Chapter 2: Energy and the First Law of Thermodynamics PDF

Chapter 2 Energy and the First Law of Thermodynamics 1  Learning Outcomes ►Explain key concepts related to energy and the first law of thermodynamics... including internal, kinetic, and potential energy, work and power, heat transfer and heat transf...

Chapter 2 Energy and the First Law of Thermodynamics 1  Learning Outcomes ►Explain key concepts related to energy and the first law of thermodynamics... including internal, kinetic, and potential energy, work and power, heat transfer and heat transfer modes, heat transfer rate, power cycle, refrigeration cycle, and heat pump cycle. 2  Learning Outcomes, cont. ►Analyze closed systems including applying energy balances, appropriately modeling the case at hand, and correctly observing sign conventions for work and heat transfer. ►Conduct energy analyses of systems undergoing thermodynamic cycles, evaluating as appropriate thermal efficiencies of power cycles and coefficients of performance of refrigeration and heat pump cycles. 3 Closed System Energy Balance (1 of 2) ►Energy is an extensive property that includes the kinetic and gravitational potential energy of engineering mechanics. ►For closed systems, energy is transferred in and out across the system boundary by two means only: by work and by heat. ►Energy is conserved. This is the first law of thermodynamics. 4 Closed System Energy Balance (2 of 2) ►The closed system energy balance states: The change in the Net amount of energy amount of energy transferred in and out contained within across the system boundary a closed system by heat and work during during some time the time interval interval ►We now consider several aspects of the energy balance, including what is meant by energy change and energy transfer. 5 Change in Energy of a System (1 of 2) In engineering thermodynamics the change in energy of a system is composed of three contributions: ►Kinetic energy ►Gravitational potential energy ►Internal energy 6  Change in Kinetic Energy ►The change in kinetic energy is associated with the motion of the system as a whole relative to an external coordinate frame such as the surface of the earth. ►For a system of mass m the change in kinetic energy from state 1 to state 2 is DKE = KE2 – KE1 = (Eq. 2.5) where ►V1 and V2 denote the initial and final velocity magnitudes. ►The symbol D denotes: final value minus initial value. 7 Change in Gravitational Potential Energy ►The change in gravitational potential energy is associated with the position of the system in the earth’s gravitational field. ►For a system of mass m the change in potential energy from state 1 to state 2 is DPE = PE2 – PE1 = mg(z2 – z1) (Eq. 2.10) where ►z1 and z2 denote the initial and final elevations relative to the surface of the earth, respectively. ►g is the acceleration of gravity. 8  Change in Internal Energy ► The change in internal energy is associated with the makeup of the system, including its chemical composition. ► There is no simple expression comparable to Eqs. 2.5 and 2.10 for evaluating internal energy change for a wide range of applications. In most cases we will evaluate internal energy change using data from tables in appendices of the textbook. ► Like kinetic and gravitational potential energy, internal energy is an extensive property. ►Internal energy is represented by U. ►The specific internal energy on a mass basis is u. ►The specific internal energy on a molar basis is 9  Change in Energy of a System (2 of 2) ►In summary, the change in energy of a system from state 1 to state 2 is (E2 – E1)sys = (U2 – U1)sys + (KE2 – KE1)sys + (PE2 – PE1)sys (Eq. 2.27a) DE = DU + DKE + DPE (Eq. 2.27b) ►Since an arbitrary value E1 can be assigned to the energy of a system at a given state 1, no particular significance can be attached to the value of energy at state 1 or any other state. Only changes in the energy of a system between 10 states have significance. UNITS of KE and PE 11  Energy Transfer by Work (1 of 2) ►Energy can be transferred to and from closed systems by two means only: ►Work ►Heat ►You have studied work in mechanics and those concepts are retained in the study of thermodynamics. However, thermodynamics deals with phenomena not included within the scope of mechanics, and this requires a broader interpretation of work. 12  To evaluate the integral in Eq. 2.12, it is necessary to know how the force varies with the displacement. This brings out an important idea about work: – The value of W depends on the details of the interactions taking place between the system and surroundings during a process and not just the initial and final states of the system. – It follows that work is not a property of the system or the surroundings. In addition, the limits on the integral of Eq. 2.12 mean “from state 1 to state 2” and cannot be interpreted as the values of work at these states. The notion of work at a state has no meaning, so the value of this integral should never be indicated as W2 − W1. (Moran, 01/2018, p. 29) 13  Work – Thermodynamic definition A particular interaction is categorized as a work interaction if it satisfies the following criterion, which can be considered the thermodynamic definition of work: – Work is done by a system on its surroundings if the sole effect on everything external to the system could have been the raising of a weight. Notice that the raising of a weight is, in effect, a force acting through a distance, so the concept of work in thermodynamics is a natural extension of the concept of work in mechanics. However, the test of whether a work interaction has taken place is not that the elevation of a weight has actually taken place, or that a force has actually acted through a distance, but that the sole effect could have been an increase in the elevation of a weight. (Moran, 01/2018, p. 28) 14  The differential of work, δW, is said to be inexact because, in general, the following integral cannot be evaluated without specifying the details of the process. Similarly, the differential of heat, δQ, is said to be inexact because, in general, the following integral cannot be evaluated without specifying the details of the process. In other words, work and heat are NOT thermodynamic properties of a system! On the other hand, the differential of a property is said to be exact because the change in a property between two particular states depends in no way on the details of the process linking the two states. – For example, the change in volume between two states can be determined by integrating the differential dV, without regard for the details of the process, as follows, where V1 is the volume at state 1 and V2 is the volume at state 2. – The differential of every property is exact. – Exact differentials are written, as above, using the symbol d. To stress the difference between exact and inexact differentials, the differential of work is written as δW. The symbol δ is also used to identify other 15 inexact differentials encountered later. (Moran, 01/2018, pp. 29-30)  Illustrations of Work ►When a spring is compressed, energy is transferred to the spring by work. ►When a gas in a closed vessel is stirred, energy is transferred to the gas by work. ►When a battery is charged electrically, energy is transferred to the battery contents by work. ►The first two examples of work are encompassed by mechanics. The third example is an example of the broader interpretation of work encountered in thermodynamics. 16  Illustration of work …cont’d. Manifestation of work due to current flow. Recall: Work is done by a system on its surroundings if the sole effect on everything external to the system could have been the raising of a weight. Based on the definition of work (above), the cartoon shows how the flow of current is a work transfer interaction. 17  Energy Transfer by Work (2 of 2) ►The symbol W denotes an amount of energy transferred across the boundary of a system by work. ►Since engineering thermodynamics is often concerned with internal combustion engines, turbines, and electric generators whose purpose is to do work, it is convenient to regard the work done by a system as positive. ►W > 0: work done by the system ►W < 0: work done on the system The same sign convention is used for the rate of energy transfer by work – called power, denoted by 18  Energy Transfer by Heat (1 of 2) ►Energy transfers by heat are induced only as a result of a temperature difference between the system and its surroundings. ►Net energy transfer by heat occurs only in the direction of decreasing temperature. 19  Energy Transfer by Heat (2 of 2) ►The symbol Q denotes an amount of energy transferred across the boundary of a system by heat transfer. ►Heat transfer into a system is taken as positive and heat transfer from a system is taken as negative: ►Q > 0: heat transfer to the system ►Q < 0: heat transfer from the system The same sign convention is used for the rate of energy transfer by heat, denoted by ►If a system undergoes a process involving no heat transfer with its surroundings, that process is called 20 adiabatic. Summary: Closed System Energy Balance (1 of 4) ►The energy concepts introduced thus far are summarized in words as follows: change in the amount net amount of energy net amount of energy of energy contained transferred in across transferred out across within a system the system boundary by the system boundary during some time heat transfer during by work during the interval the time interval time interval ►Using previously defined symbols, this can be expressed as: E2 – E1 = Q – W (Eq. 2.35a) ►Alternatively, DKE + DPE + DU = Q – W (Eq. 2.35b) In Eqs. 2.35, a minus sign appears before W because energy transfer by work from the system to the surrounding is 21 taken as positive. Summary: Closed System Energy Balance (2 of 4) ►The time rate form of the closed system energy balance is (Eq. 2.37) ►The rate form expressed in words is time rate of change net rate at which net rate at which of the energy energy is being energy is being contained within transferred in transferred out the system at by heat transfer by work at time t at time t time t 22  Summary: Closed System Energy Balance (3 of 4) When applying the energy balance in any of its forms, it is important to be careful about signs and units and to distinguish carefully between rates and amounts. In addition, it is important to recognize that the location of the system boundary can be relevant in determining whether a particular energy transfer is regarded as heat or work. (Moran, 01/2018, p. 44) When applying the energy balance in any of its forms, it is important to be careful about signs and units and to distinguish carefully between rates and amounts. In addition, it is important to recognize that the location of the system boundary can be relevant in determining whether a particular energy transfer is regarded as heat or work. (Moran, 23  Summary: Closed System Energy Balance (4 of 4) Consider Fig. 2.16, in which three alternative systems are shown that include a quantity of a gas (or liquid) in a rigid, well-insulated container. v In Fig. 2.16a, the gas itself is the system. As current flows through the copper plate, there is an energy transfer from the copper plate to the gas. Since this energy transfer occurs as a result of the temperature difference between the plate and the gas, it is classified as a heat transfer. v Next, refer to Fig. 2.16b, where the boundary is drawn to include the copper plate. It follows from the thermodynamic definition of work that the energy transfer that occurs as current crosses the boundary of this system must be regarded as work. v Finally, in Fig. 2.16c, the boundary is located so that no energy is transferred across it by heat or work. (Moran, 01/2018, p. 44) 24 Modeling Expansion and Compression Work (1 of 7) ►A case having many practical applications is a gas (or liquid) undergoing an expansion (or compression) process while confined in a piston- cylinder assembly. ►During the process, the gas exerts a normal force on the piston, F = pA , where p is the pressure at the interface between the gas and piston and A is the area of the piston face. 25 Modeling Expansion and Compression Work (2 of 7) ►From mechanics, the work done by the gas as the piston face moves from x1 to x2 is given by ►Since the product Adx = dV , where V is the volume of the gas, this becomes V2 (Eq. 2.17) V1 ►For a compression, dV is negative and so is the value of the integral, in keeping with the sign convention for work. 26 Modeling Expansion and Compression Work (3 of 7) ►To perform the integral of Eq. 2.17 requires a relationship between gas pressure at the interface between the gas and piston and the total gas volume. ►During an actual expansion of a gas such a relationship may be difficult, or even impossible, to obtain owing to non-equilibrium effects during the process – for example, effects related to combustion in the cylinder of an automobile engine. ►In most such applications, the work value can be obtained only by experiment. 27 28 Modeling Expansion and Compression Work (4 of 7) ►Eq. 2.17 can be applied to evaluate the work of idealized processes during which the pressure p in the integrand is the pressure of the entire quantity of the gas undergoing the process and not only the pressure at the piston face. ►For this we imagine the gas undergoes a sequence of equilibrium states during the process. Such an idealized expansion (or compression) is called a quasiequilibrium process. 29 30 Modeling Expansion and Compression Work (5 of 7) ►In a quasiequilibrium expansion, the gas moves along a pressure-volume curve, or path, as shown. ►Applying Eq. 2.17, the work done by the gas on the piston is given by the area under the curve of pressure versus volume. 31 Modeling Expansion and Compression Work (6 of 7) ►When the pressure-volume relation required by Eq. 2.17 to evaluate work in a quasiequilibrium expansion (or compression) is expressed as an equation, the evaluation of expansion or compression work can be simplified. ►An example is a quasiequilibrium process described by pVn = constant , where n is a constant. This is called a polytropic process. ►For the case n = 1, pV = constant and Eq. 2.17 gives where constant = p1V1 = p2V2. 32 Modeling Expansion and Compression Work (7 of 7) ►Since non-equilibrium effects are invariably present during actual expansions (and compressions), the work determined with quasiequilibrium modeling can at best approximate the actual work of an expansion (or compression) between given end states. 33  Derivation of Expression for Polytropic Work Ploytropic process  PVn=const. Discuss special cases when n=0, n=1 CONSIDER A POLYTROPIC PROCESS IN WHICH THE INITIAL STATE IS CHARACTERIZED BY PRESSURE, P1 (kPa), VOLUME, V1 (m3) AND THE FINAL STATE IS CHARACTERIZED BY PRESSURE, P2 (kPa), VOLUME, V2 (m3). v FOR THIS PROCESS DETERMINE THE WORK DONE, v DETERMINE WORK DONE WHEN THE POLYTROPIC EXPONENT ASSUMES A VALUE n=1? v DETERMINE WORK DONE WHEN THE POLYTROPIC EXPONENT ASSUMES A VALUE n=0? 34 35 36 37 38 39 40  Modes of Heat Transfer ►For any particular application, energy transfer by heat can occur by one or more of three modes: ►conduction ►radiation ►convection 41  Conduction (1 of 2) ►Conduction is the transfer of energy from more energetic particles of a substance to less energetic adjacent particles due to interactions between them. ►The time rate of energy transfer by conduction is quantified by Fourier’s law. ►An application of Fourier’s law to a plane wall at steady state is shown at right. 42  Conduction (2 of 2) ►By Fourier’s law, the rate of heat transfer across any plane normal to the x direction, , is proportional to the wall area, A, and the temperature gradient in the x direction, dT/dx, (Eq. 2.31) where ►k is a proportionality constant, a property of the wall material called the thermal conductivity. ►The minus sign is a consequence of energy transfer in the direction of decreasing temperature. ►In this case, temperature varies linearly with x, and thus and Eq. 2.31 gives 43  Thermal Radiation (1 of 2) ►Thermal radiation is energy transported by electromagnetic waves (or photons). Unlike conduction, thermal radiation requires no intervening medium and can take place in a vacuum. ►The time rate of energy transfer by radiation is quantified by expressions developed from the Stefan-Boltzman law. 44  Thermal Radiation (2 of 2) ►An application involving net radiation exchange between a surface at temperature Tb and a much larger surface at Ts (< Tb) is shown at right. ►Net energy is transferred in the direction of the arrow and quantified by (Eq. 2.33) where ►A is the area of the smaller surface, ►e is a property of the surface called its emissivity, ►s is the Stefan-Boltzman constant. 45  Convection (1 of 2) ►Convection is energy transfer between a solid surface and an adjacent gas or liquid by the combined effects of conduction and bulk flow within the gas or liquid. ►The rate of energy transfer by convection is quantified by Newton’s law of cooling. 46  Convection (2 of 2) ►An application involving energy transfer by convection from a transistor to air passing over it is shown at right. ►Energy is transferred in the direction of the arrow and quantified by (Eq. 2.34) where ►A is the area of the transistor’s surface and ►h is an empirical parameter called the convection heat transfer coefficient. 47  Thermodynamic Cycles ►A thermodynamic cycle is a sequence of processes that begins and ends at the same state. ►Examples of thermodynamic cycles include ►Power cycles that develop a net energy transfer by work in the form of electricity using an energy input by heat transfer from hot combustion gases. ►Refrigeration cycles that provide cooling for a refrigerated space using an energy input by work in the form of electricity. ►Heat pump cycles that provide heating to a dwelling using an energy input by work in the form of electricity. 48  Thermodynamic Cycles Consider an arbitrary closed cycle as shown in Figure The only requirement for a cycle is that the initial state (i) and final state (f) must be identical to one another. 49  Power Cycle (1 of 4) ►A system undergoing a power cycle is shown at right. ►The energy transfers by heat and work shown on the figure are each positive in the direction of the accompanying arrow. This convention is commonly used for analysis of thermodynamic cycles. ►Wcycle is the net energy transfer by work from the system per cycle of operation – in the form of electricity, typically. ►Qin is the heat transfer of energy to the system per cycle from the hot body – drawn from hot gases of combustion or solar radiation, for instance. ►Qout is the heat transfer of energy from the system per cycle to the cold body – discharged to the surrounding atmosphere or nearby lake or river, for example. 50  Power Cycle (2 of 4) ►Applying the closed system energy balance to each cycle of operation, DEcycle = Qcycle – Wcycle (Eq. 2.39) ►Since the system returns to its initial state after each cycle, there is no net change in its energy: DEcycle = 0, and the energy balance reduces to give Wcycle = Qin – Qout (Eq. 2.41) ►In words, the net energy transfer by work from the system equals the net energy transfer by heat to the system, each per cycle of operation. 51  Power Cycle (3 of 4) ►The performance of a system undergoing a power cycle is evaluated on an energy basis in terms of the extent to which the energy added by heat, Qin, is converted to a net work output, Wcycle. This is represented by the ratio (power cycle) (Eq. 2.42) called the thermal efficiency. ►Introducing Eq. 2.41, an alternative form is obtained (power cycle) (Eq. 2.43) 52  Power Cycle (4 of 4) ►Using the second law of thermodynamics (Chapter 5), we will show that the value of thermal efficiency must be less than unity: h < 1 (< 100%). That is, only a portion of the energy added by heat, Qin, can be obtained as work. The remainder, Qout, is discharged. Example: A system undergoes a power cycle while receiving 1000 kJ by heat transfer from hot combustion gases at a temperature of 500 K and discharging 600 kJ by heat transfer to the atmosphere at 300 K. Taking the combustion gases and atmosphere as the hot and cold bodies, respectively, determine for the cycle, the net work developed, in kJ, and the thermal efficiency. ►Substituting into Eq. 2.41, Wcycle = 1000 kJ – 600 kJ = 400 kJ. ►Then, with Eq. 2.42, h = 400 kJ/1000 kJ = 0.4 (40%). Note the 53 thermal efficiency is commonly reported on a percent basis.  Refrigeration Cycle (1 of 3) ►A system undergoing a refrigeration cycle is shown at right. ►As before, the energy transfers are each positive in the direction of the accompanying arrow. ►Wcycle is the net energy transfer by work to the system per cycle of operation, usually in the form of electricity. ►Qin is the heat transfer of energy to the system per cycle from the cold body – drawn from a freezer compartment, for example. ►Qout is the heat transfer of energy from the system per cycle to the hot body – discharged to the space surrounding the refrigerator, for instance. 54  Refrigeration Cycle (2 of 3) ►Since the system returns to its initial state after each cycle, there is no net change in its energy: DEcycle = 0, and the energy balance reduces to give Wcycle = Qout – Qin (Eq. 2.44) ►In words, the net energy transfer by work to the system equals the net energy transfer by heat from the system, each per cycle of operation. 55  Refrigeration Cycle (3 of 3) ►The performance of a system undergoing a refrigeration cycle is evaluated on an energy basis as the ratio of energy drawn from the cold body, Qin, to the net work required to accomplish this effect, Wcycle: (refrigeration cycle) (Eq. 2.45) called the coefficient of performance for the refrigeration cycle. ►Introducing Eq. 2.44, an alternative form is obtained (refrigeration cycle) (Eq. 2.46) 56  Heat Pump Cycle (1 of 4) ►The heat pump cycle analysis closely parallels that given for the refrigeration cycle. The same figure applies: ►But now the focus is on Qout, which is the heat transfer of energy from the system per cycle to the hot body – such as to the living space of a dwelling. ►Qin is the heat transfer of energy to the system per cycle from the cold body – drawn from the surrounding atmosphere or the ground, for example. 57  Heat Pump Cycle (2 of 4) ►As before, Wcycle is the net energy transfer by work to the system per cycle, usually provided in the form of electricity. ►As for the refrigeration cycle, the energy balance reads Wcycle = Qout – Qin (Eq. 2.44) 58  Heat Pump Cycle (3 of 4) ►The performance of a system undergoing a heat pump cycle is evaluated on an energy basis as the ratio of energy provided to the hot body, Qout, to the net work required to accomplish this effect, Wcycle: (heat pump cycle) (Eq. 2.47) called the coefficient of performance for the heat pump cycle. ►Introducing Eq. 2.44, an alternative form is obtained (heat pump cycle) (Eq. 2.48) 59  Heat Pump Cycle (4 of 4) Example: A system undergoes a heat pump cycle while discharging 900 kJ by heat transfer to a dwelling at 20oC and receiving 600 kJ by heat transfer from the outside air at 5oC. Taking the dwelling and outside air as the hot and cold bodies, respectively, determine for the cycle, the net work input, in kJ, and the coefficient of performance. ►Substituting into Eq. 2.44, Wcycle = 900 kJ – 600 kJ = 300 kJ. ►Then, with Eq. 2.47, g = 900 kJ/300 kJ = 3.0. Note the coefficient of performance is reported as its numerical value, as calculated here. 60