Final answer:
A reversible reaction does not occur exclusively in any particular phase and reaches a point where the rate of the forward reaction equals that of the reverse reaction, leading to chemical equilibrium.
Step-by-step explanation:
A reversible reaction is a reaction that can occur in both the forward and reverse directions, where the conversion of reactants to products and the conversion of products back to reactants happens simultaneously. Such reactions can take place in any phase - solid, liquid, gaseous, or aqueous. The key characteristic of a reversible reaction is that at some point, a state called chemical equilibrium is reached. This is when the rate of the forward reaction equals the rate of the reverse reaction, and as a result, the concentration of the reactants and products remains constant over time.
For example, when carbon dioxide dissolves in water, it can do so as a gas dissolved in water or by reacting with water to produce carbonic acid. However, a reversible reaction does not depend on the phase of the reactants or products. Therefore, none of the options A. Liquid phase, B. Gaseous phase, C. Solid phase, D. Aqueous phase exclusively define where a reversible reaction can occur.