Entropy, increase during

The second entropy increases during spontaneous changes, . ... 

In the equilibrium Second Law, the first entropy increases during spontaneous changes in structure, and when the structure stabilizes (i.e., change ceases), the first entropy is a maximum. This state is called the equilibrium state. Similarly, in the nonequilibrium Second Law, the second entropy increases during spontaneous changes in flux, and when the flux stabilizes, the second entropy is a maximum. This state is called the steady state. The present nonequilibrium Second Law has the potential to provide the same basis for the steady state that Clausius Second Law has provided for the equilibrium state. 

If the system considered is closed and thermally insulated, then its entropy increases during a transport phenomenon... 

Since In and In Ng are always negative, entropy increases during formation of a homogeneous mixture, even though there has not been any heat exchange. There would not be any change anywhere else since this type of mixing takes place spontaneously and on its own, and this term indeed is the entropy increase of the universe. 

If the expansion is adiabatic and irreversible, entropy increases during the expansion. Point 3 shows a possible hnal state. The enthalpy of the hnal state would be greater than the H2 given above, and the work produced, being equal to the decrease in H, would be reduced. 

The molecules in liquid water are moving around freely and are therefore more "disordered" than when the molecules are held rigidly in a solid lattice in ice. The entropy increases during melting. 

Thus, it is exactly as much as the value S Ti that is released by the hotter body. While the amount of entropy increases during conduction, the energy current remains cMistant Wb represents the energy used up ( burnt ) along the conducting... 

This process is endothermic, which means that AH is positive. Because the entropy increases during the process, AS is positive, which makes —TAS negative. At temperatures below 0 °C (273 K), the magnitude of AH is greater than that of —TAS. Hence, the positive enthalpy term dominates, and A G is positive. This positive value of AG means that ice melting is not spontaneous at T < 0 °C, just as our everyday experience tells us rather, the reverse process, the freezing of liquid water into ice, is spontaneous at these temperatures. 

The process of protonation allows reconstitution of hydrophobic hydration to such an extent that the temperature range for hydrophobic association drops below that of the operating temperature (Urry, 1993, 1997). The result is a contraction due to hydrophobic association. Again, during an isometric contraction (this time chemically driven), hydrophobic hydration becomes less ordered bulk water. The solvent entropy increases during the development of entropic elastic force due to a decrease in entropy. 

Another concept to be explained in this connection is the so-called steady state. This is not a state of equilibrium. In the steady state, a steady flow of energy occurs between the system and its surroundings in those forms of energy that can be exchanged by the system, and this occurs such that the variables of the system remain constant with time. In other words, the flow of energy and particles into and out of the system are equal. Here a steady-state process creates the false impression of a state. In such cases, the intensive variables are, of course, not constant in space because otherwise no flow of energy would be possible moreover, the entropy increases during steady-state processes. 

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