🧤physical chemistry i review

key term - Dynamic Equilibrium

Definition

Dynamic equilibrium refers to a state in a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction, resulting in no net change in the concentrations of reactants and products. This balance is sensitive to changes in temperature and pressure, which can shift the position of equilibrium, affecting how the system responds to external conditions.

5 Must Know Facts For Your Next Test

  1. In dynamic equilibrium, even though concentrations remain constant, both forward and reverse reactions continue to occur at equal rates.
  2. Changes in temperature can affect the position of equilibrium by favoring either the endothermic or exothermic direction of a reaction.
  3. Increasing pressure in a gaseous system at equilibrium will shift the position toward the side with fewer moles of gas.
  4. The value of the equilibrium constant (K) is temperature-dependent, meaning it can change if temperature varies, impacting the equilibrium position.
  5. Dynamic equilibrium is not limited to chemical reactions; it can also apply to physical processes like phase changes, where solid, liquid, and gas phases coexist.

Review Questions

  • How does Le Chatelier's Principle relate to dynamic equilibrium in terms of external changes?
    • Le Chatelier's Principle is directly connected to dynamic equilibrium as it describes how a system at equilibrium responds to external changes. When conditions such as temperature or pressure are altered, the system adjusts its equilibrium position to minimize that disturbance. For instance, increasing pressure will favor the side with fewer gas molecules, allowing the reaction to reach a new state of dynamic equilibrium that counteracts the change.
  • What role does temperature play in shifting the position of dynamic equilibrium?
    • Temperature plays a crucial role in determining the position of dynamic equilibrium. For an endothermic reaction, increasing temperature shifts the equilibrium toward products, while for an exothermic reaction, higher temperatures favor reactants. This means that any change in temperature will not only affect the rate at which reactions occur but also change the concentrations of reactants and products at equilibrium, demonstrating how sensitive these systems are to thermal conditions.
  • Evaluate how understanding dynamic equilibrium can influence industrial processes that rely on chemical reactions.
    • Understanding dynamic equilibrium is vital for optimizing industrial processes because it allows chemists and engineers to manipulate conditions for maximum yield. By applying principles such as Le Chatelier's Principle, industries can adjust temperature and pressure to favor product formation in reversible reactions. This knowledge helps in designing more efficient processes, reducing costs, and enhancing productivity while ensuring sustainable practices by minimizing waste through better control of reaction conditions.