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 22b
Find and fix each mistake in the equilibrium constant expressions. b. CO(g) + Cl2(g) ⇌ COCl2(g) K = [CO][Cl2]/[COCl2]
Verified step by step guidance1
Step 1: Understand the equilibrium constant expression. The equilibrium constant expression for a reaction is the product of the concentrations of the products raised to their stoichiometric coefficients, divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients.
Step 2: Identify the mistake in the given equilibrium constant expression. For the reaction CO(g) + Cl2(g) ⇌ COCl2(g), the equilibrium constant expression given is K = [CO][Cl2]/[COCl2]. This is incorrect because the reactants and products are in the wrong places.
Step 3: Correct the equilibrium constant expression. The correct equilibrium constant expression for this reaction should be K = [COCl2]/([CO][Cl2]). This is because COCl2 is the product and CO and Cl2 are the reactants.
Step 4: Remember that the concentrations in the equilibrium constant expression are equilibrium concentrations. These are the concentrations of the reactants and products at the point when the reaction has reached equilibrium.
Step 5: Always double-check your equilibrium constant expressions to make sure that the products are in the numerator and the reactants are in the denominator, each raised to their respective stoichiometric coefficients.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Equilibrium Constant Expression
The equilibrium constant expression (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a reversible reaction. It is formulated based on the balanced chemical equation, where the concentrations of gaseous and aqueous species are included, while solids and liquids are omitted. The general form is K = [products]/[reactants], raised to the power of their stoichiometric coefficients.
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Equilibrium Constant Expressions
Stoichiometry in Chemical Reactions
Stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction, derived from the balanced equation. Each substance's coefficient indicates the ratio in which they react or are produced. Understanding stoichiometry is essential for correctly formulating the equilibrium constant expression, as it dictates how concentrations are represented in the equation.
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Gaseous and Aqueous Species in K Expressions
In equilibrium constant expressions, only the concentrations of gaseous and aqueous species are included, while pure solids and liquids are excluded. This is because their activities are defined as 1, meaning they do not affect the equilibrium position. Recognizing which species to include is crucial for accurately calculating the equilibrium constant for a given reaction.
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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
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
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.