Dynamic equilibrium in chemistry is a state where reversible reactions occur at equal rates, maintaining constant reactant and product concentrations. This concept is crucial for understanding chemical processes in closed systems and differentiates from static equilibrium. It's exemplified by the Haber process and iodine sublimation, impacting industrial and natural phenomena.
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Dynamic equilibrium is a fundamental concept in chemistry that describes a state of balance in a reversible chemical reaction
Dynamic equilibrium occurs in a closed system where a reversible chemical reaction takes place
In dynamic equilibrium, the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products
In dynamic equilibrium, the concentrations of reactants and products remain constant over time
While the system may appear static, at the molecular level, there is ongoing activity as molecules are continuously reacting and interconverting
Dynamic equilibrium is different from static equilibrium, where no reactions are occurring
Dynamic equilibrium can be observed in various processes, such as the equilibrium between solid and gaseous iodine and the Haber process for producing ammonia
Dynamic equilibrium plays a crucial role in maintaining the efficiency and continuity of chemical processes
Non-equilibrium dynamics, which studies systems that are not in equilibrium, uses principles of dynamic equilibrium to understand and predict the behavior of dynamic systems
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Characteristics of a closed system in dynamic equilibrium
No exchange with surroundings, reaction rates equal, constant reactant and product concentrations.
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Effect of dynamic equilibrium on reactant and product levels
Reactant and product levels stabilize, no net change in concentration despite ongoing reactions.
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Analogy for understanding dynamic equilibrium
Similar to a room with equal numbers of people entering and leaving, maintaining a steady population inside.
