In dynamic equilibrium of a chemical reaction, the rates of forward and reverse reactions are equal, leading to constant but not necessarily equal concentrations of reactants and products. This equilibrium is dynamic, ongoing, and represented by a double-headed arrow in chemical equations.
Which statement is true of a chemical reaction in dynamic equilibrium? The true statement is that at the point when the rate of the reverse reaction becomes equal to the rate of the forward reaction, equilibrium is reached. The concentrations of the reactants and products do not change at equilibrium because they are consumed and re-formed at the same rate. However, this does not mean the amounts of reactants and products are equal; rather, their concentrations remain constant over time while the reaction is ongoing in both directions. This concept is often represented using a double-headed arrow.
Conditions for a chemical system to achieve dynamic equilibrium include that the system must be closed, with no net changes in the concentrations of reactants and products, as the rates of the forward and reverse reactions must be equal. The equilibrium constant, K, reflects the steady state at which a reversible reaction occurs and is an important concept in understanding chemical equilibrium.
The complete question is- which statement is true of a chemical reaction in dynamic equilibrium? group of answer choices
1.the amounts of reactants and products are equal.
2.all of the reactants are consumed and the forward reaction stops.
3.the concentration of reactants is equal to the concentration of products rate forward