⏱️general chemistry ii review

key term - Dynamic Equilibrium

Definition

Dynamic equilibrium is a state in a reversible reaction where the rates of the forward and reverse reactions are equal, leading to constant concentrations of reactants and products over time. This concept is crucial for understanding how systems respond to changes in conditions and is essential for grasping precipitation reactions, solubility product constants, and the influence of external factors on chemical systems.

5 Must Know Facts For Your Next Test

  1. In dynamic equilibrium, even though the concentrations of reactants and products remain constant, molecular interactions continue to occur, maintaining a balance.
  2. The addition of a common ion can shift the position of equilibrium, affecting solubility and precipitation reactions by driving the formation or dissolution of solid phases.
  3. The equilibrium constant expression for a reaction at dynamic equilibrium is temperature-dependent and varies with changes in temperature.
  4. Changing conditions such as concentration, pressure, or temperature can shift the position of dynamic equilibrium according to Le Chatelier's Principle, resulting in a new equilibrium state.
  5. Dynamic equilibrium is not static; it involves continuous processes occurring in both directions, which is vital for understanding chemical systems in real-world scenarios.

Review Questions

  • How does Le Chatelier's Principle relate to dynamic equilibrium in chemical reactions?
    • Le Chatelier's Principle is closely tied to dynamic equilibrium because it explains how a system at equilibrium responds to external changes. When a stressor, like a change in concentration or temperature, is applied, the system will adjust its position to counteract that change. This means that if you add more reactant or product, the system will shift to either favor the forward or reverse reaction to re-establish dynamic equilibrium.
  • What role does Ksp play in understanding dynamic equilibrium for sparingly soluble ionic compounds?
    • Ksp is fundamental in understanding dynamic equilibrium as it quantifies the solubility of sparingly soluble ionic compounds at equilibrium. When these compounds dissolve, they establish an equilibrium between solid and dissolved ions. The value of Ksp helps predict whether a precipitate will form when conditions change, such as when common ions are added, thereby influencing dynamic equilibrium within that system.
  • Evaluate how factors like temperature and pressure can alter dynamic equilibrium in gas-phase reactions.
    • Factors such as temperature and pressure significantly affect dynamic equilibrium in gas-phase reactions due to their direct influence on reaction rates and concentrations. Increasing temperature typically shifts the equilibrium towards endothermic reactions, while decreasing it favors exothermic reactions. For reactions involving gases, altering pressure can shift the balance towards side with fewer moles of gas, effectively changing the concentrations of reactants and products. Understanding these shifts helps predict how systems behave under various conditions, crucial for optimizing chemical processes.