key term - Heterogeneous equilibria

Definition

Heterogeneous equilibria refer to the state of balance in a chemical reaction where the reactants and products are present in different phases, such as solids, liquids, and gases. This type of equilibrium is important because it emphasizes how the concentrations of substances in various phases impact the overall equilibrium constant and how calculations for equilibrium concentrations must account for these differences in states.

5 Must Know Facts For Your Next Test

1. In heterogeneous equilibria, only the concentrations of gaseous and aqueous species appear in the equilibrium constant expression, while solids and pure liquids are not included because their concentrations remain constant.
2. The position of heterogeneous equilibria can be affected by changes in temperature, pressure, and concentration, following Le Chatelier's Principle.
3. Calculating equilibrium concentrations for reactions involving heterogeneous equilibria often requires determining the molar amounts of each phase present at equilibrium.
4. In reactions where solids are involved, the concentration of the solid does not change and is therefore considered constant, simplifying the equilibrium expression.
5. Understanding heterogeneous equilibria is crucial for processes such as catalysis and extraction, where multiple phases interact.

Review Questions

• How do the phases of reactants and products influence the expression for the equilibrium constant in heterogeneous equilibria?
  • In heterogeneous equilibria, only the concentrations of gaseous and aqueous reactants and products are included in the equilibrium constant expression. This is because solids and pure liquids have constant concentrations and do not affect the system's dynamics. Therefore, when calculating K for a reaction involving different phases, one must recognize which species contribute to the value of K based on their states.
• Discuss how Le Chatelier's Principle applies to heterogeneous equilibria when external changes are made to a system.
  • Le Chatelier's Principle states that a system at equilibrium will shift in response to external changes to re-establish balance. In heterogeneous equilibria, if pressure is increased by reducing volume, for example, the system may shift toward the side with fewer gas molecules. Similarly, adding a reactant or removing a product would drive the reaction forward to produce more products until a new equilibrium is reached. The presence of different phases complicates these adjustments but still adheres to this fundamental principle.
• Evaluate how understanding heterogeneous equilibria is crucial for practical applications such as catalysis and industrial processes.
  • Understanding heterogeneous equilibria is vital for optimizing catalytic reactions and industrial processes where multiple phases coexist. For example, in catalytic converters used in automobiles, gas-phase reactants interact with solid catalysts to facilitate reactions. Knowledge of how these reactions reach equilibrium allows engineers to manipulate conditions like temperature and pressure effectively to maximize product yield. Additionally, recognizing how concentrations of each phase influence overall reaction rates can lead to more efficient designs in chemical manufacturing processes.

Related terms

Le Chatelier's Principle:

A principle stating that if an external change is applied to a system at equilibrium, the system will adjust itself to counteract that change and restore a new equilibrium.

Equilibrium Constant (K): A numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature.

Phase: A distinct state of matter (solid, liquid, gas) that has uniform properties throughout; relevant in determining how substances interact in heterogeneous equilibria.