"In chemistry, the law of mass action is the proposition that the rate of the chemical reaction is directly proportional to the product of the activities or concentrations of the reactants."
A law that states that the rate of a chemical reaction is proportional to the product of the concentrations/pressures of the reactants, each raised to a power equal to its stoichiometric coefficient.
Chemical Equilibrium: The balanced state where the rate of the forward reaction is equal to the rate of the reverse reaction, leading to a constant concentration of reactants and products.
Reaction Quotient (Q): The mathematical expression that shows the ratio of the product of reactant concentrations to the product of product concentrations at any point in a chemical reaction.
Equilibrium Constant (Kc): The numerical value that is determined from the concentrations of reactants and products at equilibrium, indicating the extent of a chemical reaction.
Law of Mass Action: The principle that the rate of a chemical reaction is proportional to the product of the concentrations of the reactants raised to their stoichiometric coefficients.
Le Chatelier’s Principle: The principle that states that a system at equilibrium will respond to any change in conditions to re-establish equilibrium, by shifting the position of equilibrium in the direction that opposes the external change.
Homogeneous Equilibria: Chemical equilibria where all reactants and products are in the same phase.
Heterogeneous Equilibria: Chemical equilibria where reactants and products are in different phases.
Calculating Equilibrium Concentrations: The process of using the equilibrium constant and stoichiometry to calculate the equilibrium concentrations of reactants and products.
Changes in Equilibrium: The effects of changes in temperature, pressure, and concentration on the position of equilibrium and the equilibrium constant.
Acid-Base Equilibria: Chemical equilibria involving weak acids and bases, and their conjugate acid-base pairs.
Salt Hydrolysis: The process of a salt reacting with water to produce an acidic or basic solution, depending on the acidity or basicity of the anion or cation.
Multiple Equilibria: Chemical systems where more than one equilibria exist, and the equilibria are interdependent.
Ionic Equilibria: Chemical equilibria involving ionic compounds and their interactions with water.
Solubility Equilibria: Chemical equilibria involving the dissolution and precipitation of salts in water.
Redox Equilibria: Chemical equilibria involving the transfer of electrons between reactants, often in the form of an oxidation-reduction (redox) reaction.
Homogeneous Chemical Equilibrium: Homogeneous chemical equilibrium refers to a state in which the rate of forward and reverse reactions become equal, and the concentrations of reactants and products remain constant.
Heterogeneous Chemical Equilibrium: Heterogeneous chemical equilibrium refers to the state in which reactants and products exist in different physical phases, such as solid, liquid, or gas, where their concentrations remain constant over time.
Gas Phase Chemical Equilibrium: Gas phase chemical equilibrium refers to a state in which the rates of the forward and reverse reactions in a gas-phase chemical reaction become equal, resulting in a constant concentration of reactants and products.
Liquid Phase Chemical Equilibrium: Liquid Phase Chemical Equilibrium refers to the state in which the rate of forward and reverse reactions occurring in a liquid system are equal, resulting in a constant concentration of reactants and products.
Solid Phase Chemical Equilibrium: Solid phase chemical equilibrium refers to the equilibrium state between a solid substance and its dissolved ions in a solution.
Complex Chemical Equilibrium: Complex chemical equilibrium refers to the dynamic balance among multiple simultaneous reactions involving multiple reactants and products.
Reversible Chemical Equilibrium: Reversible chemical equilibrium refers to the state in a chemical reaction where the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products with time.
Irreversible Chemical Equilibrium: Irreversible Chemical Equilibrium refers to a scenario in which a reaction proceeds predominantly in one direction and does not achieve a state of balance between reactants and products.
Dynamic Chemical Equilibrium: Dynamic chemical equilibrium refers to a state in a chemical reaction where the rates of the forward and reverse reactions are equal, leading to no net change in the concentrations of reactants and products over time.
Static Chemical Equilibrium: Static chemical equilibrium refers to a state in a chemical reaction where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products.
Ionic Chemical Equilibrium: Ionic chemical equilibrium refers to the balance between ionized and unionized species in a solution where both forward and reverse reactions occur at an equal rate.
Acid-Base Equilibrium: Acid-Base Equilibrium refers to the balance between the dissociation and recombination of hydrogen ions and hydroxide ions in water, involving acids and bases.
Redox Equilibrium: Redox equilibrium refers to the balance between reduction and oxidation reactions in a chemical system.
Solubility Equilibrium: Solubility equilibrium pertains to the balance between dissolved and undissolved particles in a saturated solution at a specific temperature.
Adsorption Equilibrium: Adsorption equilibrium in chemistry refers to the balance between the adsorption and desorption of molecules onto a solid surface, determined by the concentration of the adsorbate and the affinity of the surface.
Surface Equilibrium: Surface equilibrium is the distribution of reactants and products between the surface and gas phase, determined by the law of mass action, at which the rates of adsorption and desorption are equal.
"It explains and predicts behaviors of solutions in dynamic equilibrium."
"It implies that for a chemical reaction mixture that is in equilibrium, the ratio between the concentration of reactants and products is constant."
"Guldberg and Waage between 1864 and 1879."
"The equilibrium aspect, concerning the composition of a reaction mixture at equilibrium, and the kinetic aspect concerning the rate equations for elementary reactions."
"Equilibrium constants were derived by using kinetic data and the rate equation which they had proposed."
"Guldberg and Waage also recognized that chemical equilibrium is a dynamic process in which rates of reaction for the forward and backward reactions must be equal at chemical equilibrium."
"In order to derive the expression of the equilibrium constant appealing to kinetics, the expression of the rate equation must be used."
"The expression of the rate equations was rediscovered later independently by Jacobus Henricus van 't Hoff."
"The law is a statement about equilibrium and gives an expression for the equilibrium constant, a quantity characterizing chemical equilibrium."
"In modern chemistry, this is derived using equilibrium thermodynamics."
"It can also be derived with the concept of chemical potential."
"The rate of the chemical reaction is directly proportional to the product of the activities or concentrations of the reactants."
"It explains and predicts behaviors of solutions in dynamic equilibrium."
"Guldberg and Waage conducted the research."
"Equilibrium constants were derived by using kinetic data and the rate equation."
"Guldberg and Waage recognized that chemical equilibrium is a dynamic process."
"In order to derive the expression of the equilibrium constant appealing to kinetics, the expression of the rate equation must be used."
"Jacobus Henricus van 't Hoff rediscovered the expression of the rate equations."
"The equilibrium constant can also be derived with the concept of chemical potential."