Which of the following statements is true about reversible reactions?

Reversible reactions are characterized by their ability to proceed in both the forward and reverse directions. When a reversible reaction occurs, it can reach a state known as dynamic equilibrium. At this point, the concentrations of the reactants and products remain constant because the rate of the forward reaction equals the rate of the reverse reaction. This equilibrium can be influenced by changes in temperature, pressure, and concentration, allowing for the system to shift in either direction depending on the conditions.

The statement regarding the occurrence of reversible reactions only at high temperatures is not accurate, as reversible reactions can take place at a range of temperatures. Similarly, saying that reversible reactions are inherently irreversible or can only proceed in one direction contradicts the very definition of a reversible reaction. In reality, the hallmark of reversible reactions is their capacity to reach a balance between reactants and products, which is precisely what dynamic equilibrium represents.