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Chemical Thermodynamics explores the energy changes that accompany physical and chemical transformations, helping scientists predict whether a reaction will occur spontaneously and how energy flows between substances. The field begins by defining the universe as a system interacting with its surroundings, distinguishing between state functions like internal energy and enthalpy that depend solely on initial and final conditions, and path functions like heat and work that depend on the specific route taken. The First Law of Thermodynamics establishes the conservation of energy, expressed through the internal energy equation where energy can neither be created nor destroyed. Building upon this, enthalpy measures heat changes at constant pressure, allowing chemists to calculate reaction heat using thermochemical principles. To understand why certain processes happen naturally, the Second Law introduces entropy as a measure of molecular disorder, dictating that total universal entropy always increases during a spontaneous change. Finally, Gibbs Free Energy combines enthalpy and entropy into a single criterion for spontaneity at constant temperature and pressure. A negative change in Gibbs free energy signifies a spontaneous process, enabling chemists to determine the feasibility of reactions before they even occur in a laboratory setting.
Chemical Thermodynamics explores the energy changes that accompany physical and chemical transformations, helping scientists predict whether a reaction will occur spontaneously and how energy flows between substances. The field begins by defining the universe as a system interacting with its surr...
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