Equilibrium Calculations

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The application of equilibrium concepts and equations to calculate the concentrations of reactants and products at equilibrium, and to predict the direction of the reaction.

Chemical Equilibrium: This is the state in which the rate of forward chemical reaction and the rate of the reverse chemical reaction have reached a point of balance, so that there is no further net change in the amounts of the reactants and products.
Law of Mass Action: This is a fundamental principle that defines how the concentrations of the reactants and products in a chemical reaction are related to the equilibrium constant.
Equilibrium Constant (Kc/Kp): This is a numerical value that expresses the ratio of the concentrations, or partial pressures, of the products and reactants at equilibrium for a specific chemical reaction.
Le Chatelier's Principle: This principle states that when a system at equilibrium is subjected to a change in temperature, pressure, or concentration, it will respond by shifting its equilibrium position in a direction that minimizes the effect of the change.
Equilibrium Expressions: These are algebraic expressions that define the relationship between the concentrations, or partial pressures, of the reactants and products at equilibrium.
Reaction Quotients: These are calculated values that express the relative concentrations, or partial pressures, of the reactants and products at a given point in a reaction, before it has reached equilibrium.
Acid-Base Equilibria: These are systems in which a weak acid and its corresponding weak base are present in a solution, and their relative concentrations determine the pH of that solution.
Solubility Equilibria: These are systems in which a solid substance is dissolved in a solution until a point of equilibrium is reached, and the concentrations of the dissolved solute and the undissolved solid are related by the equilibrium constant.
Complex Ion Equilibria: These are systems in which a metal ion is surrounded by ligands, or other molecules, that form a complex, and the equilibrium constant relates the concentrations of the metal ion and the ligands.
Equilibrium and Thermodynamics: These topics explore how the principles of thermodynamics, such as enthalpy, entropy, and free energy, can be applied to chemical equilibrium calculations.
Homogeneous Equilibria: In homogeneous equilibria, all the reactants and products are present in the same phase, i.e., either in the gaseous phase, liquid phase or solid phase. Examples include the Haber-Bosch process and the formation of acid-base salts.
Heterogeneous Equilibria: In heterogeneous equilibria, reactants and products are present in different phases, and their concentrations need to be considered differently. An example of a heterogeneous equilibrium is the reaction between calcium carbonate and hydrochloric acid to form calcium chloride, water, and carbon dioxide.
Acid-Base Equilibria: Acid-Base Equilibria are characterized by the transfer of H+ ions. Acids donate H+ ions, whereas bases accept them. Examples include the reaction between acetic acid and sodium acetate.
Redox Equilibria: Redox Equilibria involve the transfer of electrons from one species to another. Examples include the formation of iron (III) oxide from iron (II) ions and oxygen.
Solubility Equilibria: Solubility Equilibria occur when a slightly soluble salt is dissolved in water. Equilibrium is reached when the velocity of the dissolution reaction equals that of the precipitation reaction. Examples include the dissolution of calcium carbonate in sea water.
Complex Equilibria: Complex Equilibria occur when coordination complexes are formed due to the presence of metal ions and ligands. Examples include the reaction between silver ions and ammonia to form the complex ion [Ag(NH3)2]+.
Gas-Liquid Equilibria: Gas-Liquid Equilibria are characterized by the equilibrium between a gas and a liquid. Examples include the dissolution of gases in water.
Ionic Equilibria: Ionic Equilibria occur due to the presence of ions in the solution. Examples include the reaction between hydrogen ions and hydroxide ions to form water.
Thermodynamic Equilibria: Thermodynamic Equilibria occur due to the exchange of heat between the system and its surroundings. Examples include the formation of nitrogen oxide from nitrogen and oxygen in the presence of a catalyst.
Phase Equilibria: Phase Equilibria occur due to the equilibrium between different phases of matter. Examples include the phase changes that occur upon freezing and melting of water.
- "Chemical equilibrium is the state in which both the reactants and products are present in concentrations which have no further tendency to change with time."
- "This state results when the forward reaction proceeds at the same rate as the reverse reaction."
- "The reaction rates of the forward and backward reactions are generally not zero."
- "They are equal."
- "There are no net changes in the concentrations of the reactants and products."
- "Such a state is known as dynamic equilibrium."
- "There is no observable change in the properties of the system."
- "Both the reactants and products are present in concentrations which have no further tendency to change with time."
- "The forward reaction proceeds at the same rate as the reverse reaction."
- "There are no net changes in the concentrations of the reactants and products."
- No direct quote in the paragraph, but can be inferred as a characteristic of chemical processes.
- "There is no observable change in the properties of the system."
- "Such a state is known as dynamic equilibrium."
- "Both the reactants and products are present in concentrations which have no further tendency to change with time."
- "The forward reaction proceeds at the same rate as the reverse reaction."
- "Both the reactants and products are present in concentrations which have no further tendency to change with time."
- "Both the reactants and products are present in concentrations which have no further tendency to change with time."
- No direct quote in the paragraph about the consequences, but it would indicate the system is not at equilibrium.
- "Both the reactants and products are present in concentrations which have no further tendency to change with time."
- "Both the reactants and products are present in concentrations which have no further tendency to change with time."