Domanda del libro di testo
Find and fix each mistake in the equilibrium constant expressions. a. 2 H2S(g) ⇌ 2 H2(g) + S2(g) K = [H2][S2]/[H2S]
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Ch.15 - Chemical Equilibrium
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Capitolo 15, Problema 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
Guida verificata passo dopo passo1
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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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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Percorso guidato
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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03:20Equilibrium Constant Expressions
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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07:32Le Chatelier's Principle
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