key term - Homogeneous equilibrium

Definition

Homogeneous equilibrium is a state of balance in a chemical reaction where all reactants and products are in the same phase, typically gaseous or aqueous. This type of equilibrium is influenced by changes in temperature and pressure, which can shift the balance between reactants and products, ultimately affecting the concentrations of each species in the system.

5 Must Know Facts For Your Next Test

1. In homogeneous equilibrium, all reactants and products are in the same phase, allowing for uniform concentration throughout the system.
2. Changes in temperature can affect the position of homogeneous equilibrium by favoring either endothermic or exothermic reactions based on the direction of the temperature change.
3. Pressure changes primarily affect gaseous equilibria; increasing pressure will shift the equilibrium position towards the side with fewer moles of gas.
4. Homogeneous equilibria can be represented using equilibrium constants (K), which quantify the concentrations of reactants and products when equilibrium is achieved.
5. Dynamic processes occur at homogeneous equilibrium, meaning that while concentrations remain constant, reactions continue to take place at equal rates in both directions.

Review Questions

• How does Le Chatelier's Principle apply to homogeneous equilibrium when there is a change in temperature?
  • Le Chatelier's Principle states that a system at equilibrium will respond to external changes by shifting its position to minimize the effect of those changes. When temperature changes, it affects the rates of the forward and reverse reactions differently, favoring either the endothermic or exothermic process depending on whether heat is added or removed. As a result, the system shifts toward either reactants or products to establish a new equilibrium state.
• Discuss how pressure changes influence homogeneous equilibrium involving gaseous reactants and products.
  • In homogeneous equilibria involving gases, pressure changes can significantly influence the position of equilibrium. According to Le Chatelier's Principle, if pressure is increased, the system will shift towards the side with fewer moles of gas to reduce pressure. Conversely, if pressure is decreased, it will favor the side with more moles of gas. This shift alters the concentrations of reactants and products until a new equilibrium is established.
• Evaluate how understanding homogeneous equilibrium can enhance predictions about chemical reactions under varying conditions.
  • Understanding homogeneous equilibrium allows chemists to predict how reactions will respond to changes in conditions like temperature and pressure. By applying Le Chatelier's Principle and analyzing reaction quotients (Q) against equilibrium constants (K), one can foresee shifts in product and reactant concentrations. This knowledge is crucial for optimizing industrial processes, enhancing yield, and controlling reaction pathways effectively in real-world applications.

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 to counteract that change and restore a new equilibrium.

Reaction Quotient (Q): A ratio that compares the concentrations of products to reactants at any point in a reaction, used to predict the direction in which a reaction will proceed to reach 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.