This condition describes an endothermic process that involves a decrease in system entropy. Such a process is spontaneous at low temperatures and nonspontaneous at high temperatures. If the TΔ S term’s magnitude is greater than Δ H, the free energy change will be positive. In this case, Δ G will be negative if the magnitude of the TΔ S term is less than Δ H. This condition describes an exothermic process that involves a decrease in system entropy. Such a process is spontaneous at high temperatures and nonspontaneous at low temperatures. If the TΔ S term is less than Δ H, the free energy change will be positive. In this case, Δ G will be negative if the magnitude of the TΔ S term is greater than Δ H. This condition describes an endothermic process that involves an increase in system entropy. Four possibilities therefore exist with regard to the signs of the enthalpy and entropy changes: Since T is the absolute (kelvin) temperature, it can only have positive values. The spontaneity of a process, as reflected in the arithmetic sign of its free energy change, is then determined by the signs of the enthalpy and entropy changes and, in some cases, the absolute temperature. Appendix L: Standard Electrode (Half-Cell) Potentials.Appendix K: Formation Constants for Complex Ions.Appendix I: Ionization Constants of Weak Bases.Appendix H: Ionization Constants of Weak Acids.Appendix G: Standard Thermodynamic Properties for Selected Substances.Appendix F: Composition of Commercial Acids and Bases.Appendix D: Fundamental Physical Constants.Appendix C: Units and Conversion Factors.Second Law of Thermodynamics and Gibbs Free Energy.Application: Precipitation and Dissolution.Shifting Equilibria: LeChatelier’s Principle.Chemical Equilibria and Applications Toggle Dropdown Collision Theory and Factors Affecting Reaction Rates.Solutions and Colligative Properties Toggle Dropdown Liquids, Solids, and Modern Materials Toggle Dropdown Chemical Bonding and Molecular Geometry Toggle Dropdown Thermochemical Guidelines, Enthalpy of Formation and Hess's Law.Solution Stoichiometry and Combustion Analysis.Writing and Balancing Chemical Equations.Stoichiometry of Chemical Reactions Toggle Dropdown Determining Empirical and Molecular Formulas.Composition of Substances and Solutions Toggle Dropdown Molecular and Ionic Compounds and Their Nomenclature. Early Ideas and Evolution of Atomic Theory.Atoms, Molecules and Ions Toggle Dropdown Measurements and Uncertainty in Measurement.Classification, Physical and Chemical Properties.
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