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Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.15 - Chemical EquilibriumProblema 53
Capitolo 15, Problema 53

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)?

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1
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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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.
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Equilibrium Constant Expressions

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.
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Partial Pressure Calculation

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.
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Le Chatelier's Principle
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