- "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 topic covers the concept of chemical equilibrium, including Le Chatelier’s principle, equilibrium constants, and acid-base and solubility equilibrium.
Reaction Quotient (Qc/Qp): The ratio of concentrations of products to reactants at any point in reaction, which helps determine whether the reaction has reached equilibrium or not.
Equilibrium Constant (Kc/Kp): 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.
Le Chatelier's Principle: A principle that states that when a system in equilibrium is subjected to a stress, it will shift position to counteract the stress and re-establish equilibrium.
Factors Affecting Equilibrium: Factors such as temperature, pressure, and concentration that affect the position of the equilibrium and determine the rate of reaction.
Acid-Base Equilibria: Equilibria involving the transfer of protons between species in solution, characterized by the acid dissociation constant, Ka, and the base dissociation constant, Kb.
Solubility Equilibria: Equilibria involving the dissolution of sparingly soluble salts in water, characterized by the solubility product constant, Ksp.
Equilibrium Calculations: 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.
Heterogeneous Equilibria: Equilibria involving reactants and/or products in different physical states, such as gases, liquids, and solids.
The Law of Mass Action: 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.
Equilibrium Expressions: Mathematical expressions that describe the equilibrium concentrations/pressures of reactants and products in terms of the equilibrium constant and initial concentrations/pressures.
- "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."