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Spontaneity and Chemical Equilibrium
Spontaneity and Chemical Equilibrium
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The course Spontaneity and Chemical Equilibrium covers the natural direction and spontaneity of physical and chemical processes, centering on the concept of entropy, which quantifies energy dispersion and irreversibility. Spontaneous processes increase the total entropy of the universe, while the speed of occurrence is treated separately by chemical kinetics.
For conditions of constant temperature and pressure, the course introduces the Gibbs Energy (ΔG), combining enthalpy and entropy: spontaneous processes occur when ΔG < 0; non-spontaneous, when ΔG > 0; and chemical equilibrium, when ΔG = 0.
The material also addresses limitations of energy conversion, with the Kelvin-Planck Statement showing that no heat engine can fully convert heat into work, and that maximum efficiency is limited by the reversible Carnot cycle, which depends on the temperature difference between hot and cold sources.
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