

15장, 문제 53

At 373 K, 𝐾_𝑝= 0.416 for the equilibrium 2 NOBr(𝑔) ⇌ 2 NO(𝑔) + Br₂(𝑔) If the pressures of NOBr(𝑔) and NO(𝑔) are equal, what is the equilibrium pressure of Br₂(𝑔)?

검증된 단계별 안내

Identify the balanced chemical equation: 2 NOBr(g) ⇌ 2 NO(g) + Br_2(g).

Write the expression for the equilibrium constant K_p: K_p = (P_NO^2 * P_Br2) / (P_NOBr^2).

Since the pressures of NOBr and NO are equal, let P_NOBr = P_NO = x.

Substitute the pressures into the K_p expression: 0.416 = (x^2 * P_Br2) / (x^2).

Solve for P_Br2: P_Br2 = 0.416.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Equilibrium Constant (Kp)

The equilibrium constant, Kp, is a ratio that expresses the relationship between the partial pressures of the products and reactants at equilibrium for a given reaction at a specific temperature. For the reaction 2 NOBr(g) ⇌ 2 NO(g) + Br2(g), Kp is calculated using the formula Kp = (P_NO^2 * P_Br2) / (P_NOBr^2), where P represents the partial pressures of the gases involved.

Partial Pressure

Partial pressure is the pressure exerted by a single component of a gas mixture. In the context of the equilibrium reaction, the total pressure is the sum of the partial pressures of NOBr, NO, and Br2. Understanding how to calculate and relate these pressures is essential for determining the equilibrium state of the system.

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 this problem, if the pressures of NOBr and NO are equal, the system will shift to produce more Br2 to maintain the equilibrium constant, which is crucial for finding the equilibrium pressure of Br2.