In the equation ΔG = ΔH - TΔS, what is ΔG?

In the equation ΔG = ΔH - TΔS, what is ΔG?

• A. The change in enthalpy
• B. The change in free energy
• C. The change in entropy
• D. The change in temperature

Answer: (B)

In the equation ΔG = ΔH - TΔS, ΔG represents the change in free energy of a system. This concept is fundamental in thermodynamics and helps in predicting the spontaneity of a reaction. A negative ΔG indicates that a reaction can occur spontaneously, while a positive ΔG suggests that the reaction is non-spontaneous under standard conditions. Understanding ΔG is crucial because it incorporates both the enthalpy change (ΔH), which reflects the heat content of the system, and the entropy change (ΔS), which measures the disorder or randomness of the system at a given temperature (T). By adjusting for temperature, the equation effectively balances the contributions of both energy and disorder, providing a comprehensive view of the energy available to perform work in a chemical reaction. Thus, ΔG is a key indicator of the thermodynamic favorability of processes and reactions.

In the equation ΔG = ΔH - TΔS, ΔG represents the change in free energy of a system. This concept is fundamental in thermodynamics and helps in predicting the spontaneity of a reaction. A negative ΔG indicates that a reaction can occur spontaneously, while a positive ΔG suggests that the reaction is non-spontaneous under standard conditions.

Understanding ΔG is crucial because it incorporates both the enthalpy change (ΔH), which reflects the heat content of the system, and the entropy change (ΔS), which measures the disorder or randomness of the system at a given temperature (T). By adjusting for temperature, the equation effectively balances the contributions of both energy and disorder, providing a comprehensive view of the energy available to perform work in a chemical reaction. Thus, ΔG is a key indicator of the thermodynamic favorability of processes and reactions.