Textbook Question
Find and fix each mistake in the equilibrium constant expressions. a. 2 H2S(g) ⇌ 2 H2(g) + S2(g) K = [H2][S2]/[H2S]
Ch.16 - Chemical Equilibrium
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
Chapter 16, Problem 23
When this reaction comes to equilibrium, will the concentrations of the reactants or products be greater? Does the answer to this question depend on the initial concentrations of the reactants and products? A(g)+B(g) ⇌ 2 C(g) Kc = 1.4⨉10-5
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Identify the equilibrium constant expression for the reaction: \( K_c = \frac{[C]^2}{[A][B]} \).
Recognize that the equilibrium constant \( K_c \) is very small (\( 1.4 \times 10^{-5} \)), indicating that the reaction favors the reactants.
Understand that a small \( K_c \) value means that at equilibrium, the concentration of products \([C]\) will be much smaller compared to the concentrations of reactants \([A]\) and \([B]\).
Conclude that the concentrations of the reactants \([A]\) and \([B]\) will be greater than the concentration of the product \([C]\) at equilibrium.
Note that the answer does not depend on the initial concentrations of the reactants and products, as \( K_c \) is a constant at a given temperature.
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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. At this point, 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.
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04:21
Chemical Equilibrium Concepts
Equilibrium Constant (Kc)
The equilibrium constant (Kc) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. A small Kc value, such as 1.4x10^-5, indicates that at equilibrium, the concentration of reactants is much greater than that of products. This value helps predict the direction of the reaction and the relative amounts of substances present at equilibrium.
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Le Chatelier's Principle
Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium. This principle is essential for understanding how initial concentrations of reactants and products can influence the final equilibrium concentrations, as shifts in equilibrium can occur based on these initial conditions.
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Related Practice
Textbook Question
Write an expression for the equilibrium constant of each chemical equation.
a. SbCl5(g) ⇌ SbCl3(g) + Cl2(g)
b.2 BrNO(g) ⇌ 2 NO(g) + Br2(g)
c. CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g)
d. 2 CO(g) + O2(g) ⇌ 2 CO2(g)
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Textbook Question
Find and fix each mistake in the equilibrium constant expressions. b. CO(g) + Cl2(g) ⇌ COCl2(g) K = [CO][Cl2]/[COCl2]
Textbook Question
H2 and I2 are combined in a flask and allowed to react according to the reaction: H2(g) + I2(g) ⇌ 2 HI(g) Examine the figures (sequential in time) and answer the questions: a. Which figure represents the point at which equilibrium is reached?
Textbook Question
Ethene (C2H4) can be halogenated by this reaction: C2H4(g) + X2(g) ⇌ C2H4X2(g) where X2 can be Cl2 (green), Br2 (brown), or I2 (purple). Examine the three figures representing equilibrium concentrations in this reaction at the same temperature for the three different hal- ogens. Rank the equilibrium constants for the three reactions from largest to smallest.
Textbook Question
A chemist trying to synthesize a particular compound attempts two different synthesis reactions. The equilibrium constants for the two reactions are 23.3 and 2.2⨉104 at room temperature. However, upon carrying out both reactions for 15 minutes, the chemist finds that the reaction with the smaller equilibrium constant produces more of the desired product. Explain how this might be possible.