the question is, if concentrations do not change why is the equilibrium state considered dynamic? First of all I don't understand what makes a state dynamic?
The reaction is not stopped, it is going forward, and reverse, at the same rate. Molecules are constantly reacting in both directions.
The term "dynamic" refers to something that is constantly changing or in motion. In the context of the equilibrium state, it is considered dynamic because even though the concentrations of reactants and products do not change, the reaction is still ongoing, with molecules constantly reacting in both the forward and reverse directions.
To understand why the equilibrium state is considered dynamic, we need to understand the concept of a chemical equilibrium. In a chemical reaction, reactants are converted into products. Initially, when the reaction starts, the concentration of reactants is high, and there are fewer products. As the reaction progresses, the concentration of reactants decreases, and the concentration of products increases.
At a certain point, called the equilibrium point, the concentrations of reactants and products reach a state of balance, where the rate of the forward reaction is equal to the rate of the reverse reaction. At this point, the concentrations of reactants and products no longer change.
However, it's important to note that even though the concentrations of reactants and products remain constant, the individual molecules are still constantly moving and reacting with each other in both the forward and reverse directions. There is a dynamic exchange happening between reactants and products, where molecules are continuously forming products while simultaneously converting back into reactants.
This dynamic nature of the equilibrium state is crucial because it allows the reaction to be reversible. If the concentrations were completely static, without any molecular motion or reaction occurring, it would mean that the reaction has come to a complete stop. But in equilibrium, the balanced rates of the forward and reverse reactions ensure that the reaction is ongoing, albeit with no net change in overall concentrations.
In summary, the equilibrium state is considered dynamic because even though the concentrations of reactants and products do not change, the molecules are constantly moving and reacting, maintaining a balance between the forward and reverse reactions.