10: Processes End Up At Equilibrium — Read

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10.1: Overview and Objectives
The material in this chapter will help you to apply the concepts of thermodynamics to describe the behavior and composition of a chemical reaction at equilibrium.
10.2: The Concept of Chemical Equilibrium
This page discusses chemical equilibrium as a dynamic state where forward and reverse reactions happen at equal rates, leading to stable concentrations of reactants and products. It uses the dissociation of dinitrogen tetroxide (N2O4) into nitrogen dioxide (NO2) as an example, explaining product-favored and reactant-favored equilibria.
10.3: The Equilibrium Constant
This page covers the concept of chemical equilibrium, emphasizing equilibrium constants (K) and their relationship to reaction kinetics, Gibbs free energy (ΔG), and temperature. It differentiates between product-favored and reactant-favored equilibria, explains homogeneous and heterogeneous equilibria, and discusses the law of mass action. The text illustrates how to calculate K from concentrations and partial pressures, the effect of temperature on K, and how K values relate to reaction rates.
10.4: Solving Equilibrium Problems
This page provides comprehensive methods for calculating equilibrium concentrations and constants in chemical reactions using various examples, including n-butane isomerization and the water-gas shift reaction. It emphasizes constructing initial, change, and final concentration tables, applying stoichiometry, and the significance of the equilibrium constant (K).
10.5: Non-equilibrium Conditions
This page explores the reaction quotient (Q) and its role in determining the direction of chemical reactions and equilibrium state. It illustrates how Q compares to the equilibrium constant (K) to predict reaction behavior. The effects of changes in conditions on equilibria are detailed, employing Le Chatelier's principle to show how systems adjust to restore equilibrium.
10.6: Factors That Affect Equilibrium
This page explores how changes in concentration, pressure, and temperature impact the equilibrium composition of chemical reactions, with a focus on Le Chatelier's principle. It illustrates examples, including reactions involving gases and the formation of ammonia, highlighting how shifts occur in response to stressors. Temperature effects are detailed regarding exothermic and endothermic reactions, while equilibrium constants are discussed throughout various scenarios.
10.7: Spontaneity and Equilibrium
This page covers the principles of spontaneous reactions and equilibrium, focusing on the relationship between free energy change (ΔG), equilibrium constants (K), and reaction spontaneity. It explains how ΔG and K indicate product or reactant favorability and how factors like temperature and pressure influence these values.
10.8: Comparing Thermodynamics and Kinetics
This page explains the differences between thermodynamics and kinetics in chemical processes, illustrating that thermodynamics evaluates energy and equilibrium, while kinetics examines reaction rates. It notes that nonspontaneous reactions can still occur under certain conditions, such as temperature changes or coupling with favorable reactions.

This page titled 10: Processes End Up At Equilibrium was last modified on Thu, 13 Aug 2026 01:22:18 GMT and is shared under a CC BY 4.0 license and was authored, remixed, and/or curated by Kathy Davis, Terrie Salupo-Bryant, Mark Bryant and Jeff Osborne.

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