Which of the following can be a consequence of a negative change in free energy?

• A. The reaction is non-spontaneous
• B. The reaction is spontaneous
• C. The reaction requires additional energy to proceed
• D. The reaction results in the formation of unstable products

Answer: (B)

A negative change in free energy (ΔG < 0) indicates that a reaction can occur spontaneously. This means that the products of the reaction have lower free energy than the reactants, thereby favoring the formation of products without the need for additional energy input.

In spontaneous reactions, the system moves toward greater stability, typically resulting in the release of energy in the form of heat or work. Thus, a reaction characterized by a negative ΔG is thermodynamically favorable and occurs naturally under standard conditions.

The other options focus on criteria that do not align with a negative change in free energy. A non-spontaneous reaction would have a positive ΔG, and reactions requiring additional energy to proceed suggest an unfavorable reaction direction rather than spontaneity. Additionally, the formation of unstable products may indicate kinetic or thermodynamic barriers, which again does not reflect the characteristic of a spontaneous process indicated by a negative ΔG. Therefore, a negative change in free energy clearly indicates that the reaction is spontaneous.