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Thermodynamic Favorability

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Understanding thermodynamic favorability is crucial in predicting the spontaneity of chemical reactions. It involves the laws of thermodynamics, entropy, enthalpy, and Gibbs Free Energy. Reactions are favored when they lead to an increase in the universe's total entropy, which can be exothermic or endothermic. The distinction between thermodynamic and kinetic favorability is also essential, especially in organic chemistry where reaction conditions affect product formation.

Understanding Thermodynamic Favorability in Chemical Reactions

Thermodynamic favorability is a criterion used to predict whether a chemical reaction can proceed spontaneously after overcoming the activation energy barrier. This concept is based on the laws of thermodynamics, which govern energy and entropy in the universe. The first law, the law of conservation of energy, states that energy can neither be created nor destroyed, only converted from one form to another. The second law asserts that the entropy, or the degree of disorder, of an isolated system will tend to increase over time. The third law states that the entropy of a perfect crystal at absolute zero temperature is exactly zero. These principles help us understand the conditions under which chemical reactions occur spontaneously, which is essential for assessing thermodynamic favorability.
Glass beaker with lit blue liquid on white surface, lit Bunsen burner underneath and immersed thermometer, in laboratory.

Entropy and Enthalpy: The Drivers of Chemical Reactions

Entropy (S) and enthalpy (H) are key thermodynamic quantities that influence the spontaneity of chemical reactions. Entropy quantifies the disorder or randomness within a system, with an increase in entropy reflecting a transition to a more disordered state. The change in entropy (∆S) is determined by the difference in entropy between the products and the reactants. Enthalpy represents the total heat content of a system under constant pressure. Reactions that release heat, known as exothermic reactions, have a negative change in enthalpy (∆H), and typically raise the temperature of their surroundings. In contrast, endothermic reactions absorb heat, have a positive ∆H, and lower the temperature of their surroundings. The interplay between entropy and enthalpy is crucial for determining the thermodynamic favorability of a reaction.

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First Law of Thermodynamics

Energy conservation: Energy neither created/destroyed, only transformed.

01

Second Law of Thermodynamics

Entropy increase: Isolated systems tend towards greater disorder over time.

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Third Law of Thermodynamics

Zero-point entropy: Perfect crystal's entropy at absolute zero is zero.

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