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Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.15 - Chemical EquilibriumProblem 53
Chapter 15, Problem 53

At 373 K, 𝐾𝑝 = 0.416 for the equilibrium 2 NOBr(𝑔) β‡Œ 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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Identify the balanced chemical equation: 2 NOBr(g) β‡Œ 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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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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) β‡Œ 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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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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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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Related Practice
Textbook Question

For the equilibrium Br2(𝑔) + Cl2(𝑔) β‡Œ 2 BrCl(𝑔) at 400 K, 𝐾𝑐 = 7.0. If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentrations of Br2, Cl2, and BrCl?

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Textbook Question

At 80Β°C, 𝐾𝑐 = 1.87Γ—10βˆ’3 for the reaction PH3BCl3(𝑠) β‡Œ PH3(𝑔) + BCl3(𝑔) (a) Calculate the equilibrium concentrations of PH3 and BCl3 if a solid sample of PH3BCl3 is placed in a closed vessel at 80Β°C and decomposes until equilibrium is reached.

Textbook Question

At 218Β°C, 𝐾𝑐 = 1.2Γ—10βˆ’4 for the equilibrium NH4SH(𝑠) β‡Œ NH3(𝑔) + H2S(𝑔) Calculate the equilibrium concentrations of NH3 and H2S if a sample of solid NH4SH is placed in a closed vessel at 218Β°C and decomposes until equilibrium is reached.

Textbook Question

At 2000Β°C, the equilibrium constant for the reaction 2 NO(𝑔) β‡Œ N2(𝑔) + O2(𝑔) is 𝐾𝑐 = 2.4Γ—103. If the initial concentration of NO is 0.175 M, what are the equilibrium concentrations of NO, N2, and O2?

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