Appendix A Table and Graphs Compilations

Transcription

1 Appendix A Table and Graphs Compilations Our objective here is to study the temperature, and thus the flow of heat, in a graphlike, physical object. The continuous eigenvalue problem that arises is related to a discrete graph eigenvalue problem, and the interplay between continuous and discrete illuminates both. In particular, the eigenvalues and eigenvectors have a specific physical interpretation. Springer International Publishing AG 2017 B. Zohuri, Thermal-Hydraulic Analysis of Nuclear Reactors, DOI /

2 748 Appendix A: Table and Graphs Compilations A.1 Conduction Graphs Few heat conduction graphs are shown in this appendix as follows; Temperature, C Gold Tin Silver Lead Magnesium Zinc Copper Aluminium Liquid sodium Wrought iron (c < 0.5 persent) Iron (pure) 100 Thermal conductivity, Btu/h. ft. F F high-alumina brick SAE 10 petroleum lubricating oil Mercury ZrO 2 (dense) Water (liquid) Kerosene Rock wool (loose. 10 lb/ft 3 ) NH 3 (gas) Type 430 stainless steel Air(gas) UO 2 (dense) 3000 F high-alumina brick Asbestos (36 lb/ft 2 ) Argon (gas) Thermal conductivity, w/m. C Freon-11 (gas) Steam (H 2 O vapor) Temperature, F Fig. A.1 Thermal conductivity of typical engineering materials [1]

3 Appendix A: Table and Graphs Compilations 749 Temperature, C , , Thermal conductivity, Btu/h ft F Gold Copper Aluminum Silver Tungsten Thermal conductivity, W/m C 200 Platinum Iron Temperature, F 200 Fig. A.2 Thermal conductivity of metals at low temperatures

4 750 Appendix A: Table and Graphs Compilations Heat transfer coefficient, Btu/h ft 2 F Air at 200 F (93.3 C) under turbulent flow in a tube ID = 0.1 in = 0.5 in = 1.0 in Flow rate, kg/m 2 s Water at 200 F (93.3 C) under turbulent flow in a tube ID = 0.1 in = 0.5 in = 1.0 in , Heat transfer coefficient, W/m 2 C Flow rate, lb/ft 2 s Fig. A.3 Heat transfer coefficient for turbulent flow of water and air at 200 F in tubes

5 Appendix A: Table and Graphs Compilations 751 Fig. A.4 Correction factor for Fig. A.3 to illustrate the variation of h with the type of fluid and temperature 20 0 Temperature, C 100 H He CH Air Gasoline Freon 114 SAE-10 Water CO 2 Argon Dowtherm, A 0.02 Liquids Gases Temperature, F 400

6 Appendix B Physical Property Tables In this appendix, you will find the physical properties of gases at atmospheric pressure and of saturated liquids. More extensive tabulation of physical property data is available in reference books such as: Perry s Chemical Engineers Handbook, edited by R. H. Perry and D. W. Green, McGraw-Hill, Inc., New York, NY. CRC Handbook of Chemistry and Physics, CRC Press, Boca Raton, FL. Lange s Handbook of Chemistry, J. A. Dean, McGraw-Hill, Inc., New York, NY. Chemical Properties Handbook, C. L. Yaws, (1999) McGraw-Hill, Inc., New York, NY. Physical and Thermodynamic Properties of Pure Chemicals: Evaluated Process Design Data, T. E. Daubert et al., (1999), Taylor & Francis, Philadelphia, PA. NIST Chemistry Webbook, edited by P. J. Linstrom and W. G. Mallard, (2005) National Institute of Standards and Technology, Gaithersburg, MD. ( webbook.nist.gov.) The Knovel scientific and engineering online database ( provides searchable access to many reference books but requires a subscription. The data in this appendix were compiled from these and other sources. For critical applications, you should consult one or more of the original sources. Springer International Publishing AG 2017 B. Zohuri, Thermal-Hydraulic Analysis of Nuclear Reactors, DOI /

7 754 Appendix B: Physical Property Tables B:1 Temperature and Enthalpy of Phase Change Table B.1 Atomic mass and number of the first 100 elements Element Symbol Atomic number Atomic mass Element Symbol Atomic number Atomic mass Hydrogen H Oxygen O Helium He Fluorine F Lithium Li Neon Ne Beryllium Be Sodium Na Boron B Magnesium Mg Carbon C Aluminum Al Nitrogen N Silicon Si Phosphorous P Cadmium Cd Sulfur S Indium In Chlorine Cl Tin Sn Argon Ar Antimony Sb Potassium K Tellurium Te Calcium Ca Iodine I Scandium Sc Xenon Xe Titanium Ti Cesium Cs Vanadium V Barium Ba Chromium Cr Lanthanum La Manganese Mn Cerium Ce Iron Fe Praseodymium Pr Cobalt Co Neodymium Nd Nickel Ni Promethium Pm 61 (145) Copper Cu Samarium Sm Zinc Zn Europium Eu Gallium Ga Gadolinium Gd

8 Appendix B: Physical Property Tables 755 Germanium Ge Terbium Tb Arsenic As Dysprosium Dy Selenium Se Holmium Ho Bromine Br Erbium Er Krypton Kr Thulium Tm Rubidium Rb Ytterbium Yb Strontium Sr Lutetium Lu Yttrium Y Hafnium Hf Zirconium Zr Tantalum Ta Niobium Nb Wolfram W Molybdenum Mo Rhenium Re Technetium Tc 43 (98) Osmium Os Ruthenium Ru Iridium Ir Rhodium Rh Platinum Pt Palladium Pd Gold Au Silver Ag Mercury Hg Thallium Tl Protactinium Pa Lead Pb Uranium U Bismuth Bi Neptunium Np Polonium Po 84 (209) Plutonium Pu 94 (244) Astatine At 85 (210) Americium Am 95 (243) Radon Rn 86 (222) Curium Cm 96 (247) Francium Fr 87 (223) Berkelium Bk 97 (247) Radium Ra Californium Cf 98 (251) Actinium Ac Einsteinium Es 99 (252) Thorium Th Fermium Fm 100 (257) Mass numbers in parentheses are those for the most stable or best known isotope Source: CRC Handbook of Chemistry and Physics, 70th edition; Perry s Chemical Engineers Handbook 6th ed

9 756 Appendix B: Physical Property Tables B.2 Nonideal Gas Model Equation and Critical Properties One way to write the ideal gas law is PbV RT ¼ 1 ðb:1þ where P ¼ pressure, T ¼ temperature, R ¼ ideal gas constant, and bv ¼ specific molar volume (volume per mole). The ideal gas law is a very useful model equation for calculating specific volumes (or, equivalently, densities) of gases at low to moderate pressures. For accurate calculations at higher pressures, either experimental data or more complicated model equations are required. Many such equations have been proposed; Perry s Chemical Engineers Handbook or any chemical engineering thermodynamics textbook is a good source of information. Although differing in detail and complexity, these equations share the common feature of calculating a value for the compressibility factor Z, where Z ¼ P bv RT ðb:2þ For an ideal gas, Z ¼ 1. Most of the time, for real gases Z < 1. (You will typically see values of roughly 0.7 < Z < 1.) One of the most widely used model equations for predicting specific volumes of real gases is the Redlich Kwong equation: Z 3 Z 2 þ A B 2 B Z AB ¼ 0 ðb:3þ where A ¼ ap R 2 T 2:5 a ¼ Ω ar 2 T 2:5 c B ¼ bp RT P c b ¼ Ω brt c P c 1 Ω a ¼ ffiffi 9 3p 2 1 3p ffiffiffi 2 1 Ω b ¼ 3 Knowing just the critical temperature T and critical pressure P c for the compound of interest is sufficient to calculate Z (and hence specific volume or density) for that gas at a given T and P. Since the Redlich Kwong equation is a cubic equation, there are three roots. The largest real root is the correct value of Z for a gas. Critical temperatures and pressures for selected compounds are in Table B.2. Convert T c to an absolute temperature scale before using in the Redlich Kwong equation.

10 Appendix B: Physical Property Tables 757 Table B.2 Critical temperature T c and critical pressure P c of selected compounds Compound Formula Tc, C Pc, atm Compound Formula Tc, C Pc, atm Acetaldehyde C 2 H 4 O Carbon disulfide CS Acetic acid C 2 H 4 O Carbon monoxide CO Acetic anhydride C 4 H 6 O Chlorine Cl Acetone C 3 H 6 O Diethylamine (C 2 H 5 ) 2 NH Acetonitrile C 2 H 3 N Dimethylamine (CH 3 ) 2 NH Acetylene C 2 H Ethane C 2 H Air Ethyl acetate CH 3 COOC 2 H Ammonia NH Ethanol C 2 H 5 OH Argon Ar Ethylene C 2 H Benzene C 6 H Ethylene oxide C 2 H 4 O Bromine Br Fluorine F Butadiene, 1,3 C 4 H Helium He n-butane C 4 H Heptane C 7 H Carbon dioxide CO Hydrazine N 2 H Hydrogen H n-pentane C5H Hydrogen chloride HCl Phenol C 6 H 5 OH Hydrogen cyanide HCN Phosgene COCl Hydrogen sulfide H 2 S n-propane C 3 H Isobutane C4H Propionic acid C2H5COOH Isopentane C 5 H n-propanol C 3 H 7 OH Mercury Hg >1550 >200 Propylene C 3 H Methyl acetate CH 3 COOCH Pyridine C 6 H 5 N Methanol CH 3 OH Radon Rn Methyl ethyl ether CH 3 OC 2 H Sodium Na Neon Ne Silicon tetrafluoride SiF (continued)

11 758 Appendix B: Physical Property Tables Table B.2 (continued) Compound Formula Tc, C Pc, atm Compound Formula Tc, C Pc, atm Nitric oxide NO Sulfur dioxide SO Nitrogen N Sulfur trioxide SO Nitrogen tetroxide N2O Toluene C6H5CH Nitrous oxide N 2 O Triethylamine (C 2 H 5 ) 3 N n-octane C 8 H Trimethylamine (CH 3 ) 3 N Oxygen O Water H 2 O To convert to T(K), add To convert to P (bar), divide by Source: Perry s Chemical Engineers Handbook, 6th ed

12 Appendix B: Physical Property Tables 759 B.3 Gibbs Energy, Enthalpy of Formation, and Enthalpy of Combustion The standard Gibbs energy of formation is useful for calculating the Gibbs energy change with reaction at 298 K, as in following equation (Eq. B.4): Δ b G o r ¼ X v i Δ b G o i, f ðb:4þ To a good approximation, we can calculate the Gibbs energy change at any temperature T by using the van t Hoff expression, as in following equation (Eq. B.5): " # ln K a, r ¼ Δ bg r o RT ¼1 ΔbG r o Δ bh r o Δ bh r o ðb:5þ R 298 T where or ΔbH o r ¼ X v i ΔbH o i, f ΔbH o r ¼ X v i ΔbH o i,c Table B.3 Standard Gibbs energy of formation ΔbG f o, enthalpy of formation Δ bh f o, and enthalpy of combustion at 298 K Compound Formula ΔbG f o kj=gmol Δ bh f o kj=gmol Δ bh c o kj=gmol Acetaldehyde (g) C 2 H 4 O Acetic acid (g) C 2 H 4 O (l) Acetic anhydride (g) C 4 H 6 O Acetone (g) C 3 H 6 O (l) Acetonitrile (g) C 2 H 3 N Acetylene (g) C 2 H Adipic acid (l) C 6 H 10 O Ammonia (g) NH Ammonium nitrate (s) N 2 H 5 NO (aq) Argon (g) Ar Benzene(g) C 6 H Butadiene, 1,3 (g) C 4 H (continued)

13 760 Appendix B: Physical Property Tables Table B.3 (continued) Compound Formula ΔbG f o kj=gmol Δ bh f o kj=gmol Δ bh c o kj=gmol n-butane (g) C 4 H Calcium carbonate (s) CaCO Calcium chloride (s) CaCl Carbon dioxide (g) CO Carbon disulfide (g) CS Carbon monoxide (g) CO Carbonyl sulfide (g) COS Chlorine (g) Cl Chlorobenzene (l) C 6 H 5 Cl Chloroform (g) CHCl Cyclohexane (g) C 6 H (l) Diethylamine (g) (C 2 H 5 ) 2 NH Diethyl ether (g) (C 2 H 5 ) 2 O (l) Dimethylamine (g) (CH 3 ) 2 NH Dimethyl carbonate (l) C 3 H 6 O Dimethyl ether (g) (CH 3 ) 2 O Ethane (g) C 2 H Ethanol (g) C 2 H 5 OH (l) Ethyl acetate (g) CH 3 COOC 2 H (l) Ethylamine (g) C 2 H 5 NH Ethylbenzene (g) C 8 H (l) Ethylene (g) C 2 Η Ethylene glycol (g) C 2 HO (l) Ethylene oxide (g) C 2 H 4 O Formaldehyde (g) CH 2 O Formic acid (g) CH 2 O Gallium nitride (s) GaN Glycerol (glycerin) (g) C 3 H 8 O (l) n-heptane (g) C 7 H (l) Hexamethylenediamine C 6 H 16 N (g) n-hexane (g) C 6 H (l) Hydrazine (g) N 2 H (continued)

14 Appendix B: Physical Property Tables 761 Table B.3 (continued) Compound Formula ΔbG f o kj=gmol Δ bh f o kj=gmol Δ bh c o kj=gmol (l) Hydrogen (g) H Hydrogen chloride (g) HCl Hydrogen peroxide (g) H 2 O (l) Hydrogen cyanide (g) HCN Hydrogen sulfide (g) H 2 S Iron oxide (ferrous) (s) FeO (ferric, hematite) (s) Fe 2 O (magnetite) (s) Fe 3 O Isobutane (g) C 4 H Isobutene (g) C 4 H Isopentane (g) C 5 H Magnesium chloride (s) MgCl Methane (g) CH Methyl acetate (g) CH 3 COOCH Methanol (g) CH 3 OH (l) Methyl ethyl ether CH 3 OC 2 H Naphthalene (g) C 8 H Nitric acid (g) HNO (l) Nitric oxide (g) NO Nitroglycerin C 3 H 5 (NO 3 ) Nitrogen (g) N Nitrogen dioxide (g) NO Nitrogen tetroxide (g) N 2 O Nitrous oxide (g) N 2 O n-octane (g) C 8 H (l) Oxygen (g) O n-pentane (g) C 5 H (l) Phenol (g) C 6 H 5 OH (l) Phosgene (g) COCl n-propane (g) C 3 H Propionic acid (g) C 2 H 5 COOH (l) n-propanol (g) C 3 H 7 OH (l) Propylene (g) C 3 H (continued)

15 762 Appendix B: Physical Property Tables Table B.3 (continued) Compound Formula ΔbG f o kj=gmol Δ bh f o kj=gmol Δ bh c o kj=gmol Silicon tetrachloride (l) SiCl Silicon dioxide (c, SiO quartz) Sodium borohydride (aq) NaBH Sodium carbonate (c) Na 2 CO Sodium chloride (c) NaCl Sodium cyanide (c) NaCN 94.0 Sodium hydroxide (s) NaOH (aq) Sodium metaborate (aq) NaBO Styrene C 8 H Sulfur dioxide (g) SO Sulfur trioxide (g) so Sulfuric acid (l) H 2 SO (aq) Toluene (g) C 6 H 5 CH (l) Triethylamine (g) (C 2 H 5 ) 3 N Trimethylamine (CH 3 ) 3 N Trinitrotoluene (g) C 7 H 5 (NO 2 ) (s) 65.6 Urea (g) (NH 2 ) 2 CO (l) (s) Vinyl chloride (g) C 2 H 3 Cl Water (g) H 2 O (l) o-xylene (g) C 8 H (l) m-xylene (g) C 8 H (l) p-xylene (g) C 8 H (l) ΔHc o is the enthalpy change associated with combustion of the compound in the gas phase, with CO 2 (g),h 2 O (g),cl 2 (g), N 2 (g), and SO 2 (g) as products. With H 2 O (l) as product, Δ bh c o decreases (becomes more negative) by 44.0n kj/gmol, where n is the number of moles of H 2 O. ΔH c is sometimes called the lower heating value with water vapor and the higher heating value with liquid water as the product Source: Compiled from data in Perry s Chemical Engineers Handbook, 6th and 7th eds., Lange s Handbook of Chemistry, 14th ed., and NIST Chemistry webbook

16 Appendix B: Physical Property Tables 763 B.4 Antoine Equation Constants The Antoine equation is given as: log 10 P sat ðmmhg B Þ ¼ A Tð CÞþC ðb:6þ This is a useful equation for modeling saturation pressures of liquids and solids. The constants should not be used outside the indicated temperature range. Table B.4 Antoine equation constants for selected compounds Compound Formula Range, C A B C Acetaldehyde CH 3 CHO 45 to Acetic acid CH 3 COOH Acetic anhydride C 4 H 6 O Acetone CH 3 COCH Acetonitrile CH 3 CN Acrylonitrile C 3 H 3 N 20 to Ammonia NH 3 83 to Benzene C 6 H to Benzoic acid C 6 H 5 COOH 96 to Bromine Br n-butanol C 4 H 9 OH + 15 to Butadiene, 1,3 C 4 H 6 58 to Carbon disulfide CS 2 3 to Chlorine Cl Chloroform CHCl 3 35 to Diethanolamine (C 2 H 5 O) 2 NH 194 to Diethylamine (C 2 H 5 ) 2 NH 31 to Dimethylamine (CH 3 ) 2 NH 72 to Ethanol C 2 H 5 OH 2 to Ethanolamine C 2 H 7 ON 65 to Ethyl acetate CH 3 COOC 2 H 5 15 to Ethylamine C 2 H 5 NH 2 20 to Ethylbenzene C 8 H to Ethylene glycol C 2 H 6 O 2 50 to Ethylene oxide C 2 H 4 O 49 to Formic acid CH 2 O 2 37 to Glycerol C 3 H 8 O to n-heptane C 7 H 16 2 to n-hexane C 6 H to Hydrogen cyanide HCN 16 to Hydrogen peroxide H 2 O Isopentane C 5 H (continued)

17 764 Appendix B: Physical Property Tables Table B.4 (continued) Compound Formula Range, C A B C Isopropanol C 3 H 7 OH 0 to Lactic acid C 3 H 6 O Methanol CH 3 OH 14 to to Methyl acetate CH 3 COOCH 3 1 to Methyl ethyl ketone CH 3 COC 2 H Naphthalene (s) C 10 H 8 86 to (l) 125 to Nitrogen N n-octane C 8 H to Oxygen O n-pentane C 5 H to Phosgene COCl 2 68 to Phenol C 6 H 5 OH 107 to n-propanol C 3 H 7 ΟΗ 2 to Propionic acid C 2 H 5 COOH 56 to Silicon tetrachloride SiCl 4 0 to Styrene C 8 H 8 32 to Tetramethyl lead C 4 H 12 Pb 0 to Toluene C 7 H 8 6 to Water H 2 O 0 to to n-xylene C 8 H to m-xylene C 8 H to p-xylene C 8 H to Source: Lange s Handbook of Chemistry, 14th ed and NIST Chemistry Webbook B.5 Phase Equilibrium Data Table B.5 Henry s law constant (atm), H i ¼ y i P x i ¼ p i x i, for gas dissolved in water 0 C 10 C 20 C 30 C 40 C 50 C He 129, , , , , ,000 H 2 57,900 63,600 68,300 72,900 75,100 76,500 N 2 52,900 66,800 80,400 92, , ,000 CO 35,200 44,200 53,600 62,000 69,600 76,100 O 2 25,500 32,700 40,100 47,500 53,500 58,800 CH 4 22,400 29,700 37,600 44,900 52,000 57,700 C 2 H 6 12,600 18,900 26,300 34,200 42,300 50,000 C 2 H ,200 12,700 CO H 2 S Adapted from Hines and Maddox. Mass Transfer Fundamentals and Applications, 1985

18 Appendix B: Physical Property Tables 765 Table B.6 Partial pressures of SO 2 in equilibrium with dissolved SO 2 in water Partial pressure of SO 2, p so2, mmhg Grams SO 2 per 100 g water 10 C 20 C 30 C 40 C 50 C 60 C 70 C 80 C 90 C 100 C Source: Perry s Chemical Engineers Handbook, 6th ed Table B.7 Partial pressures of NH 3 in equilibrium with dissolved NH 3 in water Grams NH 3 per 100 g solution 0 C 10 C 21 C 32 C 43 C 54 C 65.5 C 77 C 88 C Source: Adapted from data in Perry s Chemical Engineers Handbook, 6th ed

19 766 Appendix B: Physical Property Tables Table B.8 Solubility of salts in water Compound Formula 0 C 10 C 20 C 30 C 40 C 50 C 60 C 70 C 80 C 90 C 100 C Calcium bicarbonate Ca(HCO 3 ) Magnesium chloride MgCl 2 6H 2 O Potassium nitrate KNO Potassium sulfate K 2 SO Sodium chloride NaCl Sodium sulfate Na2SO4 10H2O Na 2 SO 4 H 2 O Na 2 SO Data are listed as gram of anhydrous substance per 100 g water, in a saturated liquid solution. The formula shows the solid phase (hydrated or anhydrous) that is in equilibrium with the saturated solution Source: Perry s Chemical Engineers Handbook, 6th ed

20 Appendix B: Physical Property Tables 767 Table B.9 Benzene naphthalene solid liquid equilibrium Mole fraction naphthalene in liquid phase, x n Temperature, C Solid phase Benzene Benzene Benzene Benzene Benzene Naphthalene Naphthalene Naphthalene Naphthalene Naphthalene Naphthalene Naphthalene Naphthalene Naphthalene Naphthalene Saturated liquid solution of benzene and naphthalene in equilibrium with a single-component solid phase (Calculated by assuming ideal solution behavior and using melting points and enthalpies of melting of pure components) Table B.10 m-xylene p-xylene solid liquid equilibrium Mole fraction p-xylene in liquid phase, x p Temperature, C Solid phase m-xylene m-xylene m-xylene p-xylene p-xylene p-xylene p-xylene p-xylene p-xylene p-xylene p-xylene Saturated liquid solution of m-xylene and p-xylene in equilibrium with a single-component solid phase (Calculated by assuming ideal solution behavior and using melting points and enthalpies of melting of pure components)

21 768 Appendix B: Physical Property Tables Table B.11 Ethanol-water vapor liquid equilibrium at 1 atm Temperature, C Mole fraction ethanol in liquid phase, x e Source: Perry s Chemical Engineers Handbook, 6th ed Molt fraction ethanol in vapor phase, y e Table B.12 Methanol-benzene vapor liquid equilibrium at 1 atm Temperature, C Mole fraction methanol in liquid phase, x m Source: Perry s Chemical Engineers Handbook, 6th ed Mole fraction methanol in vapor phase, y m

22 Appendix B: Physical Property Tables 769 Table B.13 Water-acetic acid-methyl isobutyl ketone liquid liquid equilibrium, at 25 C Weight % in raffinate Weight % in extract Water Acetic acid MIBK Water Acetic acid MIBK Each row shows the compositions of the raffinate and extract phase at equilibrium Source: Perry s Chemical Engineers Handbook, 6th ed Table B.14 Ethylbenzene-styrene-ethylene glycol liquid liquid equilibrium, at 25 C Weight % in raffinate Weight % in extract Ethylbenzene Styrene Ethylene glycol Ethylbenzene Styrene Ethylene glycol Each row shows the compositions of the raffinate and extract phase at equilibrium Source: Perry s Chemical Engineers Handbook, 6th ed

23 770 Appendix B: Physical Property Tables Table B.15 Distribution coefficient, K D ¼ x A, phase II /x A,phase I, for solute a distributing between two immiscible liquids Solute A Solvent phase I Solvent phase II K D Acetic acid Water Methyl acetate Acetic acid Water Furfural (26.7 C) Acetic acid Water Heptadecanol Acetic acid Water Benzene Acetic acid Water 1-Butanol (26.7 C) Oleic acid Cottonseed oil Propane (85 C) Chlorine Water Carbon tetrachloride 5.0 Bromine Water Carbon tetrachloride 27 Iodine Water Carbon tetrachloride 55 Ammonia Water Carbon tetrachloride Diethylamine Water Chloroform 2.2 Dielhylamine Water Benzene 1.8 Dielhylamine Water Toluene 0.63 Dielhylamine Water Xylene 0.20 Ethanol Water Benzene Ethanol Water Heptadecanol Ethanol Water n-butanol 3.00 (20 C) Methyl ethyl ketone Water Gasoline Methyl ethyl ketone Water 2-Methyl furan 84.0 Penicillin F Water (ph 6.0) Amyl acetate 0.06 Penicillin F Water (ph 4.0) Amyl acetate 32 Data at 25 C unless otherwise noted. Reliable only at dilute solute concentrations Compiled from data in Perry s Chemical Engineers Handbook, 6th ed., Biochemical and Biotechnology Handbook, 1991, 2nd ed., and Process Synthesis, D.F. Rudd, G.J. Powers and J.J. Siiroia, 1973 B.6 Steam Table bh and bu are given in units of kj/kg, with the reference condition as the triple point of liquid water ( K, bar). bv is given in units of m 3 /kg. Source: E. W. Lemmon, M. O. McLinden and D. G. Friend, Thermophysical Properties of Fluid Systems in NIST Chemistry WebBook, NIST Standard Reference Database Number 69, Eds. P. J. Linstrom and W. G. Mallard, June 2005, National Institute of Standards and Technology, Gaithersburg MD, (

24 Appendix B: Physical Property Tables 771 Table B.16 Specific enthalpy bh, internal energy bu, and volume bv of H 2 O at several temperatures and pressures Ternperature ( C) P, bar (T sat, C) Sat d liquid Sat d vapor Hˆ (0.01) ^U bv Hˆ (45.806) ^U bv Hˆ (99.606) ^U bv Hˆ (151.83) ^U bv Hˆ (179.88) ^U bv Hˆ (212.38) ^U bv Hˆ (250.35) ^U bv Hˆ (continued)

25 772 Appendix B: Physical Property Tables Table B.16 (continued) Ternperature ( C) P, bar (T sat, C) Sat d liquid Sat d vapor (275.58) ^U bv Hˆ (311.00) ^U bv Hˆ (342.16) ^U bv Hˆ (365.75) ^U bv Hˆ (373.95) ^U bv

26 Appendix B: Physical Property Tables 773 Temperature ( C) P, bar (T sat, C) Sat d liquid Sat d vapor Hˆ (0.01) ^U bv Hˆ (45.806) ^U bv Hˆ (99.606) ^U bv Hˆ (151.83) ^U bv Hˆ (179.88) ^U bv Hˆ (212.38) ^U bv Hˆ (250.35) ^U bv Hˆ (275.58) ^U bv (continued)

27 774 Appendix B: Physical Property Tables Table B.16 (continued) Temperature ( C) P, bar (T sat, C) Sat d liquid Sat d vapor Hˆ (311.00) ^U bv Hˆ (342.16) ^U bv Hˆ (365.75) ^U bv Hˆ (373.95) ^U bv

28 Appendix B: Physical Property Tables 775 B:7 Heat Capacities Table B.17 Heat capacity C p of selected liquids and vapors Compound Formula Cp (approx.) A B C D Acetaldehyde (g) C 2 H 4 O 54.7 (l) Acetic acid (g) C 2 H 4 O e e 8 (l) Acetone (g) C 3 H 6 O e e 8 (l) Acetonitrile (g) C 2 H 3 N e e 9 Acetylene (g) C 2 H e e 8 Ammonia (g) NH e e 8 Argon (g) Ar Benzene (g) C6H e e 8 (l) e 4 Bromine (g) Br e e 9 Butadiene, 1,3(g) C 4 H e e 8 n-butane (g) C4H e e 9 Carbon dioxide (g) CO e e 8 Carbon disulfide (g) CS e e 8 Carbon monoxide (g) CO e e 8 Carbon tetrachloride (g) CCl e e 8 Chlorine (g) Cl e e 8 Chloroform (g) CHCl e e 8 (l) e 4 (continued)

29 776 Appendix B: Physical Property Tables Table B.17 (continued) Compound Formula Cp (approx.) A B C D Chlorobenzene (l) C 6 H 5 C e 4 Cyclohexane (l) C 6 H e 3 Diethylamine (g) (C2H5)2NH (l) Diethyl ether (g) (C 2 H 5 ) 2 O e e 9 Dimethylamine (g) (CH 3 ) 2 NH (l) Dimethyl ether (g) (CH 3 ) 2 O 65.6 (l) Ethane (g) C 2 H e e 9 (e) 68 Ethanol (g) C 2 H 5 OH e e 9 (l) Ethyl acetate (g) CH 3 COOC 2 H (l) Ethylbenzene (g) C 8 H e e 7 (l) Ethylene (g) C 2 H e 5 l.755e 8 Ethylene glycol (g) C 2 HO Ethylene oxide (g) C 2 H 4 O e e 8 Formaldehyde (g) CH 2 O 35.4 Glycerol (glycerin) (l) C 3 H 8 O n-heptane (g) C 7 H e e 8 (l) 212 n-hexane (g) C 6 H e e 8 (l) 189.1

30 Appendix B: Physical Property Tables 777 Hydrazine (g) N 2 H e e 8 (l) 98.9 Hydrogen (g) H e e 9 Hydrogen chloride (g) HCl e e 9 Hydrogen cyanide (g) HCN e e 8 Hydrogen sulfide (g) H 2 S e e 8 Isobutane (g) C 4 H e e 8 Isobutene (g) C 4 H e e 9 Isopentane (g) C 5 H e e 8 Isopropanol (g) C 3 H 7 OH e e 8 (l) 155 Lactic acid (g) C 3 H 6 O (l) 262 Methane (g) CH e e 8 Methyl acetate (l) CH 3 COOCH Methanol (g) CH 3 OH e e 8 (l) 81.2 Nitric oxide (g) NO e e e 9 Nitrogen (g) N e e e 8 Nitrogen dioxide (g) NO Nitrogen tetroxide (g) N 2 O (l) Nitrous oxide (g) N 2 O e e e 8 n-octane (g) C8H e e 8 (l) 255 Oxygen O e e 8 n-pentane (g) C 5 H e e 8 (l) (continued)

31 778 Appendix B: Physical Property Tables Table B.17 (continued) Compound Formula Cp (approx.) A B C D Phenol (g) C 6 H 5 OH Phosgene (g) COCl Potassium nitrate (l) KNO n-propane (g) C 3 H e e 8 n-propanol (g) C 3 H 7 OH e e 8 (l) e 3 Propylene (g) C3H e e 8 Silicon tetrachloride (l) SiCl Sodium nitrate (l) NaNO Styrene (g) C 8 H e e 8 (l) Sulfur (g) S (l) S 32 Sulfur dioxide (g) SO e e 8 Sulfur trioxide (g) SO e e 8 Toluene (g) C 6 H 5 CH e e 8 (l) e 4 Triethylamine (g) (C 2 H 5 ) 3 N Trimethylamine (g) (CH 3 ) 3 N 91.8 Water (g) H 2 O e e 9 (l) o-xylene (g) C 8 H e e 8 m-xylene (g) C 8 H e e 8 p-xylene (g) C8H e e 8 For approximate calculation, use the number in the column labeled C p (approx.), which is the heat capacity at 25 C. For more accurate calculations, use the polynomial expression Cp A + BT + CT 2 + DT 3,whereCp is in J/gmol K (or J/gmol C) and T is in K. To convert to cal/gmol K or to Btu/Ibmol F, multiply by Source: Compiled from data in Introductory Chemical Engineering Thermodynamics. J. P. Elliott and C. T. Lira, Prentice-Hall, 1999; Perry s Chemical Engineers Handbook, 6th ed.; and Lang s Handbook of Chemistry, 14th ed

32 Appendix B: Physical Property Tables 779 Table B.18 Heat capacity C p of selected solids Compound Formula C p, J/gmol K (with T in K) Benzoic acid C 6 H 5 COOH 147 Calcium carbonate CaCO T l.287e6/t 2 Carbon (graphite) C T 4.89e5/T 2 Glucose C 6 H 12 O (25 C) Gold Au T Iron oxide FeO T 3.188e5/T 2 Fe 2 O T l.77e6/t 2 Fe 3 O T 4.1e 6/T 2 Magnesium chloride MgCl T Naphthalene C 10 H T Phenol C 6 H 5 OH (20 C) Silicon Si T 4.225e5/T 2 Silicon dioxide (quartz) SiO T 101e6/T 2 Sodium chloride NaCl T Sucrose C 12 H 22 O (at 20 C) Titanium dioxide TiO T 1.75e5/T 2 Urea CH 4 N 2 O 80.3 (at 20 C) Source: Compiled from data in Perry s Chemical Engineers Handbook, 6th ed., and NIST Chemistry Webbook Table B.19 Heat capacity C p of miscellaneous materials Material C p, J/g K Cellulose 1.34 Clay 0.94 Coal Concrete 0.65 Diamond 0.61 Fireclay brick 1.25 (1500 C) Glass (pyrex) 0.8 Limestone 0.91 Rubber 1.74 Sand 0.8 Silk 1.38 Steel 0.50 Wood Wool 1.36 Source: Perry s Chemical Engineers Handbook, 6th ed

33 780 Appendix B: Physical Property Tables B.8 Temperature and Enthalpy of Phase Change Table B.20 Enthalpy of melting Δ bh m at the normal melting temperature T m and enthalpy of vaporization Δ bh v at the normal boiling temperature T b at 1 atm Compound Formula T m ( C) Δ bh m kj=gmol T b ( C) Δ bh v kj=gmol n-pentane C 5 H Phenol C 6 H 5 OH Phosgene COCl Propane C 3 H Propionic acid C 2 H 5 COOH n-propanol C 3 H 7 OH Propylene C 3 H Silicon Si Silicon SiCl tetrachloride Silicon dioxide SiO (quartz) Sodium Na 2 CO carbonate Sodium NaCl chloride Sodium cyanide NaCN Sodium NaOH hydroxide Sulfur S Sulfur dioxide SO Sulfur trioxide SO 3 17 Sulfuric acid H 2 SO Styrene C 8 H Toluene C 6 H 5 CH Triethylamine (C 2 H 5 ) 3 N Trimethylamine (CH 3 ) 3 N Trinitrotoluene C 7 H 5 N 3 O Explodes Urea CH 4 N 2 O Decomposes 87.9 (sublim.) Water H 2 O o-xylene C 8 H m-xylene C 8 H p-xylene C 8 H Source: Compiled from the data in Perry s Chemical Engineers Handbook, 6th ed., CRC Handbook of chemistry and Physics, 70th ed., Lang s Handbook of Chemistry, 14th ed

34 Appendix B: Physical Property Tables 781 B.9 Enthalpies of Solution and of Mixing Table B.21 Enthalpy of solution of organic solids dissolved in water, Δ bh solution, at infinite dilution and 25 C Compound Formula Δ bh soln kj/gmol solute Acetic acid C 2 H 4 O Citric acid C 6 H 8 O Lactose C 11 H 22 O 11 H 2 O Maleic acid C 4 H 4 O Menthol C 10 H 20 O 0 Phenol C 6 H 5 OH 10.9 Phthalic acid C 8 H 6 O Picric acid C 6 H 3 N 3 O Potassium citrate Sodium citrate(tri) Sucrose C 12 H 22 O Urea CH 4 N 2 O 15.1 Vanillin denotes heat evolved (exothermic), denotes heat absorbed (endothermic) Source: Compiled from data in Perry s Chemical Engineers Handbook Table B.22 Enthalpy of solution of inorganic solids dissolved in water, Δ bh soln, at indicated dilution and 18 C Compound Formula Dilution, gmol water per g substance Δ bh soln kj/gmol solute Aluminum chloride AlCl Ammonium chloride NH 4 Cl Ammonium sulfate (NH 4 ) 2 SO Calcium chloride CaCl Calcium chloride CaCl 2 H 2 O Ferric chloride FeCl Phosphoric acid H 3 PO Sodium bicarbonate NaHCO Sodium carbonate Na 2 CO Sodium carbonate Na 2 CO 3 H 2 O Sodium carbonate Na 2 CO 3 7H 2 O Sodium carbonate Na 2 CO 3 10H 2 O Sodium hydroxide NaOH denotes heat evolved (exothermic), + denotes heat absorbed (endothermic) Note: Δ bh soln is very sensitive to waters of hydration and to dilution factor Source: Compiled from data in Perry s Chemical Engineers Handbook

35 782 Appendix B: Physical Property Tables Table B.23 Enthalpy of mixing of liquids or gases with water at 25 C Compound Formula Δ bh mix kj/gmol solute Acetic acid (l) CH 3 COOH Ammonia (g) HN Formic acid (l) HCOOH 0.85 Hydrogen chloride (g) HCl Nitric acid (l) HNO denotes heat evolved Source: Perry s Chemical Engineers Handbook, 6th ed

36 Appendix C Units, Dimensions, and Conversion Factors In the field of engineering and particular dealing with heat transfer, the physical quantities such as specific heat, thermal conductivity, heat transfer coefficient, heat flux, etc. are expressed in terms of a few fundamental dimensions which include length, time, mass, and temperature (see Table B.1) and each of these dimensions is associated with a unit when it is to be expressed numerically. In this appendix we present the two most commonly used systems of units that includes (1) the SI system (Systèm International d Unitès), also known as MKSA system, and (2) the English engineering system (ft.lb.lb f.s). C.1 Some Useful Definitions A quantity in the general sense is a property ascribed to phenomena, bodies, or substances that can be quantified for, or assigned to, a particular phenomenon, body, or substance. Examples are mass and electric charge. A quantity in the particular sense is a quantifiable or assignable property ascribed to a particular phenomenon, body, or substance. Examples are the mass of the moon and the electric charge of the proton. A physical quantity is a quantity that can be used in the mathematical equations of science and technology. A unit is a particular physical quantity, defined and adopted by convention, with which other particular quantities of the same kind are compared to express their value. The value of a physical quantity is the quantitative expression of a particular physical quantity as the product of a number and a unit, the number being its numerical value. Thus, the numerical value of a particular physical quantity depends on the unit in which it is expressed. Springer International Publishing AG 2017 B. Zohuri, Thermal-Hydraulic Analysis of Nuclear Reactors, DOI /

37 784 Appendix C: Units, Dimensions, and Conversion Factors For example, the value of the height h W of the Washington Monument is h W ¼ 169 m ¼ 555 ft. Here h W is the physical quantity, its value expressed in the unit meter, unit symbol m, is 169 m, and its numerical value when expressed in meters is 169. However, the value of h W expressed in the unit foot, symbol ft, is 555 ft, and its numerical value when expressed in feet is 555. C.2 Metric or International System of Units (SI) This is a brief summary of the SI (Systèm International d Unitès), the modern metric system of measurement. Long the language universally used in science, the SI has become the dominant language of international commerce and trade. These essentials are adapted from NIST Special Publication 811 (SP 811), prepared by B. N. Taylor and entitled Guide for the Use of the International System of Units (SI), and NIST Special Publication 330 (SP 330), edited by B. N. Taylor and entitled The International System of Units (SI). Users requiring information that is more detailed may access SP 811 and SP 330 online from the Bibliography, or order SP 811 for postal delivery. Information regarding the adoption and maintenance of the SI may be found in the section International aspects of the SI. This unit is also known as MKSA System. C.3 SI Based and British System Engineering Based Units The SI is founded on seven SI base units for seven base quantities assumed to be mutually independent, as given in Table C.1.

38 Appendix C: Units, Dimensions, and Conversion Factors 785 Table C.1 SI base units SI base unit English base unit Base quantity Name Symbol Symbol Length Meter m ft Mass Kilogram kg lb Time Second s s Electric current Ampere A A Thermodynamic temperature Kelvin K 0 R Amount of substance Mole mol mol Luminous intensity Candela cd cd Force Newton N lb f Energy Joule J Btu Table C.2 Examples of SI derived units Derived quantity SI derived unit Name Symbol Area Square meter m 2 Volume Cubic meter m 3 Speed, velocity Meter per second m/s Acceleration Meter per second squared m/s 2 Wave number Reciprocal meter m 1 Mass density Kilogram per cubic meter kg/m 3 Specific volume Cubic meter per kilogram m 3 /kg Current density Ampere per square meter A/m 2 Magnetic field strength Ampere per meter A/m Amount-of-substance concentration Mole per cubic meter mol/m 3 Luminance Candela per square meter cd/m 2 Mass fraction Kilogram per kilogram, which may be represented by the number 1 kg/kg ¼ 1 C.4 SI Based Derived Units Other quantities, called derived quantities, are defined in terms of the seven base quantities via a system of quantity equations. The SI derived units for these derived quantities are obtained from these equations and the seven SI base units. Examples of such SI derived units are given in Table C.2, where it should be noted that the symbol 1 for quantities of dimension 1 such as mass fraction is generally omitted. For ease of understanding and convenience, 22 SI derived units have been given special names and symbols, as shown in Table C.3.

39 786 Appendix C: Units, Dimensions, and Conversion Factors Table C.3 SI derived units with special names and symbols Derived quantity SI derived unit Name Symbol Expression in terms of other SI units Expression in terms of SI base units Plane angle Radian a rad m m 1 ¼ 1 b Solid angle Steradian a sr c m 2 m 2 ¼ 1 b Frequency Hertz Hz s 1 Force Newton N m kg s 2 Pressure, stress Pascal Pa N/m 2 m 1 kg s 2 Energy, work, quantity of Joule J N m m 2 kg s 2 heat Power, radiant flux Watt W J/s m 2 kg s 3 Electric charge, quantity of Coulomb C s A electricity Electric potential difference, Volt V W/A m 2 kg s 3 A 1 electromotive force Capacitance Farad F C/V m 2 kg 1 s 4 A 2 Electric resistance Ohm Ω V/A m 2 kg s 3 A 2 Electric conductance Siemens S A/V m 2 kg 1 s 3 A 2 Magnetic flux Weber Wb V s m 2 kg s 2 A 1 Magnetic flux density Tesla T Wb/m 2 kg s 2 A 1 Inductance Henry H Wb/A m 2 kg s 2 A 2 Celsius temperature Degree Celsius C K Luminous flux Lumen lm cd sr c m 2 m 2 cd ¼ cd Illuminance Lux lx lm/m 2 m 2 m 4 cd ¼ m cd Activity (of a radionuclide) Becquerel Bq s 1 Absorbed dose, specific Gray Gy J/kg m 2 s 2 energy (imparted), kerma Dose equivalent d Sievert Sv J/kg m 2 s 2 Catalytic activity Katal kat s 1 mol a The radian and steradian may be used advantageously in expressions for derived units to distinguish between quantities of a different nature but of the same dimension; some examples are given in Table C.4 b In practice, the symbols rad and sr are used where appropriate, but the derived unit 1 is generally omitted c In photometry, the unit name steradian and the unit symbol sr are usually retained in expressions for derived units d Other quantities expressed in sieverts are ambient dose equivalent, directional dose equivalent, personal dose equivalent, and organ equivalent dose For a graphical illustration of how the 22 derived units with special names and symbols given in Table C.3 are related to the seven SI base units, see relationships among SI units.