Untitled - Aerobib - Universidad Politécnica de Madrid

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1.2. THERMODYNAMIC FUNCTIONS OF AN IDEAL GAS. 9 Alcohols Substance Formula State h 0 s 0 ∆G 0 Methanol CH 3OH g -1501.15 1.773 38 700 Methanol CH 3 OH l -1780.04 0.946 -39 750 Ethanol C 2H 5OH g -1220.80 1.463 -40 300 Ethanol C 2 H 5 OH l -1440.39 0.834 -41 770 1-Propanol C 3H 7OH l -1212.43 0.767 -40 900 2-Propanol C 3 H 7 OH l -1279.00 0.716 -44 000 1-Butanol C 4H 9OH l -1074.07 0.735 -40 400 2-methyl-2-Propanol (CH 3 ) 3 COH l -1206.29 0.611 -47 500 1-Pentanol C 5H 11OH l -976.33 0.691 -39 100 2-methyl-2-Butanol C 2 H 5 COH(CH 3 ) 2 l -1094.32 0.622 -47 700 Diphenyl Carbinol (C 6H 5) 2CHOH s -110.62 0.311 30 700 Triphenyl Carbinol (C 6 H 5 ) 3 COH s 15.21 0.302 69 700 Cydohexanol C 6H 11OH l -85.47 0.476 -34 300 Ethylene Glycol CH 2 OHCH 2 OH l -1749.37 0.643 -77 120 Glycerol CH 2OHCHOHCH 2OH l -1728.23 0.540 -113 600 Phenol C 6 H 5 OH s -407.72 0.362 -11 000 Thiophenol C 6 H 5 SH s 0.477 Pyrocatechol C 6 H 4 (OH) 2 s -795.31 0.326 -51 400 Resorcinol C 6 H 4 (OH) 2 s -795.31 0.321 -53 200 Hydroquinone C 6 H 4 (OH) 2 s -795.31 0.304 -52 700 Aniline C 6 H 5 NH 2 l 78.82 0.492 35 400 Table 1.3: Formation enthalpies (cal/gr), (cal/mol). Alcohols. entropies (cal gr −1 K −1 ) and free energies Free Energy Gibbs free energy which can be written in the form g = h − T s, (1.19) g = g 0 + R g T ln ( p p 0 ) , (1.20) where g 0 = h − T s 0 (1.21) is the free energy at standard pressure. gas The free energy G = Mg per mole is also called chemical potential µ of the ( ) p µ = G = G 0 + RT ln , (1.22) p 0
10 CHAPTER 1. THERMOCHEMISTRY where G 0 = H − T S 0 = µ 0 , (1.23) and H, S 0 and µ 0 are, respectively, the molar enthalpy and entropy of the gas and its chemical potential at standard pressure. Hydrocarbons Substance Formula State h 0 s 0 ∆G 0 Methane CH 4 g -1 115.14 2.774 -12 140 Ethane C 2 H 6 g -673.01 1.824 -7 860 Propane C 3 H 8 g -562.89 1.463 -56 14 n-Butane C 4 H 10 g -512.94 1.275 -3 754 n-Pentane C 5H 12 g -485.13 1.154 -1 960 Ethylene C 2 H 4 g 445.49 1.87 1 6282 Propilene C 3 H 6 g 115.95 1.516 14 990 1-Butene C 4H 8 g 4.99 1.31 17 217 cis-2-Butene - g -24.28 1.282 16 046 trans-2-Butene - g -42.87 1.263 15 315 Isobutene - g -59.59 1.251 14 582 1-Pentene C 5H 10 g -71.30 1.185 18 787 Acetylene C 2 H 2 g 2081.5 1.843 50 000 Methylacetylene C 3 H 4 g 1106.26 1.48 46 313 Cyclopentane C 5H 10 l -360.76 0.696 8 700 Methylcyclopentane C 6 H 12 l -392.96 0.704 7 530 Cyclohexane C 6 H 12 l -443.7 0.58 6 370 Methylcyclohexane C 7H 14 l -462.92 0.604 4 860 Benzene C 6 H 6 g 253.75 0.824 30 989 Benzene C 6 H 6 l 150.02 0.529 29 756 Toluene C 7H 8 g 129.7 0.829 29 228 Toluene C 7H 8 l 31.12 0.57 27 282 o-Xylene C 8 H 10 g 42.77 0.794 29 177 o-Xylene C 8 H 10 l -55.02 0.555 26 370 m-Xylene - g 38.81 0.805 28 405 m-Xylene - g -57.22 0.568 25 730 p-Xylene - g 40.41 0.793 28 952 p-Xylene - l -54.99 0.557 26 310 Durene C 6 H 2 (CH 3 ) 4 s -242.68 0.437 19 000 Cumene C 6 H 5 CH(CH 3 ) 2 l -81.94 0.556 20 700 Mesitylene C 6 H 3 (CH 3 ) 3 l -126.34 0.544 24 830 Diphenyl C 6H 5-C 6H 5 s 135.34 0.319 57 400 Diphenylmethane C 6 H 5 -CH 2 -C 6 H 5 s 117.22 0.340 63 600 Triphenylmethane (C 6 H 5 ) 3 s 170.92 0.305 101 400 Naphthalene C 10H 8 s 124.53 0.311 45 200 Anthracene C 14 H 10 s 154.86 0.278 64 800 Phenanthrene C 14 H 10 s 129.62 0.284 60 000 Table 1.4: Formation enthalpies (cal/gr), (cal/mol). Hydrocarbons. entropies (cal gr −1 K −1 ) and free energies
Page 2 and 3: Aerothermochemistry Gregorio Millá
Page 4 and 5: PRESENTACIÓN Amable Liñán Es un
Page 6 and 7: que no cambiaron los resultados, y
Page 8: INSTITUTO NACIONAL DE TÉCNICA AERO
Page 11 and 12: aim to become acquainted with Aerot
Page 13 and 14: Tarifa, Manuel de Sendagorta and Ig
Page 15 and 16: 3.4 Energy equation . . . . . . . .
Page 17 and 18: 8.4 Quenching . . . . . . . . . . .
Page 20 and 21: Chapter 1 Thermochemistry 1.1 Intro
Page 22 and 23: 1.1. INTRODUCTION 3 GAS ε/k (K) σ
Page 24 and 25: 1.1. INTRODUCTION 5 14 12 10 N 2 CH
Page 26 and 27: 1.2. THERMODYNAMIC FUNCTIONS OF AN
Page 30 and 31: 1.3. MIXTURE OF GASES 11 Helmholtz
Page 32 and 33: 1.3. MIXTURE OF GASES 13 is the par
Page 34 and 35: 1.3. MIXTURE OF GASES 15 Entropy Si
Page 36 and 37: 1.4. CALCULATION OF THE THERMODYNAM
Page 38 and 39: 1.4. CALCULATION OF THE THERMODYNAM
Page 40 and 41: 1.5. CHEMICAL REACTIONS IN A MIXTUR
Page 42 and 43: 1.6. CHEMICAL EQUILIBRIUM 23 Since
Page 44 and 45: ∆G 0 j = ∑ i 1.7. CASE OF A MIX
Page 46 and 47: 1.7. CASE OF A MIXTURE OF IDEAL GAS
Page 48 and 49: 1.8. CHEMICAL KINETICS 29 1.8 Chemi
Page 50 and 51: 1.8. CHEMICAL KINETICS 31 Mechanics
Page 52 and 53: 1.8. CHEMICAL KINETICS 33 This stru
Page 54 and 55: 1.8. CHEMICAL KINETICS 35 [3] Hirsc
Page 56 and 57: Chapter 2 Transport phenomena in ga
Page 58 and 59: 2.2. DIFFUSION 39 Hereinafter, nota
Page 60 and 61: 2.2. DIFFUSION 41 where r is the di
Page 62 and 63: 2.2. DIFFUSION 43 T ∗ Ω (1,1)∗
Page 64 and 65: 2.2. DIFFUSION 45 Gas Pair σ 12 (
Page 66 and 67: 2.2. DIFFUSION 47 coefficients. 14
Page 68 and 69: 2.3. VISCOSITIES 49 2.3 Viscosities
Page 70 and 71: 2.3. VISCOSITIES 51 Here µ and µ
Page 72 and 73: 2.3. VISCOSITIES 53 Its value depen
Page 74 and 75: 2.4. THERMAL CONDUCTIVITY 55 2000 1
Page 76 and 77: 2.4. THERMAL CONDUCTIVITY 57 4000 3
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Chapter 3 General equations 3.1 Int
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3.2. EQUATION OF CONTINUITY 61 The
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3.2. EQUATION OF CONTINUITY 63 A i
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3.4. ENERGY EQUATION 65 where the s
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3.4. ENERGY EQUATION 67 The energy
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3.5. GENERAL EQUATIONS 69 obtained
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3.6. ENTROPY VARIATION 71 Taking in
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3.7. ONE-DIMENSIONAL MOTIONS 73 red
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3.8. STATIONARY, ONE-DIMENSIONAL MO
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3.9. THE CASE OF ONLY TWO CHEMICAL
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3.10. STATIONARY, ONE-DIMENSIONAL M
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3.11. APPENDIX: NOTATION AND REPERT
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3.11. APPENDIX: NOTATION AND REPERT
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Chapter 4 Combustion Waves 4.1 Deto
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4.2. KINDS OF DETONATIONS AND DEFLA
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4.2. KINDS OF DETONATIONS AND DEFLA
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4.3. VELOCITY OF THE BURNT GASES 95
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4.3. VELOCITY OF THE BURNT GASES 97
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4.4. PROPAGATION VELOCITY 99 p H’
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4.5. APPLICATIONS 101 By substituti
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4.7. INDETERMINACY OF THE SOLUTION
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Chapter 5 Structure of the combusti
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5.2. WAVE EQUATIONS 107 of diffusio
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5.2. WAVE EQUATIONS 109 2) Burnt ga
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5.4. LIMITING FORM OF THE WAVE EQUA
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5.4. LIMITING FORM OF THE WAVE EQUA
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5.5. DETONATIONS 115 Of these two v
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5.5. DETONATIONS 117 waves. Such th
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5.5. DETONATIONS 119 This relation
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5.5. DETONATIONS 121 curves, repres
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5.6. DEFLAGRATIONS 123 mum temperat
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5.6. DEFLAGRATIONS 125 8 7 v/v 1 =T
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5.7. TRANSITION FROM DEFLAGRATION T
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5.7. TRANSITION FROM DEFLAGRATION T
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Chapter 6 Laminar flames 6.1 Introd
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6.1. INTRODUCTION 133 papers presen
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6.3. BOUNDARY CONDITIONS 135 c) Dif
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6.4. MODIFICATION OF THE CONDITIONS
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6.4. MODIFICATION OF THE CONDITIONS
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6.6. EXAMPLE 141 generally impossib
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6.6. EXAMPLE 143 Two more relations
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6.7. REACTION VELOCITY 145 1.0 0.8
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6.8. FLAME EQUATIONS 147 6.8 Flame
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6.9. SOLUTION OF THE FLAME EQUATION
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6.10. STRUCTURE OF THE COMBUSTION W
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6.11. IGNITION TEMPERATURE 161 6.11
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6.12. GENERAL EQUATIONS FOR THE COM
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6.13. OZONE DECOMPOSITION FLAME 169
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6.14. HYDRAZINE DECOMPOSITION FLAME
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6.15. FLAME PROPAGATION IN HYDROGEN
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Chapter 7 Turbulent flames 7.1 Intr
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7.1. INTRODUCTION 209 300 250 TURBU
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7.2. TURBULENT COMBUSTION THEORIES
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7.4. COMPARISON WITH EXPERIMENTAL R
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Chapter 8 Ignition, flammability an
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8.2. IGNITION 223 comparison betwee
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8.3. FLAMMABILITY LIMITS 225 The pr
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8.4. QUENCHING 227 8.4 Quenching So
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8.4. QUENCHING 229 [19] Simon, D. M
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Chapter 9 Flows with combustion wav
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9.2. CONDITIONS THAT MUST BE SATISF
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9.3. NORMAL FLAME FRONT 235 9.3 Nor
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9.4. INCLINED FLAME FRONT 237 60 50
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9.5. ENTROPY JUMP ACROSS THE FLAME
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9.5. ENTROPY JUMP ACROSS THE FLAME
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9.6. VORTICITY ACROSS THE FLAME 243
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Chapter 10 Aerothermodynamic field
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10.1. INTRODUCTION 247 form numeric
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10.1. INTRODUCTION 249 ∆ P /∆ P
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10.2. TSIEN METHOD 251 As aforesaid
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10.2. TSIEN METHOD 253 1.0 λ=6.0 M
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10.3. METHOD OF FABRI-SIESTRUNCK-FO
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10.3. METHOD OF FABRI-SIESTRUNCK-FO
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10.5. CHAMBER WITH SLOWLY VARYING C
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Chapter 11 Similarity in combustion
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11.2. DIMENSIONLESS PARAMETERS OF A
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11.2. DIMENSIONLESS PARAMETERS OF A
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11.3. SCALING OF ROCKETS 267 Furthe
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11.3. SCALING OF ROCKETS 269 From h
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11.4. SCALING OF ROCKETS FOR NON-ST
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11.4. SCALING OF ROCKETS FOR NON-ST
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11.5. FLAME STABILIZATION 275 Flame
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11.5. FLAME STABILIZATION 277 Flame
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11.5. FLAME STABILIZATION 279 which
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Chapter 12 Diffusion flames 12.1 In
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12.1. INTRODUCTION 283 In fact, oth
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12.1. INTRODUCTION 285 which preced
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12.1. INTRODUCTION 287 remains appr
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12.2. GENERAL EQUATIONS FOR LAMINAR
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12.3. BOUNDARY CONDITIONS ON THE FL
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12.4. SIMPLIFIED EQUATIONS 293 As f
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12.4. SIMPLIFIED EQUATIONS 295 whil
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12.5. SOLUTIONS OF THE SIMPLIFIED S
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12.5. SOLUTIONS OF THE SIMPLIFIED S
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Chapter 13 Combustion of liquid fue
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13.2. ATOMIZATION 303 lem has been
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13.4. COMBUSTION 305 solution corre
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13.5. NOTATION 307 2) The phenomeno
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13.6. CONTINUITY EQUATIONS 309 Chem
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13.7. ENERGY EQUATION 311 The value
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13.8. DIFFUSION EQUATIONS 313 13.8
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13.9. COMBUSTION VELOCITY OF THE DR
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13.10. INTEGRATION OF THE EQUATIONS
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13.11. NUMERICAL APPLICATION 319 wh
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13.11. NUMERICAL APPLICATION 321 10
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13.12. COMPARISON WITH EXPERIMENTAL
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13.14. COMBUSTION OF FUEL SPRAYS 32
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13.15. DROPLET EVAPORATION 327 4 0.
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13.15. DROPLET EVAPORATION 329 1 0.
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13.16. APPENDIX: APPLICATION OF PRO
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