Questions: Which of the following statements about equilibrium of chemical reactions is correct?

Solution Steps

Let's evaluate each statement to determine its correctness regarding chemical equilibrium:

1. Reactions can only go in the direction toward equilibrium.
   This statement is generally true. Reactions tend to proceed in the direction that moves them toward equilibrium, where the rates of the forward and reverse reactions are equal.

2. A reaction that is at equilibrium is not capable of doing any work.
   This statement is true. At equilibrium, there is no net change in the concentrations of reactants and products, and the system is at its lowest free energy state, meaning it cannot perform work.

3. The equilibrium point is where the system has the highest free energy.
   This statement is false. The equilibrium point is where the system has the lowest free energy, not the highest.

4. Most reactions in a living cell are close to equilibrium.
   This statement is generally false. Many reactions in living cells are far from equilibrium, as they are often driven by energy inputs to maintain life processes.

5. The equilibrium point of a reaction represents the least stable configuration for that reaction.
   This statement is false. The equilibrium point represents a stable configuration where the free energy is minimized.

Based on the analysis above, the correct statement about the equilibrium of chemical reactions is:

• A reaction that is at equilibrium is not capable of doing any work.

Final Answer