By ECZ Study Tool, September 25, 2023
Equilibrium in chemistry refers to a state in which a chemical reaction has reached a balance, where the rates of the forward and reverse reactions are equal. In other words, in a chemical equilibrium, the concentrations of reactants and products remain relatively constant over time, though individual molecules continue to react.
Key points about equilibrium include:
Dynamic Balance: Equilibrium is a dynamic state, meaning that even
though individual molecules are constantly reacting, the overall concentrations
of reactants and products do not change. It's like a tug-of-war where the two
teams pull with equal strength, resulting in a stable position.
Reversible Reactions: Equilibrium is most commonly associated with
reversible reactions, where reactants can interconvert into products and vice
versa. The reaction can proceed in both directions simultaneously.
Equilibrium Constant: Equilibrium is characterized by an
equilibrium constant (K), which expresses the ratio of the concentrations of
products to reactants at equilibrium. The specific value of K depends on the
reaction and the temperature.
Applications: Equilibrium is essential in various chemical
processes, including chemical reactions in solution, industrial processes, and
biological systems. It plays a crucial role in understanding reaction rates and
predicting the composition of a system at equilibrium.
Physical Equilibrium: Equilibrium is not limited to chemical
reactions; it also applies to physical processes such as phase changes (e.g.,
solid-liquid equilibrium during melting) and the solubility of substances.
Understanding chemical equilibrium
is fundamental in chemistry, helping scientists predict and control the
outcomes of reactions and processes, and it has applications in fields such as
chemical engineering and environmental science.
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