Abstract
The reaction quotient Q can be expressed in partial pressures as \(\hbox {Q}_\mathrm{P}\) or in mole fractions as \(\hbox {Q}_{\mathrm{x}}\). \(\hbox {Q}_\mathrm{P}\) is ostensibly more useful than \(\hbox {Q}_{\mathrm{x}}\) because the related \(\hbox {K}_{\mathrm{x}}\) is a constant for a chemical equilibrium in which T and P are kept constant while \(\hbox {K}_{\mathrm{P}}\) is an equilibrium constant under more general conditions in which only T is constant. However, as demonstrated in this work, \(\hbox {Q}_{\mathrm{x}}\) is in fact more important both theoretically and technically. The relationships between \(\hbox {Q}_{\mathrm{x}}\), \(\hbox {Q}_\mathrm{P}\), and \(\hbox {Q}_{\mathrm{C}}\) are discussed. Four examples of applications are given in detail.
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Acknowledgments
We acknowledge support from Shanghai Key Laboratory of Rare Earth Functional Materials (1551), and Shenyang Normal University (Shiyanshi Zhuren Jijin Syzx1004 and Syzx1102).
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Liu, Y., Drew, M.G.B. & Liu, Y. A mathematical approach to chemical equilibrium theory for gaseous systems—III: \(\hbox {Q}_\mathrm{p}\), \(\hbox {Q}_\mathrm{c}\), and \(\hbox {Q}_{\mathrm{x}}\) . J Math Chem 52, 1191–1200 (2014). https://doi.org/10.1007/s10910-014-0306-4
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DOI: https://doi.org/10.1007/s10910-014-0306-4