"The equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical equilibrium, a state approached by a dynamic chemical system after sufficient time has elapsed at which its composition has no measurable tendency towards further change."
The ratio of concentrations/pressures of products to reactants at equilibrium, which varies with temperature and is a measure of how far the reaction proceeds to the right.
Chemical Equilibrium: Equilibrium is a state of chemical balance in which the concentrations of reactants and products remain constant over time.
Introduction to Equilibrium Constant (Kc/Kp): Equilibrium constant is an expression that relates the concentrations or partial pressures of reactants and products at equilibrium.
Calculation of Equilibrium Constant: Equilibrium constant can be calculated using the balanced chemical equation and the concentrations or partial pressures of reactants and products at equilibrium.
Relationship between Equilibrium Constant and Reaction Quotient: Reaction quotient is an expression that relates the concentrations or partial pressures of reactants and products at any point during the reaction. The relationship between the equilibrium constant and reaction quotient determines the direction in which the reaction proceeds.
Le Chatelier's Principle: Le Chatelier's principle states that a system at equilibrium will respond to any external stress in such a way as to counteract the stress and reestablish equilibrium.
Effect of Concentration on Equilibrium Constant: Changes in the concentration of reactants or products at equilibrium can cause a shift in the equilibrium position. Equilibrium constant remains constant, however.
Effect of Pressure on Equilibrium Constant: Changes in pressure can affect the equilibrium position, particularly if the reaction involves gas-phase components.
Effect of Temperature on Equilibrium Constant: Changes in temperature can affect the equilibrium position and the value of the equilibrium constant.
Equilibrium Constant and Reaction Rate: Evaluation of equilibrium constant can help to determine the rate of a reaction as well as the thermodynamic feasibility of the reaction.
Acid-Base Equilibria: The equilibrium constant for acid-base reactions can be expressed in terms of the concentrations of the acid and the base at equilibrium.
Solubility Equilibria: The equilibrium constant for solubility equilibria can be expressed in terms of the concentrations of the solid solute and the ions that are in the solution.
Heterogeneous Equilibria: Equilibria that involve a mixture of phases (e.g., gas and liquid) like the adsorption of gases on metals can be dealt with in the formalism of Kc and Kp eq constants.
Application of Equilibrium Constant: Equilibrium constant has several applications in chemistry, particularly in acid-base chemistry, solubility equilibria, and in the estimation of reaction feasibility.
Application of Equilibrium Constant in Industry: Equilibrium constant has an important role in the chemical industry and is frequently used for the design of chemical processes, particularly in the field of chemical engineering.
Homogeneous Equilibrium Constant (Kc): This is the equilibrium constant for reactions that take place in the same phase. It is defined as the product of the concentrations of the reactants raised to their stoichiometric coefficients, divided by the product of the concentrations of the products raised to their stoichiometric coefficients.
Heterogeneous Equilibrium Constant (Kp): This is the equilibrium constant for reactions that take place in different phases. It is defined as the product of the partial pressures of the reactants raised to their stoichiometric coefficients, divided by the product of the partial pressures of the products raised to their stoichiometric coefficients.
Ionization Constant (Ka/Kb): This is the equilibrium constant for the ionization of weak acids or bases. It is defined as the product of the concentration of the products (H+ or OH-) raised to their stoichiometric coefficients, divided by the concentration of the acid or base.
Dissociation Constant (Kd): This is the equilibrium constant for the dissociation of a complex molecule into its constituent parts. It is defined as the product of the concentrations of the products raised to their stoichiometric coefficients, divided by the concentration of the complex.
Solubility Product Constant (Ksp): This is the equilibrium constant for the dissolution of a sparingly soluble salt. It is defined as the product of the concentrations of the dissolved ions raised to their stoichiometric coefficients, divided by the concentration of the solid salt.
Reaction Quotient (Qc/Qp): This is the mathematical expression of the concentration or partial pressure of the reactants and products in the reaction, calculated at any point in time during the reaction. It can be compared to the equilibrium constant to determine the direction and extent of the reaction.
Equilibrium Constant Expressions (Keq): This is the general notation used to represent the equilibrium constant for any chemical reaction. The expression is obtained by substituting the concentrations or partial pressures of the reactants and products into the equation for the equilibrium constant.
"a state approached by a dynamic chemical system after sufficient time has elapsed at which its composition has no measurable tendency towards further change."
"For a given set of reaction conditions, the equilibrium constant is independent of the initial analytical concentrations of the reactant and product species in the mixture."
"Thus, given the initial composition of a system, known equilibrium constant values can be used to determine the composition of the system at equilibrium."
"reaction parameters like temperature, solvent, and ionic strength may all influence the value of the equilibrium constant."
"A knowledge of equilibrium constants is essential for the understanding of many chemical systems."
"biochemical processes such as oxygen transport by hemoglobin in blood and acid–base homeostasis in the human body."
"Stability constants, formation constants, binding constants, association constants and dissociation constants are all types of equilibrium constants."
"temperature... may all influence the value of the equilibrium constant."
"solvent... may all influence the value of the equilibrium constant."
"acid–base homeostasis in the human body."
"oxygen transport by hemoglobin in blood."
"its composition has no measurable tendency towards further change."
"For a given set of reaction conditions, the equilibrium constant is independent of the initial analytical concentrations of the reactant and product species in the mixture."
"Stability constants, formation constants, binding constants, association constants and dissociation constants are all types of equilibrium constants."
"determine the composition of the system at equilibrium."
"The equilibrium constant is independent of the initial analytical concentrations of the reactant and product species in the mixture."
"a state approached by a dynamic chemical system after sufficient time has elapsed"
"The equilibrium constant is independent of the initial analytical concentrations of the reactant and product species in the mixture."
"Stability constants, formation constants, binding constants, association constants, and dissociation constants are all types of equilibrium constants."