The freedom in that part of the universe may increase with no change in the freedom of the rest of the universe. Statistical Entropy - Mass, Energy, and Freedom The energy or the mass of a part of the universe may increase or decrease, but only if there is a corresponding decrease or increase somewhere else in the universe.Qualitatively, entropy is simply a measure how much the energy of atoms and molecules become more spread out in a process and can be defined in terms of statistical probabilities of a system or in terms of the other thermodynamic quantities. Statistical Entropy Entropy is a state function that is often erroneously referred to as the 'state of disorder' of a system.Earlier the value of 185.3 J/molK was calculated from experimental data Giauque W.F., 1931. Phase Change, gas expansions, dilution, colligative properties and osmosis. The calorimetric value is significantly higher than the statistically calculated entropy, 186.26 J/molK, which remains the best value for use in thermodynamic calculations Vogt G.J., 1976, Friend D.G., 1989, Gurvich, Veyts, et al., 1989. Simple Entropy Changes - Examples Several Examples are given to demonstrate how the statistical definition of entropy and the 2nd law can be applied.Calculate the entropy change for 1.0 mole of ice melting to form liquid at 273 K. The enthalpy of fusion for water is 6.01 kJ/mol. A microstate is one of the huge number of different accessible arrangements of the molecules' motional energy* for a particular macrostate. The entropy change for a phase change at constant pressure is given by. Instead, they are two very different ways of looking at a system. Microstates Dictionaries define “macro” as large and “micro” as very small but a macrostate and a microstate in thermodynamics aren't just definitions of big and little sizes of chemical systems. Entropy of air at 0☌ and 1 bara: 0.1100 kJ/mol K 3.796 kJ/kg K 0.9067 Btu (IT)/lb ☏ Liquid density at boiling point and 1 bar: 875.50 kg/m 3 54.656 lb/ft 3 Molar mass: 28.“Disorder” was the consequence, to Boltzmann, of an initial “order” not - as is obvious today - of what can only be called a “prior, lesser but still humanly-unimaginable, large number of accessible microstate it was his surprisingly simplistic conclusion: if the final state is random, the initial system must have been the opposite, i.e., ordered. ‘Disorder’ in Thermodynamic Entropy Boltzmann’s sense of “increased randomness” as a criterion of the final equilibrium state for a system compared to initial conditions was not wrong.
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