__5.7 The Inequality of Clausius__

The Carnot cycle is a reversible cycle and produces work which we will refer to as *W*rev. Consider an irreversible cycle operating between the same two reservoirs, shown in Fig. 5.9. Obviously, since the Carnot cycle possesses the maximum possible

**F****i****g****u****re 5.9 **A reversible and an irreversible engine operating between two reservoirs.

efﬁciency, the efﬁciency of the irreversible cycle must be less than that of the Carnot cycle. In other words, for the same amount of heat addition *Q* , we must have

*W*_{irr }< *W*_{rev }**(5.41)**

From the ﬁrst law applied to a cycle (*W *= *Q* – *Q *) we see that, assuming that (*Q *) and (*Q *) are the same,

since the above integral for a reversible cycle is zero.

If we were considering an irreversible refrigerator rather than an engine, we would require more work for the same amount of refrigeration *Q . *By applying the ﬁrst law to refrigerators, we would arrive at the same inequality as that of Eq. (5.43). Hence, for all cycles, reversible or irreversible, we can write

This is known as *th**e inequality of Clausius. *It is a consequence of the second law of thermodynamics. It will be used to establish entropy relationships for real processes.

5.8 Entropy Change for an Irreversible Process

Consider a cycle to be composed of two reversible processes, shown in Fig. 5.10. Suppose that we can also return from state 2 to state 1 along the irreversible process marked by path *C*. For the system experiencing the reversible cycle we have

**F****i****g****u****re 5.10 **A cycle that includes the possibility of an irreversible process.

For the system experiencing the cycle involving the irreversible process, the Clausius inequality demands that

The equality holds for a system experiencing a reversible process and the inequality for an irreversible process.

We can also introduce the *entropy production **σ *into Eq. (5.48):

where we have used *δσ *since it is a path dependent function. It is obvious that entropy production is zero for a reversible process and positive for an irreversible process, i.e., any real process.

Relationship (5.48) leads to an important conclusion in thermodynamics. Con- sider an inﬁnitesimal process of a system at absolute temperature *T*. If the process is reversible, the differential change in entropy is *δ**Q*/*T*; if the process is irreversible, the change in entropy is greater than *δ**Q*/*T*. We thus conclude that the effect of irreversibility (e.g., friction) is to increase the entropy of a system. Alternatively, observe that the entropy production *σ *in Eq. (5.49), for any real process, must be positive.

Finally, consider an *isolated *system, a system that exchanges no work or heat with its surroundings. For such a system the ﬁrst law demands that *E*2 = *E*1 for any process. Equation (5.48) takes the form

**Δ S ≥ 0 (5.50)**

demanding that the entropy of an isolated system either remains constant or

increases, depending on whether the process is reversible or irreversible. Hence, for any real process the entropy of an isolated system must increase. Alternatively, we can state that the entropy production associated with a real process of an isolated

system must be positive since for an isolated system Δ*S *= σ .

We can restate Eq. (5.50) by considering an isolated system to be composed of

any system under consideration plus the surroundings to that system as a second larger system. The heat and work transferred to the system under consideration are negative the heat and work transferred from the surroundings. This combination of the system and surroundings is often referred to as the universe. For the universe we can write

where σ = 0 applies to a reversible (ideal) process and the inequality to an irreversible (real) process. Relation (5.51), the *principle of entropy increase*, is often used as the mathematical statement of the second law. In Eq. (5.51), *σ *has also been referred to as Δ*S*gen , the entropy generated.

__EXAMPLE 5.11__

Air is contained in one half of an insulated tank. The other half is completely evacuated. The membrane separating the two halves is punctured and the air quickly ﬁlls the entire volume. Calculate the speciﬁc entropy change of this iso- lated system.

__Solution __

The entire tank is chosen as the system boundary. No heat transfer occurs across the boundary and the air does no work. The ﬁrst law then takes the form Δ*U *= *m**C**v *(*T*2 − *T*1 ) = 0. Hence, the ﬁnal temperature is equal to the initial temperature. Using Eq. (5.25) for the entropy change, we have, with *T _{1}=T_{2}*

Note that this satisﬁes Eq. (5.48) since for this example *Q *= 0, so that ∫δ*Q */*T *= 0 < *m*Δ*s*.

__EXAMPLE 5.12__

Two kilograms of steam at 400°C and 600 kPa are cooled at constant pressure by transferring heat from a cylinder until the steam is completely condensed. The surroundings are at 25°C. Determine the net entropy production.

__Solution __

The entropy of the steam that deﬁnes our system decreases since heat is transferred from the system to the surroundings. From the steam tables this change is found to be

Δ*S*_{sys} = *m*(*s*_{2} − *s*_{1} ) = 2(1.9316 − 7.708) = −11.55 kJ/K

The heat transfer to the surroundings occurs at constant temperature. Hence, the entropy change of the surroundings [see Eq. (5.18)] is

The heat transfer for the constant-pressure process needed to condense the steam is

The entropy production is positive, as it must be.

__5.9 The Second Law Applied to a Control Volume__

__5.9 The Second Law Applied to a Control Volume__

Return once again to a ﬁxed control volume, a device, with one inlet and one outlet. At ime *t *the system occupies a small volume 1 (that enters the device from the inlet pipe over a time increment Δ*t*) plus the device; then at *t *+ Δ*t*, the system occupies the device plus the small volume 2 that leaves the device. The second law for the steady-state device, can be stated by applying Eq. (5.48):

Recognizing that *S*device (*t *+ Δ*t*) = *S*device (*t*) due to the steady ﬂow (all quantities are

independent of time), we have

where *δ**Q*c.s. is the incremental heat transfer into the device at a boundary location where the temperature is *T *, the subscript “c.s.” representing the control surface c.s. surrounding the device. Introducing the entropy production of Eq. (5.49),

Let’s assume that the entire control surface is at a constant temperature *T* _{c.s}, a rather common assumption. If we divide Eq. (5.54) by Δ*t *and use dots to denote rates, we arrive at the steady-state rate equation

Zero rate of entropy production is associated with a reversible process whereas positive entropy production is associated with the many irreversibilities that may exist within a control volume; these are due to viscous effects, separation of the

ﬂow from turbine or compressor blades, and large temperature differences over which heat transfer takes place, to name a few.

By transferring energy to the control volume via heat transfer, we can obviously increase the entropy of the ﬂuid ﬂowing from the control volume so that *s* > *s *. If irreversibilities are present, σ·device will be positive and *s*2 will be greater than the exiting entropy for the same rate of heat transfer without irreversibilities. We also note that for an adiabatic steady-ﬂow process, the entropy also increases from inlet to exit due to irreversibilities since, for that case, Eq. (5.56) shows that

*s*_{2} ≥ *s*_{1} **(5.56)**

since σ·_{device} must be positive or zero. For the reversible adiabatic process the inlet entropy and exit entropy are equal since σ·device = 0; this is the isentropic process. We use this fact when studying a reversible adiabatic process involving, for example, steam or a refrigerant flowing through an ideal turbine or compressor.

We have calculated the efﬁciency of a cycle earlier in this chapter. Now we desire a quantity that can be used as a measure of the irreversibilities that exist in a particular device. The *efﬁciency *of a device is one such measure; it is deﬁned as the ratio of the actual performance of a device to the ideal performance. The ideal performance is often that associated with an isentropic process. For example, the efﬁciency of a turbine would be

where *w**a *is the actual shaft work output and *w**s *is the maximum shaft work output, i.e., the work associated with an isentropic process. In general, the efﬁciency is deﬁned using the optimum output; for a nozzle we would use the maximum kinetic energy increase. For a compressor the actual work required is greater than the min- imum work requirement of an isentropic process. For a compressor or pump the efﬁciency is deﬁned to be

Each efﬁciency above is often called the *adiabatic efﬁciency *since each efﬁciency is based on an adiabatic process.

__EXAMPLE 5.13__

Superheated steam enters a turbine, as shown, and exits at 10 kPa. For a mass ﬂow rate of 2 kg/s, determine the maximum power output.

__Solution __

If we neglect kinetic energy and potential energy changes, the ﬁrst law, for an

adiabatic process, is −*W**T *= *m*(*h*2 – *h*1)*. *Since we desire the maximum power output, the process is assumed to be reversible, the entropy exiting is the same as the entropy entering, as shown (such a sketch is quite useful in visualizing the process). From the steam tables, at 600°C and 2 MPa,

With the above value for *s* we see that state 2 is in the quality region. The quality is determined as follows:

__EXAMPLE 5.14__

The turbine of Example 5.13 is assumed to be 80 percent efﬁcient. Determine the entropy and temperature of the ﬁnal state. Sketch the real process on a *T**-**s *diagram.

__Solution __

Using the deﬁnition of efﬁciency, the actual power output is

Using this value and *P*2′ = 10 kPa, we see that state 2′ lies in the superheated region, since *h*2′ > *h**g*. This is shown schematically below. At *P*2 = 10 kPa and *h*2′ = 2770, we interpolate to ﬁnd the value of *T*2′ :

The entropy is interpolated to be *s*2′ = 8.46 kJ/kg ⋅ K.

Note that the irreversibility has the desired effect of moving state 2 into the super- heated region, thereby eliminating the formation of droplets due to the condensation of moisture. In an actual turbine, moisture formation cannot be tolerated because of damage to the turbine blades, so the irreversibility is somewhat desirable.

__EXAMPLE 5.15__

A preheater is used to preheat water in a power plant cycle, as shown. The super- heated steam is at a temperature of 250°C and the entering water is at 45°C. All pressures are 600 kPa. Calculate the rate of entropy production.

__Solution __

The conservation of mass requires that

*m*_{3}= *m*_{2} + *m*· 1 = 0.5 + 4 = 4.5 kg/s

The ﬁrst law allows us to calculate the temperature of the exiting water. Neglecting kinetic energy and potential energy changes and assuming zero heat transfer, the ﬁrst law takes the form *m*· 3*h*3 = *m*· 2*h*2 + *m*· 1*h*1. Using the steam tables (*h *is the enthalpy of saturated liquid at 45°C),

This enthalpy is less than that of saturated liquid at 600 kPa. Thus, the exiting water is subcooled. Its temperature is interpolated from the saturated steam tables (ﬁnd *T *that gives *h *= 496 kJ/kg) to be

The entropy at this temperature is then interpolated (using *s**f*) to be *s*3 = 1.508 kJ/kg · K. The entropy of the entering superheated steam is found to be *s*2 = 7.182 kJ/kg · K. The entering entropy of the water is *s**f *at *T*1 = 45°C, or *s*1 = 0.639 kJ/kg · K. Finally, modifying Eq. (5.56), to account for two inlets, we have, with no heat transfer,

This is positive, indicating that entropy is produced, a consequence of the second law. The mixing process between the superheated steam and the sub- cooled water is indeed an irreversible process.

__Quiz No. 1__

__Quiz No. 1__

1. An inventor claims a thermal engine operates between ocean layers at 27 and

10°C. It produces 10 kW and discharges 9900 kJ/min. Such an engine is

(A) Impossible

(B) Reversible

(C) Possible

(D) Probable

2. A heat pump is to provide 2000 kJ/h to a house maintained at 20°C. If it is

−20°C outside, what is the minimum power requirement?

(A) 385 kJ/h

(B) 316 kJ/h

(C) 273 kJ/h

(D) 184 kJ/h

3. Select an acceptable paraphrase of the Kelvin-Planck statement of the second law.

(A) No process can produce more work than the heat that it accepts.

(B) No engine can produce more work than the heat that it intakes.

(C) An engine cannot produce work without accepting heat.

(D) An engine has to reject heat.

4. A power plant burns 1000 kg of coal each hour and produces 500 kW of power. Calculate the overall thermal efﬁciency if each kg of coal produces 6 MJ of energy.

(A) 0.35

(B) 0.30

(C) 0.25

(D) 0.20

5. Two Carnot engines operate in series between two reservoirs maintained at 327 and 27°C, respectively. The energy rejected by the ﬁrst engine is input into the second engine. If the ﬁrst engine’s efﬁciency is 20 percent greater than the second engine’s efﬁciency, calculate the intermediate temperature.

(A) 106°C

(B) 136°C

(C) 243°C

(D) 408°C

6. A heat pump is to maintain a house at 20°C when the outside air is at

−25°C. It is determined that 1800 kJ is required each minute to accomplish

this. Calculate the minimum power required.

(A) 3.87 kW

(B) 4.23 kW

(C) 4.61 kW

(D) 3.99 kW

7. Which of the following entropy relationships is incorrect?

(A) Air, *V *= const: Δ*s *= *C**v *ln*T*2 /*T*1

(B) Water: Δ*s *= *C**p *ln*T*2 /*T*1

(C) Reservoir: Δ*s *= *C**p *ln*T*2 /*T*1

(D) Copper: Δ*s *= *C**p *ln*T*2 /*T*1

8. Two kilograms of air are heated at constant pressure of 200 kPa to 500°C.

Calculate the entropy change if the initial volume is 0.8 m3.

(A) 2.04 kJ/K

(B) 2.65 kJ/K

(C) 3.12 kJ/K

(D) 4.04 kJ/K

9. Two kilograms of air are compressed from 120 kPa and 27°C to 600 kPa in a rigid container. Calculate the entropy change.

(A) 5.04 kJ/K

(B) 4.65 kJ/K

(C) 3.12 kJ/K

(D) 2.31 kJ/K

10. A paddle wheel provides 200 kJ of work to the air contained in a 0.2-m3 rigid volume, initially at 400 kPa and 40°C. Determine the entropy change if the volume is insulated.

(A) 0.504 kJ/K

(B) 0.443 kJ/K

(C) 0.312 kJ/K

(D) 0.231 kJ/K

11. 0.2 kg of air is compressed slowly from 150 kPa and 40°C to 600 kPa, in an adiabatic process. Determine the ﬁnal volume.

(A) 0.0445 m3

(B) 0.0662 m3

(C) 0.0845 m3

(D) 0.0943 m3

12. A rigid, insulated 4-m3 volume is divided in half by a membrane. One chamber is pressurized with air to 100 kPa and the other is completely evacuated. The membrane is ruptured and after a period of time equilibrium is restored. The entropy change of the air is nearest

(A) 0.624 kJ/K

(B) 0.573 kJ/K

(C) 0.473 kJ/K

(D) 0.351 kJ/K

13. Ten kilograms of air are expanded isentropically from 500°C and 6 MPa to

400 kPa. The work accomplished is nearest

(A) 7400 kJ

(B) 6200 kJ

(C) 4300 kJ

(D) 2990 kJ

14. Find the work needed to isentropically compress 2 kg of air in a cylinder at

400 kPa and 400°C to 2 MPa.

(A) 1020 kJ

(B) 941 kJ

(C) 787 kJ

(D) 563 kJ

15. Calculate the total entropy change if 10 kg of ice at 0°C are mixed in an insulated container with 20 kg of water at 20°C. Heat of melting for ice is

340 kJ/kg.

(A) 6.19 kJ/K

(B) 3.95 kJ/K

(C) 1.26 kJ/K

(D) 0.214 kJ/K

16. A 5-kg block of copper at 100°C is submerged in 10 kg of water at 10°C, and after a period of time, equilibrium is established. If the container is insulated, calculate the entropy change of the universe.

(A) 0.082 kJ/K

(B) 0.095 kJ/K

(C) 0.108 kJ/K

(D) 0.116 kJ/K

17. Find *w**T *of the insulated turbine shown.

(A) 910 kJ/kg

(B) 1020 kJ/kg

(C) 1200 kJ/kg

(D) 1430 kJ/kg

18. The efﬁciency of the turbine of Prob. 17 is nearest

(A) 92%

(B) 89%

(C) 85%

(D) 81%

19. A nozzle accelerates steam at 120 kPa and 200°C from 20 m/s to the atmosphere. If it is 85 percent efﬁcient, the exiting velocity is nearest

(A) 290 m/s

(B) 230 m/s

(C) 200 m/s

(D) 185 m/s

20. A turbine produces 4 MW by extracting energy from 4 kg of steam which ﬂows through the turbine every second. The steam enters at 600°C and 1600 kPa and exits at 10 kPa. The turbine efﬁciency is nearest

(A) 82%

(B) 85%

(C) 87%

(D) 91%

__Quiz No. 2__

__Quiz No. 2__

1. An engine operates on 100°C geothermal water. It exhausts to a 20°C stream. Its maximum efﬁciency is nearest

(A) 21%

(B) 32%

(C) 58%

(D) 80%

2. Which of the following can be assumed to be reversible?

(A) A paddle wheel

(B) A burst membrane

(C) A resistance heater

(D) A piston compressing gas in a race engine

3. A Carnot engine operates between reservoirs at 20 and 200°C. If 10 kW of

power is produced, ﬁnd the rejected heat rate.

(A) 26.3 kJ/s

(B) 20.2 kJ/s

(C) 16.3 kJ/s

(D) 12.0 kJ/s

4. An automobile that has a gas mileage of 13 km/L is traveling at 100 km/h.

At this speed essentially all the power produced by the engine is used to overcome air drag. If the air drag force is given by 1 ρ*V *2 *A**C*

determine the thermal efﬁciency of the engine at this speed using projected area *A *= 3 m2, drag coefﬁcient *C*

= 0.28, and heating value of gasoline 9000 kJ/kg. Gasoline

has a density of 740 kg/m3.

(A) | 0.431 |

(B) | 0.519 |

(C) | 0.587 |

(D) | 0.652 |

5. A proposed power cycle is designed to operate between temperature

reservoirs of 900 and 20°C. It is supposed to produce 43 hp from the

2500 kJ of energy extracted each minute. Is the proposal feasible?

(A) No

(B) Yes

(C) Maybe

(D) Insufﬁcient information

6. A Carnot refrigeration cycle is used to estimate the energy requirement in an attempt to reduce the temperature of a specimen to absolute zero.

Suppose that we wish to remove 0.01 J of energy from the specimen when

it is at 2 × 10−6 K. How much work is necessary if the high-temperature

reservoir is at 20°C?

(A) 622 kJ

(B) 864 kJ

(C) 1170 kJ

(D) 1465 kJ

7. One kilogram of air is heated in a rigid container from 20 to 300°C. The

entropy change is nearest

(A) 0.64 kJ/K

(B) 0.54 kJ/K

(C) 0.48 kJ/K

(D) 0.34 kJ/K

8. Which of the following second law statements is incorrect?

(A) The entropy of an isolated system must remain constant or increase.

(B) The entropy of a hot copper block decreases as it cools.

(C) If ice is melted in water in an insulated container, the net entropy decreases.

(D) Work must be input if energy is transferred from a cold body to a hot body.

9. A piston allows air to expand from 6 MPa to 200 kPa. The initial volume and temperature are 500 cm3 and 800°C. If the temperature is held constant, calculate the entropy change.

(A) 10.9 kJ/K

(B) 9.51 kJ/K

(C) 8.57 kJ/K

(D) 7.41 kJ/K

10. The entropy change in a certain expansion process is 5.2 kJ/K. The nitrogen, initially at 80 kPa, 27°C, and 4 m3, achieves a ﬁnal temperature of 127°C. Calculate the ﬁnal volume.

(A) 255 m3

(B) 223 m3

(C) 158 m3

(D) 126 m3

11. A piston is inserted into a cylinder causing the pressure in the air to change from 50 to 4000 kPa while the temperature remains constant at 27°C. To accomplish this, heat transfer must occur. Determine the entropy change.

(A) −0.92 kJ/kg ⋅ K

(B) −0.98 kJ/kg ⋅ K

(C) −1.08 kJ/kg ⋅ K

(D) −1.26 kJ/kg ⋅ K

12. A torque of 40 N · m is needed to rotate a shaft at 40 rad/s. It is attached to a paddle wheel located in a rigid 2-m3 volume. Initially the temperature is 47°C and the pressure is 200 kPa; if the paddle wheel rotates for 10 min and 500 kJ of heat is transferred to the air in the volume, determine the entropy increase assuming constant speciﬁc heats.

(A) 3.21 kJ/K

(B) 2.81 kJ/K

(C) 2.59 kJ/K

(D) 2.04 kJ/K

13. Four kilograms of air expand in an insulated cylinder from 500 kPa and 227°C to 20 kPa. What is the work output?

(A) 863 kJ

(B) 892 kJ

(C) 964 kJ

(D) 1250 kJ

14. Steam, at a quality of 85 percent, is expanded in a cylinder at a constant pressure of 800 kPa by adding 2000 kJ/kg of heat. Compute the entropy increase.

(A) 3.99 kJ/ kg ⋅ K

(B) 3.74 kJ/ kg ⋅ K

(C) 3.22 kJ/ kg ⋅ K

(D) 2.91 kJ/ kg ⋅ K

15. Two kilograms of saturated steam at 100°C are contained in a cylinder. If the

steam undergoes an isentropic expansion to 20 kPa, determine the work output.

(A) 376 kJ

(B) 447 kJ

(C) 564 kJ

(D) 666 kJ

16. Ten kilograms of iron at 300°C are chilled in a large volume of ice and

water. Find the total entropy change.

(A) 0.88 kJ/K

(B) 1.01 kJ/K

(C) 1.26 kJ/K

(D) 1.61 kJ/K

17. Five kilograms of ice at −20°C are mixed with 10 kg of water initially at

20°C. If there is no signiﬁcant heat transfer from the container, determine

the net entropy change. It takes 330 kJ to melt a kg of ice.

(A) 0.064 kJ/K

(B) 0.084 kJ/K

(C) 1.04 kJ/K

(D) 1.24 kJ/K

18. Two kilograms of air are stored in a rigid volume of 2 m3 with the temperature initially at 300°C. Heat is transferred from the air until the pressure reaches 120 kPa. Calculate the entropy change of the air.

(A) −0.292 kJ/K

(B) −0.357 kJ/K

(C) −0.452 kJ/K

(D) −0.498 kJ/K

19. Calculate the entropy change of the universe for Prob. 18 if the surroundings are at 27°C.

(A) 0.252 kJ/K

(B) 0.289 kJ/K

(C) 0.328 kJ/K

(D) 0.371 kJ/K

20. Two hundred kilowatts are to be produced by a steam turbine. The outlet steam is to be saturated at 80 kPa and the steam entering will be at 600°C. For an isentropic process, determine the mass ﬂow rate of steam.

(A) 0.342 kg/s

(B) 0.287 kg/s

(C) 0.198 kg/s

(D) 0.116 kg/s