Chemical Equilibrium: Characteristics and Definition

Study Notes

State in which the rates of forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products.
Equilibrium is a dynamic state, meaning that reactions are still occurring, but at equal rates.

Reversible reactions: Can proceed in both forward and reverse directions.
Equilibrium constant (K): A measure of the extent to which a reaction proceeds towards equilibrium.
Equilibrium expression: A mathematical expression that describes the equilibrium constant in terms of the concentrations of reactants and products.

Homogeneous equilibrium: Equilibrium in which all reactants and products are in the same phase (e.g., gas or liquid).
Heterogeneous equilibrium: Equilibrium in which reactants and products are in different phases (e.g., solid and gas).

Concentration: Increasing the concentration of a reactant or product can shift the equilibrium towards the product or reactant side.
Temperature: Changes in temperature can alter the equilibrium constant and shift the equilibrium.
Pressure: Changes in pressure can affect the equilibrium of reactions involving gases.
Catalysts: Substances that increase the rates of both forward and reverse reactions, but do not affect the equilibrium constant.

If a system at equilibrium is subjected to a change, the equilibrium will shift in a direction that counteracts the change.
This principle can be used to predict the response of a system to changes in concentration, temperature, or pressure.

Equilibrium constant (K): Can be calculated using the equilibrium expression and the concentrations of reactants and products.
Equilibrium concentrations: Can be calculated using the equilibrium constant and the initial concentrations of reactants and products.

Chemical equilibrium is a state where the rates of forward and reverse reactions are equal, resulting in no net change in concentrations of reactants and products.
Equilibrium is a dynamic state, meaning reactions are still occurring, but at equal rates.
Reversible reactions can proceed in both forward and reverse directions.

The equilibrium constant (K) measures the extent to which a reaction proceeds towards equilibrium.
The equilibrium expression is a mathematical expression that describes the equilibrium constant in terms of reactant and product concentrations.

Homogeneous equilibrium occurs when all reactants and products are in the same phase (e.g., gas or liquid).
Heterogeneous equilibrium occurs when reactants and products are in different phases (e.g., solid and gas).

Increasing the concentration of a reactant or product can shift the equilibrium towards the product or reactant side.
Changes in temperature can alter the equilibrium constant and shift the equilibrium.
Changes in pressure can affect the equilibrium of reactions involving gases.
Catalysts increase the rates of both forward and reverse reactions, but do not affect the equilibrium constant.

If a system at equilibrium is subjected to a change, the equilibrium will shift in a direction that counteracts the change.
This principle can be used to predict the response of a system to changes in concentration, temperature, or pressure.

The equilibrium constant (K) can be calculated using the equilibrium expression and reactant and product concentrations.
Equilibrium concentrations can be calculated using the equilibrium constant and initial reactant and product concentrations.