Predicting the invisible: How Gibbs Free Energy determines chemical fate
In short: Why do some chemical reactions happen spontaneously while others require a constant push? This video explains how scientists use the Gibbs Free Energy equation to predict the feasibility of reactions by balancing heat, entropy, and temperature.
The Gibbs Free Energy ($\Delta G$) serves as a vital tool in chemical thermodynamics to determine if a process is spontaneous. By calculating $\Delta G$ using enthalpy ($\Delta H$), entropy ($\Delta S$), and temperature ($T$), scientists can predict the direction of a reaction. A negative $\Delta G$ indicates a spontaneous process, while a positive value means it is non-spontaneous. When $\Delta G$ equals zero, the system has reached equilibrium.
While total entropy change can also predict reaction direction, chemists often prefer Gibbs Free Energy because it frames these changes in terms of energy—a more familiar concept for analyzing chemical feasibility and equilibrium constants.
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Sources
- Summary by Intellect · source: Using Gibbs Free Energy
- Also: The Gibbs free energy | Post-16 thermodynamics tutorials
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