Textbook Question
(a) Is the dissociation of fluorine molecules into atomic fluorine, F2(𝑔) ⇌ 2 F(𝑔), an exothermic or endothermic process?
Ch.15 - Chemical Equilibrium
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 15, Problem 72
If Kc = 1 for the equilibrium 2A ⇌ B, what is the relationship between [A] and [B] at equilibrium?
Verified step by step guidance1
Step 1: Write the expression for the equilibrium constant (Kc) for the reaction 2A ⇌ B. The expression is Kc = \( \frac{[B]}{[A]^2} \).
Step 2: Since Kc = 1, set the expression equal to 1: \( \frac{[B]}{[A]^2} = 1 \).
Step 3: Rearrange the equation to express [B] in terms of [A]: [B] = [A]^2.
Step 4: Interpret the relationship: At equilibrium, the concentration of B is equal to the square of the concentration of A.
Step 5: Conclude that if Kc = 1, then [B] = [A]^2, indicating a specific mathematical relationship between the concentrations of A and B at equilibrium.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Equilibrium Constant (Kc)
The equilibrium constant, Kc, is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For the reaction 2A ⇌ B, Kc is calculated as [B]/[A]^2. A Kc value of 1 indicates that at equilibrium, the concentrations of products and reactants are equal when raised to their respective stoichiometric coefficients.
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Equilibrium Constant Expressions
Chemical Equilibrium
Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products over time. In the context of the reaction 2A ⇌ B, this means that the concentrations of A and B will stabilize at certain values, reflecting the balance between the formation of B from A and the conversion of B back to A.
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Concentration Relationships at Equilibrium
At equilibrium, the concentrations of reactants and products are related through the equilibrium constant. For Kc = 1 in the reaction 2A ⇌ B, it implies that the concentration of B is equal to the square of the concentration of A, or [B] = [A]^2. This relationship helps predict how changes in concentration will affect the system and the position of equilibrium.
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Related Practice
Textbook Question
When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) (a) Calculate Kc for this reaction at this temperature.
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Textbook Question
(b) If the temperature is raised by 100 K, does the equilibrium constant for this reaction increase or decrease?