Question

Chemical reactions are reversible; they can proceed in both the forward and reverse directions. If the ΔG° for the reaction Y!X is energetically favorable, how can you explain the fact that not all of the Y molecules will be converted to X molecules?

Answer 1

Chemical reactions are reversible, meaning they can proceed in both the forward and reverse directions. The fact that not all of the Y molecules will be converted to X molecules, even if the reaction is energetically favorable (has a negative ΔG°), can be explained by the concept of equilibrium.

Step-by-step explanation:

Chemical reactions are reversible, meaning they can proceed in both the forward and reverse directions.

The fact that not all of the Y molecules will be converted to X molecules, even if the reaction is energetically favorable (has a negative ΔG°), can be explained by the concept of equilibrium.

In a reversible reaction, reactants are turned into products, but when the concentration of products goes beyond a certain threshold, some of these products will be converted back into reactants.

This back and forth continues until a state of equilibrium is reached, where the concentrations of reactants and products remain constant.