GIBBS FREE ENERGY Meaning and
Definition
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Gibbs free energy, also referred to as Gibbs energy or G, is a thermodynamic function that measures the maximum amount of reversible work that can be obtained from a system under constant temperature and pressure conditions. Named after the American physicist Josiah Willard Gibbs, this concept plays a crucial role in determining the spontaneity of a chemical or physical process.
Gibbs free energy encompasses both enthalpy (the heat energy exchanged during a process) and entropy (the measure of disorder or randomness in a system). It is denoted as ∆G, where ∆ represents the change in free energy between the initial and final states of the system. A negative ∆G implies that the process is spontaneous, as it indicates a decrease in the overall energy of the system.
The Gibbs free energy is widely used in chemistry and physics to predict the direction of chemical reactions and phase changes. By comparing the calculated ∆G value to a standard value, known as the standard Gibbs free energy (∆G°), scientists can determine whether a reaction is energetically favorable or not. If the ∆G value is lower than ∆G°, the reaction will proceed spontaneously. Conversely, if the ∆G value is higher than ∆G°, the reaction will not proceed spontaneously and requires an input of energy to occur.
Overall, the Gibbs free energy serves as a fundamental tool for understanding the energetic aspect of chemical processes, providing valuable insights into the viability and spontaneity of reactions.
