What does a negative Gibbs free energy change indicate about a reaction?

What does a negative Gibbs free energy change indicate about a reaction?

• A. It indicates the reaction is non-spontaneous
• B. It indicates the reaction is at equilibrium
• C. It indicates the reaction is spontaneous
• D. It indicates a high activation energy

Answer: (C)

A negative Gibbs free energy change indicates that the reaction is spontaneous under the given conditions. This means that the reaction can proceed forward without the need for external energy input. When the Gibbs free energy is negative, it signifies that the products of the reaction are at a lower energy state than the reactants, which suggests that the reaction is thermodynamically favorable. The spontaneous nature does not guarantee the speed of the reaction; it simply means that there is a drive for the reaction to occur. The concept of spontaneity is crucial in electrochemistry, as it relates directly to the feasibility of reactions occurring in an electrochemical cell. In contrast, a positive Gibbs free energy would indicate a non-spontaneous reaction that requires energy input to proceed, while an equilibrium state would show a Gibbs free energy change of zero, reflecting that there is no net change in the concentration of products and reactants. High activation energy pertains more to the rate of the reaction rather than its spontaneity, indicating that while a reaction may be thermodynamically favorable, it may still proceed at a slow rate if the activation barrier is significant.

A negative Gibbs free energy change indicates that the reaction is spontaneous under the given conditions. This means that the reaction can proceed forward without the need for external energy input. When the Gibbs free energy is negative, it signifies that the products of the reaction are at a lower energy state than the reactants, which suggests that the reaction is thermodynamically favorable.

The spontaneous nature does not guarantee the speed of the reaction; it simply means that there is a drive for the reaction to occur. The concept of spontaneity is crucial in electrochemistry, as it relates directly to the feasibility of reactions occurring in an electrochemical cell.

In contrast, a positive Gibbs free energy would indicate a non-spontaneous reaction that requires energy input to proceed, while an equilibrium state would show a Gibbs free energy change of zero, reflecting that there is no net change in the concentration of products and reactants. High activation energy pertains more to the rate of the reaction rather than its spontaneity, indicating that while a reaction may be thermodynamically favorable, it may still proceed at a slow rate if the activation barrier is significant.