Physical Properties APPENDIX B. B.1 Atomic Mass and Number of the Elements B.2 Critical Temperature T c. and Pressure P c

Transcription

1 mur52933_app.qxd 9/26/05 10:01 AM Page 641 B APPENDIX B Physical Properties Table Pages B.1 Atomic Mass and Number of the Elements B.2 Critical Temperature T c and Pressure P c of Selected Compounds B.3 Gibbs Energy of Formation G f, Enthalpy of Formation H, and Enthalpy of Combustion H f c at 298 K B.4 Antoine Equation Constants for Selected Compounds B.5 Henry s Law Constant H i for Gas Dissolved in Water 654 B.6 Partial Pressures of SO 2 in Equilibrium with Dissolved SO 2 in Water B.7 Partial Pressures of NH 3 in Equilibrium with Dissolved NH 3 in Water 655 B.8 Solubility of Salts in Water 656 B.9 Benzene-Naphthalene Solid-Liquid Equilibrium 656 B.10 m-xylene p-xylene Solid-Liquid Equilibrium 657 B.11 Ethanol-Water Vapor-Liquid Equilibrium 657 B.12 Methanol-Benzene Vapor-Liquid Equilibrium 658 B.13 Water Acetic Acid Methyl Isobutyl Ketone Liquid-Liquid Equilibrium 658 B.14 Ethylbenzene Styrene-Ethylene Glycol Liquid-Liquid Equilibrium 659 B.15 Distribution Coefficient K D for Solute Distributing between Two Immiscible Liquids B.16 Specific Enthalpy H, Internal Energy U, and Volume V of H 2 O at Several Temperatures and Pressures B.17 Heat Capacity C p of Selected Liquids and Vapors B.18 Heat Capacity C p of Selected Solids 666 B.19 Heat Capacity C p of Miscellaneous Materials 667 B.20 Enthalpy of Melting H m and Enthalpy of Vaporization H v at 1.0 atm B.21.Enthalpy of Solution of Organic Solids Dissolved in Water H soln

2 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties B.22 Enthalpy of Solution of Inorganic Solids Dissolved in Water, H soln, at Indicated Dilution and 18 C, per gmol Solute B.23 Enthalpy of Mixing of Liquids or Gases with Water at 25 C 672 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. (http.//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. B.1 Atomic Mass and Number of the Elements Table B.1 Atomic Mass and Number of the First 100 Elements Atomic Atomic Atomic Atomic Element Symbol number mass Element Symbol number 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

3 mur52933_app.qxd 9/26/05 10:01 AM Page 643 Section B.1 Atomic Mass and Number of the Elements 643 Atomic Atomic Atomic Atomic Element Symbol number mass Element Symbol number mass 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 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

4 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties Table B.1 Atomic Atomic Atomic Atomic Element Symbol number mass Element Symbol number mass 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. B.2 Nonideal Gas Model Equation and Critical Properties One way to write the ideal gas law is PV RT 1 where P pressure, T temperature, R ideal gas constant, and 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 PV RT For an ideal gas, Z 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 V

5 mur52933_app.qxd 9/26/05 10:01 AM Page 645 Section B.2 Nonideal Gas Model Equation and Critical Properties 645 equations for predicting specific volumes of real gases is the Redlich-Kwong equation: Z 3 Z 2 1A B 2 B2 Z AB 0 where A ap R 2 T 2.5 a ar T c P c a 1 9A 3 2 1B B bp RT b b RT c P c b Knowing just the critical temperature T c 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. Table B.2 Critical Temperature T c and Critical Pressure P c of Selected Compounds Compound Formula T c, C P c,atm Compound Formula T c, C P c, atm Acetaldehyde C 2 O Carbon CS disulfide Acetic acid C 2 O Carbon CO monoxide Acetic C 4 O Chlorine Cl anhydride Acetone C 3 O Diethylamine (C 2 NH Acetonitrile C 2 H 3 N Dimethylamine (CH 3 NH Acetylene C 2 H Ethane C Air Ethyl acetate CH 3 COOC Ammonia NH Ethanol C 2 OH Argon Ar Ethylene C Benzene C Ethylene oxide C 2 O Bromine Br Fluorine F Butadiene, 1,3 C Helium He n-butane C Heptane C 7 H Carbon dioxide CO Hydrazine N

6 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties Table B.2 Compound Formula T c, C P c,atm Compound Formula T c, C P c, atm Hydrogen H n-pentane C 5 H Hydrogen HCl Phenol C 6 O chloride Hydrogen HCN Phosgene COCl cyanide Hydrogen H 2 S n-propane C sulfide Isobutane C Propionic acid C 2 COOH Isopentane C 5 H n-propanol C 3 H 7 OH Mercury Hg Propylene C Methyl acetate CH 3 COOCH Pyridine C 6 N Methanol CH 3 OH Radon Rn Methyl ethyl CH 3 OC Sodium Na ether Neon Ne Silicon SiF tetrafluoride Nitric oxide NO Sulfur dioxide SO Nitrogen N Sulfur trioxide SO Nitrogen N 2 O Toluene C 6 CH tetroxide Nitrous oxide N 2 O Triethylamine (C 2 ) 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. 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 Eq. (4.14): G r v i G i, f

7 mur52933_app.qxd 9/26/05 10:01 AM Page 647 Section B.3 Gibbs Energy, Enthalpy of Formation, and Enthalpy of Combustion 647 To a good approximation, we can calculate the Gibbs energy change at any temperature T by using the van t Hoff expression, Eq. (4.15): where lnk a,t - G T RT - 1 R c G r H r 298 H r T d or H r v i H i, f H r v i H i,c Table B.3 Standard Gibbs Energy of Formation G f, Enthalpy of Formation H f, and Enthalpy of Combustion H c at 298 K G f H f H c Compound Formula kj/gmol kj/gmol kj/gmol Acetaldehyde (g) C 2 O Acetic acid (g) C 2 O (l) Acetic anhydride (g) C 4 O Acetone (g) C 3 O (l) Acetonitrile (g) C 2 H 3 N Acetylene (g) C 2 H Adipic acid (l) C 6 O Ammonia (g) NH Ammonium nitrate (s) N 2 NO (aq) Argon (g) Ar Benzene (g) C Butadiene, 1,3 (g) C n-butane (g) C Calcium carbonate (s) CaCO

8 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties Table B.3 G f H f H c Compound Formula kj/gmol kj/gmol kj/gmol 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 Cl Chloroform (g) CHCl Cyclohexane (g) C 6 H (l Diethylamine (g) (C 2 NH Diethyl ether (g) (C 2 O (l) Dimethylamine (g) (CH 3 N Dimethyl carbonate (l) C 3 O Dimethyl ether (g) (CH 3 O Ethane (g) C Ethanol (g) C 2 OH (l) Ethyl acetate (g) CH 3 COOC (l) Ethylamine (g) C 2 NH Ethylbenzene (g) C (l) Ethylene (g) C Ethylene glycol (g) C 2 HO (l) Ethylene oxide (g) C 2 O Formaldehyde (g) CH 2 O Formic acid (g) CH 2 O

9 mur52933_app.qxd 9/26/05 10:01 AM Page 649 Section B.3 Gibbs Energy, Enthalpy of Formation, and Enthalpy of Combustion 649 G f H f H c Compound Formula kj/gmol kj/gmol kj/gmol Gallium nitride (s) GaN Glycerol (glycerin) (g) C 3 O (l) n-heptane (g) C 7 H (l) Hexamethylenediamine (g) C 6 H 16 N n-hexane (g) C 6 H (l) Hydrazine (g) N (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 Isobutene (g) C Isopentane (g) C 5 H Magnesium chloride (s) MgCl Methane (g) C Methyl acetate (g) CH 3 COOCH Methanol (g) CH 3 OH (l) Methyl ethyl ether CH 3 OC Naphthalene (g) C Nitric acid (g) HNO (l)

10 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties Table B.3 G f H f H c Compound Formula kj/gmol kj/gmol kj/gmol Nitric oxide (g) NO Nitroglycerin C 3 (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 OH (l) Phosgene (g) COCl n-propane (g) C Propionic acid (g) C 2 COOH (l) n-propanol (g) C 3 H 7 OH (l) Propylene (g) C Silicon tetrachloride (l) SiCl Silicon dioxide (c,quartz) SiO Sodium borohydride (aq) NaB 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

11 mur52933_app.qxd 9/26/05 10:01 AM Page 651 Section B.3 Gibbs Energy, Enthalpy of Formation, and Enthalpy of Combustion 651 G f H f H c Compound Formula kj/gmol kj/gmol kj/gmol Sulfur dioxide (g) SO Sulfur trioxide (g) SO Sulfuric acid (l) H 2 SO (aq) Toluene (g) C 6 CH (l) Triethylamine (g) (C 2 ) 3 N Trimethylamine (CH 3 ) 3 N Trinitrotoluene (g) C 7 (NO 2 ) (s) 65.6 Urea (g) (NH 2 CO (l) (s) Vinyl chloride (g) C 2 H 3 Cl Water (g) H 2 O (l) o-xylene (g) C (l) m-xylene (g) C (l) p-xylene (g) C (l) H c 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, H c decreases (becomes more negative) by 44.0n kj/gmol, where n is the number of moles of H 2 O. H 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.

12 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties B.4 Antoine Equation Constants The Antoine equation log 10 P sat 1mmHg2 A B T 1 C2 C 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 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 8 to Benzoic acid C 6 COOH 96 to Bromine Br n-butanol C 4 H 9 OH 15 to Butadiene, 1,3 C 4 58 to Carbon disulfide CS 2 3 to Chlorine Cl Chloroform CHCl 3 35 to Diethanolamine (C 2 O NH 194 to Diethylamine (C 2 NH 31 to Dimethylamine (CH 3 NH 72 to Ethanol C 2 OH 2 to Ethanolamine C 2 H 7 ON 65 to Ethyl acetate CH 3 COOC 2 15 to Ethylamine C 2 NH 2 20 to Ethylbenzene C 8 26 to Ethylene glycol C 2 O 2 50 to

13 mur52933_app.qxd 9/26/05 10:01 AM Page 653 Section B.4 Antoine Equation Constants 653 Compound Formula Range, C A B C Ethylene oxide C 2 O 49 to Formic acid CH 2 O 2 37 to Glycerol C 3 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 Isopropanol C 3 H 7 OH 0 to Lactic acid C 3 O Methanol CH 3 OH 14 to to Methyl acetate CH 3 COOCH 3 1 to Methyl ethyl ketone CH 3 COC Naphthalene (s) C 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 O7 to n-propanol C 3 H 7 OH 2 to Propionic acid C 2 COO6 to Silicon tetrachloride SiCl 4 0 to Styrene C 8 32 to Tetramethyl lead C 4 H 12 Pb 0 to Toluene C 7 6 to Water H 2 O 0 to to n-xylene C 8 32 to m-xylene C 8 28 to p-xylene C 8 27 to Source: Lange s Handbook of Chemistry, 14th ed and NIST Chemistry Webbook.

14 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties B.5 Phase Equilibrium Data Table B.5 Henry s Law Constant (atm), H i yip xi p i xi, 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 C 22,400 29,700 37,600 44,900 52,000 57,700 C 2 12,600 18,900 26,300 34,200 42,300 50,000 C 2 5,520 7,680 10,200 12,700 CO ,040 1,420 1,860 2,330 2,830 H 2 S Adapted from Hines and Maddox, Mass Transfer Fundamentals and Applications, Table B.6 Partial Pressures of SO 2 in Equilibrium with Dissolved SO 2 in Water Partial pressure of SO 2,, mmhg Grams SO 2 per 100 grams water 10 C 20 C 30 C 40 C 50 C 60 C 70 C 80 C 90 C 100 C p SO2

15 mur52933_app.qxd 9/26/05 10:01 AM Page 655 Section B.5 Phase Equilibrium Data 655 Partial pressure of SO 2,, mmhg Grams SO 2 per 100 grams 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. p SO2 Table B.7 Partial Pressures of NH 3 in Equilibrium with Dissolved NH 3 in Water Partial Pressure of NH 3,, mmhg Grams NH 3 per 100 grams 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. p NH3

16 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties 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 Magnesium chloride MgCl 2 6H 2 O Potassium nitrate KNO Potassium sulfate K 2 SO Sodium chloride NaCl Sodium sulfate Na 2 SO 4 10H 2 O Na 2 SO 4 7H 2 O Na 2 SO Data are listed as grams 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. 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.)

17 mur52933_app.qxd 9/26/05 10:01 AM Page 657 Section B.5 Phase Equilibrium Data 657 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.) Table B.11 Ethanol-Water Vapor-Liquid Equilibrium at 1 atm Mole fraction ethanol Mole fraction ethanol Temperature, C in liquid phase, x e in vapor phase, y e Source: Perry s Chemical Engineers Handbook, 6th ed.

18 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties Table B.12 Methanol-Benzene Vapor-Liquid Equilibrium at 1 atm Mole fraction methanol Mole fraction methanol Temperature, C in liquid phase, x m in vapor phase, y m Source: Perry s Chemical Engineers Handbook, 6th ed. 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 phases at equilibrium. Source: Perry s Chemical Engineers Handbook, 6th ed.

19 mur52933_app.qxd 9/26/05 10:01 AM Page 659 Section B.5 Phase Equilibrium Data 659 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 phases at equilibrium. Source: Perry s Chemical Engineers Handbook, 6th ed. Table B.15 Distribution Coefficient, K D 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

20 mur52933_app.qxd 9/26/05 1:48 PM Page Appendix B Physical Properties Table B.15 Solute A Solvent phase I Solvent phase II K D Diethylamine Water Benzene 1.8 Diethylamine Water Toluene 0.63 Diethylamine 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 (p.0) Amyl acetate 0.06 Penicillin F Water (p.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, B.6 Steam Tables H U and are given in units of kj/kg, with the reference condition as the triple point of liquid water ( K, bar). V 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, ( (See table on next page.)

21 mur52933_app.qxd 9/26/05 10:01 AM Page 661 Table B.16 Specific Enthalpy H, Internal Energy U, and Volume V of H 2 O at Several Temperatures and Pressures Temperature ( C) P, bar Sat d Sat d (T sat, C) liquid vapor H (0.01) U V H (45.806) U V (99.606) U V H (151.83) U V H (179.88) U V H (212.38) U V (250.35) U V H (275.58) U V H (311.00) U V H (342.16) U V H (365.75) U V H (373.95) U V

22 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties Table B.16 Temperature ( C) P, bar Sat d Sat d (T sat, C) liquid vapor H (0.01) U V H (45.806) U V (99.606) U V H (151.83) U V H (179.88) U V H (212.38) U V (250.35) U V H (275.58) U V H (311.00) U V H (342.16) U V H (365.75) U V H (373.95) U V

23 mur52933_app.qxd 9/26/05 10:01 AM Page 663 Section B.7 Heat Capacities 663 B.7 Heat Capacities Table B.17 Heat Capacity C p of Selected Liquids and Vapors C p Compound Formula (approx.) A B C D Acetaldehyde (g) C 2 O 54.7 (l) Acetic acid (g) C 2 O e e-8 (l) Acetone (g) C 3 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) C e e-8 (l) e-4 Bromine (g) Br e e-9 Butadiene, 1,3 (g) C e e-8 n-butane (g) C 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 Chlorobenzene (l) C 6 Cl e-4 Cyclohexane (l) C 6 H e-3 Diethylamine (g) (C 2 NH (l) Diethyl ether (g) (C 2 O e e-9 Dimethylamine (g) (CH 3 NH (l) 136.8

24 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties Table B.17 C p Compound Formula (approx.) A B C D Dimethyl ether (g) (CH 3 O 65.6 (l) Ethane (g) C e e-9 (e) 68 Ethanol (g) C 2 O e e-9 (l) Ethyl acetate (g) CH 3 COOC (l) Ethylbenzene (g) C e e-7 (l) Ethylene (g) C e e-8 Ethylene glycol (g) C 2 HO Ethylene oxide (g) C 2 O e e-8 Formaldehyde (g) CH 2 O 35.4 Glycerol (glycerin) (l) C 3 O n-heptane (g) C 7 H e e-8 (l12 n-hexane (g) C 6 H e e-8 (l) Hydrazine (g) N 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 e e-8 Isobutene (g) C e e-9 Isopentane (g) C 5 H e e-8 Isopropanol (g) C 3 H 7 O e e-8 (l) 155 Lactic acid (g) C 3 O (l62

25 mur52933_app.qxd 9/26/05 10:01 AM Page 665 Section B.7 Heat Capacities 665 C p Compound Formula (approx.) A B C D Methane (g) C e e-8 Methyl acetate (l) CH 3 COOCH Methanol (g) CH 3 O 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) C 8 H e e-8 (l55 Oxygen O e e-8 n-pentane (g) C 5 H e e-8 (l) Phenol (g) C 6 O3.6 Phosgene (g) COCl Potassium nitrate (l) KNO n-propane (g) C e e-8 n-propanol (g) C 3 H 7 O e e-8 (l) e-3 Propylene (g) C e e-8 Silicon tetrachloride (l) SiCl Sodium nitrate (l) NaNO Styrene (g) C 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 CH e e-8 (l) Triethylamine (g) (C 2 ) 3 N 160.9

26 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties Table B.17 C p Compound Formula (approx.) A B C D Trimethylamine (g) (CH 3 ) 3 N 91.8 Water (g) H 2 O e e-9 (l) o-xylene (g) C e e-8 m-xylene (g) C e e-8 p-xylene (g) C e e-8 For approximate calculations, 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 C p A BT CT 2 DT 3, where C p is in J/gmol K (or J/gmol C) and T is in K. To convert to cal/gmol K or to Btu/lbmol F, multiply by Source: Compiled from data in Introductory Chemical Engineering Thermodynamics, J. R. Elliott and C. T. Lira, Prentice-Hall, 1999; Perry s Chemical Engineers Handbook, 6th ed.; and Lange s Handbook of Chemistry, 14th ed. 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 COOH 147 Calcium carbonate CaCO T 1.287e6/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 1.77e6/T 2 Fe 3 O T 4.1e-6/T 2 Magnesium chloride MgCl T Naphthalene C T Phenol C 6 OH (20 C) Silicon Si T 4.225e5/T 2 Silicon dioxide (quartz) SiO T 1.01e6/T 2 Sodium chloride NaCl T Sucrose C 12 H 22 O (at 20 C) Titanium dioxide TiO T 1.75e5/T 2 Urea C N 2 O 80.3 (at 20 C) Source: Compiled from data in Perry s Chemical Engineers Handbook, 6th ed, and NIST Chemistry Webbook.

27 mur52933_app.qxd 9/26/05 10:01 AM Page 667 Section B.8 Temperature and Enthalpy of Phase Change 667 Table B.19 Heat Capacity C p of Miscellaneous Materials Material C p, J/g K Cellulose 1.34 Clay 0.94 Coal 1.09 to 1.55 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 1.9 to 2.7 Wool 1.36 Source: Perry s Chemical Engineers Handbook, 6th ed. B.8 Temperature and Enthalpy of Phase Change Table B.20 Enthalpy of Melting H m at the Normal Melting Temperature T m and Enthalpy of Vaporization H v at the Normal Boiling Temperature T b at 1.0 atm H H m v Compound Formula T m ( C) kj/gmol T b ( C) kj/gmol Acetaldehyde C 2 O Acetic acid C 2 O Acetic anhydride C 4 O Acetone C 3 O Acetonitrile C 2 H 3 N Acetylene C 2 H Acrylonitrile C 3 H 3 N Adipic acid C 6 O

28 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties Table B.20 H H m v Compound Formula T m ( C) kj/gmol T b ( C) kj/gmol Ammonia NH Argon Ar Benzene C Benzoic acid C 6 COOH Bromine Br Bromoform CHBr Butadiene, 1,3 C n-butane C Calcium carbonate CaCO (53) Calcium chloride CaCl Carbon (graphite) C Carbon dioxide CO Carbon disulfide CS Carbon monoxide CO Carbon tetrachloride CCl Chlorine Cl Chlorobenzene C 6 Cl Chloroform CHCl Diethylamine (C 2 NH Diethyl ether (C 2 O Dimethylamine (CH 3 NH Dimethyl carbonate C 3 O Dimethyl ether (CH 3 O Ethane C Ethyl acetate CH 3 COOC Ethylbenzene C Ethanol C 2 OH Ethylamine C 2 NH Ethylene C Ethylene glycol C 2 O Ethylene oxide C 2 O Formaldehyde CH 2 O

29 mur52933_app.qxd 9/26/05 10:01 AM Page 669 Section B.8 Temperature and Enthalpy of Phase Change 669 H H m v Compound Formula T m ( C) kj/gmol T b ( C) kj/gmol Formic acid CH 2 O Gallium Ga Glycerol C 3 O n-heptane C 7 H n-hexane C 6 H Hydrazine N Hydrogen H Hydrogen chloride HCl Hydrogen peroxide H 2 O Hydrogen cyanide HCN Hydrogen sulfide H 2 S Iron Fe Iron oxide FeO 1380 Isobutane C Isopentane C 5 H Isopropanol C 3 O Lactic acid C 3 O Methane C Methyl acetate CH 3 COOCH Methanol CH 3 OH Methylamine CH 2 NH Methyl ethyl ether CH 3 OC Naphthalene C Nitric acid HNO Nitric oxide NO Nitrogen N Nitrogen dioxide NO Nitrogen tetroxide N 2 O Nitroglycerin C 3 N 3 O Nitrous oxide N 2 O n-octane C 8 H Oxygen O

30 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties Table B.20 H H m v Compound Formula T m ( C) kj/gmol T b ( C) kj/gmol n-pentane C 5 H Phenol C 6 O Phosgene COCl Propane C Propionic acid C 2 COOH n-propanol C 3 H 7 OH Propylene C Silicon Si Silicon tetrachloride SiCl Silicon dioxide (quartz) SiO Sodium carbonate Na 2 CO Sodium chloride NaCl Sodium cyanide NaCN Sodium hydroxide NaOH Sulfur S Sulfur dioxide SO Sulfur trioxide SO 3 17 Sulfuric acid H 2 SO Styrene C Toluene C 6 CH Triethylamine (C 2 ) 3 N Trimethylamine (CH 3 ) 3 N Trinitrotoluene C 7 N 3 O explodes Urea C N 2 O decomposes 87.9 (sublim.) Water H 2 O o-xylene C m-xylene C p-xylene C Source: Compiled from data in Perry s Chemical Engineers Handbook, 6th ed., CRC Handbook of Chemistry and Physics, 70th ed., Lange s Handbook of Chemistry, 14th ed.

31 mur52933_app.qxd 9/26/05 10:01 AM Page 671 Section B.9 Enthalpies of Solution and of Mixing 671 B.9 Enthalpies of Solution and of Mixing Table B.21 Enthalpy of Solution of Organic Solids Dissolved in Water,, at Infinite Dilution and 25 C H soln Compound Formula kj/gmol solute Acetic acid C 2 O Citric acid C 6 O Lactose C 11 H 22 O 11 H 2 O Maleic acid C 4 O Menthol C 10 H 20 O 0 Phenol C 6 OH 10.9 Phthalic acid C 8 O Picric acid C 6 H 3 N 3 O Potassium citrate 11.8 Sodium citrate(tri) Sucrose C 12 H 22 O Urea C N 2 O 15.1 Vanillin 21.8 denotes heat evolved (exothermic), denotes heat absorbed (endothermic). Source: Compiled from data in Perry s Chemical Engineers Handbook. H soln Table B.22 Enthalpy of Solution of Inorganic Solids Dissolved in Water,, at Indicated Dilution and 18 C H soln Dilution, gmol water H soln Compound Formula per g substance kj/gmol solute Aluminum chloride AlCl Ammonium chloride N Cl q Ammonium sulfate (N SO 4 q 11.5 Calcium chloride CaCl 2 q 20.5 Calcium chloride CaCl 2.H 2 O q 51.46

32 mur52933_app.qxd 9/26/05 10:01 AM Page Appendix B Physical Properties Table B.22 Dilution, gmol water H soln Compound Formula per g substance kj/gmol solute Ferric chloride FeCl Phosphoric acid H 3 PO Sodium bicarbonate NaHCO Sodium carbonate Na 2 CO 3 q Sodium carbonate Na 2 CO 3.H 2 O q 9.16 Sodium carbonate Na 2 CO 3.7H 2 O q Sodium carbonate Na 2 CO 3.10H 2 O q Sodium hydroxide NaOH q denotes heat evolved (exothermic), denotes heat absorbed (endothermic). Note: H soln is very sensitive to waters of hydration and to dilution factor. Source: Compiled from data in Perry s Chemical Engineers Handbook. Table B.23 Enthalpy of Mixing of Liquids or Gases with Water at 25 C Compound Formula 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. H mix