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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 52
Chapter 15, Problem 52

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?

Verified step by step guidance
1
Identify the initial concentrations of Br_2 and Cl_2 by dividing the moles by the volume of the container: [Br_2]_0 = \(\frac{0.25 \text{ mol}\)}{3.0 \(\text{ L}\)}, [Cl_2]_0 = \(\frac{0.55 \text{ mol}\)}{3.0 \(\text{ L}\)}.
Set up an ICE (Initial, Change, Equilibrium) table to track the changes in concentrations as the system reaches equilibrium. Let x be the change in concentration of Br_2 and Cl_2 that reacts to form BrCl.
Write the expression for the equilibrium constant K_c: K_c = \(\frac{[BrCl]^2}{[Br_2][Cl_2]}\).
Substitute the equilibrium concentrations from the ICE table into the K_c expression: K_c = \(\frac{(2x)^2}{([Br_2]_0 - x)([Cl_2]_0 - x)}\).
Solve the equation for x, which represents the change in concentration, and use it to find the equilibrium concentrations: [Br_2] = [Br_2]_0 - x, [Cl_2] = [Cl_2]_0 - x, [BrCl] = 2x.

Key Concepts

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

Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In this state, the system is dynamic, meaning that reactions continue to occur, but there is no net change in concentration. Understanding this concept is crucial for analyzing how concentrations shift in response to changes in conditions, such as concentration or temperature.
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Equilibrium Constant (Kc)

The equilibrium constant (Kc) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium, each raised to the power of their coefficients in the balanced equation. For the reaction Br<sub>2</sub>(g) + Cl<sub>2</sub>(g) β‡Œ 2 BrCl(g), Kc = [BrCl]<sup>2</sup> / ([Br<sub>2</sub>][Cl<sub>2</sub>]). This constant provides insight into the extent of the reaction and helps predict the direction in which the reaction will shift to reach equilibrium.
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Concentration Calculations

Concentration calculations involve determining the molarity of substances in a solution, which is defined as the number of moles of solute divided by the volume of the solution in liters. In this problem, the initial concentrations of Br<sub>2</sub> and Cl<sub>2</sub> must be calculated based on the given moles and the volume of the container. These initial concentrations are essential for applying the equilibrium expression and finding the equilibrium concentrations of all species involved.
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Related Practice
Textbook Question

At 900 K, the following reaction has 𝐾𝑝 = 0.345: 2 SO2(𝑔) + O2(𝑔) β‡Œ 2 SO3(𝑔) In an equilibrium mixture the partial pressures of SO2 and O2 are 0.135 atm and 0.455 atm, respectively. What is the equilibrium partial pressure of SO3 in the mixture?

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Textbook Question

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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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.

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