Page 681 - Chemistry--atom first
P. 681
Chapter 12 | Thermodynamics 671
Key Terms
entropy (S) state function that is a measure of the matter and/or energy dispersal within a system, determined by the number of system microstates often described as a measure of the disorder of the system
Gibbs free energy change (G) thermodynamic property defined in terms of system enthalpy and entropy; all spontaneous processes involve a decrease in G
microstate (W) possible configuration or arrangement of matter and energy within a system
nonspontaneous process process that requires continual input of energy from an external source
reversible process process that takes place so slowly as to be capable of reversing direction in response to an infinitesimally small change in conditions; hypothetical construct that can only be approximated by real processes removed
second law of thermodynamics entropy of the universe increases for a spontaneous process
spontaneous change process that takes place without a continuous input of energy from an external source
standard entropy (S°) entropy for a substance at 1 bar pressure; tabulated values are usually determined at 298.15 K and denoted
standard entropy change (ΔS°) change in entropy for a reaction calculated using the standard entropies, usually at room temperature and denoted
standard free energy change (ΔG°) change in free energy for a process occurring under standard conditions (1 bar pressure for gases, 1 M concentration for solutions)
standard free energy of formation change in free energy accompanying the formation of one mole of substance from its elements in their standard states
third law of thermodynamics entropy of a perfect crystal at absolute zero (0 K) is zero Key Equations
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• S=klnW
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• ΔSuniv = ΔSsys + ΔSsurr
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• ΔG=ΔH−TΔS
• ΔG=ΔG°+RTlnQ
• ΔG°=−RTlnK
