Chemical Equilibrium Quiz

Chemical Equilibrium

Definition

• Chemical equilibrium: a state where the rates of forward and reverse reactions are equal, and the concentrations of reactants and products remain constant.

Characteristics

• Equilibrium is a dynamic state, not a static one.
• The reaction is still occurring, but at equal rates in both directions.
• The equilibrium state is characterized by a constant ratio of concentrations of products to reactants.

Equilibrium Constant (K)

• A measure of the extent to which a reaction proceeds to completion.
• Represented by the symbol K (or Keq).
• Defined as the ratio of the concentrations of products to reactants at equilibrium.

Types of Equilibrium Constants

• Kc: equilibrium constant in terms of concentration (moles per liter).
• Kp: equilibrium constant in terms of partial pressures.

Factors Affecting Equilibrium

• Concentration: increasing the concentration of reactants drives the reaction forward.
• Temperature: increasing temperature can shift the equilibrium to the right (forward reaction) or left (reverse reaction).
• Pressure: increasing pressure can shift the equilibrium to the right (forward reaction) or left (reverse reaction).

Le Chatelier's Principle

• When a system in equilibrium is subjected to a change in concentration, temperature, or pressure, the equilibrium will shift to counteract the change.
• The system will respond to the change to re-establish equilibrium.

Applications of Equilibrium

• Industrial processes: optimizing reaction conditions to maximize yield and efficiency.
• Biological systems: understanding the regulation of metabolic pathways.
• Environmental systems: modeling the fate of pollutants in the environment.