Astrofluids are characterized with the help of various thermodynamic properties and associated conservation laws. In this context, can anyone give a realistic correlation between the specific entropy conservation and logatropic pressure of such fluids?
Relevant References and materials dealing with new equations of state are as well welcome.
Any isothermal change in the system keeping the pressure constant the variation in the Gibbs free energy may be written as:
Del G = Del U -T Del S +P Del V According to the postulated entropy conservation (That means one has an adiabatic process, DEl S=0 in this question) above equation takes the following form:
Del G = Del U + P Del V According to the Thermodynamics for closed system Del G is negative for irreversible changes and is equal to zero for reversible changes, and it can never be positive since that iöplies unnatural process which never takes in nature!! The mathematical inequality may be put into the following form.
Del U EQ L ( - P del V) , In the case of reversible change one has:
Del U = -P DelV Decrease in the volume increases the internal energy or visa versa. In the case irreversible process the increase is less than the work done on the system during contraction, and that difference appears as a dissipation of energy.
In my work on the irreversible processes under the isobaric isothermal conditions, one has: - Del G/T = Del Internal S is Positive definite quantity called internal entropy production.
Any isothermal change in the system keeping the pressure constant the variation in the Gibbs free energy may be written as:
D G = D U -T Dl S +P D V According to the postulated entropy conservation (That means one has an adiabatic process, DEl S=0 in this question) above equation takes the following form:
D G = D U + P DV According to the Thermodynamics for closed system D G is negative for irreversible changes and is equal to zero for reversible changes, and it can never be positive since that iöplies unnatural process which never takes in nature!! The mathematical inequality may be put into the following form.
D U EQ L ( - P D V) , In the case of reversible change one has:
DU = -P DV Decrease in the volume increases the internal energy or visa versa. In the case irreversible process the increase is less than the work done on the system during contraction, and that difference appears as a dissipation of energy.
In my work on the irreversible processes under the isobaric isothermal conditions, one has: - D G/T = D Internal S is Positive definite quantity called internal entropy production.
Any isothermal change in the system keeping the pressure constant the variation in the Gibbs free energy may be written as:
D G = D U -T Dl S +P D V According to the postulated entropy conservation (That means one has an adiabatic process, D S=0 in this question) above equation takes the following form:
D G = D U + P DV According to the Thermodynamics for closed system D G is negative for irreversible changes and is equal to zero for reversible changes, and it can never be positive since that iöplies unnatural process which never takes in nature!! The mathematical inequality may be put into the following form.
D U EQ L ( - P D V) , In the case of reversible change one has:
DU = -P DV Decrease in the volume increases the internal energy or visa versa. In the case irreversible process the increase is less than the work done on the system during contraction, and that difference appears as a dissipation of energy.
In my work on the irreversible processes under the isobaric isothermal conditions, one has: - D G/T = D Internal S is Positive definite quantity called internal entropy production.
ΔG = Δ U -TΔS +P Δ V According to the postulated entropy conservation (That means one has an adiabatic process, D S=0 in this question) above equation takes the following form:
ΔG = ΔU + P ΔV According to the Thermodynamics for closed system ΔG is negative for irreversible changes and is equal to zero for reversible changes, and it can never be positive since that iöplies unnatural process which never takes in nature!! The mathematical inequality may be put into the following form.
ΔU EQ L ( - P Δ V) , In the case of reversible change one has:
ΔU = -P ΔV Decrease in the volume increases the internal energy or visa versa. In the case irreversible process the increase is less than the work done on the system during contraction, and that difference appears as a dissipation of energy.
In my work on the irreversible processes under the isobaric isothermal conditions, one has: - Δ G/T = S Internal S is Positive definite quantity called internal entropy production.
ΔG = Δ U -TΔS +P Δ V According to the postulated entropy conservation (That means one has an adiabatic process, D S=0 in this question) above equation takes the following form:
ΔG = ΔU + P ΔV According to the Thermodynamics for closed system ΔG is negative for irreversible changes and is equal to zero for reversible changes, and it can never be positive since that iöplies unnatural process which never takes in nature!! The mathematical inequality may be put into the following form.
ΔU EQ L ( - P Δ V) , In the case of reversible change one has:
ΔU = -P ΔV Decrease in the volume increases the internal energy or visa versa. In the case irreversible process the increase is less than the work done on the system during contraction, and that difference appears as a dissipation of energy.
In my work on the irreversible processes under the isobaric isothermal conditions, one has: - Δ G/T = S Internal S is Positive definite quantity called internal entropy production.
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