Download presentation

Presentation is loading. Please wait.

1
**Thermodynamics processes and cycles**

HEAT PROCESSES TZ2 HP2 Thermodynamics processes and cycles Thermodynamics fundamentals. State variables, Gibbs phase rule, state equations, internal energy, enthalpy, entropy. First law and the second law of thermodynamics. Phase changes and phase diagrams. Ts and hs diagrams (example: Ts diagrams for air). Thermodynamic cycles Carnot, Clausius Rankine, Ericson, Stirling, thermoacoustics. Rudolf Žitný, Ústav procesní a zpracovatelské techniky ČVUT FS 2010

2
**FUNDAMENTALS of THERMODYNAMICS**

HP2 TZ1 FUNDAMENTALS of THERMODYNAMICS Estes

3
**BASIC NOTIONS HP2 TZ1 SYSTEM Closed (without mass transfer)**

Subsystem flame zone = opened SYSTEM Insulated- without mass or energy transfer Closed (without mass transfer) Opened (mass and heat transport through boundary). Thermal units operating in continuous mode (heat exchangers, evaporators, driers, tubular reactors, burners) are opened systems Thermal units operating in a batch mode (some chemical reactors) are closed systems Subsystem candlewick = opened Subsystem candle = opened with moving boundary Subsystem stand = closed

4
StaTE VARIABLES HP2 TZ1 state of system is characterized by THERMODYNAMIC STATE VARIABLES related with directly measurable mechanical properties: T [K], p [Pa=J/m3], v [m3/kg] (temperature, pressure, specific volume) Thermodynamické state variables related to energy (could be derived from T,p,v): u [J/kg] internal energy s [J/kg/K] specific entropy h [J/kg] enthalpy g [J/kg] gibbs energy e [J/kg] exergy

5
**Gibbs phase rule NDOF = Ncomponents – Nphases + 2 HP2 TZ1**

Not all state variables are independent. Number of independent variables (DOF, Degree Of Freedom) is given by Gibbs rule NDOF = Ncomponents – Nphases + 2 1 component, 1 phase (e.g.gaseous oxygen) NDOF=2 . In this case only two state variables can be selected arbitrarily, e.g. p,v, or p,T or v,T. 1 component, 2 phases (e.g. equilibrium mixture of water and steam at the state of evaporation/condensation). In this case only one state variable can be selected, e.g. pressure (boiling point temperature is determined by p)

6
**State EquATIONS p-v-T Van der Waals equation isotherms HP2 TZ2**

Critical point, solution of these two equations give a,b parameters as a function of critical temperature and critical pressure Above critical temperature Tc the substance exists only as a gas (liquefaction is not possible even at infinitely great pressure)

7
**Pv=RT tutorial Baloon = 599 kg TZ2 HP2**

Example: Calculate load capacity of a baloon filled by hot air. D=20m, T=600C, Te=200C, p=105 Pa. M=29 (air) D m = 599 kg

8
**Adiabatic change (thermally insulated)**

TZ2 HP2 Pv=RT tutorial Syringe Record time change of temperature of air compressed in syringe. V x D Thermocouple P-pressure transducer Kulite XTM 140 Adiabatic change (thermally insulated) Example: V2/V1= =cp/cv=1.4 T1=300 K T2=396 K temperature increase 96 K!!

9
**tested sample, viscoelastic tube (blood vessel)**

TZ2 HP2 Pv=RT tutorial - expansion Dynamic inflation test of a viscoelastic pipe (carried out in our laboratory of cardiovascular mechanics) was based upon recorded oscillation of pressure after a sudden release of pressure in a container. We did not know a reason for a gradual pressure increase in the end of experiment. Possible explanation: Temperature of adiabatically expanded air initially drops and later on slowly increases to the room temperature (and this is accompanied by a gradual increase of pressure). T1=300K, p1=60kPa T2=257K, p2=35kPa T3=300K, p3=41kPa Example: p2/p1=35/60= =cp/cv= T1=300 K T2=257 K Slow heating (closed vessel) to the final temperature 300K tested sample, viscoelastic tube (blood vessel) In this way only a final value p3 is analysed. It is necessary to know heat transfer rate (heat transf.coef.) to calculate the time change of p.

10
**Internal energy u [J/kg]**

TZ2 HP2 Internal energy u [J/kg] u-all forms of energy of matter inside the system (J/kg), invariant with respect to coordinate system (potential energy of height /gh/ and kinetic energy of motion of the whole system /½w2/ are not included in the internal energy). Internal energy is determined by structure, composition and momentum of all components, i.e. all atoms and molecules. Nuclear energy (nucleus) ~1017J/kg Chemical energy of ionic/covalent bonds in molecule ~107 J/kg Intermolecular VdW forces (phase changes) ~106 J/kg Thermal energy (kinetic energy of molecules) ~104 J/kg Frequently only the following item (thermal energy) is included into the internal energy notion (sometimes distinguished as the sensible internal energy) It follows from energy balances that the change of internal energy of a closed system at a constant volume equals amount of heat delivered to the system du = dq (heat added at isochoric change)

11
**Enthalpy h [J/kg] h=u+pv**

TZ2 HP2 Enthalpy h [J/kg] h=u+pv enthalpy is always greater than the internal energy. The added term pv (pressure multiplied by specific volume) simplifies energy balancing of continuous systems. The pv term automatically takes into account mechanical work (energy) necessary to push/pull the inlet/outlet material streams to/from the balanced system. It follows from energy balances that the change of enthalpy of a closed system at a constant pressure equals amount of heat delivered to the system dh = dq (heat added at isobaric change)

12
TZ2 HP2 Entropy s [J/kg/K] Thermodynamic definition of entropy s by Clausius where ds is the specific entropy change of system corresponding to the heat dq [J/kg] added in a reversible way at temperature T [K]. Boltzmann’s statistical approach: Entropy represents probability of a macroscopic state (macrostate is temperature, concentration,…). This probability is proportional to the number of microstates corresponding to a macrostate (number of possible configurations, e.g. distribution of molecules to different energy levels, for given temperature). It follows from energy balances that the change of entropy of a closed system at a constant temperature equals amount of heat delivered to the system / T Tds = dq (heat added at an isothermal and reversible change)

13
**Laws of thermodynamics**

HP2 TZ2 Modigliani

14
**Laws of thermodynamics**

HP2 TZ2 First law of thermodynamics (conservation of energy) δq = heat added to system δw = work done by system expansion work (p.dV) in case of compressible fluids, surface work (surface tension x increase of surface), shear stresses x displacement, but also electrical work (intensity of electric field x current). Later on we shall use only the p.dV mechanical expansion work. δq = du + δw Second law of thermodynamics (entropy of closed insulated system increases) Tds δq δq = heat added to system is Tds only in the case of reversible process Combined first and second law of thermodynamics Tds = du+pdv

15
**THERMODYNAMIC relationships**

TZ2 HP2 Be careful at interpretation: First law of thermodynamic was presented in the form corresponding only to reversible changes (therefore for infinitely slow changes, without viscous friction, at uniform temperature) This equation enables to calculate the entropy change during a reversible process. However, entropy is a state variable, and its changes are independent of the way, how the changes were realized (there are always infinitely many ways how to proceed from a state 1 to a state 2). So, why not to select the reversible way even in the case, when the real process is irreversible? It is always simpler and results (for example calculated entropy changes) hold generally even for irreversible (real) processes. In the following it will be demonstrated how to calculate internal energy and enthalpy changes from the measured changes of temperature, pressure and volume (and results hold not only for the reversible processes). reversible processes are generally defined as changes of state (12) which can be recovered (21) without any change of the system environment. In an irreversible process it is also possible to return back (to the initial state) but heat or work must be added from environment.

16
**Example: insulated system**

TZ2 HP2 Let us consider a perfectly insulated calorimeter (Deware flask, e.g.) containing a cold metallic block (temperature Tm) and hot water (Tw). At a time interval dt the temperature of water Tw decreases by dTw=-dQwm/(mwcpw) and the temperature Tm increases by dTm=dQwm/(mmcpm), however the sum of inner energies U=ummm+uwmw remains, therefore dU=0. Volume V is constant and dV=0. Therefore the entropy increase of the whole system dS should be zero (dS=0) Water Tw=300K dQwm This conclusion is wrong, because the whole process is irreversible and dS is actually positive. So that the previous equation could be used the whole process must be substituted by an equivalent but reversible process. For example the water can be used for heating Metal Tm=273K of a fictive gas at constant temperature Tw (reversibly, entropy of water will be decreased by dQwm/Tw), followed by an adiabatic expansion cooling down the gas to the temperature Tm (reversible expansion, not changing the entropy of gas). The gas then isothermally and reversibly heats the metallic block, thus increasing its entropy by dQwm/Tm. Summing the entropy changes gives

17
**Energies and Temperature**

TZ2 HP2 The temperature increase increases thermal energy (kinetic energy of molecules). For constant volume (fixed volume of system) internal energy change is proportional to the change of thermodynamic temperature (Kelvins) du = cv dT where cv is specific heat at constant volume For constant pressure (e.g. atmospheric pressure) the enthalpy change is also proportional to the thermodynamic temperature dh = cp dT where cp is specific heat at constant pressure. Specific heat at a constant pressure is always greater than the specific heat at a constant volume (it is always necessary to supply more heat to increase temperature at constant pressure, because part of the delivered energy is converted to the volume increase, therefore to the mechanical work). Only for incompressible materials it holds cp=cv.

18
**Energies and Temperature**

TZ2 HP2 Internal energy (kinetic energy of translatory motion) of one monoatomic molecule of an ideal gas is given by where k is Boltzmann constant ×10−23 Kinetic energy (1/2mw2) of chaotic thermal motion is therefore independent of molecular mass (lighter molecules are moving faster)! Knowing molecular mass it is therefore possible to estimate the specific heat capacity cv [J/kg/K] theoretically (molar internal energy , therefore molar heat capacity Specific heat capacity is where M is molecular mass [kg/mol]. For helium (M=0.004) thus calculated specific heat capacity cv=12.5/0.004=3125 J/kg/K. The tabulated cp value at 300K is cp=5193 J/kg/K. This agrees quite well, because cp-cv=R/M=8.314/0.004=2078 J/kg/K, see the Mayer’s equation). For more complicated molecules the equipartition principle can be applied, stating that any mode of motion (translational, vibrational, rotational) has the same energy kT/2 (monoatomic gas has 3 translational modes in the x,y,z directions, therefore u=3kT/2). According to the equipartition theorem the specific heat capacities are constants independent of temperature. This is not quite true especially at low temperatures, when cv decreases – and in this case quantum mechanics must be applied. At low temperatures (<100 K) only three translational degrees of freedom are excited (cv=3/2R), at higher temperatures two additional rotational degrees increase cv to 5/2R (for diatomic molecules N2, H2, O2) and contribution of vibrational degrees of freedom is significant at even higher temperatures (>500 K). In water rotational and vibrational degrees of freedom are excited at very low temperatures. This nice animated gif (molecule of a peptide with atoms C,N,O,H) is captured from Wikipedia.org

19
**Energies and Temperature**

TZ2 HP2 According to the equipartition theorem the specific heat capacities are constants independent of temperature. This is not quite true especially at low temperatures, when cv decreases – and in this case quantum mechanics must be applied. At low temperatures (<100 K) only three translational degrees of freedom are excited (cv=3/2R), at higher temperatures two additional rotational degrees increase cv to 5/2R (for diatomic molecules N2, H2, O2) and contribution of vibrational degrees of freedom is significant at even higher temperatures (>500 K). In water rotational and vibrational degrees of freedom are excited at very low temperatures.

20
**u(T,v) internal energy change**

TZ2 HP2 How to evaluate internal energy change? Previous relationship du=cvdT holds only at a constant volume. However, according to Gibbs rule the du should depend upon a pair of state variables (for a one phase system). So how to calculate du as soon as not only the temperature (dT) but also the specific volume (dv) are changing? Solution is based upon the 1st law of thermodynamic (for reversible changes) where du is expressed in terms dT and dv (this is what we need), coefficient at dT is known (cv), however entropy appears at the dv term. It is not possible to measure entropy directly (so how to evaluate ds/dv?), but it is possible to use Maxwell relationships, stating for example that Instead of exact derivation I can give you only an idea based upon dimensional analysis: dimension of s/v is Pa/K and this is just the dimension of p/T! So there is the final result ds cv This term is zero for ideal gas (pv=RT)

21
**h(T,p) enthalpy changes**

TZ2 HP2 The same approach can be applied for the enthalpy change. So far we can calculate only the enthalpy change at constant pressure (dh=cpdT). Using definition h=u+pv and the first law of thermodynamics And the same problem how to express the entropy term ds/dp by something that is directly measurable. Dimensional analysis: s/p has dimension J/(kg.K.Pa)=m3/(kg.K) and this is dimension of v/T. Corresponding Maxwells relationship is After substuting we arrive to the final expression for enthalpy change Negative sign in the Maxwell equation is probably confusing, and cannot be derived from dimensional analysis. Correct derivation is presented in the following slide. cp Tds

22
**Maxwell relationships**

TZ2 HP2 Basic idea consists in design of a state function with total differential depending only upon dT and dp . Such a function is Gibbs energy g (previously free enthalpy) Notice the fact, that using this combination of enthalpy and entropy (h-Ts) the differentials dh and ds are mutually cancelled. Comparing coefficients at dp and dT the partial derivatives of Gibbs energy can be expressed as Because the mixed derivatives equal, the Maxwell equation follows

23
**Maxwell relationships**

TZ2 HP2 For first law For incompressible elongation (f force positive when extended) For magnetisation H-intensity of magnetic. field -specific magnetisation 0-magnetic permeability of vacuum

24
**s(T,v) s(T,p) entropy changes**

TZ2 HP2 Changes of entropy follow from previous equations for internal energy and enthalpy changes Special case for IDEAL GAS (pv=RmT, where Rm is individual gas constant) Please notice the difference between universal and individual gas constant. And the difference between molar and specific volume.

25
**u,h,s finite changes (without phase changes or reactions)**

TZ2 HP2 Previous equations describe only differential changes. Finite changes must be calculated by their integration. This integration can be carried out analytically for constant values of heat capacities cp, cp and for state equation of ideal gas

26
**u,h,s finite changes during phase changes**

TZ2 HP2 During phase changes (evaporation, condensation, melting,…) both temperature T and pressure p remain constant. Only specific volume varies and the enthalpy/entropy changes depend upon only one state variable (for example temperature). These functions are tabulated (e.g. h-enthalpy of evaporation) as a function of temperature (see table for evaporation of water), or approximated by correlation T[0C] p[Pa] h[kJ/kg] 593 2538 50 12335 2404 100 101384 2255 200 1898 300 1373 Tc=647 K, T1=373 K, r=2255 kJ/kg, n=0.38 for water Pressure corresponding to the phase change temperature is calculated from Antoine’s equation C=-46 K, B= , A= for water Entropy change is calculated directly from the enthalpy change

27
**h,s during phase changes (phase diagram p-T)**

TZ2 HP2 Melting hSL>0, sSL>0,, S-solid L-liquid G-gas T p Evaporation hLG>0, sLG>0, Sublimation hSG>0, sSG>0, Phase transition lines in the p-T diagram are described by the Clausius Clapeyron equation hLG Specific volume changes, e.g. vG-vL

28
**Initial state T1=0C, p1=1bar**

h finite changes EXAMPLE TZ2 HP2 There are infinitely many ways how to proceed from the state 1 to the state 2. For example Red way increases first the pressure to the final value and continues by heating. Water boils at 120C (Antoine’s equation). Compression hcompres=0 Liquid water h=cpL.120 for cpL=4.21 Evaporation hLG=2203 J/kg (from table) Steam h=cpG.380, cpG=2.07 Taken together h=3495 J/kg Green way holds initial pressure when heating up to final temperature and isothermal compression follows. Liquid water h=cpL.100 for cpL=4.20 Evaporation hLG=2255 J/kg (from table) Steam h=cpG.400, cpG=2.05 Isothermal compression hcompres=0 Sum (1-4) gives the same result h=3495 J/kg Final state T2=500C, p2=2bar S-solid L-liquid G-gas T p Initial state T1=0C, p1=1bar 1000C 1200C Remark: cp depends upon temperature (use tables)

29
**Initial state T1=20C, p1=1bar**

s finite changes EXAMPLE TZ2 HP2 Entropy change follows directly from definition Final state T2=80C, p2=1bar S-solid L-liquid G-gas T p Initial state T1=20C, p1=1bar

30
SUMMARY TZ2 HP2 State equation p,v,T. Ideal gas pV=nRT (n-number of moles, R=8.314 J/mol.K) First law of thermodynamics (and entropy change) Internal energy increment (du=cv.dT for constant volume dv=0) Enthalpy increment (dh=cp.dT for constant pressure dp=0) These terms are zero for ideal gas (pv=RT)

31
Check units TZ2 HP2 It is always useful to check units – all terms in equations must have the same dimension. Examples

32
**Important values TZ2 HP2 cv=cp ice = 2 kJ/(kg.K)**

cv=cp water = 4.2 kJ/(kg.K) cp steam = 2 kJ/(kg.K) cp air = 1 kJ/(kg.K) Δhenthalpyof evaporation water = 2.2 MJ/kg R = kJ/(kmol.K) Rm water = 8.314/18 = kJ/(kg.K) Example: Density of steam at 200 oC and pressure 1 bar.

33
**THERMODYNAMIC DIAGRAMS**

TZ2 HP2 THERMODYNAMIC DIAGRAMS Delvaux

34
DIAGRAM T-s TZ2 HP2 isobars Critical point isochors Left curve-liquid Right curve-saturated steam Implementation of previous equations in the T-s diagram with isobars and isochoric lines.

35
**DIAGRAM h-s TZ2 HP2 Critical point Left curve liquid**

Right curve saturated steam

36
**Thermodynamic processes**

TZ2 HP2 Basic processes in thermal apparatuses are Isobaric dp=0 (heat exchangers, ducts, continuous reactors) Isoentropic ds=0 (adiabatic-thermally insulated apparatus, ideal flow without friction, enthalpy changes are fully converted to mechanical energy: compressors, turbines, nozzles) Isoenthalpic dh=0 (also adiabatic without heat exchange with environment, but no mechanical work is done and pressure energy is dissipated to heat: throttling in reduction valves)

37
**Thermodynamic processes**

TZ2 HP2 s T h STEAM expansion in a turbine the enthalpy decrease is transformed to kinetic energy, entropy is almost constant (slight increase corresponds to friction) T h Expansion of saturated steam in a nozzle the same as turbine (purpose: convert enthalpy to kinetic energy of jet) s s s T h Steam compression power consumption of compressor is given by enthalpy increase Throttling of steam in a valve or in a porous plug. Enthalpy remains constant while pressure decreases. See next lecture Joule Thomson effect. s T h

38
**Thermodynamic processes**

TZ2 HP2 s T h Superheater of steam. Pressure only slightly decreases (friction), temperature and enthalpy increases. Heat delivered to steam is the enthalpy increase (isobaric process). The heat is also hatched area in the Ts diagram (integral of dq=Tds). s T h Boiler (evaporation at the boiling point temperatrure) constant temperature, pressure. Density decreases, enthalpy and entropy increases. Hatched area is the enthalpy of evaporation. Mixing of condensate and superheated steam purpose of mixing is to generate a saturated steam from a superheated steam. Resulting state is determined by masses of condensate and steam (lever rule). s T h

39
**Thermodynamic cycles TZ2 HP2**

Periodically repeating processes with working fluid (water, hydrocarbons, CO2,…) when heat is supplied to the fluid in the first phase of the process followed by the second phase of heat removal (final state of the working medium is the same as the initial one, therefore the cycle can be repeated infinitely many times). Because more heat is supplied in the first phase than in the second phase, the difference is the mechanical work done by the working medium in a turbine (e.g.). It follows from the first law of thermodynamics.

40
**Thermodynamic cycles TZ2 HP2 Carnot cycle s T s T**

Mechanical work 1 2 3 4 s T 1 2 3 4 s T 1 2 3 4 Clausius Rankine cycle Cycle makes use phase changes. Example POWERPLANTS. 1-2 feed pump boiler and heat exchangers turbine and generator condenser 1 2 3 4 s T 1 2 3 4 Ericsson cycle John Ericsson designed (200 years ago) several interesting cycles working with only gaseous phase. Reversed cycle (counterclock orientation) is applied in air conditioning – see Brayton cycle shown in diagrams. 2 3 1 4

41
**Thermodynamic cycles TZ2 HP2**

H. Chen et al. / Renewable and Sustainable Energy Reviews 14 (2010) 3059–3067 ORC – Organic Rankine Cycles supercritical Rankine cycle (CO2)

42
**Stirling machine TZ2 HP2 Engine (work produced) Stirling cycle**

Gas cycle having thermodynamic efficiency of Carnot cycle. Can be used as engine or heat pump (Stirling machines fy.Philips are used in cryogenics). Efficiency can be increased by heat regenerator (usually a porous insert in the displacement channel capable to absorb heat from the flowing gas). Compression 1-2 and transport of cool gas to heater 2-3 Expansion of hot gas Displacement of gas from hot to cool section 4-1 Compression (1-2) 1 3 2 4 β-Stirling Refrigeration (work consumed) s T 1 2 3 4 4-1 displacement v=const. and heating in regenerator 1-2 isothermal compression 2-3 cooling in regenerator 3-4 isothermal expansion -Stirling with regenerator

43
**Thermoacoustical engine**

TZ2 HP2 Thermoacoustic analogy of Stirling engine Very simple design can be seen on Internet video engines. Cylinder can be a glass test tube with inserted porous layer (stack). Besides toys there exist applications with rather great power driven by solar energy or there exist equipments for cryogenics – liquefaction of natural gas. Hot HE Cold HE Stack (regeneratir) Velocity amplitude pressure x u,p Standing waves – mutually shifted pressure and velocity waves (90o) Wave equation for pressure, velocity. C is speed of sound Mechanical design is simple, unlike theoretical description (N.Rott published series of papers Thermally driven acoustic oscillations, I.,II.,III.,IV.,V. in Journal of Applied Mathematics and Physics in years 1969,1973, 1975,1976). Standing temperature and pressure waves generated inside the cylinder are mutually shifted (phase shift is similar to the Stirling engine, where compression/expansion phases are shifted with respect to the heating/cooling phase). Solution of oscillating pressure, temperature and gas velocity is frequently realized by Computer Fluid Dynamics codes (Fluent). Travelling waves mode – in phase pressure and velocity waves Travelling waves – analogy with Stirling Tuned resonator

44
Thermoacoustics TZ2 HP2 Phenomena and principles of thermoacoustics are more than hundred years old. Singing Rijke tube Rijke P.L. Annalen der Physik 107 (1859), 339 Sondhauss tube Sondhauss C. Annalen der Physik 79 (1850), 1 Taconis oscillations Taconis K.W. Physica 15 (1949) 738 Heated wire screen Air flowing through an empty tube Generated sound waves Thin tube Thin tube inserted into a cryogenic liquid Heated bulb Liquid helium Lord Rayleigh | author=Lord Rayleigh | title=The explanation of certain acoustical phenomena | journal=Nature (London) | year=1878 | volume=18 | pages=319–321] formulated principles as follows: thermoacoustic oscillations are generated as soon as Heat is supplied to the gas at a place of greatest condensation (maximum density) Heat is removed at a place of maximum rarefaction (minimum pressure)

45
**Thermoacoustics TZ2 HP2 Refrigerator (heat pump if )**

Scott Backhaus and Greg Swift: New varieties of thermoacoustic engines, 2002 Thermoacoustic machines can operate either as heat pumps (usually refrigerators) when forced oscillations are driven by an oscillating membrane (usually loadspeaker), or as an engine (prime mover) that turns heat into mechanical energy (sound). Spontaneous oscillations (engine mode) exist only if the axial temperature gradient in stack is high enough so that the Rayleigh criterion will be satisfied (see fig. showing axial gradient Tstack in a stack and Tcrit in a gas parcel oscillating in the x-direction at a large distance from the wall of stack). Babaei H.,Siddiqui K.: Design and optimisation of thermoacoustic devices. Energy Conversion and Management, 49 (2008), -frequency, -therm.expansion [1/K], p-mean pressure amplitude, u-mean velocity amplitude, -mean density Refrigerator (heat pump if ) Engine (oscillations generated if ) T Heat supplied to gas parcel at max.density stack Cold HE Hot HE Hot HE loadspeaker Critical gradient Tcrit (insulated parcel) Piston or piezocrystal Axial temperature of stack Tstack Heat removed from gas to stack x Gas parcel oscillating back and forth in accordance with pressure (motion left – increasing pressure – compression – gas temperature increases - heat is removed from gas to stack and work is consumed by gas parcel)

46
Thermoacoustics TZ2 HP2 How to understand the expression for the critical axial temperature gradient? -frequency, -therm.expansion [1/K], p-mean pressure amplitude, u-mean velocity amplitude, -mean density T describes temperature difference during pressure oscillation of a thermally insulated gas parcel (adiabatic compression/expansion) Mean velocity of gas parcel times time of period For ideal gas thermal expansion coefficient =1/T T For adiabatic compression Ts=0 T temperature change during adiabatic compression of gas parcel x displacement of a gas parcel during one oscillation

47
**Thermoacoustics - modelling**

TZ2 HP2 Theoretical background of thermoacoustics developed by Nicolas Rott and published as a serie of articles (Thermally driven acoustic oscillations) in Journal of Applied Mathematics and Physics is not freely available in Internet, on contrary to the recent PhD thesis Mathematical Aspects of Thermoacoustics 2009 (Eidhoven) or the Technical Research Institute of Sweden report written by Freddy Rietdijk Thermoacoustic refrigeration using a standing-wave device Some papers are available from Science direct, for example This paper presents analytical solution of oscillating velocity, pressure and temperature field in a tube (capillary of a stack). The solution is almost the same as that derived by Nicolas Rott Continuity equation relating axial (u1) and transversal (v1) velocities and density . is prescribed frequency and a is speed of sound, L is length of tube Momentum balance for axial velocity (pressure is independent of radius and radial velocity profile is expressed in terms of bessel function J0). v is viscous penetration depth (therefore velocities are not exactly in phase with oscillation of pressure). Enthalpy balance of gaseous layer. The first RHS term corresponds to the time derivative of pressure. Only the radial heat transport characterised by the thermal penetration depth t is important. Penetration depth shifts temperature oscillations. Enthalpy balance in the wall of stack must be solved too (stack represents an regenerator). s is the penetration depth in solid material of wall. State equation of ideal gas (after expansion, index 1 means the first term of expansion)

48
**Thermoacoustics TZ2 HP2 CFD combustion thermoacoustics**

Low computational cost CFD analysis of thermoacoustic oscillations Applied Thermal Engineering, Volume 30, Issues 6-7, May 2010, Pages Andrea Toffolo, Massimo Masi, Andrea Lazzaretto Timing of the pressure fluctuation due to the acoustic mode at 36 Hz and of the heat released by the fuel injected through the main radial holes (if the heat is released in the gray zones, the necessary condition stated by Rayleigh criterion is satisfied and thermoacoustic oscillations at this frequency are likely to grow).

49
**Magnetic refrigeration**

TZ2 HP2 Application of magnetic field upon ferromagnetic material causes orientation of magnetic spin of molecules therefore decreases the magnetic entropy. Total entropy (sum of magnetisation entropy and lattice entropy, thermal vibration of molecules in a crystal lattice) remains constant assuming a thermally insulated (adiabatic) system, therefore the magnetic entropy decrease must be compensated by the thermal entropy (and temperature) increase. The first law of thermodynamic can be formulated in terms of internal energy as (o magnetic permeability of vacuum, H intensity of magnetic field [T], specific magnetisation) For constant volume the relationship between entropy, temperature and H is For most materials magnetisation decreases with temperature therefore d/dT<0 and matter heats when H increases. This equation enables to construct the T-s diagrams and demonstrate thermodynamic cycles of refrigeration.

50
**Magnetic refrigeration**

TZ2 HP2 Principle of Active Magnetic Regenerator (AMR) cycle….

51
**Magnetic refrigeration**

TZ2 HP2 Romero Gómez, J., Ferreiro Garcia, R., Carbia Carril, J., Romero Gómez, M., Experimental analysis of a reciprocating magnetic refrigeration prototype, International Journal of Refrigeration (2013) The working principle is as follows: during the first semicycle of operation one of the regenerators (2) is subjected to the magnetic field action generated by the permanent magnets (6). As a consequence of this field, the material contained in this part of the regenerator undergoes the MCE. The HTF, consisting of glycol water, is pumped via the circulation pump (4) through the servo-valve (5a) activated during the first semi-cycle to absorb the heat generated by the magnetocaloric material whilst it is cooled. The heat absorbed from the magnetocaloric material is ceded to the environment in the HHEX(1). Once the heat is ceded, the HTF is returned through the other regenerator. Upon contact with the magnetocaloric material, whose temperature has decreased as a result of being removed in the previous semi-cycle from the presence of the magnetic field, the HTF is cooled. The cooled HTF passes through the two-position three-way valve (5b) toward the CHEX(3). Once the first semi-cycle is finished, the valve positions change simultaneously (5a) and (5b) whilst the AMR moves (2) within the magnetic field, thus inverting the flow direction of the circulating HTF. (1) HHEX, (2)mobile AMR, (2a) regenerator A, (2b) regenerator B, (3) CHEX, (4) pump, (5a), (5b) solenoid valve, (6) static NdFeB magnets, (7) motor, (8) magnet fixed to yoke to compensate F, (9) magnet fixed to the AMR, (10) AMR displacement guide

52
**Magnetic refrigeration**

TZ2 HP2 Romero Gómez, J., Ferreiro Garcia, R., Carbia Carril, J., Romero Gómez, M., A review of room temperature linear reciprocating magnetic refrigerators. Renewable and Sustainable Energy Reviews, Volume 21, May 2013, Pages 1-12 AMR cycle cannot be described by Ts diagrams. Rotary AMR Reciprocating AMR

53
**Magnetic refrigeration**

TZ2 HP2 H.R.E.H. Bouchekara, A. Kedous-Lebouc, J.P. Yonnet: Design of a new magnetic refrigeration field source running with rotating bar-shaped magnets. International Journal of Refrigeration 35 (2012) A Halbach magnet array is an arrangement of permanent magnets to increase the magnetic field on one side of the array while canceling it on the other side This paper is only a theoretical analysis calculated by MATLAB. Permanent magnets NdFeB (Neodymium-Iron-Boron alloy, diameter of 7 rods is 20 mm, magnetic induction 1.4T). Active blocks are Gadolinium.

54
Laser cooling TZ2 HP2 Ruan X.L. et al. Entropy and efficiency in laser cooling solids. Physical Review B, 75 (2007), A phonon is a quantum of collective excitation in a periodic, elastic arrangement of atoms or molecules in condensed matter. Chu, Steven, Science 253, , 1991 Lasers to achieve extremely low temperatures has advanced to the point that temperatures of 10-9 K have been reached. Idea of Doppler effect atom Na moving with velocity about 570 m/s at 300K collision with photon from behind has too low energy laser should be tuned below the resonance frequency (difference f should be the Doppler frequency given by velocity of atom)

55
EXAM HP2 Thermodynamic cycles. Heat pumps and Heat engines

56
**EXAM HP2 Carnot T s Clausius Rankine T s Ericsson T s 3 2 1 4 3 2 4 1**

57
**What is important (at least for exam)**

HP2 regenerator T STIRLING displacing piston 1 3 2 4 Thermoacoustic standing wave compression/expansion wave stack s Thermoacoustic travelling wave regenerator N S AMR Active Magnetic Refrigerator

Similar presentations

OK

Aka the Law of conservation of energy, Gibbs in 1873 stated energy cannot be created or destroyed, only transferred by any process The net change in energy.

Aka the Law of conservation of energy, Gibbs in 1873 stated energy cannot be created or destroyed, only transferred by any process The net change in energy.

© 2017 SlidePlayer.com Inc.

All rights reserved.

Ads by Google

Ppt on balanced diet completes physical health Ppt on institute management system Ppt on nitrogen cycle Can keynote read ppt on iphone Ppt on power transmission drives Show ppt on samsung tv Ppt on rational and irrational numbers for class 9 Ppt on virus and antivirus Ppt on technical analysis of indian stocks Free download ppt on unity in diversity