Chemical Equilibrium: Characteristics and Definition

Chemical Equilibrium

Definition

• 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.

Characteristics

• 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.

Types of Equilibrium

• 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).

Factors Affecting Equilibrium

• 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.

Le Chatelier's Principle

• 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 Calculations

• 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

Definition and Characteristics

• 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.

Equilibrium Constant and Expression

• 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.

Types of Equilibrium

• 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).

Factors Affecting Equilibrium

• 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.

Le Chatelier's Principle

• 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 Calculations

• 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.