Negative electrocaloric effect and its use for solid-state refrigeration. International Journal of Numerical Methods for Heat & Fluid Flow 2023, 33 Is the tendency to maximise energy distribution an optimal collective activity for biological purposes? A proposal for a global principle of biological organization. The Statistical Interpretation of Classical Thermodynamic Heating and Expansion Processes. The Misinterpretation of Entropy as “Disorder”. Chemistry in Past and New Science Frameworks and Standards: Gains, Losses, and Missed Opportunities. Review of Entropy and the Second Law: Interpretation and Misss-Interpretationsss. Visualizing the Entropy Change of a Thermal Reservoir. Statistical Teleodynamics: Toward a Theory of Emergence. Macroscopic Observations of Dissolving, Insolubility, and Precipitation: General Chemistry and Physical Chemistry Students’ Ideas about Entropy Changes and Spontaneity. Development of the Enthalpy and Entropy in Dissolution and Precipitation Inventory. Teaching Entropy from Phase Space Perspective: Connecting the Statistical and Thermodynamic Views Using a Simple One-Dimensional Model. This article is cited by 83 publications. It should be replaced by describing entropy change as energy dispersal-from a molecular viewpoint, by changes in molecular motions and occupancy of microstates. Frequently misleading, order-disorder as a description of entropy change is also an anachronism. From a molecular viewpoint all such entropy increases involve the dispersal of energy over a greater number, or a more readily accessible set, of microstates. In contrast, when ideal gases or liquids are allowed to expand or to mix in a larger volume, the entropy increase is due to a greater dispersion of their original unchanged thermal energy. In thermodynamics, the entropy of a substance increases when it is warmed because more thermal energy has been dispersed within it from the warmer surroundings. Entropy is the measure or index of that dispersal. Energy's diffusion or dispersal to more microstates is the driving force in chemistry. Ten examples illustrate the problem.Entropy is not disorder, not a measure of chaos, not a driving force. This seems to be a useful visual support, but it can be so misleading as actually to be a failure-prone crutch. To aid students in visualizing an increase in entropy, many elementary chemistry texts use artists' before-and-after drawings of groups of 'orderly' molecules that become 'disorderly'.

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