Isentropic process
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}} In thermodynamics, an isentropic process or isoentropic process (ισον = "equal" (Greek); εντροπία entropy = "disorder"(Greek)) is one in which, for purposes of simplified engineering analysis and calculations, one may assume that the process takes place from initiation to completion without an increase or decrease in the entropy of the system, i.e., the entropy of the system remains constant throughout.^{[1]}^{[2]} It can be proven that any reversible adiabatic process is an isentropic process. A simple more common definition of isentropic would be one that produces "No change in entropy".
Background
The second law of thermodynamics states that,
where is the amount of energy the system gains by heating, is the temperature of the system, and is the change in entropy. The equal sign will hold for a reversible process. For a reversible isentropic process, there is no transfer of heat energy and therefore the process is also adiabatic. For an irreversible process, the entropy will increase. Hence removal of heat from the system (cooling) is necessary to maintain a constant entropy for an irreversible process in order to make it isentropic. Thus an irreversible isentropic process is not adiabatic.
For reversible processes, an isentropic transformation is carried out by thermally "insulating" the system from its surroundings. Temperature is the thermodynamic conjugate variable to entropy, thus the conjugate process would be an isothermal process in which the system is thermally "connected" to a constanttemperature heat bath.
Isentropic Processes in Thermodynamic Systems
The entropy of a fixed mass does not change during a process that is internally reversible and adiabatic. A process during which the entropy remains constant is called an isentropic process.^{[3]}
Many thermodynamic devices are essentially isentropic when the irreversibilities, for example friction, are idealized as 0 or minimized to almost 0.
Some isentropic thermodynamic devices include:
Pump
Gas compressor
Turbine
Nozzle
Diffuser
Isentropic Efficiencies of SteadyFlow Devices in Thermodynamic Systems
Most steadyflow devices operate under adiabatic conditions, and the ideal process for these devices is the isentropic process.The parameter that describes how efficiently a device approximates a corresponding isentropic device is called isentropic or adiabatic efficiency.^{[4]}
Isentropic efficiency of Turbines:
Isentropic efficiency of Compressors
Isentropic efficiency of Nozzles
For all above equations:
 is the enthalpy at the entrance state
 is the enthalpy at the exit state for the actual process
 is the enthalpy at the exit state for the isentropic process
Isentropic Devices in Thermodynamic Cycles
Ideal Rankine Cycle 1>2 Isentropic compression in a pump
Ideal Rankine Cycle 3>4 Isentropic expansion in a turbine
Ideal Carnot Cycle 2>3 Isentropic expansion
Ideal Carnot Cycle 4>1 Isentropic compression
Ideal Otto Cycle 1>2 Isentropic compression
Ideal Otto Cycle 3>4 Isentropic expansion
Ideal Diesel Cycle 1>2 Isentropic compression
Ideal Diesel Cycle 3>4 Isentropic expansion
Ideal Brayton Cycle 1>2 Isentropic compression in a compressor
Ideal Brayton Cycle 3>4 Isentropic expansion in a turbine
Ideal Vaporcompression refrigeration Cycle 1>2 Isentropic compression in a compressor
NOTE: The isentropic assumptions are only applicable with ideal cycles. Real world cycles have inherent losses due to inefficient compressors and turbines. The real world system are not truly isentropic but are rather idealized as isentropic for calculation purposes.
Isentropic flow
An isentropic flow is a flow that is both adiabatic and reversible. That is, no heat is added to the flow, and no energy transformations occur due to friction or dissipative effects. For an isentropic flow of a perfect gas, several relations can be derived to define the pressure, density and temperature along a streamline.
Note that energy can be exchanged with the flow in an isentropic transformation, as long as it doesn't happen as heat exchange. An example of such an exchange would be an isentropic expansion or compression that entails work done on or by the flow.
Derivation of the isentropic relations
For a closed system, the total change in energy of a system is the sum of the work done and the heat added,
The reversible work done on a system by changing the volume is,
where is the pressure and is the volume. The change in enthalpy () is given by,
Then for a process that is both reversible and adiabatic (i.e. no heat transfer occurs), , and so . All reversible adiabatic processes are isentropic. This leads to two important observations,
Next, a great deal can be computed for isentropic processes of an ideal gas. For any transformation of an ideal gas, it is always true that
Using the general results derived above for and , then
So for an ideal gas, the heat capacity ratio can be written as,
For an ideal gas is constant. Hence on integrating the above equation, assuming a perfect gas, we get
Using the equation of state for an ideal gas, ,
also, for constant (per mole),
Thus for isentropic processes with an ideal gas,
Table of isentropic relations for an ideal gas
Derived from:
 Where:
 = Pressure
 = Volume
 = Ratio of specific heats =
 = Temperature
 = Mass
 = Gas constant for the specific gas =
 = Universal gas constant
 = Molecular weight of the specific gas
 = Density
 = Specific heat at constant pressure
 = Specific heat at constant volume
References
 Van Wylen, G.J. and Sonntag, R.E. (1965), Fundamentals of Classical Thermodynamics, John Wiley & Sons, Inc., New York. Library of Congress Catalog Card Number: 6519470
Notes
 ↑ Van Wylen, G.J. and Sonntag, R.E., Fundamentals of Classical Thermodynamics, Section 7.4
 ↑ Massey, B.S. (1970), Mechanics of Fluids, Section 12.2 (2nd edition) Van Nostrand Reinhold Company, London. Library of Congress Catalog Card Number: 6725005
 ↑ Cengel, Yunus A., and Michaeul A. Boles. Thermodynamics: An Engineering Approach. 7th Edition ed. New York: McgrawHill, 2012. Print.
 ↑ Cengel, Yunus A., and Michaeul A. Boles. Thermodynamics: An Engineering Approach. 7th Edition ed. New York: McgrawHill, 2012. Print.