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PHYSICAL PROPERTIES OF PURE SUBSTANCESTABLE 2-1 Physical Properties of the Elements and Inorganic Compounds* Abbreviations Used in the Table Formula Color, crystalline form Specific Melt

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DOI: 10.1036/0071511253

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GENERAL REFERENCES PHYSICAL PROPERTIES OF PURE SUBSTANCES

Tables

2-1 Physical Properties of the Elements and Inorganic

Compounds 2-7

2-2 Physical Properties of Organic Compounds 2-28

VAPOR PRESSURES OF PURE SUBSTANCES

Units Conversions 2-48

Additional References 2-48

Tables

2-3 Vapor Pressure of Water Ice from 0 to −40 °C 2-48

2-4 Vapor Pressure of Supercooled Liquid Water

2-314, and 2-315 Sorted by Chemical Family 2-49

2-7 Formula Index of Substances in Tables 2-8, 2-32,

2-11 Partial Pressures of Water over Aqueous Solutions

of HCl 2-802-12 Partial Pressures of HCl over Aqueous Solutions

of HCl 2-80Vapor Pressures of H3PO4Aqueous: Partial Pressure of

H2O Vapor (Fig 2-1) 2-81Vapor Pressures of H3PO4Aqueous: Weight of H2O

in Saturated Air (Fig 2-2) 2-812-13 Partial Pressures of H2O and SO2over Aqueous

Solutions of Sulfur Dioxide 2-812-14 Water Partial Pressure, bar, over Aqueous Sulfuric

Acid Solutions 2-822-15 Sulfur Trioxide Partial Pressure, bar, over Aqueous

Sulfuric Acid Solutions 2-842-16 Sulfuric Acid Partial Pressure, bar, over Aqueous

Sulfuric Acid 2-862-17 Total Pressure, bar, of Aqueous Sulfuric Acid Solutions 2-872-18 Partial Pressures of HNO3and H2O over Aqueous

Solutions of HNO3 2-882-19 Partial Pressures of H2O and HBr over Aqueous

Solutions of HBr at 20 to 55 °C 2-89

2-1

Section 2 Physical and Chemical Data*

Bruce E Poling Department of Chemical Engineering, University of Toledo (Physical and

Richard L Rowley Department of Chemical Engineering, Brigham Young University

(Prediction and Correlation of Physical Properties)

W Vincent Wilding Department of Chemical Engineering, Brigham Young University

(Prediction and Correlation of Physical Properties)

*Contribution in part of the National Institute of Standards and Technology; not subject to copyright in the United States

Copyright © 2008, 1997, 1984, 1973, 1963, 1950, 1941, 1934 by The McGraw-Hill Companies, Inc Click here for terms of use.

2-20 Partial Pressures of HI over Aqueous Solutions

2-28 Partial Pressures of H2O and CH3OH over Aqueous

Solutions of Methyl Alcohol 2-94

2-29 Partial Pressures of H2O over Aqueous Solutions

of Sodium Hydroxide 2-94

WATER-VAPOR CONTENT OF GASES

Chart for Gases at High Pressures 2-95

Water Content of Air (Fig 2-4) 2-95

DENSITIES OF PURE SUBSTANCES

Tables

2-30 Density (kg/m3) of Saturated Liquid Water from

the Triple Point to the Critical Point 2-96

2-31 Density (kg/m3) of Mercury from 0 to 350°C 2-97

2-32 Densities of Inorganic and Organic Liquids (mol/dm3) 2-98

DENSITIES OF AQUEOUS INORGANIC SOLUTIONS AT 1 ATM

Units and Units Conversions 2-104

2-41 Arsenic Acid (H3AsO4) 2-104

2-42 Barium Chloride (BaCl2) 2-105

2-43 Cadmium Nitrate [Cd(NO3)2] 2-105

2-44 Calcium Chloride (CaCl2) 2-105

2-45 Calcium Hydroxide [Ca(OH)2] 2-105

2-46 Calcium Hypochlorite (CaOCl2) 2-105

2-47 Calcium Nitrate [Ca(NO3)2] 2-105

2-48 Chromic Acid (CrO3) 2-105

2-49 Chromium Chloride (CrCl3) 2-105

2-50 Copper Nitrate [Cu(NO3)2] 2-105

2-51 Copper Sulfate (CuSO4) 2-105

2-52 Cuprous Chloride (CuCl2) 2-105

2-53 Ferric Chloride (FeCl3) 2-105

2-54 Ferric Sulfate [Fe2(SO4)3] 2-106

2-55 Ferric Nitrate [Fe(NO3)3] 2-106

2-56 Ferrous Sulfate (FeSO4) 2-106

2-64 Magnesium Sulfate (MgSO4) 2-106

2-65 Nickel Chloride (NiCl2) 2-106

2-66 Nickel Nitrate [Ni(NO3)2] 2-106

2-67 Nickel Sulfate (NiSO4) 2-106

2-68 Nitric Acid (HNO3) 2-107

2-69 Perchloric Acid (HClO4) 2-108

DENSITIES OF AQUEOUS ORGANIC SOLUTIONS

Units and Units Conversions 2-114Tables

2-108 Formic Acid (HCOOH) 2-1142-109 Acetic Acid (CH3COOH) 2-1152-110 Oxalic Acid (H2C2O4) 2-1162-111 Methyl Alcohol (CH3OH) 2-1162-112 Ethyl Alcohol (C2H5OH) 2-1172-113 Densities of Mixtures of C2H5OH and H2O at 20°C 2-1182-114 Specific Gravity {60°/60°F [(15.56°/15.56°C)]} of

Mixtures by Volume of C2H5OH and H2O 2-1192-115 n-Propyl Alcohol (C3H7OH) 2-1202-116 Isopropyl Alcohol (C3H7OH) 2-1202-117 Glycerol 2-1212-118 Hydrazine (N2H4) 2-1212-119 Densities of Aqueous Solutions of Miscellaneous

Organic Compounds 2-122

DENSITIES OF MISCELLANEOUS MATERIALS

Tables2-120 Approximate Specific Gravities and Densities of Miscellaneous Solids and Liquids 2-1242-121 Density (kg/m3) of Selected Elements as a

Function of Temperature 2-125

SOLUBILITIES

Units Conversions 2-125Tables

2-122 Solubilities of Inorganic Compounds in Water at Various Temperatures 2-1262-123 Solubility as a Function of Temperature and

Henry’s Constant at 25°C for Gases in Water 2-1302-124 Henry’s Constant H for Various Compounds in

Water at 25°C 2-1302-125 Henry’s Constant H for Various Compounds in Water

at 25°C from Infinite Dilution Activity Coefficients 2-1312-126 Air 2-1312-127 Ammonia-Water at 10 and 20°C 2-1312-128 Carbon Dioxide (CO2) 2-1312-129 Carbonyl Sulfide (COS) 2-1312-130 Chlorine (Cl2) 2-1322-131 Chlorine Dioxide (ClO2) 2-132

2-135 Linear Expansion of the Solid Elements 2-134

2-136 Linear Expansion of Miscellaneous Substances 2-135

2-137 Volume Expansion of Liquids 2-136

2-138 Volume Expansion of Solids 2-136

2-141 Critical Constants and Acentric Factors of Inorganic

and Organic Compounds 2-138

COMPRESSIBILITIES

Introduction 2-143

Units conversions 2-143

Tables

2-142 Composition of Selected Refrigerant Mixtures 2-143

2-143 Compressibility Factors for R 407A (Klea 60) 2-143

2-144 Compressibility Factors for R 407B (Klea 61) 2-143

2-147 Heats of Fusion and Vaporization of the Elements

and Inorganic Compounds 2-145

2-148 Heats of Fusion of Miscellaneous Materials 2-147

2-149 Heats of Fusion of Organic Compounds 2-148

2-150 Heats of Vaporization of Inorganic and Organic

2-152 Specific Heat [kJ/(kg⋅K)] of Selected Elements 2-164

2-153 Heat Capacities of Inorganic and Organic Liquids

[J/(kmol⋅K)] 2-165

2-154 Specific Heats of Organic Solids 2-171

2-155 Heat Capacity at Constant Pressure of Inorganic and

Organic Compounds in the Ideal Gas State Fit to a

Polynomial Cp [J/(kmol⋅K)] 2-174

2-156 Heat Capacity at Constant Pressure of Inorganic and

Organic Compounds in the Ideal Gas State Fit

to Hyperbolic Functions Cp [J/(kmol⋅K)] 2-176

2-157 C p /C v : Ratios of Specific Heats of Gases at

SPECIFIC HEATS OF MISCELLANEOUS MATERIALS

Tables2-176 Specific Heats of Miscellaneous Liquids and Solids 2-1852-177 Oils (Animal, Vegetable, Mineral Oils) 2-185

PROPERTIES OF FORMATION AND COMBUSTION REACTIONS

Units Conversions 2-185Table

2-178 Heats and Free Energies of Formation of Inorganic Compounds 2-1862-179 Enthalpies and Gibbs Energies of Formation, Entropies,and Net Enthalpies of Combustion of Inorganic andOrganic Compounds at 298.15 K 2-1952-180 Ideal Gas Sensible Enthalpies, h T − h298(kJ/kmol),

of Combustion Products 2-2012-181 Ideal Gas Entropies s°, kJ/(kmol⋅K), of

Combustion Products 2-202

HEATS OF SOLUTION

Tables2-182 Heats of Solution of Inorganic Compounds in Water 2-2032-183 Heats of Solution of Organic Compounds in Water

(at Infinite Dilution and Approximately Room Temperature) 2-206

THERMODYNAMIC PROPERTIES

Explanation of Tables 2-207Notation 2-207Units Conversions 2-207Additional References 2-207Tables

2-184 List of Substances for Which Thermodynamic Property Tables Were Generated from NIST Standard Reference Database 23 2-2082-185 Thermodynamic Properties of Acetone 2-2092-186 Saturated Acetylene 2-2102-187 Thermodynamic Properties of Air 2-211Pressure-Enthalpy Diagram for Dry Air (Fig 2-5) 2-2152-188 Air 2-216Air, Moist 2-2162-189 Thermodynamic Properties of Ammonia 2-217Pressure-Enthalpy Diagram for Ammonia (Fig 2-6) 2-219Enthalpy-Concentration Diagram for Aqueous

Ammonia (Fig 2-7) 2-2202-190 Thermodynamic Properties of Argon 2-2212-191 Liquid-Vapor Equilibrium Data for the Argon-

Nitrogen-Oxygen System 2-2242-192 Thermodynamic Properties of the International

Standard Atmosphere 2-2282-193 Thermodynamic Properties of Benzene 2-2292-194 Saturated Bromine 2-2312-195 Thermodynamic Properties of Butane 2-2322-196 Thermodynamic Properties of 1-Butene 2-2342-197 Thermodynamic Properties of cis-2-Butene 2-2362-198 Thermodynamic Properties of trans-2-Butene 2-2382-199 Thermodynamic Properties of Carbon Dioxide 2-2402-200 Thermodynamic Properties of Carbon Monoxide 2-242Temperature-Entropy Diagram for Carbon

Monoxide (Fig 2-8) 2-2442-201 Thermophysical Properties of Saturated Carbon

Tetrachloride 2-245

2-202 Saturated Carbon Tetrafluoride (R14) 2-245

2-203 Thermodynamic Properties of Carbonyl Sulfide 2-246

2-204 Saturated Cesium 2-248

2-205 Thermophysical Properties of Saturated Chlorine 2-249

Enthalpy–Log-Pressure Diagram for Chlorine (Fig 2-9) 2-250

2-206 Saturated Chloroform (R20) 2-251

2-207 Thermodynamic Properties of Cyclohexane 2-252

2-208 Thermodynamic Properties of Decane 2-254

2-209 Thermodynamic Properties of Deuterium Oxide

(Heavy Water) 2-256

2-210 Thermodynamic Properties of 2,2-Dimethylpropane

(Neopentane) 2-258

2-211 Saturated Diphenyl 2-260

2-212 Thermodynamic Properties of Dodecane 2-261

2-213 Thermodynamic Properties of Ethane 2-263

2-214 Thermodynamic Properties of Ethanol 2-265

Enthalpy-Concentration Diagram for Aqueous Ethyl

Alcohol (Fig 2-10) 2-267

2-215 Thermodynamic Properties of Ethylene 2-268

2-216 Thermodynamic Properties of Fluorine 2-270

2-217 Flutec 2-271

2-218 Halon 2-271

2-219 Thermodynamic Properties of Helium 2-272

2-220 Thermodynamic Properties of Heptane 2-274

2-221 Thermodynamic Properties of Hexane 2-276

2-222 Saturated Hydrazine 2-278

2-223 Thermodynamic Properties of Normal Hydrogen 2-279

2-224 Thermodynamic Properties of para-Hydrogen 2-281

2-225 Saturated Hydrogen Peroxide 2-282

2-226 Thermodynamic Properties of Hydrogen Sulfide 2-283

Enthalpy-Concentration Diagram for Aqueous Hydrogen

Chloride at 1 atm (Fig 2-11) 2-285

2-227 Thermodynamic Properties of Isobutane 2-286

2-228 Thermodynamic Properties of Isobutene

Enthalpy–Log-Pressure Diagram for Mercury (Fig 2-12) 2-295

2-233 Thermodynamic Properties of Methane 2-296

2-234 Thermodynamic Properties of Methanol 2-298

2-235 Thermodynamic Properties of 2-Methyl Butane (Isopentane) 2-300

2-236 Thermodynamic Properties of 2-Methyl Pentane

(Isohexane) 2-302

2-237 Saturated Methyl Chloride 2-304

2-238 Thermodynamic Properties of Neon 2-305

2-239 Thermodynamic Properties of Nitrogen 2-307

Pressure-Enthalpy Diagram for Nitrogen (Fig 2-13) 2-309

2-240 Saturated Nitrogen Tetroxide 2-310

2-241 Thermodynamic Properties of Nitrogen Trifluoride 2-311

2-242 Thermodynamic Properties of Nitrous Oxide 2-313

Mollier Diagram for Nitrous Oxide (Fig 2-14) 2-315

2-243 Thermodynamic Properties of Nonane 2-316

2-244 Thermodynamic Properties of Octane 2-318

2-245 Thermodynamic Properties of Oxygen 2-320

Pressure-Enthalpy Diagram for Oxygen (Fig 2-15) 2-322

Enthalpy-Concentration Diagram for Oxygen-Nitrogen

Mixture at 1 atm (Fig 2-16) 2-323

2-246 Thermodynamic Properties of Pentane 2-324

2-247 Saturated Potassium 2-326

Mollier Diagram for Potassium (Fig 2-17) 2-326

2-248 Thermodynamic Properties of Propane 2-327

2-249 Thermodynamic Properties of Propylene 2-329

2-250 Thermodynamic Properties of R-11, Trichlorofluoromethane 2-331

Pressure-Enthalpy Diagram for Refrigerant 11 (Fig 2-18) 2-333

2-251 Thermodynamic Properties of R-12,

Dichlorodifluoromethane 2-334

Pressure-Enthalpy Diagram for Refrigerant 12 (Fig 2-19) 2-336

2-252 Thermodynamic Properties of R-13, Chlorotrifluoromethane 2-337

Refrigerant 20 2-339

Refrigerant 14 2-339

2-253 Saturated Refrigerant 13B1, Bromotrifluoromethane 2-339

2-254 Saturated Refrigerant 21, Dichlorofluoromethane 2-339

2-255 Thermodynamic Properties of R-22, Chlorodifluoromethane 2-340

Pressure-Enthalpy Diagram for Refrigerant 22 (Fig 2-20) 2-342

2-256 Thermodynamic Properties of R-23, Trifluoromethane 2-343

2-257 Thermodynamic Properties of R-32, Difluoromethane 2-345

Pressure-Enthalpy Diagram for Refrigerant 32 (Fig 2-21) 2-347

2-258 Thermodynamic Properties of R-41, Fluoromethane 2-3482-259 Saturated R-401A (SUVA MP 39) 2-3502-260 R-401A (SUVA MP 39) at Atmospheric Pressure 2-3502-261 Thermodynamic Properties of Saturated R-407A (Klea 60) 2-3512-262 Thermodynamic Properties of Saturated R-407B (Klea 61) 2-351Enthalpy–Log-Pressure Diagram for R-407A (Klea 60)

(Fig 2-22) 2-352Enthalpy–Log-Pressure Diagram for R-407B (Klea 61)

(Fig 2-23) 2-3532-263 Saturated R-404A (SUVA HP 62) 2-3542-264 R-404A (SUVA HP 62) at Atmospheric Pressure 2-354Enthalpy–Log-Pressure Diagram for Refrigerant 123

2-265 Saturated R-401B (SUVA MP 66) 2-3552-266 R-401B (SUVA MP 66) at Atmospheric Pressure 2-3552-267 Saturated R-402A (SUVA HP 80) 2-3552-268 R-402A (SUVA HP 80) at Atmospheric Pressure 2-3562-269 Saturated R-402B (SUVA HP 81) 2-3562-270 R-402B (SUVA HP 81) at Atmospheric Pressure 2-3562-271 Thermodynamic Properties of R-113, 1,1,

2-Trichlorotrifluoroethane 2-3572-272 Thermodynamic Properties of R-114, 1,

2-Dichlorotetrafluoroethane 2-3592-273 Saturated Refrigerant 115, Chloropentafluoroethane 2-3612-274 Thermodynamic Properties of R-116, Hexafluoroethane 2-3622-275 Thermodynamic Properties of R-123,

2,2-Dichloro-1,1,1-Trifluoroethane 2-365Enthalpy–Log-Pressure Diagram for Refrigerant 123

(Fig 2-24) 2-3662-276 Thermodynamic Properties of R-124,

2-Chloro-1,1,1,2-Tetrafluoroethane 2-3672-277 Thermodynamic Properties of R-125, Pentafluoroethane 2-369Enthalpy–Log-Pressure Diagram for Refrigerant

125 (Fig 2-25) 2-3712-278 Thermodynamic Properties of R-134a, 1,1,1,2-

Tetrafluoroethane 2-372Pressure-Enthalpy Diagram for Refrigerant 134a (Fig 2-26) 2-3742-279 Thermodynamic Properties of R-141b, 1,1-Dichloro-1-

Fluoroethane 2-3752-280 Thermodynamic Properties of R-142b, 1-Chloro-1,1-

Difluoroethane 2-3772-281 Thermodynamic Properties of R-143a, 1,1,1-Trifluoroethane 2-3792-282 Thermodynamic Properties of R-152a, 1,1-Difluoroethane 2-3812-283 Saturated Refrigerant 216a, 1,3-Dichloro-1,1,2,2,3,3-

Hexafluoropropane 2-3832-284 Thermodynamic Properties of R-218, Octafluoropropane 2-3842-285 Thermodynamic Properties of R-227ea, 1,1,1,2,3,3,3-

Heptafluoropropane 2-3862-286 Saturated Refrigerant 245cb 1,1,1,2,2-Pentafluoropropane 2-3882-287 Refrigerant RC 318, Octafluorocyclobutane 2-3882-288 Thermodynamic Properties of R-404A 2-3892-289 Thermodynamic Properties of R-407C 2-391Pressure-Enthalpy Diagram for Refrigerant 407C (Fig 2-27) 2-3932-290 Thermodynamic Properties of R-410A 2-3942-291 Saturated Refrigerant 500 2-3962-292 Saturated Refrigerant 502 2-3962-293 Saturated Refrigerant 503 2-3972-294 Saturated Refrigerant 504 2-3972-295 Thermodynamic Properties of Refrigerant 507 2-3972-296 Thermodynamic Properties of R-507A 2-3982-297 Saturated Rubidium 2-4002-298 Thermophysical Properties of Saturated Seawater 2-4002-299 Saturated Sodium 2-401Mollier Diagram for Sodium (Fig 2-28) 2-402Enthalpy-Concentration Diagram for Aqueous Sodium

Hydroxide at 1 atm (Fig 2-29) 2-4032-300 Thermodynamic Properties of Sulfur Dioxide 2-4042-301 Thermodynamic Properties of Sulfur Hexafluoride 2-406Pressure-Enthalpy Diagram for Sulfur Hexafluoride (SF6)(Fig 2-30) 2-4082-302 Saturated SUVA AC 9000 2-409Enthalpy-Concentration Diagram for Aqueous Sulfuric Acid

at 1 atm (Fig 2-31) 2-4092-303 Thermodynamic Properties of Toluene 2-4102-304 Saturated Solid/Vapor Water 2-4122-305 Thermodynamic Properties of Water 2-4132-306 Thermodynamic Properties of Water Substance

along the Melting Line 2-4162-307 Thermodynamic Properties of Xenon 2-4172-308 Surface Tension (N/m) of Saturated Liquid Refrigerants 2-4192-309 Surface Tension σ (dyn/cm) of Various Liquids 2-419

2-311 Velocity of Sound (m/s) in Saturated Liquid Refrigerants 2-420

2-312 Vapor Viscosity of Inorganic and Organic Substances (Pas) 2-421

2-313 Viscosity of Inorganic and Organic Liquids (Pas) 2-427

2-314 Vapor Thermal Conductivity of Inorganic and Organic

2-317 Lower and Upper Flammability Limits,

Flash Point, and Autoignition Temperature for

Selected Hydrocarbons 2-446

2-318 Viscosities of Liquids: Coordinates for Use with Fig 2-32 2-448

Nomograph for Viscosities of Liquids at 1 atm (Fig 2-32) 2-449

Tables

2-319 Viscosity of Sucrose Solutions 2-450

Nomograph for Thermal Conductivity of Organic Liquids

(Fig 2-33) 2-450

2-320 Thermal Conductivity Nomograph Coordinates 2-450

2-321 Prandtl Number of Air 2-451

2-322 Prandtl Number of Liquid Refrigerants 2-451

2-323 Thermophysical Properties of Miscellaneous Saturated

2-327 Thermal-Conductivity-Temperature for Metals 2-460

2-328 Thermal Conductivity of Chromium Alloys 2-461

2-329 Thermal Conductivity of Some Alloys at High Temperature 2-461

2-330 Thermal Conductivities of Some Materials for

Refrigeration and Building Insulation 2-461

2-331 Thermal Conductivities of Insulating Materials at High

Temperatures 2-461

2-332 Thermal Conductivities of Insulating Materials at

Moderate Temperatures (Nusselt) 2-462

2-333 Thermal Conductivities of Insulating Materials

at Low Temperatures (Gröber) 2-462

2-334 Thermal Diffusivity (m2/s) of Selected Elements 2-462

2-335 Thermophysical Properties of Selected Nonmetallic Solid

Substances 2-463

PREDICTION AND CORRELATION OF PHYSICAL PROPERTIES

Introduction 2-463

Units 2-464

Classification of Estimation Methods 2-467

Theory and Empirical Extension of Theory 2-467

2-336 Ambrose Group Contributions for Critical Constants 2-469

2-337 Joback Group Contributions for Critical Constants 2-470

Normal Melting Point 2-471

Normal Boiling Point 2-471

2-338 Fedors Method Atomic and Structural Contributions 2-471

2-339 First-Order Groups and Their Contributions for Melting

Point 2-472

2-340 Second-Order Groups and Their Contributions for Melting

Point 2-472

Characterizing and Correlating Constants 2-473

2-341 Group Contributions for the Nannoolal Method for Normal Boiling Point 2-4742-342 Intermolecular Interaction Corrections for the

Nannoolal et al Method for Normal Boiling Point 2-476Vapor Pressure 2-477Liquids 2-477Solids 2-478Thermal Properties 2-478Enthalpy of Formation 2-4782-343 Domalski-Hearing Group Contribution Values for

Standard State Thermal Properties 2-479Entropy 2-485Gibbs’ Energy of Formation 2-486Latent Enthalpy 2-486Enthalpy of Vaporization 2-486Enthalpy of Fusion 2-487Enthalpy of Sublimation 2-4882-344 Cs (CH) Group Values for Chickos Estimation of ∆Hfus 2-4882-345 Ct (Functional) Group Values for Chickos Estimation of ∆Hfus2-488Heat Capacity 2-489Gases 2-4892-346 Group Contributions and Corrections for ∆Hsub 2-489Liquids 2-4902-347 Benson and CHETAH Group Contributions for Ideal Gas Heat Capacity 2-491Solids 2-4952-348 Liquid Heat Capacity Group Parameters for

Ruzicka-Domalski Method 2-496Mixtures 2-497Density 2-497Gases 2-4972-349 Group Values and Nonlinear Correction Terms for

Estimation of Solid Heat Capacity with the Goodman et al.Method 2-4982-350 Element Contributions to Solid Heat Capacity for the

Modified Kopp’s Rule 2-498

2-351 Simple Fluid Compressibility Factors Z(0) 2-500

2-352 Acentric Deviations Z(1)from the Simple Fluid Compressibility Factor 2-5012-353 Constants for the Two Reference Fluids Used in Lee-Kesler Method 2-5022-354 Relationships for Eq (2-66) for Common Cubic EoS 2-502Solids 2-503Mixtures 2-503Viscosity 2-504Gases 2-5042-355 Reichenberg Group Contribution Values 2-505Liquids 2-506Liquid Mixtures 2-5062-356 Group Contributions for the Hsu et al Method 2-5072-357 UNIFAC-VISCO Group Interaction Parameters αmn 2-509Thermal Conductivity 2-509Gases 2-510Liquids 2-5102-358 Correlation Parameters for Baroncini et al Method for

Estimation of Thermal Conductivity 2-5112-359 Sastri-Rao Group Contributions for Liquid Thermal

Conductivity at the Normal Boiling Point 2-511Liquid Mixtures 2-512Surface Tension 2-513Pure Liquids 2-513Liquid Mixtures 2-5142-360 Knotts Group Contributions for the Parachor in Estimating Surface Tension 2-514Flammability Properties 2-5152-361 Group Contributions for Pintar Flammability Limits

Method for Organic Compounds 2-5162-362 Group Contributions for Pintar Flammability Limits

Method for Inorganic Compounds 2-5162-363 Group Contributions for Pintar Autoignition Temperature Method for Organic Compounds 2-5172-364 Group Contributions for Pintar Autoignition Temperature Method for Inorganic Compounds 2-517

Considerations of reader interest, space availability, the system or systems of units

employed, copyright considerations, etc., have all influenced the revision of

mate-rial in previous editions for the present edition Reference is made at numerous

places to various specialized works and, when appropriate, to more general works

A listing of general works may be useful to readers in need of further information

ASHRAE Handbook—Fundamentals, SI edition, ASHRAE, Atlanta,

2005; Benedek, P., and F Olti, Computer-Aided Chemical

Thermody-namics of Gases and Liquids, Wiley, New York, 1985; Brule, M R., L.

L Lee, and K E Starling, Chem Eng., 86, 25, Nov 19, 1979, pp.

155–164; Cox, J D., and G Pilcher, Thermochemistry of Organic and

Organometallic Compounds, Academic Press, New York, 1970; Cox, J.

D., D D Wagman, and V A Medvedev, CODATA Key Values for

Ther-modynamics, Hemisphere Publishing Corp., New York, 1989; Daubert,

T E., R P Danner, H M Sibel, and C C Stebbins, Physical and

Ther-modynamic Properties of Pure Chemicals: Data Compilation, Taylor &

Francis, Washington, 1997; Domalski, E S., and E D Hearing, Heat

capacities and entropies of organic compounds in the condensed phase,

vol 3, J Phys Chem Ref Data 25(1):1–525, Jan-Feb 1996; Dykyj, J.,

and M Repas, Saturated vapor pressures of organic compounds, Veda,

Bratislava, 1979 (Slovak); Dykyj, J., M Repas, and J Svoboda, Saturated

vapor pressures of organic compounds, Veda, Bratislava, 1984 (Slovak);

Glushko, V P., Ed., Thermal Constants of Compounds, Issues I–X.,

Moscow, 1965–1982 (Russian only); Gmehling, J., Azeotropic Data, 2

vols., VCH Weinheim, Germany, 1994; Gmehling, J., and U Onken,

Vapor-Liquid Equilibrium Data Collection, Dechema Chemistry Data

Series, Frankfurt, 1977–1978; International Data Series, Selected Data

on Mixtures, Series A: Thermodynamics Research Center, National

Institute of Standards and Technology, Boulder, Colo.; Kaye, S M.,

Encyclopedia of Explosives and Related Items, U.S Army R&D

com-mand, Dover, N.J., 1980; King, M B., Phase Equilibrium in Mixtures,

Pergamon, Oxford, 1969; Landolt-Boernstein, Numerical Data and

Functional Relationships in Science and Technology (New Series),

http://www.springeronline.com/sgw/cda/frontpage/0,11855,4-10113-2-95859-0,00.html; Lide, D R., CRC Handbook of Chemistry and

Physics, 86th ed., CRC Press, Boca Raton, Fla., 2005; Lyman, W J., W.

F Reehl, and D H Rosenblatt, Handbook of Chemical Property

Esti-mation Methods, McGraw-Hill, New York, 1990; Majer, V., and V

Svo-boda, Enthalpies of Vaporization of Organic Compounds: A Critical

Review and Data Compilation, Blackwell Science, 1985; Majer V., V.

Svoboda, and J Pick, Heats of Vaporization of Fluids, Elsevier,

Amster-dam, 1989 (general discussion); Marsh, K N., Recommended Reference

Materials for the Realization of Physicochemical Properties, Blackwell

Science, 1987; NIST-IUPAC Solubility Data Series, Pergamon Press,

http://www.iupac.org/publications/ci/1999/march/solubility.html; Ohse,

R W., and H von Tippelskirch, High Temp.—High Press., 9:367–385,

1977; Ohse, R W., Handbook of Thermodynamic and Transport

Prop-erties of Alkali Metals, Blackwell Science Pubs., Oxford, England, 1985;

Pedley, J B., R D Naylor, and S P Kirby, Thermochemical Data of

Organic Compounds, Chapman and Hall, New York, 1986; Physical

Property Data for the Design Engineer, Hemisphere, New York, 1989;

Poling, B E., J M Prausnitz, and J P O’Connell, The Properties of

Gases and Liquids, 5th ed., McGraw-Hill, New York, 2001; Rothman,

D, et al., Max Planck Inst f Stromungsforschung, Ber 6, 1978; Smith,

B D., and R Srivastava, Thermodynamic Data for Pure Compounds, Part A: Hydrocarbons and Ketones, Elsevier, Amsterdam, 1986, Physi-

cal sciences data 25, scription.librarians/BS_PSD/description; Sterbacek, Z., B Biskup, and

http://www.elsevier.com/wps/find/bookseriesde-P Tausk, Calculation of Properties Using Corresponding States

Meth-ods, Elsevier, Amsterdam, 1979; Stull, D R., E F Westrum, and G C.

Sink, The Chemical Thermodynamics of Organic Compounds, Wiley, New York, 1969; TRC Thermodynamic Tables—Hydrocarbons, Ther-

modynamics Research Center, National Institute of Standards and

Technology, Boulder, Colo.; TRC Thermodynamic

Tables—Non-Hydrocarbons, Thermodynamics Research Center, National Institute

of Standards and Technology, Boulder, Colo.; Young, D A., “Phase grams of the Elements,” UCRL Rep 51902, 1975 republished in expanded form by the University of California Press, 1991; Zabransky, M., V Ruzicka, Jr., V Majer, and E S Domalski, Heat Capacity of Liq-

Dia-uids: Critical Review and Recommended Values, J Phy Chem Ref.

Data, Monograph No 6, 1996.

C RITICAL D ATA ARE C OMPILED IN :

Ambrose, D., “Vapor-Liquid Critical Properties,” N P L Teddington, Middlesex, Rep 107, 1980; Kudchaker, A P., G H Alani, and B J.

Zwolinski, Chem Revs 68:659–735, 1968; Matthews, J F., Chem.

Revs 72:71–100, 1972; Simmrock, K., R Janowsky, and A Ohnsorge,

Critical Data of Pure Substances, Parts 1 and 2, Dechema Chemistry

Data Series, 1986; Other recent references for critical data can be

found in Lide, D R., CRC Handbook of Chemistry and Physics, 86th

ed., CRC Press, Boca Raton, Fla., 2005.

P UBLICATIONS ON T HERMOCHEMISTRY

Pedley, J B., Thermochemical Data and Structures of Organic

Com-pounds, 1, Thermodynamic Research Center, Texas A&M Univ., 1994

(976 pp., 3000 cpds.); Frenkel, M., et al., Thermodynamics of Organic

Compounds in the Gas State, 2 vols., Thermodynamic Research Center,

Texas A&M Univ., 1994 (1825 pp., 2000 cpds.); Barin, I.,

Thermochem-ical Data of Pure Substances, 2 vols., 2d ed., VCH Weinheim, Germany,

1993 (1834 pp., 2400 substances); Gurvich, L.V., et al., Thermodynamic

Properties of Individual Substances, 3 vols., 4th ed., Hemisphere, New

York, 1989, 1990, and 1993 (2520 pp.); Lide, D R., and G W A Milne,

Handbook of Data on Organic Compounds, 7 vols., 3d ed., Chemical

Rubber, Miami, 1993 (7000 pp.); Daubert, T E., et al., Physical and

Thermodynamic Properties of Pure Chemicals: Data Compilation,

extant 1995, Taylor & Francis, Bristol, Pa., 1995; Database 11, NIST, Gaithersburg, Md U.S Bureau of Mines publications include Bulletins

584, 1960 (232 pp.); 592, 1961 (149 pp.); 595, 1961 (68 pp.); 654, 1970

(26 pp.); Chase, M W., et al., JANAF Thermochemical Tables, 3d ed., J.

Phys Chem Ref Data 14 suppl 1., 1986 (1896 pp.); Journal of Physical and Chemical Reference Data is available online at http://listserv.

nd.edu/cgi-bin/wa?A2=ind0501&L=pamnet&F=&S=&P=8490 and at http://www.nist.gov/srd/reprints.htm

GENERAL REFERENCES

2-6

al., 95 percent ethyl alcohol

alk, alkali (i.e., aq NaOH or

KOH)

am., amyl (C5H11)

amor., amorphous

anh., anhydrous

aq., aqueous or water

aq reg., aqua regia

atm., atmosphere or 760 mm ofmercury pressure

bk., blackbrn., brownbz., benzenec., coldcb., cubic

cc, cubic centimeterchl., chloroformcol., colorless or whiteconc., concentratedcr., crystals or crystallined., decomposesD., specific gravity with refer-ence to hydrogen = 1

d 50, decomposes at 50°C; 50d., melts at 50°C withdecompositiondelq., deliquescentdil., dilutedk., darkeff., effloresces or efflorescentet., ethyl ether

expl., explodesgel., gelatinousgly., glycerol (glycerin)gn., green

h., hothex., hexagonal

hyg., hygroscopici., insolubleign., igniteslq., liquidlt., light

m al., methyl alcoholmn., monoclinicnd., needles

NH3, liquid ammonia

NH4OH, ammonium hydroxidesolution

oct., octahedralor., orangepd., powder

pl., platespr., prisms or prismaticpyr., pyridinerhb., rhombic (orthorhombic)s., soluble

satd., saturatedsl., slightlysoln., solutionsubl., sublimessulf., sulfidestart a., tartaric acidtet., tetragonaltr., transitiontri., triclinic

trig., trigonalv., veryvac., in vacuovl., violetvolt., volatile or volatilizeswh., white

yel., yellow

∞, soluble in all proportions

<, less than

>, greater than42, about or near 42

−3H2O, 100, loses 3 moles ofwater per formula weight at100°C

Formula weights are based upon the International Atomic Weights in “Atomic Weights of the

Ele-ments 2001,” Pure Appl Chem., 75, 1107, 2003, and are computed to the nearest hundredth.

Refractive index, where given for a uniaxial crystal, is for the ordinary (ω) ray; where given for a

biax-ial crystal, the index given is for the median (β) value Unless otherwise specified, the index is given for

the sodium D-line (λ = 589.3 mµ)

Specific gravity values are given at room temperatures (15 to 20 °C) unless otherwise indicated by

the small figures which follow the value: thus, “5.618°

4 ” indicates a specific gravity of 5.6 for the substance

at 18 °C referred to water at 4°C In this table the values for the specific gravity of gases are given with

reference to air (A) = 1, or hydrogen (D) = 1

Melting point is recorded in a certain case as “82 d.” and in some other case as “d 82,” the

distinc-tion being made in this manner to indicate that the former is a melting point with decomposidistinc-tion at 82°C,

while in the latter decomposition only occurs at 82 °C Where a value such as “−2H2O, 82” is given it

indi-cates loss of 2 moles of water per formula weight of the compound at a temperature of 82 °C

Boiling point is given at atmospheric pressure (760 mm of mercury) unless otherwise indicated;

thus, “8215 mm.” indicates the boiling point is 82°C when the pressure is 15 mm

Solubility is given in parts by weight (of the formula shown at the extreme left) per 100 parts by

weight of the solvent; the small superscript indicates the temperature In the case of gases the solubility

is often expressed in some manner as “510°cc” which indicates that at 10 °C, 5 cc of the gas are soluble in

100 g of the solvent The symbols of the common mineral acids: H2SO4, HNO3, HCl, etc., representdilute aqueous solutions of these acids See also special tables on Solubility

REFERENCES: The information given in this table has been collected mainly from the following sources:

Mellor, A Comprehensive Treatise on Inorganic and Theoretical Chemistry, Longmans, New York, 1922 Abegg, Handbuch der anorganischen Chemie, S Hirzel, Leipzig, 1905 Gmelin-Kraut, Handbuch der anor-

ganischen Chemie, 7th ed., Carl Winter, Heidelberg; 8th ed., Verlag Chemie, Berlin, 1924 Friend, Textbook

of Inorganic Chemistry, Griffin, London, 1914 Winchell, Microscopic Character of Artificial Inorganic Solid Substances or Artificial Minerals, Wiley, New York, 1931 International Critical Tables, McGraw-Hill,

New York, 1926 Tables annuelles internationales de constants et donnes numeriques, McGraw-Hill, New York Annual Tables of Physical Constants and Numerical Data, National Research Council, Princeton, N.J., 1943 Comey and Hahn, A Dictionary of Chemical Solubilities, Macmillan, New York, 1921 Seidell,

Solubilities of Inorganic and Metal Organic Compounds, Van Nostrand, New York, 1940.

PHYSICAL PROPERTIES OF PURE SUBSTANCESTABLE 2-1 Physical Properties of the Elements and Inorganic Compounds*

Abbreviations Used in the Table

Formula Color, crystalline form Specific Melting Boiling Solubility in 100 partsName Formula weight and refractive index gravity point, °C point, °C Cold water Hot water Other reagents

subl 178

oxide (corundum) Al2O3 wh., trig., 1.768 4.00 1999 to 2032 2210 i i v sl s a., alk

*By N A Lange, Ph.D., Handbook Publishers, Inc., Sandusky, Ohio Abridged from table of Physical Constants of Inorganic Compounds in Lange’s Handbook of Chemistry.

26.98204.11162.08266.69374.78143.96133.34241.43101.99294.0678.00375.1381.98101.96101.96121.95

TABLE 2-1 Physical Properties of the Elements and Inorganic Compounds (Continued)

Formula Color, crystalline form Specific Melting Boiling Solubility in 100 partsName Formula weight and refractive index gravity point, °C point, °C Cold water Hot water Other reagents

Aluminum (Cont.)

potassium silicate (muscovite) 3Al2O3K2O6SiO2· mn., 1.590 2.9 d i

2H2Opotassium silicate (orthoclase) Al2O3K2O6SiO2 col., mn., 1.524 2.56 1450 (1150) i

24H2Opotassium (kalinite) Al2(SO4)3K2SO4 col., mn., 1.4564 1.7626°

4 92 −18H2O, 64.5 5.70° ∞93°

24H2Opotassium chrome Cr2(SO4)3K2SO4 red or gn., cb., 1.4814 1.83 89 20 50 i al

24H2Osodium Al2(SO4)3Na2SO4 col., oct., 1.4388 1.675 20°

24H2OAmmonia† NH3 col gas, 1.325 (lq.) 0.817−79° −77.7 −33.4 89.90° 7.496° 14.820°al.; s et

0.5971 (A)

4 subl 542 6810° 145.6100° s al., et., act

NH2CO2NH4‡

2NH4HCO3H2Ochloride (salammoniac) NH4Cl wh., cb., 1.639, 1.6426 1.5317° d 350 subl 520 29.40° 77.3100° s NH3; sl s al., m al

in vac

nitrate (α), stable −16° to 32° NH4NO3 col., tet., 1.611 1.6625°

perchlorate NH4ClO4 col., rhb., 1.4833 1.95 d 10.90° 46.9100° 220°al.; s act.; i et

phosphate, monobasic NH4H2PO4 col., tet., 1.5246 1.80319°

796.61556.66362.22209.94524.44342.15906.66956.69964.38948.78998.81916.5617.0377.08337.0979.0697.94114.10157.13272.2153.49443.87372.97367.50152.0744.06252.06392.1937.0457.0463.0651.1135.05196.011235.8680.0480.0464.04439.02142.11125.08117.49228.20115.03

Ammonium phosphomolybdate (NH4)3PO412MoO3 yel d 0.0315° i s alk.; i al., HNO3

3H2O (?)

sulfate (mascagnite) (NH4)2SO4 col., rhb., 1.5230 1.76920°

4 235 d 70.60° 103.3100° i al., act., CS2

thiocyanate NH4CNS col., mn., 1.685 1.305 149.6 d 170 1200° 17020° s al., act., NH3, SO2

H2SO4chloride, tri- (butter of SbCl3 col., rhb., delq 3.1420°

4 73.4 220.2 601.60° ∞72° s al., HCl, HBr,

oxide, tri- (valentinite) Sb2O3 rhb., 2.35 5.67 656 1570 v sl s sl s s HCl, KOH, H2C4H4O6

sulfide, tri- (stibnite) Sb2S3 bk., rhb., 4.046 4.64 550 0.0001718° d s HCl; alk., NH4HS,

K2S; i ac

Antimonyl potassium tartrate

(tartar emetic) (SbO)KC4H4O6aH2O wh., rhb 2.60 −aH2O, 100 5.268.7° 35.7100° s gly.; i al

1.402−185.7°;1.38 (A)

aq Cl2, h alk

sulfide, di- (realgar) As2S2 red, mn., 2.68 (α)3.50619°; (α)tr 267; 565 i d s K2S, NaHCO3

(β)3.25419° (β)307

Arsenious chloride (butter of

oxide (arsenolite) As2O3 col., cb., fibrous, 1.755 3.86525°

i al., et

NH3

Cf also under Gold

acetate Ba(C2H3O2)2H2O wh., tri pr., 1.517 2.19 −H2O, 41 7530°(anh.) 7940°(anh.) i al

*Usually the solution

†See special tables

‡Usual commercial form

132.06388.041930.39178.15114.12132.14115.1168.14196.40134.1699.11184.1576.12116.98121.76228.12291.52291.52339.72403.85626.32333.94371.58683.2039.95

299.69299.69299.69150.95123.93265.87229.84213.97310.17181.2877.95197.84197.84197.84339.36383.11232.42222.98137.33255.42273.43297.14

TABLE 2-1 Physical Properties of the Elements and Inorganic Compounds (Continued)

Formula Color, crystalline form Specific Melting Boiling Solubility in 100 partsName Formula weight and refractive index gravity point, °C point, °C Cold water Hot water Other reagents

Barium (Cont.)

carbonate (witherite) BaCO3 wh., rhb., 1.676 4.29 tr 811 to α d 1450 0.002218° 0.0065100° s a.; i al

4 tr 925 1560 310° 59100° sl s HCl, HNO3; i al

chloride BaCl22H2O† col., mn., 1.646 3.09724°

4 −2H2O, 100 39.30° 76.8100° sl s HCl, HNO3; i al

hydroxide Ba(OH)28H2O col., mn., 1.5017 2.18816° 77.9 −8H2O, 550 5.615° v sl s al.; i et.nitrate (nitrobarite) Ba(NO3)2 col., cb., 1.572 3.24428° 592 d 5.00° 34.2100° sl s a.; i al

i NH3, act

sulfate (barite, barytes) BaSO4 col., rhb., 1.636 4.49915° 1580 d tr to mn 1149 0.0001150° 0.00028530° s conc H2SO4; 0.006,

3% HCl

Bromine Br2 rhb., or red lq 3.11920°; −7.2 58.78 4.220° 3.1330° s al., et., alk., CS2

5.87 (A)

i NH3

333.17197.34197.34197.34304.23322.24208.23208.23244.26171.34315.46261.34225.35153.33169.33313.45331.30233.31601.92448.60279.40233.39169.39233.52301.629.01208.98527.98279.89315.34485.07305.00465.96465.96465.96260.4361.8310.8155.2569.62123.67128.91159.81339.96112.41230.50266.53172.42183.32

4 d 300 0.0002625° s a., NH4salts; i alk

sulfide (greenockite) CdS yel.-or., hex., 2.506 4.58 1750100atm subl in N2, 980 0.000001 Colloidal s a.; v s NH4OH

aluminum silicate (anorthite) CaOAl2O32SiO2 tri., 1.5832 2.765 1551

4 760 1810 1250° 312105° s al., act.; sl s NH3carbonate (aragonite) CaCO3 col., rhb., 1.6809 2.93 d 825 0.001220°† 0.002100° s a., NH4Cl

carbonate (calcite) CaCO3 col., hex., 1.550 2.71125°

chloride (hydrophilite) CaCl2* wh., delq., cb, 1.52 2.15215°

4 772 >1600 59.50° 347260° s al

chloride CaCl26H2O col., trig., 1.417 1.6817° 29.92 −6H2O, 200 v s v s s al

citrate Ca3(C6H5O7)24H2O col nd −2H2O, 130 −4H2O, 185 0.08518° 0.09626° 0.006518°al

fluoride (fluorite) CaF2 wh., cb., 1.4339 3.18020° 1330 0.001618° 0.001726° sl s a

magnesium carbonate

nitrate (nitrocalcite) Ca(NO3)2 col., cb 2.36 561 1020° 376151° 1415°al.; s amyl al., NH3

Ca(OH)2

phosphate, monobasic CaH4(PO4)2H2O wh., tri 2.22016°

phosphate, dibasic CaHPO42H2O wh., mn pl 2.30616°

silicate (α) (pseudowollastonite) CaSiO3 col., pseudo hex., 2.905 1540 0.009517° s HCl

1.6150 or mn.(?)silicate (β) (wollastonite) CaSiO3 col., mn., 1.610 2.915 tr 1190 to α

sulfate (anhydrite) CaSO4 col., rhb., 1.576, or 2.96 1450(mn.) tr 1193 to rhb 0.29820° 0.1619100° s a., Na2S2O3, NH4salts

mn, 1.50

*Usual commercial form

†The solubility of CaCO3in H2O is greatly increased by increasing the amount of CO2in the H2O

228.36164.45146.43236.42308.48128.41128.41240.82208.47226.49769.54280.53334.58144.4840.08176.18158.04278.21398.07199.89100.09100.09110.98129.00219.08570.4980.10508.2978.07130.1142.0974.09215.04274.13308.29184.40216.55164.09236.15148.25150.10128.10146.1156.08216.20252.07172.09310.18198.02254.10344.18182.18116.16116.16136.14

2-12 TABLE 2-1 Physical Properties of the Elements and Inorganic Compounds (Continued)

Formula Color, crystalline form Specific Melting Boiling Solubility in 100 partsName Formula weight and refractive index gravity point, °C point, °C Cold water Hot water Other reagents

Calcium (Cont.)

sulfate (gypsum) CaSO42H2O col., mn., 1.5226 2.32 −1aH2O, 128 −2H2O, 163 0.2230° 0.25750° s a., gly., Na2S2O3,

NH4salts

sulfite CaSO32H2O wh., cr., 1.595 −2H2O, 100 d 650 0.004318° 0.002790° s H2SO3

Carbon, cf table of organic

compounds

dioxide CO2 col gas lq 1.101−87°; −56.65.2atm. subl.−78.5 179.70°cc 90.120°cc s a., alk

oxysulfide COS gas lq 1.24−87°; −138.2 −50.2760mm 1330°cc 40.330°cc v s alk., al

2.10 (A)

Chlorine Cl2 rhb., or gn.-yel gas lq 1.56−33.6°; −101.6 −34.6 1.460°; 0.5730°; s alk

chloride CrCl36H2O* vl or gn., hex pl 1.83525°

sulfate Cr2(SO4)318H2O vl., cb., 1.564 1.722° −12H2O, 100 12020° d s al

172.17214.3272.14156.17260.21210.29260.30287.92

12.0112.0112.0144.0176.1428.01

98.9260.0868.03114.98398.28397.18172.11404.30140.12568.42712.54132.91210.5770.91215.03517.90441.54116.52494.29158.36266.45108.99103.02139.05400.15373.13151.99392.18482.26662.41716.46200.19

i HNO3trioxide (chromic acid) CrO3 red, rhb 2.70 197 d 164.90° 206.7100° s H2SO4, al., et

Cobaltic chloride, purpureo Co(NH3)5Cl3 rhb 1.81925°

Cobaltous acetate Co(C2H3O2)24H2O red-vl., mn., 1.542 1.705318.7° −4H2O, 140 s s s a., al

25 86 −6H2O, 110 116.50° 17780° v s et., act

nitrate Co(NO3)26H2O red, mn., 1.4 1.88325°

25 <100 d 84.030°(anh.) 334.990° 10012.5°al.; s act.;

(anh.) sl s NH3

1.639sulfate (biebeorite) CoSO47H2O* red, mn., 1.483 1.94825°

25 96.8 −7H2O, 420 3380° s 2.58°al

acetate Cu(C2H3O2)2H2O dark gn., mn 1.882 115 240 d 7.2 20 7 al.; s et.; gly

Cu(C2H3O2)2*ammonium chloride CuCl22NH4Cl2H2O blue, tet., 1.670, 1.98 d 110 33.80° 99.380° s a

1.744

carbonate, basic (azurite) 2CuCO3Cu(OH)2 blue, mn., 1.758 3.88 d 220 i d s NH4OH, h aq

NaHCO3carbonate, basic (malachite) CuCO3Cu(OH)2 dark gn., mn., 1.875 3.9 d i d s KCN; 0.03 aq COchloride (eriochalcite) CuCl2 brn.-yel pd 3.054 498 Forms Cu2Cl2 70.70° 107.9100° 5315°al.; 6815°m al

993chloride CuCl22H2O gn., rhb., 1.684 2.3922.4° −2H2O, 110 d 110.40° 192.4100° s al.; et., NH4Cl

nitrate Cu(NO3)23H2O* blue, delq 2.0473.9° 114.5 −HNO3, 170 38140° 66680° 10012.5°al

*Usual commercial form

†Also a soluble modification

52.0099.99122.9086.0168.00274.1784.06154.9058.93170.97123.06165.29234.40267.48251.43250.44268.46109.96165.86406.05214.06240.80249.08129.84237.93291.0374.93155.00173.01281.1091.0063.55181.63199.651013.79277.47245.75344.67221.12134.45170.48374.66115.58315.56614.54465.15153.5897.56277.72241.60295.65

TABLE 2-1 Physical Properties of the Elements and Inorganic Compounds (Continued)

Formula Color, crystalline form Specific Melting Boiling Solubility in 100 partsName Formula weight and refractive index gravity point, °C point, °C Cold water Hot water Other reagents

Cupric acetate (Cont.)

sulfate (hydrocyanite) CuSO4 gn.-wh., rhb., 3.60615° d.>600 Forms CuO, 14.30° 75.4100° i al

chalcanthite) CuSO45H2O* blue, tri., 1.5368 2.28615.6°

4 −4H2O, 110 −5H2O, 250 24.30° 205100° 1.18°al

1.45

sl s NH3

Cyanogen C2N2 poisonous gas lq 0.866−17.2°; −34.4 −20.5 45020°cc 230020°cc al.; 50018°cc et

1.806 (A)

Cyanogen compounds, cf table

of organic compounds

ammonium sulfate, cf Alum

chloride (molysite) FeCl3 bk.-brn., hex delq 2.80411° 282 315 74.40° 535.8100° v s al.; et +HCl

i al., et

3.042

magnetic iron oxide)

190.94162.20270.30859.23106.87323.06349.95159.69399.88562.02775.431662.61231.53303.59392.14126.75571.73591.43323.64181.9189.86287.9571.84

phosphate (vivianite) Fe3(PO4)28H2O blue, mn., 1.592,

sulfate (copperas) FeSO47H2O* blue-gn., mn 1.89914.8° 64 −7H2O, 300 32.80° 14950° i al

cf also under iron

Gold salts cf under Auric

1 atm., and at −11.3°and 2.5 atm

Hydrochloric acid HCl† col gas; 1.256 (lq.) 1.2680°(A) −111 −85 82.30° 56.160° s al., et

col lq., 1.254

Hydrogen H2 col gas or cb lq 0.0709−252.7° −259.1 −252.7 2.10°cc 0.8580°cc sl s Fe, Pd, Pt

0.06948 (A)

4 −0.89 151.4760mm ∞ s a., et.; i petr et

*Usual commercial form

†Usual commercial form about 31 percent

‡Usual commercial forms 3 or 30 percent

501.60131.93241.98278.0187.9187.8138.00144.09157.25309.44196.97196.97

178.494.0032.05124.1050.0668.51104.9795.06158.0781.08130.1243.03127.91145.93163.94181.96199.9780.9198.93

80.91118.9636.4636.4672.4990.5127.0320.0120.012.0234.0180.9834.0833.0369.4996.0482.07

TABLE 2-1 Physical Properties of the Elements and Inorganic Compounds (Continued)

Formula Color, crystalline form Specific Melting Boiling Solubility in 100 partsName Formula weight and refractive index gravity point, °C point, °C Cold water Hot water Other reagents

et., chl

H2SO4

Cf also under ferric and

ferrous

20 327.5 1620 i i s HNO3; i c HCl, H2SO4

4 280 19.70° 22150° s gly.; v sl s al.acetate (sugar of lead) Pb(C2H3O2)23H2O† wh., mn 2.55 −3H2O, 75 45.6415° 200100° s gly.; sl s al

Pb(OH)2H2O

2Pb(OH)2

arsenate, dibasic (schultenite) PbHAsO4 wh., mn., 1.9097 5.94 d >200 −H2O, 280 i sl s s HNO3, NaOH

1.7815

CaCl2oxide, mono (massicotite) PbO yel., rhb., 2.61 8.0

96.91114.82175.91253.81333.811120.66192.2255.8555.8555.8555.8555.85179.55195.90125.7083.93119.98119.98647.44

83.80138.91207.20325.29379.33505.44608.54584.52807.72489.07347.13453.04676.24291.24367.01267.21775.63278.11323.19546.39297.23687.61331.21430.40223.20223.20

CaCl2

sulfate (anglesite) PbSO4 wh., mn or rhb.,

1.8823 6.2 1170 0.00280° 0.005640° s conc a., NH4salts; i al

4 547 1265 1430°(2H2O) 266100° s al., act

carbonate Li2CO3 col., mn., 1.567 2.110° 618 d 1.540° 0.72100° s dil a.; i al., act., NH3

4 614 1360 670° 127.5100° 2.4815°al.; s et.1.662

4 subl.<1000 forms LiOH

phosphate, tribasic Li3PO4 wh., rhb 2.53717.5° 837 0.03418° v sl s s a., NH4Cl; i act

HNO3ammonium chloride MgCl2NH4Cl6H2O wh., rhb., delq 1.456 −4H2O, 195 16.7 s

ammonium phosphate MgNH4PO46H2O col., rhb., 1.496 1.715 d 100 0.02310° 0.019580° s a.; i al

(struvite)

ammonium sulfate MgSO4(NH4)2SO4 col., mn 1.72 >120 16.860° 130100°

(boussingaultite) 6H2O

carbonate (magnesite) MgCO3 wh., trig 1.700 3.037 d 350 0.0106 s a., aq CO2; i act., NH3carbonate (nesquehonite) MgCO33H2O col., rhb., 1.501 1.852 −H2O, 100 0.151819° d s a., aq CO2

carbonate, basic 3MgCO3Mg(OH)23H2O wh., rhb., 1.530 2.16 d 0.04 0.011 s a., NH4salts; i al.(hydromagnesite)

(chloromagnesite)

chloride (bischofite) MgCl26H2O† wh., delq., mn., 1.507 1.56 118 d d 2810° 918100° 50 al

oxide (magnesia; periclase) MgO col., cb., 1.7364 3.65 2800 3600 0.00062 s a., NH4salts; i al

0.29 et

*See also a table of alloys

†Usual commercial form

223.20685.60462.40239.20283.28303.26419.36526.46239.27323.366.94128.0586.85122.8873.8942.39281.9825.9469.977.9523.9541.9668.95122.9929.88103.93115.79331.98144.05109.94127.96104.01174.9724.31142.39214.45142.26256.79245.41360.60320.5884.31138.36365.3195.21203.3058.32100.9340.30223.21

TABLE 2-1 Physical Properties of the Elements and Inorganic Compounds (Continued)

Formula Color, crystalline form Specific Melting Boiling Solubility in 100 partsName Formula weight and refractive index gravity point, °C point, °C Cold water Hot water Other reagents

Magnesium chloride (Cont.)

phosphate, pyro- Mg2P2O73H2O wh., amor 2.56 −3H2O, 100 i sl s s a.; i al

potassium chloride (carnallite) MgCl2KCl6H2O delq., rhb., 1.475 1.6019.4°

potassium sulfate (picromerite) MgSO4K2SO46H2O mn., 1.4629 2.15 d 72 19.260° 81.775°

silicofluoride MgSiF66H2O col., trig., 1.3439 1.78817.5°

sulfate (epsom salt; epsomite) MgSO47H2O* col., rhb., 1.4554 1.68 70 d 72.40° 17840° s al

carbonate (rhodocrosite) MnCO3 rose, trig., 1.817 3.125 d 0.006525° s aq CO2, dil a.; l

NH3, al

chloride (scacchite) MnCl2 rose, delq., cb 2.97725°

4 650 1190 63.40° 123.8100° s al.; i et., NH3chloride MnCl24H2O* rose red, delq., mn 2.01 58.0 −H2O, 106; 1518° ∞ s al.; i et

hydroxide (ous) (pyrochroite) Mn(OH)2 wh., trig 3.25818° d 0.00220° i s a., NH4salts; i alk

polianite)

sulfate (ous) (szmikite) MnSO4H2O pa pink, mn., 1.595 2.87 Stable 57 to 98.4748° 79.77100°

−5; 19 d

conc H2SO4, HNO3

chloride (corrosive sublimate) HgCl2 wh., rhb., 1.859 5.44 277 304 3.60° 61.3100° 3325°99% al.; 33 et

oxide (montroydite) HgO yel or red, rhb., 2.5 11.14 d 100 0.005225° 0.041100° s a.; i al

56.30222.55276.60277.85402.72274.47171.67120.37246.4754.94173.03245.09114.95125.84197.91196.7588.95175.89287.0470.94157.8786.94151.00169.02187.03205.05223.06241.08259.09277.11398.06318.68360.40693.78271.50284.62234.60216.59921.26613.30296.65729.83259.63280.49461.19

chloride (calomel) HgCl wh., tet., 1.9733 7.150 302 383.7 0.0014 0.0007 s aq reg., Hg(NO3)2;

sl s HNO3, HCl;

i al., etc

NH3

oxide, tri- (molybdite) MoO3 col., rhb 4.5019.5° 795 subl 0.10718° 2.10679° s a., NH4OH

Molybdic acid H2MoO4H2O yel., mn 3.12415° −H2O, 70 −2H2O, 200 0.13318° 2.1370° s a., NH4OH, NH4, salts

Neon Ne col gas lq 1.204−245.9° −248.67 −245.9 2.60°cc 1.145°cc s lq O2, al., act., bz

0.674 (A)

HCl; i NH3

ammonium sulfate NiSO4(NH4)2SO4 blue-gn., mn., 1.923 2.53.5° 39.288° v sl s (NH4)2SO4

4 d 112.80° 156100° s al., et., NH4OH

4H2O

1.57

NH4OH

nitrate Ni(NO3)26H2O gn., mn 2.05 56.7 136.7 243.00° ∞56.7° s NH4OH; i abs al

oxide, mono- (bunsenite) NiO gn.-bk., cb., 2.37 7.45 Forms Ni2O3at 400 i i s a., NH4OH

*Usual commercial form

†See also Tables 2-28 and 2-280

236.04

327.49280.61417.18497.24200.5995.94166.85202.30237.75273.21143.94160.07192.14224.20161.95161.95144.2420.18239.0558.69176.78291.18394.99422.59218.50272.55320.68841.29118.70587.59170.73129.60237.69231.78182.79288.91184.76109.7297.21290.79286.8674.69258.97154.76

TABLE 2-1 Physical Properties of the Elements and Inorganic Compounds (Continued)

Formula Color, crystalline form Specific Melting Boiling Solubility in 100 partsName Formula weight and refractive index gravity point, °C point, °C Cold water Hot water Other reagents

Nickel (Cont.)

sulfate NiSO46H2O* gn mn or blue, tet., 2.07 tr 53.3 −6H2O, 280 13150° 280100° v s NH4OH, al

1.5109sulfate (morenosite) NiSO47H2O gn., rhb., 1.4893 1.948 98–100 −6H2O, 103 63.50° 117.830° s al

Nitrogen N2 col gas or cb cr 1.026−252.5° −209.86 −195.8 2.350°cc 1.5520°cc sl s al

0.808−195.8°

12.50°(D)Nitrogen oxide, mono- (ous) N2O col gas lq 1.226−89° −102.3 −90.7 130.520°cc 60.8224° s H2SO4, al

oxide, di- (ic) NO or (NO)2 col gas lq 1.269−150.2° −161 −151 7.340°cc 0.0100° 26.6 cc al.; 3.5 cc H2SO4;

lq or solidoxide, tetra- (per- or di-) NO2or (NO2)2 yel lq., col solid, 1.44820° −9.3 21.3 d s HNO3, H2SO4, chl.,

Oxygen O2 col gas or hex solid 1.14−188° −218.4 −183 4.890°cc 2.630°cc sl s al., s fused Ag

i dil a

Perchloric acid HClO42H2O* stable lq., col 1.7125°

73.6% anh

1.146 (A)

262.85280.8663.0181.03117.06127.0828.0144.0130.0160.0176.0146.0192.01108.01109.9165.4681.46190.23261.14296.59332.0432.0048.00106.42266.23177.33213.36158.45213.85211.39100.46118.47136.49191.91227.94119.94196.98194.1497.012365.7134.0070.46

H3PO4Phosphoric acid, ortho- H3PO4† col., rhb 1.83418.2° 42.35 −aH2O, 213 234026° v s s al

H3PO4

Phosphorus, red P4 red, cb 2.2020° 59043atm ign in air, 725 i i s alk.; i CS2, NH3, et.Phosphorus, yellow P4 yel., hex., 2.1168 1.8220°; lq 44.1; ign 34 280 0.0003 sl s 0.4 al.; 100010°CS2; 1.50°,

chromate (tarapacaite) K2CrO4 yel., rhb., 1.7261 2.73218° 975 58.00° 75.6100° i al

cyanide KCN wh., cb., delq., 1.410 1.5216° 634.5 s 122.2108.8° s gly.; 0.919.5°al.; 1.3 h al

ferricyanide K3Fe(CN)6 red, mn pr., 1.5689 1.84 d 334.4° 77.5100° s act.; sl s al.; i NH3ferrocyanide K4Fe(CN)63H2O yel., mn., 1.5772 1.85317° −3HO2, 70 27.812.2° 90.696.8° s act.; i NH3, al., et

*One commercial form 70 to 72 per cent

†Common commercial form 85 per cent HPO in aqueous solution

161.9879.9898.00177.9866.0082.00145.98123.90123.90123.90137.33208.24141.94153.332880.05195.08336.89265.98481.01247.11238.05239.0539.1098.14158.19250.2055.12180.03367.16288.10100.12136.17167.00119.00138.21174.24330.46122.5574.55485.99194.1981.1265.12294.18329.24422.3984.1240.1172.1756.11214.00166.00

TABLE 2-1 Physical Properties of the Elements and Inorganic Compounds (Continued)

Formula Color, crystalline form Specific Melting Boiling Solubility in 100 partsName Formula weight and refractive index gravity point, °C point, °C Cold water Hot water Other reagents

Potassium (Cont.)

nitrate (saltpeter) KNO3 col., rhb., 1.5038 2.1110.6° tr 129; 333 d 400 13.30° 246100° 0.130°al.; i et

4 d 400 0.750° 21.8100° 0.10520°m al.; i et

1.5095

phosphate, pyro- K4P2O73H2O delq 2.33 −2H2O, 180 −3H2O, 300 s v s i al

sulfate (arcanite) K2SO4 col., rhb., 1.4947 2.662 tr 588 7.350° 24.1100° i al., act., CS2

tartrate K2C4H4O6aH2O col., mn., 1.526 1.98 d 12.517.5° 278100° sl s al

thiocyanate KCNS col., delq., mn., 1.886 172.3 d 500 1770° 21720° 20.822°act.; s al

(D)

HNO3

1.5320°

hex

419.811034.70197.13222.32101.1085.10184.23128.13137.1394.20138.55158.03190.32136.09174.18212.27118.07508.31384.38204.22431.39154.28352.55174.26254.32200.34194.29120.17235.28188.1897.18190.32588.99140.91226.03385.83222.02186.21102.91209.26281.3385.47101.07101.07150.3644.96144.97162.99631.68631.68

Pb, Zn; i HF

alk.; i HF

1.412

oxide, di- (opal) SiO2xH2O iridescent, amor 2.2 1600–1750 subl 1750 i i s HF, h alk., fused CaCl2

1.487

bromide (bromyrite) AgBr pa yel., cb., 2.252 6.47325°

4 434 d 700 0.0000220° 0.00037100° 0.5118°NH4OH; s KCN,

Na2S2O3

chloride (cerargyrite) AgCl wh., cb., 2.071 5.56 455 1550 0.00008910° 0.00217100° s NH4OH, KCN; sl s

HCl

nitrate (lunar caustic) AgNO3 col., rhb., 1.744 4.35219°

4 212 444 d 1220° 952100° s gly.; v sl s al

NaOH

arsenate, acid (monobasic) NaH2AsO4H2O rhb., 1.5535 2.535 d 100 s

arsenate, acid (dibasic) Na2HAsO47H2O* col., mn., 1.4658 1.871 125 −7H2O, 100 6115° v s sl s al

arsenate, acid (dibasic) Na2HAsO412H2O mn., 1.4496 1.72 28 −12H2O, 100 5.590.1° 140.730° sl s al

borate, tetra Na2B4O75H2O col., rhb., 1.461 1.815 2262°(anh.) 52.3100°

(anh.)borate, tetra- (borax) Na2B4O710H2O* wh., mn., 1.4694 1.73 75 −10H2O, 200 1.30.5(anh) 20.380° s gly.; i abs al

(anh.)

(anh.)

1.509

*Usual commercial form

631.68128.9778.1096.1128.0928.0928.0940.10268.89169.90104.0832.1260.0860.0860.0860.08107.87187.77275.75143.32133.89169.8722.9982.03136.0881.9739.01209.07511.60424.07181.94312.01402.09169.91144.1084.0161.99120.06104.06201.22291.30381.37150.89102.89138.92105.99124.00232.10286.14

TABLE 2-1 Physical Properties of the Elements and Inorganic Compounds (Continued)

Formula Color, crystalline form Specific Melting Boiling Solubility in 100 partsName Formula weight and refractive index gravity point, °C point, °C Cold water Hot water Other reagentsSodium ammonium phosphate

(Cont.)

carbonate, sesqui- (trona) Na3H(CO3)22H2O wh., mn., 1.5073 2.112 d 130° 42100°

1.5151

(anh.) i al

s molten metal

nitrate (soda niter) NaNO3 col., trig., 1.5874 2.257 308 d 380 730° 180100° s NH3; sl s gly., al.nitrite NaNO2 pa yel., rhb 2.1680° 271 d 320 72.10° 163.2100° 0.320°et.; 0.3 abs al.;

4.420°m al.; v s NH3

NaOH

phosphate, monobasic NaH2PO4H2O* col., rhb., 1.4852 2.040 −H2O, 100 d 200 710° 39083° i al

phosphate, monobasic NaH2PO42H2O col., rhb., 1.4629 1.91 60 91.10° 30840°

phosphate, dibasic Na2HPO47H2O col., mn., 1.4424 1.679 d 18540° 2000100°

phosphate, dibasic Na2HPO412H2O col., mn., 1.4361 1.52 34.6 −12H2O, 180 4.30° 76.730° i al

phosphate, tribasic Na3PO412H2O* wh., trig., 1.4458 1.62 73.4 −11H2O, 100 28.315° ∞ i CS2

phosphate (pyrodisodium) Na2H2P2O7 col., mn., 1.510 1.862 d 220 4.50° 2140°

phosphate (pyrodisodium) Na2H2P2O76H2O col., mn., 1.4645 1.848 6.90° 3640°

potassium tartrate NaKC4H4O64H2O rhb., 1.493 1.790 70 to 80 −4H2O, 215 260° 6626° sl s al

sulfate (thenardite) Na2SO4 col., rhb., 1.477 2.698 tr 100 to mn 50° 42100° i al

226.03106.4458.44161.97342.13714.3149.01298.00298.93484.0641.9968.0124.0092.09110.11210.1440.00103.0574.44149.89185.92112.0684.9969.0061.9899.81122.44140.4677.98222.10137.99156.01268.07358.14163.94380.12407.85265.90446.06221.94330.03282.22122.06284.20184.04188.06266.73142.04142.04

sulfate (Glauber’s salt) Na2SO410H2O col., mn., 1.396 1.464 32.4 −10H2O, 100 3615° 41234° i al

chloride (tin salt) SnCl22H2O* wh., tri 2.7115.5° 37.7 d 118.70° ∞ s tart a., alk., al

Sr(OH)2

carbonate (strontianite) SrCO3 wh., rhb., 1.664 3.70 149760atm −CO2, 1350 0.001118° 0.065100° s a., NH4salts, aq CO2

chloride SrCl26H2O* wh., rhb., 1.5364 1.93317° −4H2O, 61 −6H2O, 100 1040° 19840°

hydroxide Sr(OH)28H2O* col., tet., 1.499 1.90 −7H2O in 0.900° 47.7100° s NH4Cl; i act

dry air

Sr(OH)2

sulfate (celestite) SrSO4 col., rhb., 1.6237 3.96 1580 d 0.01130° 0.011432° sl s a.; i dil H2SO4, al

4 205 d 200° 4070° sl s al., act.; i et

oxide, di- SO2 col gas lq., 1.4340°; −75.5 −10.0 22.80° 4.550° s H2SO4; al., ac

2.264 (A)

2.75 (A)

TABLE 2-1 Physical Properties of the Elements and Inorganic Compounds (Concluded)

Formula Color, crystalline form Specific Melting Boiling Solubility in 100 partsName Formula weight and refractive index gravity point, °C point, °C Cold water Hot water Other reagents

HNO3, H2SO4

Thio, cf sulfo or sulfur

Tin salts, cf stannic and stannous

i al

air

2.534–2.564

2.586oxide, di- (rutile) TiO2 col if pure, tet., 4.26 1640 d <3000 i i s H2SO4, alk

2.615

NH3, HNO3, aq reg

H2SO4

Uranyl acetate UO2(C2H3O2)22H2O yel., rhb 2.8915° −2H2O, 110 9.217° d s al., act

nitrate UO2(NO3)26H2O yel., rhb., 1.4967 2.807 60.2 118 170.30° ∞60° v s ac., al., et.; i dil., alk

4 800 d 1750 0.820° s a., alk.; i abs al

hex solid, 1.309 0.9150°(ice)

4.53 (A)

acetate Zn(C2H3O2)2 mn 1.840 242 subl in vac 3025° 44.6100° 2.825°, 16679°al

acetate Zn(C2H3O2)22H2O* wh., mn., 1.494 1.735 237 −2H2O, 100 4025° 66.6100° v s al

i act., NH3

1.650sulfate (zincosite) ZnSO4 wh., rhb., 1.669 3.7415°

sulfide (β) (sphalerite) ZnS wh., cb.; glass (?) 4.10225°

2.18–2.25

*Usual commercial form

†Cf special tables on water and steam, Tables 2-3, 2-4, 2-5, 2-185, 2-186 and 2-351 through 2-357.

:°F =9⁄ °C + 32

842.08502.22424.15330.04502.13420.1499.95217.9150.94121.85157.30192.75133.88149.88165.88181.8886.39169.33137.85173.3018.0220.029131.29

173.0488.9165.41183.50219.53225.22125.42136.32117.4499.42319.22297.5181.4181.4197.41258.17141.49161.47179.49269.56287.5897.4797.4797.47190.5191.22123.22123.22

(A), density referred to air

al., ethyl alcohol

i-, iso-, containing the group (CH3)2CH-

i., insolubleign., ignitesl-, laevorotatorylf., leafletslq., liquidm-, metamn., monoclinicn-, normal

nd., needleso-, orthoor., orangep-, parapd., powderpet., petroleum etherpl., platespr., prismsrhb., rhombics., soluble

s-, sec-, secondarysilv., silverysl., slightlysubl., sublimessym., symmetricalt-, tertiarytet., tetragonaltri., triclinicuns., unsymmetricalv., very

v s., very soluble

v sl s., very slightly solublewh., white

yel., yellow(+), right rotation

>, greater than

<, less than

∞, infinitely

This table of the physical properties includes the organic compounds of most general interest For the

properties of other organic compounds, reference must be made to larger tables in Lange’s Handbook of

Chemistry (Handbook Publishers), Handbook of Chemistry and Physics (Chemical Rubber Publishing

Co.), Van Nostrand’s Chemical Annual, International Critical Tables (McGraw-Hill), and similar works.

The molecular weights are based on the atomic weight values in “Atomic weights of the Elements

2001,” PURE Appl Chem., 75, 1107, 2003 The densities are given for the temperature indicated and

are usually referred to water at 4°C, e.g., 1.02895/4a density of 1.028 at 95° C referred to water at 4° C, the

4 being omitted when it is not clear whether the reference is to water at 4°C or at the temperature cated by the upper figure The melting and boiling points given have been selected from available data as

indi-probably the most accurate The solubility is given in grams of the substance in 100 of the solvent In the

case of gases, the solubility is often expressed in some manner as “510cc.” which indicates that, at 10°C, 5

cc of the gas are soluble in 100 of the solvent

TABLE 2-2 Physical Properties of Organic Compounds*

Abbreviations Used in the Table

302.45154.21118.1744.05132.1661.0859.07135.16179.22149.19149.1960.05102.0941.0558.08128.13120.1578.50150.1826.0496.9496.94174.1156.0672.0653.06146.14144.17108.14183.2089.0988.11240.2158.08120.9876.5299.15116.18223.23223.23197.24137.14

2-29

TABLE 2-2 Physical Properties of Organic Compounds (Continued)

cyanol

green oil

dihydrodiketoanthracene

ylenedioxybenzene

phenomide

cyclohexatriene

70.1370.1370.1370.13148.20315.4193.13129.59156.14176.21152.15136.15123.15123.15108.14193.24193.24137.14256.21208.21502.38484.36538.41310.26310.26240.21222.24150.13312.53217.05132.12148.16267.37290.31242.27182.22198.22146.19106.12121.1478.11142.18157.19176.62184.24344.36210.23122.12

212.24182.22244.24140.57242.23108.14107.15183.25178.23126.58198.26164.20247.16103.08154.25154.25196.29157.01231.13233.10207.07173.01173.01183.05183.05171.03171.03252.7354.0978.1158.1258.12116.16116.16116.16116.1674.1274.1274.1274.1273.1473.1473.14165.23165.23149.23149.23178.23178.23137.02137.02137.02144.21144.21172.26117.15

TABLE 2-2 Physical Properties of Organic Compounds (Continued)

92.5792.5792.5792.57162.27102.13102.13102.13184.02184.02184.02146.1890.1990.19142.20142.20150.22130.18130.18340.58115.20115.20115.20158.24158.24158.2456.1156.1172.1188.1188.1187.12158.19158.19163.22212.21136.23136.23200.23196.20172.26116.16144.21167.2176.1428.0168.03331.63153.8288.0060.08492.39150.22

149.23150.2290.12132.16162.14284.48147.39165.40245.88169.6194.5092.52154.59112.94127.57127.57242.66242.66140.57140.57112.56156.57156.5788.5488.54197.02202.55202.55188.65188.65144.56162.62157.55157.55171.58171.58128.56128.56108.52126.58126.58119.38893.49404.67228.29212.25167.12154.25148.16132.16134.18264.32152.23192.12154.25127.23

TABLE 2-2 Physical Properties of Organic Compounds (Continued)

164.16164.16146.14149.15113.12138.16108.14108.14108.14212.24212.2486.0970.09120.19164.2042.0443.0285.06105.9261.47165.1056.1198.1984.16100.1698.1482.14142.2099.17163.06118.6066.1070.1342.08134.22134.22240.30180.16138.25142.28158.28162.14212.25199.25198.26157.30158.28158.28306.40306.40290.35197.24225.29

332.49197.28273.37210.27298.33235.90235.90312.00258.35258.35129.24221.34205.34174.24174.24130.23130.23142.24142.24202.25278.34262.30128.94126.97162.02277.10277.10277.10277.10277.10277.10147.00147.00127.0198.96197.06197.06141.04163.00240.1184.08105.14202.2573.14165.23149.23229.30118.13188.22188.2286.13160.17160.17199.29199.29222.24154.18

TABLE 2-2 Physical Properties of Organic Compounds (Continued)

154.21214.22264.58182.26211.26168.23260.33186.27218.27212.25230.30101.19101.19146.18102.17102.17114.19174.19174.19239.3278.11310.60182.17134.22282.46165.2392.52110.97302.1130.0761.0874.12330.5088.11130.1446.0745.0881.54121.18201.24180.20165.19150.17211.30108.97116.16200.32144.2164.51122.55108.52113.1174.08140.1480.51155.97