Gibbs Free Energy of Dissolution is pivotal in thermodynamics, determining the spontaneity of solutes dissolving in solvents. It involves the enthalpy change (ΔH), absolute temperature (T), and entropy change (ΔS). Negative ΔG indicates spontaneous dissolution, crucial for solubility predictions. Real-world examples and experiments, like sugar in tea and borax in water, demonstrate its practical significance. Its calculation is vital in industries like pharmaceuticals for drug solubility and environmental science for water treatment strategies.
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The Gibbs Free Energy of Dissolution is calculated using the equation ΔG = ΔH - TΔS, where ΔH is the enthalpy change, T is the absolute temperature in Kelvin, and ΔS is the entropy change
Spontaneity of dissolution
A negative ΔG indicates a spontaneous dissolution process, while a positive ΔG suggests that the process is non-spontaneous
Predicting solubility
The Gibbs Free Energy of Dissolution is critical for predicting solubility under various conditions
ΔG is influenced by changes in both enthalpy and entropy, which together determine the system's thermodynamics
The enthalpy change can be either exothermic or endothermic, depending on whether heat is released or absorbed
The entropy term, TΔS, quantifies the change in disorder as solute and solvent particles intermingle
The effect of temperature on the Free Energy of Dissolution is apparent when observing how sugar dissolves more readily in hot water compared to cold
Sugar dissolves in hot water through an endothermic process that increases the system's entropy, resulting in a negative Gibbs free energy change
Effervescent tablets demonstrate how dissolution is influenced by changes in energy and entropy
The dissolution of borax in water provides valuable data on the temperature dependence of solubility and free energy changes
The calculation of the Gibbs Free Energy of Dissolution is critical for predicting solubility under various conditions
The Standard Free Energy of Dissolution provides a benchmark for comparing different substances
The Gibbs Free Energy of Dissolution has applications in industries such as pharmaceuticals and environmental science
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Gibbs Free Energy of Dissolution (ΔG) Equation Components
ΔG = ΔH - TΔS; ΔH = enthalpy change, T = temperature in Kelvin, ΔS = entropy change.
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Positive ΔG Implication for Solute Dissolution
A positive ΔG suggests the dissolution process is non-spontaneous and not favored at a given temperature.
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Role of ΔG in Predicting Solubility
ΔG determines spontaneity of dissolution; crucial for predicting substance solubility in various conditions.
