Section 2 Physical and Chemical Data* Peter E. Liley, Ph.D., D.I.C., (physical and chemical data) School of Mechanical Engineering, Purdue University. George H. Thomson, AIChE Design Institute for Physical Property Data. (Tables 2-6, 2-30, 2-164, 2-193, 2-196, 2-198, 2-221) D.G. Friend, National Institutes of Standards and Technology, Boulder, CO. (Tables 2-333, 2-334, Figs. 2-25, 2-26) Thomas E. Daubert, Ph.D., Professor, Department of Chemical Engineering, The Pennsylvania State University. (Prediction and Correlation of Physical Properties) Evan Buck, M.S.Ch.E., Manager, Thermophysical Property Skill Center, Central Technology, Union Carbide Corporation. (Prediction and Correlation of Physical Properties) 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 15 to 0 C............ 2-48 2-4 Vapor Pressure of Liquid Water from 16 to 0 C......... 2-48 2-5 Vapor Pressure of Liquid Water from 0 to 100 C......... 2-49 2-6 Vapor Pressure of Inorganic and Organic Liquids......... 2-50 2-6a Alphabetical Index to Substances in Tables 2-6, 2-30, 2-164, 2-193, 2-196, 2-198, and 2-221................. 2-55 2-7 Vapor Pressures of Inorganic Compounds, up to 1 atm.... 2-57 2-8 Vapor Pressures of Organic Compounds, up to 1 atm...... 2-61 VAPOR PRESSURES OF SOLUTIONS Units Conversions........................................... 2-76 Tables and Figures 2-9 Partial Pressures of Water over Aqueous Solutions of HCl.. 2-76 2-10 Partial Pressures of HCl over Aqueous Solutions of HCl... 2-76 Vapor Pressures of H 3 PO 4 Aqueous: Partial Pressure of H 2 O Vapor (Fig. 2-1)............................... 2-77 Vapor Pressures of H 3 PO 4 Aqueous: Weight of H 2 O in Saturated Air (Fig. 2-2)............................. 2-77 2-11 Partial Pressures of H 2 O and SO 2 over Aqueous Solutions of Sulfur Dioxide.................................. 2-77 2-12 Water Partial Pressure, bar, over Aqueous Sulfuric Acid Solutions......................................... 2-78 2-13 Sulfur Trioxide Partial Pressure, bar, over Aqueous Sulfuric Acid Solutions.................................... 2-80 2-14 Sulfuric Acid Partial Pressure, bar, over Aqueous Sulfuric Acid..................................... 2-82 2-15 Total Pressure, bar, of Aqueous Sulfuric Acid Solutions.... 2-83 2-16 Partial Pressures of HNO 3 and H 2 O over Aqueous Solutions of HNO 3................................. 2-84 2-17 Partial Pressures of H 2 O and HBr over Aqueous Solutions of HBr at 20 to 55 C............................... 2-85 2-18 Partial Pressures of HI over Aqueous Solutions of HI at 25 C.......................................... 2-85 2-19 Vapor Pressures of the System: Water-Sulfuric Acid-Nitric Acid............................................ 2-85 2-20 Total Vapor Pressures of Aqueous Solutions of CH 3 COOH.. 2-85 2-21 Partial Pressures of H 2 O over Aqueous Solutions of HN 3.. 2-85 Vapor Pressure of Aqueous Diethylene Glycol Solutions (Fig. 2-3)........................................ 2-85 2-22 Mole Percentages of H 2 O over Aqueous Solutions of NH 3.. 2-86 2-23 Partial Pressures of NH 3 over Aqueous Solutions of NH 3... 2-87 * The contributions of J.K. Fink, Argonne National Laboratory; U. Grigull, Tech. Universität, Munich, Germany; and H. Sato, Keio University, Japan, are acknowledged. 2-1
2-2 PHYSICAL AND CHEMICAL DATA 2-24 Total Vapor Pressures of Aqueous Solutions of NH 3....... 2-88 2-25 Partial Pressures of H 2 O over Aqueous Solutions of Sodium Carbonate................................. 2-89 2-26 Partial Pressures of H 2 O and CH 3 OH over Aqueous Solutions of Methyl Alcohol......................... 2-89 2-27 Partial Pressures of H 2 O over Aqueous Solutions of Sodium Hydroxide................................. 2-89 WATER-VAPOR CONTENT OF GASES Chart for Gases at High Pressures.............................. 2-90 Water Content of Air (Fig. 2-4)................................ 2-90 DENSITIES OF PURE SUBSTANCES Units Conversions........................................... 2-91 Tables 2-28 Density (kg/m 3 ) of Water from 0 to 100 C............... 2-91 2-29 Density (kg/m 3 ) of Mercury from 0 to 350 C............. 2-93 2-30 Densities of Inorganic and Organic Liquids............. 2-94 DENSITIES OF AQUEOUS INORGANIC SOLUTIONS Units and Units Conversions.................................. 2-99 Additional References....................................... 2-99 Tables 2-31 Aluminum Sulfate [A1 2 (SO 4 ) 3 ]......................... 2-99 2-32 Ammonia (NH 3 ).................................... 2-99 2-33 Ammonium Acetate (CH 3 COONH 4 ).................... 2-99 2-34 Ammonium Bichromate [(NH 4 ) 2 Cr 2 O 7 ].................. 2-99 2-35 Ammonium Chloride (NH 4 Cl)......................... 2-99 2-36 Ammonium Chromate [(NH 4 ) 2 CrO 4 ].................... 2-99 2-37 Ammonium Nitrate (NH 4 NO 3 )......................... 2-99 2-38 Ammonium Sulfate [(NH 4 ) 2 SO 4 ]....................... 2-99 2-39 Arsenic Acid (H 3 A 3 O 4 )................................ 2-99 2-40 Barium Chloride (BaCl 2 ).............................. 2-100 2-41 Cadmium Nitrate [Cd(NO 3 ) 2 ].......................... 2-100 2-42 Calcium Chloride (CaCl 2 )............................. 2-100 2-43 Calcium Hydroxide [Ca(OH) 2 ]......................... 2-100 2-44 Calcium Hypochlorite (CaOCl 2 )........................ 2-100 2-45 Calcium Nitrate [Ca(NO 3 ) 2 ]........................... 2-100 2-46 Chromic Acid (CrO 3 )................................ 2-100 2-47 Chromium Chloride (CrCl 3 )........................... 2-100 2-48 Copper Nitrate [Cu(NO 3 ) 2 ]............................ 2-100 2-49 Copper Sulfate (CuSO 4 ).............................. 2-100 2-50 Cuprous Chloride (Cu 2 Cl 2 )............................ 2-100 2-51 Ferric Chloride (FeCl 3 )............................... 2-100 2-52 Ferric Sulfate [Fe 2 (SO 4 ) 3 ]............................. 2-101 2-53 Ferric Nitrate [Fe(NO 3 ) 3 ]............................. 2-101 2-54 Ferrous Sulfate (FeSO 4 ).............................. 2-101 2-55 Hydrogen Bromide (HBr)............................. 2-101 2-56 Hydrogen Cyanide (HCN)............................ 2-101 2-57 Hydrogen Chloride (HCl)............................. 2-101 2-58 Hydrogen Fluoride (HF)............................. 2-101 2-59 Hydrogen Peroxide (H 2 O 2 )............................ 2-101 2-60 Hydrofluosilic Acid (H 2 SiF 6 )........................... 2-101 2-61 Magnesium Chloride (MgCl 2 )......................... 2-101 2-62 Magnesium Sulfate (MgSO 4 ).......................... 2-101 2-63 Nickel Chloride (NiCl 2 ).............................. 2-101 2-64 Nickel Nitrate [Ni(NO 3 ) 2 ]............................. 2-101 2-65 Nickel Sulfate (NiSO 4 )............................... 2-101 2-66 Nitric Acid (HNO 3 ).................................. 2-102 2-67 Perchloric Acid (HClO 4 ).............................. 2-103 2-68 Phosphoric Acid (H 3 PO 4 )............................. 2-103 2-69 Potassium Bicarbonate (KHCO 3 )....................... 2-103 2-70 Potassium Bromide (KBr)............................. 2-103 2-71 Potassium Carbonate (K 2 CO 3 )......................... 2-104 2-72 Potassium Chromate (K 2 CrO 4 )......................... 2-104 2-73 Potassium Chlorate (KClO 3 )........................... 2-104 2-74 Potassium Chloride (KCl)............................. 2-104 2-75 Potassium Chrome Alum [K 2 Cr 2 (SO 4 ) 4 ].................. 2-104 2-76 Potassium Hydroxide (KOH).......................... 2-104 2-77 Potassium Nitrate (KNO 3 )............................ 2-104 2-78 Potassium Dichromate (K 2 Cr 2 O 7 )....................... 2-104 2-79 Potassium Sulfate (K 2 SO 4 )............................ 2-104 2-80 Potassium Sulfite (K 2 SO 3 )............................. 2-104 2-81 Sodium Acetate (NaC 2 H 3 O 2 ).......................... 2-104 2-82 Sodium Arsenate (Na 3 AsO 4 )........................... 2-104 2-83 Sodium Bichromate (Na 2 Cr 2 O 7 )........................ 2-104 2-84 Sodium Bromide (NaBr).............................. 2-104 2-85 Sodium Formate (HCOONa).......................... 2-104 2-86 Sodium Carbonate (Na 2 CO 3 ).......................... 2-105 2-87 Sodium Chlorate (NaClO 3 )............................ 2-105 2-88 Sodium Chloride (NaCl)............................. 2-105 2-89 Sodium Chromate (Na 2 CrO 4 )......................... 2-105 2-90 Sodium Hydroxide (NaOH).......................... 2-105 2-91 Sodium Nitrate (NaNO 3 )............................ 2-105 2-92 Sodium Nitrite (NaNO 2 )............................. 2-105 2-93 Sodium Silicates.................................... 2-105 2-94 Sodium Sulfate (Na 2 SO 4 )............................ 2-106 2-95 Sodium Sulfide (Na 2 S).............................. 2-106 2-96 Sodium Sulfite (Na 2 SO 3 )............................. 2-106 2-97 Sodium Thiosulfate (Na 2 S 2 O 3 )........................ 2-106 2-98 Sodium Thiosulfate Pentahydrate (Na 2 S 2 O 3 5H 2 O)........ 2-106 2-99 Stannic Chloride (SnCl 4 )............................. 2-106 2-100 Stannous Chloride (SnCl 2 )........................... 2-106 2-101 Sulfuric Acid (H 2 SO 4 )............................... 2-107 2-102 Zinc Bromide (ZnBr 2 )............................... 2-109 2-103 Zinc Chloride (ZnCl 2 )............................... 2-109 2-104 Zinc Nitrate [Zn(NO 3 ) 2 ]............................. 2-109 2-105 Zinc Sulfate (ZnSO 4 )................................ 2-109 DENSITIES OF AQUEOUS ORGANIC SOLUTIONS Units and Units Conversions.................................. 2-109 Tables 2-106 Formic Acid (HCOOH)............................. 2-109 2-107 Acetic Acid (CH 3 COOH)............................ 2-110 2-108 Oxalic Acid (H 2 C 2 O 4 )................................ 2-111 2-109 Methyl Alcohol (CH 3 OH)............................ 2-111 2-110 Ethyl Alcohol (C 2 H 5 OH)............................. 2-112 2-111 Densities of Mixtures of C 2 H 5 OH and H 2 O at 20 C....... 2-113 2-112 Specific Gravity (60 /60 F [(15.56 /15.56 C)]) of Mixtures by Volume of C 2 H 5 OH and H 2 O.............. 2-114 2-113 n-propyl Alcohol (C 3 H 7 OH).......................... 2-115 2-114 Isopropyl Alcohol (C 3 H 7 OH)......................... 2-115 2-115 Glycerol.......................................... 2-116 2-116 Hydrazine (N 2 H 4 ).................................. 2-116 2-117 Densities of Aqueous Solutions of Miscellaneous Organic Compounds....................................... 2-117 DENSITIES OF MISCELLANEOUS MATERIALS Tables 2-118 Approximate Specific Gravities and Densities of Miscellaneous Solids and Liquids..................... 2-119 2-119 Density (kg/m 3 ) of Selected Elements as a Function of Temperature..................................... 2-120 SOLUBILITIES Units Conversions........................................... 2-120 Tables 2-120 Solubilities of Inorganic Compounds in Water at Various Temperatures.............................. 2-121 2-121 Acetylene (C 2 H 2 )................................... 2-125 2-122 Air............................................... 2-125 2-123 Ammonia (NH 3 )................................... 2-125 2-124 Ammonia (NH 3 ) Low Pressures..................... 2-125 2-125 Carbon Dioxide (CO 2 )............................... 2-125 2-126 Carbon Monoxide (CO)............................. 2-125 2-127 Carbonyl Sulfide (COS)............................. 2-125 2-128 Chlorine (Cl 2 )..................................... 2-126 2-129 Chlorine Dioxide (ClO 2 )............................. 2-126 2-130 Ethane (C 2 H 6 )..................................... 2-126 2-131 Ethylene (C 2 H 4 ).................................... 2-126 2-132 Helium (He)...................................... 2-126 2-133 Hydrogen (H 2 ) Temperature........................ 2-126 2-134 Hydrogen (H 2 ) Pressure............................ 2-127 2-135 Hydrogen Chloride (HCl)............................ 2-127 2-136 Hydrogen Sulfide (H 2 S)............................. 2-127 2-137 Methane (CH 4 ).................................... 2-127 2-138 Nitrogen (N 2 ) Temperature......................... 2-127 2-139 Nitrogen (N 2 ) Pressure............................. 2-127 2-140 Oxygen (O 2 ) Temperature.......................... 2-127 2-141 Oxygen (O 2 ) Pressure.............................. 2-127 2-142 Ozone (O 3 )........................................ 2-128 2-143 Propylene (C 3 H 6 )................................... 2-128 2-144 Sulfur Dioxide (SO 2 )................................ 2-128 THERMAL EXPANSION Units Conversions........................................... 2-128 Additional References....................................... 2-128 Thermal Expansion of Gases.................................. 2-128 Tables 2-145 Linear Expansion of the Solid Elements................ 2-129
PHYSICAL AND CHEMICAL DATA 2-3 2-146 Linear Expansion of Miscellaneous Substances........... 2-130 2-147 Cubical Expansion of Liquids......................... 2-131 2-148 Cubical Expansion of Solids.......................... 2-131 JOULE-THOMSON EFFECT Units Conversions........................................... 2-132 Tables 2-149 Additional References Available for the Joule-Thomson Coefficient....................................... 2-132 2-150 Approximate Inversion-Curve Locus in Reduced Coordinates (T r = T/T c ; P r = P/P c )..................... 2-133 2-151 Joule-Thomson Data for Air.......................... 2-133 2-152 Approximate Inversion-Curve Locus for Air............. 2-133 2-153 Joule-Thomson Data for Argon....................... 2-133 2-154 Approximate Inversion-Curve Locus for Argon........... 2-134 2-155 Joule-Thomson Data for Carbon Dioxide............... 2-134 2-156 Approximate Inversion-Curve Locus for Carbon Dioxide.. 2-134 2-157 Approximate Inversion-Curve Locus for Deuterium...... 2-134 2-158 Approximate Inversion-Curve Locus for Ethane.......... 2-134 2-159 Joule-Thomson Data for Helium...................... 2-135 2-160 Approximate Inversion-Curve Locus for Normal Hydrogen.. 2-135 2-161 Approximate Inversion-Curve Locus for Methane........ 2-135 2-162 Joule-Thomson Data for Nitrogen..................... 2-135 2-163 Approximate Inversion-Curve Locus for Propane......... 2-135 CRITICAL CONSTANTS Additional References....................................... 2-136 Table 2-164 Critical Constants and Acentric Factors of Inorganic and Organic Compounds........................... 2-136 COMPRESSIBILITIES Introduction............................................... 2-140 Units Conversions........................................... 2-140 Tables 2-165 Compressibility Factors for Air........................ 2-140 2-166 Compressibility Factors for Argon..................... 2-140 2-167 Compressibility Factors for Carbon Dioxide............. 2-141 2-168 Compressibility Factors for Carbon Monoxide........... 2-141 2-169 Compressibility Factors for Ethanol.................... 2-141 2-170 Compressibility Factors for Ethylene................... 2-142 2-171 Compressibility Factors for Normal Hydrogen........... 2-142 2-172 Compressibility Factors for KLEA 60.................. 2-142 2-173 Compressibility Factors for KLEA 61.................. 2-143 2-174 Compressibility Factors for KLEA 66.................. 2-143 2-175 Compressibility Factors for Krypton................... 2-143 2-176 Compressibility Factors for Methane (R50)............. 2-144 2-177 Compressibility Factors for Methanol.................. 2-144 2-178 Compressibility Factors for Neon...................... 2-144 2-179 Compressibility Factors for Nitrogen................... 2-145 2-180 Compressibility Factors for Oxygen.................... 2-145 2-181 Compressibility Factors for Refrigerant 32.............. 2-145 2-182 Compressibility Factors for Refrigerant 123............. 2-146 2-183 Compressibility Factors for Refrigerant 124............. 2-146 2-184 Compressibility Factors for Refrigerant 134a............ 2-146 2-185 Compressibility Factors for Water Substance (fps units)... 2-147 2-186 Compressibility Factors of Water Substance (SI units)..... 2-148 2-187 Compressibility Factors for Xenon..................... 2-149 2-188 Compressibilities of Liquids.......................... 2-149 2-189 Compressibilities of Solids........................... 2-150 LATENT HEATS Units Conversions........................................... 2-150 Tables 2-190 Heats of Fusion and Vaporization of the Elements and Inorganic Compounds.............................. 2-151 2-191 Heats of Fusion of Miscellaneous Materials............. 2-153 2-192 Heats of Fusion of Organic Compounds................ 2-154 2-193 Heats of Vaporization of Inorganic and Organic Compounds 2-156 SPECIFIC HEATS OF PURE COMPOUNDS Units Conversions........................................... 2-161 Additional References....................................... 2-161 Tables 2-194 Heat Capacities of the Elements and Inorganic Compounds 2-161 2-195 Specific Heat [kj/(kg K)] of Selected Elements........... 2-169 2-196 Heat Capacities of Inorganic and Organic Liquids........ 2-170 2-197 Specific Heats of Organic Solids....................... 2-175 2-198 Heat Capacities of Inorganic and Organic Compounds in the Ideal Gas State................................ 2-178 2-199 C p /C v : Ratios of Specific Heats of Gases at 1-atm Pressure.. 2-183 2-200 Specific Heat Ratio, C p /C v, for Air..................... 2-183 SPECIFIC HEATS OF AQUEOUS SOLUTIONS Units Conversions........................................... 2-184 Additional References....................................... 2-184 Tables 2-201 Acetic Acid (at 38 C)................................ 2-184 2-202 Ammonia......................................... 2-184 2-203 Aniline (at 20 C)................................... 2-184 2-204 Copper Sulfate..................................... 2-184 2-205 Ethyl Alcohol...................................... 2-184 2-206 Glycerol.......................................... 2-184 2-207 Hydrochloric Acid.................................. 2-184 2-208 Methyl Alcohol.................................... 2-184 2-209 Nitric Acid........................................ 2-184 2-210 Phosphoric Acid.................................... 2-184 2-211 Potassium Chloride................................. 2-185 2-212 Potassium Hydroxide (at 19 C)....................... 2-185 2-213 Normal Propyl Alcohol.............................. 2-185 2-214 Sodium Carbonate.................................. 2-185 2-215 Sodium Chloride................................... 2-185 2-216 Sodium Hydroxide (at 20 C)......................... 2-185 2-217 Sulfuric Acid...................................... 2-185 2-218 Zinc Sulfate....................................... 2-185 SPECIFIC HEATS OF MISCELLANEOUS MATERIALS Tables 2-219 Specific Heats of Miscellaneous Liquids and Solids....... 2-186 2-219a Oils (Animal, Vegetable, Mineral Oils).................. 2-186 HEATS AND FREE ENERGIES OF FORMATION Units Conversions........................................... 2-186 Table 2-220 Heats and Free Energies of Formation of Inorganic Compounds...................................... 2-187 HEATS OF COMBUSTION Table 2-221 Enthalpies and Gibbs Energies of Formation, Entropies, and Net Enthalpies of Combustion of Inorganic and Organic Compounds at 298.15 K..................... 2-195 2-222 Ideal Gas Sensible Enthalpies, h T h 298 (kj/kgmol), of Combustion Products.............................. 2-199 2-223 Ideal Gas Entropies, s, kj/kgmol K, of Combustion Products......................................... 2-200 HEATS OF SOLUTION Tables 2-224 Heats of Solution of Inorganic Compounds in Water...... 2-201 2-225 Heats of Solution of Organic Compounds in Water (at Infinite Dilution and Approximately Room Temperature)........ 2-204 THERMODYNAMIC PROPERTIES Explanation of Tables........................................ 2-205 Units Conversions........................................... 2-205 Additional References....................................... 2-205 Tables 2-226 Thermophysical Properties of Saturated Acetone......... 2-206 2-227 Saturated Acetylene................................ 2-206 2-228 Saturated Air...................................... 2-207 2-229 Thermophysical Properties of Compressed Air........... 2-208 2-230 Enthalpy and Psi Functions for Ideal-Gas Air........... 2-212 Temperature-Entropy Diagram for Air (Fig. 2-5)......... 2-213 2-231 Air............................................... 2-214 2-232 Saturated Ammonia................................. 2-214 Enthalpy Log-Pressure Diagram for Ammonia (Fig. 2-6).. 2-215 Enthalpy-Concentration Diagram for Aqueous Ammonia (Fig. 2-7)........................................ 2-216 2-233 Saturated Argon (R740)............................. 2-217 2-234 Thermodynamic Properties of Compressed Argon........ 2-217 2-235 Liquid-Vapor Equilibrium Data for the Argon-Nitrogen- Oxygen System.................................... 2-218 2-236 Thermodynamic Properties of the International Standard Atmosphere...................................... 2-221 2-237 Saturated Benzene................................. 2-221 2-238 Saturated Bromine................................. 2-222 2-239 Saturated Normal Butane (R600)...................... 2-222 2-240 Superheated Normal Butane......................... 2-223
2-4 PHYSICAL AND CHEMICAL DATA 2-241 Saturated Carbon Dioxide........................... 2-224 2-242 Superheated Carbon Dioxide......................... 2-225 2-243 Saturated Carbon Monoxide.......................... 2-225 Temperature-Entropy Diagram for Carbon Monoxide (Fig. 2-8)........................................ 2-226 2-244 Thermophysical Properties of Saturated Carbon Tetrachloride..................................... 2-227 2-245 Saturated Carbon Tetrafluoride (R14).................. 2-227 2-246 Saturated Cesium.................................. 2-228 2-247 Thermophysical Properties of Saturated Chlorine........ 2-229 Enthalpy Log-Pressure Diagram for Chlorine (Fig. 2-9)... 2-230 2-248 Saturated Chloroform (R20).......................... 2-231 2-249 Saturated Decane.................................. 2-231 2-250 Saturated Normal Deuterium......................... 2-232 2-251 Saturated Deuterium Oxide.......................... 2-232 2-252 Deuterium Oxide Gas at 1-kg/cm 3 Pressure............. 2-232 2-253 Saturated Diphenyl................................. 2-233 2-254 Saturated Ethane (R170)............................ 2-233 2-255 Superheated Ethane................................ 2-234 2-256 Saturated Ethanol.................................. 2-235 Enthalpy-Concentration Diagram for Aqueous Ethyl Alcohol (Fig. 2-10)................................. 2-235 2-257 Saturated Ethylene (Ethene R1150).................. 2-236 2-258 Compressed Ethylene............................... 2-237 2-259 Saturated Fluorine................................. 2-239 2-260 Fluorine Gas at Atmospheric Pressure.................. 2-239 2-261 Flutec............................................ 2-239 2-262 Halon............................................ 2-239 2-263 Saturated Helium 3.................................. 2-239 2-264 Saturated Helium 4.................................. 2-240 2-265 Superheated Helium................................ 2-241 2-266 Helium 4 Gas at Atmospheric Pressure.................. 2-241 2-267 Saturated n-heptane................................ 2-242 2-268 Hexane........................................... 2-242 2-269 Saturated Hydrazine................................ 2-243 2-270 Saturated n-hydrogen............................... 2-243 2-271 Compressed n-hydrogen............................ 2-244 2-272 Saturated para-hydrogen............................ 2-246 2-273 Saturated Hydrogen Peroxide......................... 2-246 2-274 Hydrogen Sulfide.................................. 2-246 Enthalpy-Concentration Diagram for Aqueous Hydrogen Chloride at 1 atm (Fig. 2-11)........................ 2-247 2-275 Saturated Isobutane (R600a)......................... 2-248 2-276 Saturated Krypton.................................. 2-248 2-277 Compressed Krypton............................... 2-249 2-278 Saturated Lithium.................................. 2-249 2-279 Lithium Bromide Water Solutions.................... 2-249 2-280 Saturated Mercury.................................. 2-250 2-281 Saturated Methane................................. 2-251 Enthalpy Log-Pressure Diagram for Mercury (Fig. 2-12).. 2-252 2-282 Superheated Methane............................... 2-253 2-283 Thermophysical Properties of Saturated Methanol........ 2-254 2-284 Thermodynamic Properties of Compressed Methanol..... 2-255 2-285 Saturated Methyl Chloride........................... 2-256 2-286 Saturated Neon.................................... 2-256 2-287 Compressed Neon.................................. 2-257 2-288 Saturated Nitrogen (R728)........................... 2-257 Temperature-Entropy Diagram for Nitrogen (Fig. 2-13)... 2-258 2-289 Thermophysical Properties of Nitrogen (R728) at Atmospheric Pressure.............................. 2-259 2-290 Saturated Nitrogen Tetroxide......................... 2-259 2-291 Saturated Nitrous Oxide............................. 2-259 Mollier Diagram for Nitrous Oxide (Fig. 2-14)........... 2-260 2-292 Nonane........................................... 2-261 2-293 Octane........................................... 2-261 2-294 Saturated Oxygen (R732)............................ 2-262 Temperature-Entropy Chart for Oxygen (Fig. 2-15)....... 2-263 Enthalpy-Concentration Diagram for Oxygen-Nitrogen Mixture at 1 atm (Fig. 2-16)......................... 2-264 2-295 Pentane.......................................... 2-264 2-296 Saturated Potassium................................ 2-264 Mollier Diagram for Potassium (Fig. 2-17).............. 2-265 2-297 Saturated Propane (R290)............................ 2-266 2-298 Saturated Propylene (Propene, R1270)................. 2-267 2-299 Compressed Propylene (Propene, R1270)............... 2-268 2-300 Saturated Refrigerant 11............................. 2-269 Enthalpy Log-Pressure Diagram for Refrigerant 11 (Fig. 2-18)....................................... 2-269 2-301 Saturated Refrigerant 12............................. 2-270 2-302 Saturated Refrigerant 13............................. 2-270 Enthalpy Log-Pressure Diagram for Refrigerant 12 (Fig. 2-19)....................................... 2-271 2-303 Saturated Refrigerant 13B1.......................... 2-272 2-304 Saturated Refrigerant 21............................. 2-272 2-305 Saturated Refrigerant 22............................. 2-273 Enthalpy Log-Pressure Diagram for Refrigerant 22 (Fig. 2-20)....................................... 2-273 2-306 Thermophysical Properties of Compressed R22.......... 2-274 2-307 Saturated Refrigerant 23............................. 2-274 2-308 Thermophysical Properties of Saturated Difluoromethane (R32)........................................... 2-275 2-309 Specific Heat at Constant Pressure, Thermal Conductivity, Viscosity, and Prandtl of R32 Gas..................... 2-276 2-310 Saturated SUVA MP 39.............................. 2-276 2-311 SUVA MP 39 at Atmospheric Pressure................. 2-276 Enthalpy Log-Pressure Diagram for Refrigerant 32 (Fig. 2-21)....................................... 2-277 2-312 Thermodynamic Properties of Saturated KLEA 60....... 2-278 2-313 Thermodynamic Properties of Saturated KLEA 61....... 2-278 Enthalpy Log-Pressure Diagram for KLEA 60 (Fig. 2-22).. 2-279 Enthalpy Log-Pressure Diagram for KLEA 61 (Fig. 2-23).. 2-280 2-314 Saturated SUVA HP 62.............................. 2-281 2-315 SUVA HP 62 at Atmospheric Pressure.................. 2-281 2-316 Thermodynamic Properties of Saturated KLEA 66....... 2-281 Enthalpy Log-Pressure Diagram for KLEA 66 (Fig. 2-24)....................................... 2-282 2-317 Saturated SUVA MP 66.............................. 2-283 2-318 SUVA MP 66 at Atmospheric Pressure................. 2-283 2-319 Saturated SUVA HP 80.............................. 2-283 2-320 SUVA HP 80 at Atmospheric Pressure.................. 2-284 2-321 Saturated SUVA HP 81.............................. 2-284 2-322 SUVA HP 81 at Atmospheric Pressure.................. 2-284 2-323 Saturated Refrigerant 113............................ 2-285 2-324 Saturated Refrigerant 114............................ 2-286 2-325 Saturated Refrigerant 115............................ 2-286 2-326 Thermodynamic Properties of Refrigerant 123........... 2-287 2-327 Saturated Refrigerant 124............................ 2-287 Enthalpy Log-Pressure Diagram for Refrigerant 123 (Fig. 2-25)....................................... 2-288 2-328 Thermophysical Properties of Saturated Refrigerant 125... 2-289 2-329 Thermophysical Properties of Refrigerant 134a.......... 2-289 Enthalpy Log-Pressure Diagram for Refrigerant 125 (Fig. 2-26)....................................... 2-290 2-330 Thermophysical Properties of Compressed Gaseous Refrigerant 134a.................................. 2-291 2-331 Refrigerant 141b................................... 2-292 Enthalpy Log-Pressure Diagram for Refrigerant 134a (Fig. 2-27)....................................... 2-293 2-332 Refrigerant 142b................................... 2-294 2-333 Saturated Refrigerant R143a......................... 2-294 2-334 Saturated Refrigerant R152a......................... 2-295 2-335 Saturated Refrigerant 216............................ 2-295 2-336 Saturated Refrigerant 245............................ 2-296 2-337 Refrigerant C 318.................................. 2-296 2-338 Saturated Refrigerant 500............................ 2-297 2-339 Saturated Refrigerant 502............................ 2-297 2-340 Saturated Refrigerant 503............................ 2-298 2-341 Saturated Refrigerant 504............................ 2-298 2-342 Thermodynamic Properties of Refrigerant 507........... 2-298 2-343 Saturated Rubidium................................ 2-299 2-344 Thermophysical Properties of Saturated Seawater........ 2-299 2-345 Saturated Sodium.................................. 2-300 Mollier Diagram for Sodium (Fig. 2-28)................ 2-301 Enthalpy-Concentration Diagram for Aqueous Sodium Hydroxide at 1 atm (Fig. 2-29)....................... 2-302 2-346 Saturated Sulfur Dioxide............................. 2-302 2-347 Thermodynamic Properties of Saturated Sulfur Hexafluoride (SF 6 )................................. 2-303 Enthalpy-Concentration Diagram for Aqueous Sulfuric Acid at 1 atm (Fig. 2-30)................................ 2-303 Enthalpy Log-Pressure Diagram for Sulfur Hexafluoride (Fig. 2-31)....................................... 2-303 2-348 Saturated SUVA AC 9000............................ 2-304 2-349 Saturated Toluene.................................. 2-304 2-350 Saturated Solid/Vapor Water.......................... 2-304 2-351 Saturated Water Substance Temperature (fps units)...... 2-305 2-352 Saturated Water Substance Temperature (SI units)....... 2-306 2-353 Saturated Liquid Water Miscellaneous Properties........ 2-308 2-354 Thermodynamic Properties of Compressed Steam........ 2-309 2-355 Density, Specific Heats at Constant Pressure and at Constant Volume and Velocity of Sound for Compressed Water, 1 1000 bar, 0 150 C......................... 2-311 2-356 Specific Heat and Other Thermophysical Properties of Water Substance.................................. 2-313
PHYSICAL AND CHEMICAL DATA 2-5 2-357 Thermodynamic Properties of Water Substance along the Melting Line.................................. 2-315 2-358 Saturated Xenon................................... 2-315 2-359 Compressed Xenon................................. 2-316 2-360 Surface Tension (N/m) of Saturated Liquid Refrigerants... 2-317 2-361 Velocity of Sound (m/s) in Gaseous Refrigerants at Atmospheric Pressure.............................. 2-317 2-362 Velocity of Sound (m/s) in Saturated Liquid Refrigerants... 2-318 TRANSPORT PROPERTIES Introduction............................................... 2-318 Units Conversions........................................... 2-318 Additional References....................................... 2-318 Tables 2-363 Transport Properties of Selected Gases at Atmospheric Pressure......................................... 2-319 2-364 Viscosities of Gases: Coordinates for Use with Fig. 2-32.... 2-320 Nomograph for Determining (a) Absolute Viscosity of a Gas as a Function of Temperature Near Ambient Pressure and (b) Relative Viscosity of a Gas Compared with Air (Fig. 2-32)................................ 2-321 2-365 Viscosities of Liquids: Coordinates for Use with Fig. 2-33.. 2-322 Nomograph for Viscosities of Liquids at 1 atm (Fig. 2-33).. 2-323 2-366 Viscosity of Sucrose Solutions......................... 2-324 Nomograph for Thermal Conductivity of Organic Liquids (Fig. 2-34)....................................... 2-324 2-367 Thermal Conductivity Nomograph Coordinates.......... 2-324 2-368 Prandtl Number of Air.............................. 2-325 2-369 Prandtl Number of Liquid Refrigerants................. 2-325 2-370 Thermophysical Properties of Miscellaneous Saturated Liquids.......................................... 2-326 2-371 Diffusivities of Pairs of Gases and Vapors (1 atm)......... 2-328 2-372 Diffusivities in Liquids (25 C)........................ 2-330 2-373 Thermal Conductivities of Some Building and Insulating Materials........................................ 2-333 2-374 Thermal-Conductivity-Temperature Table for Metals..... 2-334 2-375 Thermal Conductivity of Chromium Alloys.............. 2-335 2-376 Thermal Conductivity of Some Alloys at High Temperature..................................... 2-335 2-377 Thermal Conductivities of Some Materials for Refrigeration and Building Insulation............................. 2-335 2-378 Thermal Conductivities of Insulating Materials at High Temperatures..................................... 2-335 2-379 Thermal Conductivities of Insulating Materials at Moderate Temperatures (Nusselt)............................. 2-336 2-380 Thermal Conductivities of Insulating Materials at Low Temperatures (Gröber)............................. 2-336 2-381 Thermal Diffusivity (m 2 /s) of Selected Elements......... 2-336 2-382 Thermophysical Properties of Selected Nonmetallic Solid Substances....................................... 2-337 PREDICTION AND CORRELATION OF PHYSICAL PROPERTIES Introduction............................................... 2-337 Units..................................................... 2-337 Nomenclature.............................................. 2-338 References................................................ 2-339 Pure Component Constants................................... 2-340 Critical Temperature...................................... 2-340 Critical Pressure.......................................... 2-340 Example 1 Estimate the Critical Temperature and Critical Pressure of 2-Butanol Using the Ambrose Method..................... 2-342 Example 2 Estimate the Critical Temperature and Critical Pressure of 2-Butanol, Which Has an Experimental Normal Boiling Point of 372.7 K.............................................. 2-342 Critical Volume........................................... 2-344 Example 3 Estimate the Critical Volume of 2-Butanol........... 2-344 Critical Compressibility Factor.............................. 2-344 Normal Freezing Temperature (Melting Point)................. 2-344 Normal Boiling Temperature................................ 2-344 Example 4 Estimate the Normal Boiling Point of 2-Butanol....... 2-345 Acentric Factor........................................... 2-345 Miscellaneous Characterizing Constants....................... 2-345 Vapor Pressure............................................. 2-345 Correlation Methods...................................... 2-345 Prediction Methods....................................... 2-346 Example 5 Estimate the Vapor Pressure of 1-Butene at 98 C...... 2-346 Example 6 Estimate the Vapor Pressure of Tetralin at 150 C...... 2-346 Example 7 Estimate the Vapor Pressure of Thiophene at 500 K.... 2-347 Example 8 Estimate the Vapor Pressure of Acetaldehyde at 0 C... 2-347 Ideal Gas Thermal Properties................................. 2-347 Heat Capacity, Cp o......................................... 2-347 Example 9 Using Eq. 2-48 to Estimate the Ideal Gas Heat Capacity of Acetone (C 3 H 6 O) at 600 K....................... 2-348 Enthalpy of Formation..................................... 2-348 Example 10 H f 298 of 2-Butanol............................. 2-348 Gibbs Energy of Formation................................. 2-348 Example 11 G f 298 of Phenol............................... 2-348 Entropy of Formation...................................... 2-348 Enthalpy of Vaporization and Fusion............................ 2-349 Enthalpy of Vaporization................................... 2-349 Example 12 Estimate H v of Propionaldehyde at 350 K.......... 2-350 Example 13 Estimate H v of Ethyl Acetate.................... 2-350 Example 14 Estimate H v of Ethyl Acetate at 450 K............. 2-350 Enthalpy of Fusion........................................ 2-350 Solid and Liquid Heat Capacity................................ 2-351 Solid Heat Capacity....................................... 2-351 Example 15 Estimate Solid Heat Capacity of Dinenzothiophene... 2-351 Liquid Heat Capacity...................................... 2-351 Example 16 Estimate Liquid Heat Capacity of 2-Butanol......... 2-351 Example 17 Estimate Liquid Heat Capacity of 1,4 Pentadiene.... 2-354 Density................................................... 2-355 Correlation Methods...................................... 2-355 Vapor Density Prediction................................... 2-355 Example 18 Estimate the Molar Volume of Isobutane at 155 C and 1.0 MPa Pressure..................................... 2-355 Example 19 Estimate the Molar Volume of Isobutane at 155 C and 8.6 MPa Pressure..................................... 2-357 Liquid Density Prediction.................................. 2-358 Example 20 Estimate the Density of Saturated Liquid Propane at 0 C.................................................. 2-359 Example 21 Estimate the Liquid Density of n-nonane at 104.5 C and 6.893 MPa Pressure................................... 2-360 Solid Density Prediction.................................... 2-361 Viscosity................................................... 2-361 Correlation Methods...................................... 2-362 Vapor Viscosity........................................... 2-362 Example 22 Estimate the Vapor Viscosity of Propane at 101.3 kpa and 80 C............................................... 2-363 Example 23 Estimate the Vapor Viscosity of a Mixture of Propane and Methane.................................... 2-363 Example 24 Estimate the Vapor Viscosity of Isopropyl Alcohol at 251 C and Atmospheric Pressure......................... 2-363 Example 25 Estimate the Vapor Viscosity of Carbon Dioxide at 350 K and a Total Pressure of 20 MPa........................ 2-364 Liquid Viscosity........................................... 2-365 Example 26 Estimate the Liquid Viscosity of cis-1,4- dimethylcyclohexane at 0 C................................ 2-366 Vapor and Liquid Thermal Conductivity......................... 2-367 Gases................................................... 2-367 Example 27 Estimate Thermal Conductivity for n-hexane........ 2-367 Example 28 Estimate Thermal Conductivity of Carbon Dioxide at 370 K and Low Pressure................................. 2-367 Example 29 Estimate the Thermal Conductivity of Carbon Dioxide at 370 K and 10 MPa Pressure.............................. 2-368 Example 30 Estimate Thermal Conductivity of a Mixture......... 2-368 Liquids................................................... 2-368 Example 31 Estimate Thermal Conductivity of n-octane at 373.15 K............................................... 2-368 Example 32 Estimate Thermal Conductivity of n-octane at 473.15 K............................................... 2-369 Example 33 Estimate Thermal Conductivity of n-butanol........ 2-369 Example 34 Estimate the Thermal Conductivity of n-propionaldehyde....................................... 2-369 Example 35 Estimate Thermal Conductivity of n-butanol........ 2-369 Example 36 Estimate Thermal Conductivity of a Mixture......... 2-370 Diffusivity................................................. 2-370 Gas Diffusivity........................................... 2-370 Example 37 Estimate the Diffusivity of Benzene Vapor Diffusing into Air at 30 C and 96.5 kpa Total Pressure.................. 2-370 Example 38 Estimate the Diffusivity of Hydrogen (1) in Nitrogen (2) at 60 C and 17.23 MPa................................. 2-371 Example 39 Estimate the Infinite Dilution Diffusivity of Propane (1) in Chlorobenzene (2) at 25 C............................ 2-371 Liquid Diffusivity......................................... 2-371 Surface Tension............................................. 2-372 Example 40 Estimate Surface Tension for Mercaptan............ 2-372 Example 41 Estimate Surface Tension for Isobutytic Acid........ 2-372 Example 42 Estimate Surface Tension of a Mixture............. 2-372 Example 43 Estimate Surface Tension of a Water-Methanol Mixture................................................ 2-373 Flammability Properties...................................... 2-374
GENERAL REFERENCES Considerations of reader interest, space availability, the system or systems of units employed, copyright considerations, etc., have all influenced the revision of material in previous editions for the present edition. Reference is made at numerous places to various specialized works and also, when appropriate, to more general works. A listing of general works may be useful to readers in need of further information. ASHRAE Handbook Fundamentals, IP and SI editions, ASHRAE, Atlanta, various dates; Beaton, C.F. and G.F. Hewitt, Physical Property Data for the Design Engineer, Hemisphere, New York, 1989 (394 pp.); Benedek, P. and F. Olti, Computer-Aided Chemical Thermodynamics of Gases and Liquids, Wiley, New York, 1985 (731 pp.); Daubert, T.E. and R.P. Danner, Physical and Thermodynamic Properties of Pure Chemicals, 4 vols., Hemisphere, New York, 1989 (2030 pp.); suppl. 1, 1991 (456 pp.); suppl. 2, 1992 (736 pp.); Gmehling, J., Azeotropic Data, 2 vols., VCH Weinheim, Germany, 1994 (1900 pp.); Kaye, S.M., Encyclopedia of Explosives and Related Items, U.S. Army R&D command, Dover, NJ, 1980; King, M.B., Phase Equilibrium in Mixtures, Pergamon, Oxford, 1969; Lyman, W.J., W.F. Reehl et al., Handbook of Chemical Property Estimation Methods, McGraw-Hill, N.Y., 1982 (929 pp.); Ohse, R.W., Handbook of Thermodynamic and Transport Properties of Alkali Metals, Blackwell Sci. Pubs., Oxford, England, 1985 (1020 pp.); Reid, R.C., J.M. Prausnitz et al., The Properties of Gases and Liquids, McGraw-Hill, New York, 1987 (742 pp.); Sterbacek, Z., B. Biskup et al., Calculation of Properties Using Corresponding States Methods, Elsevier, Amsterdam, 1979. Compilations of critical data include Ambrose, D., Vapor-Liquid Critical Properties, N.P.L. Teddington, Middx. rept. Chem 107, 1980 (62 pp.); Brule, M.R., L.L Lee et. al., Chem. Eng., 86, 25 (Nov. 19, 1979) 155 164; Kudchaker, A.P., G.H. Alani et al., Chem. Revs., 68 (1968) 659 735; Matthews, J.F., Chem. Revs., 72 (1972) 71 100; Reid, R.C., J.M. Prausnitz et al., The Properties of Gases and Liquids, 4th ed., McGraw-Hill, New York, 1987 (741 pp.); Ohse, R.W. and H. von Tippelskirch, High Temp. High Press., 9 (1977) 367 385; Young, D.A., Phase Diagrams of the Elements, UCRL Rept. 51902, 1975 (64 pp.); republished in expanded form by the University of California Press, 1991. Rothman, D. et al., Max Planck Inst. f. Stromungsforschung, Ber 6, 1978 (77 pp.). PUBLICATIONS ON THERMOCHEMISTRY Pedley, J.B., Thermochemical Data and Structures of Organic Compounds, 1, Thermodyn. Res. Ctr., Texas A&M Univ., 1994 (976 pp., 3000 cpds.); Frenkel, M., G.J. Kabo et al., Thermodynamics of Organic Compounds in the Gas State, 2 vols., Thermodyn. Res. Ctr., Texas A&M Univ., 1994 (1825 pp., 2000 cpds.); Barin, I., Thermochemical Data of Pure Substances, 2 vols., 2d ed., VCH Weinheim, Germany 1993 (1834 pp., 2400 substances); and Gurvich, L.V., I.V. Veyts et al., Thermodynamic Properties of Individual Substances, 3 vols., 4th ed., Hemisphere, New York, 1989, 1990, and 1993 (2520 pp.). See also 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., R.P. Danner et al., Physical and Thermodynamic Properties of Pure Chemicals: Data Compilation, extant 1995, Taylor & Francis, Bristol, PA, 1995; Database 11, N.I.S.T. 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., C.A. Davies et al., JANAF Thermochemical Tables, 3d ed., J. Phys. Chem. Ref. Data 14 suppl 1., 1986 (1896 pp.). 2-6
PHYSICAL PROPERTIES OF PURE SUBSTANCES TABLE 2-1 Physical Properties of the Elements and Inorganic Compounds* Abbreviations Used in the Table a., acid A., specific gravity with reference to air = 1 abs., absolute ac., acetic acid act., acetone al., 95 percent ethyl alcohol alk, alkali (i.e., aq. NaOH or KOH) am., amyl (C 5 H 11 ) amor., amorphous anh., anhydrous aq., aqueous or water aq. reg., aqua regia atm., atmosphere or 760 mm. of mercury pressure bk., black brn., brown bz., benzene c., cold cb., cubic cc, cubic centimeter chl., chloroform col., colorless or white conc., concentrated cr., crystals or crystalline d., decomposes D., specific gravity with reference to hydrogen = 1 d. 50, decomposes at 50 C; 50 d., melts at 50 C with decomposition delq., deliquescent dil., dilute dk., dark eff., effloresces or efflorescent et., ethyl ether expl., explodes gel., gelatinous gly., glycerol (glycerin) gn., green h., hot hex., hexagonal hyg., hygroscopic i., insoluble ign., ignites lq., liquid lt., light m. al., methyl alcohol mn., monoclinic nd., needles NH 3, liquid ammonia NH 4 OH, ammonium hydroxide solution oct., octahedral or., orange pd., powder pl., plates pr., prisms or prismatic pyr., pyridine rhb., rhombic (orthorhombic) s., soluble satd., saturated sl., slightly soln., solution subl., sublimes sulf., sulfides tart. a., tartaric acid tet., tetragonal tr., transition tri., triclinic trig., trigonal v., very vac., in vacuo vl., violet volt., volatile or volatilizes wh., white yel., yellow, soluble in all proportions <, less than >, greater than 42, about or near 42 3H 2 O, 100, loses 3 moles of water per formula weight at 100 C Formula weights are based upon the International Atomic Weights of 1941 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 biaxial 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, 5.6 18 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 distinction being made in this manner to indicate that the former is a melting point with decomposition at 82 C, while in the latter decomposition only occurs at 82 C. Where a value such as 2H 2 O, 82 is given it indicates 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, 82 15 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 5 10 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: H 2 SO 4, HNO 3, HCl, etc., represent dilute 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 anorganischen 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. Formula Color, crystalline form Specific Melting Boiling Solubility in 100 parts Name Formula weight and refractive index gravity point, C point, C Cold water Hot water Other reagents Aluminum Al 26.97 silv., cb. 2.70 20 660 2056 i. i. s. HCl, H 2 SO 4, alk. acetate, normal Al(C 2 H 3 O 2 ) 3 204.10 wh. pd. d. 200 s. d. acetate, basic Al(OH)(C 2 H 3 O 2 ) 2 162.07 wh., amor. d. i. s.a.; i. NH 4 salts bromide AlBr 3 266.72 trig. 3.01 25 4 97.5 268 s. s.al., act., CS 2 bromide AlBr 3 6H 2 O 374.82 col., delq. cr. d. 100 s. s. s. al., CS 2 carbide Al 4 C 3 143.91 yel., hex., 2.70 2.95 d. >2200 d. to CH 4 s. a.; i. act. chloride AlCl 3 133.34 wh., delq., hex. 2.44 25 4 194 5.2atm. 182.7 752mm ; 69.87 15 s. d. s. et., chl., CCl 4 ; i. bz. subl. 178 chloride AlCl 3 6H 2 O 241.44 col., delq., trig., 1.560 400 v. s. 50 al.; s. et. fluoride (fluellite) AlF 3 H 2 O 101.99 col., rhb., 1.490 2.17 d. sl. s. fluoride Al 2 F 6 7H 2 O 294.05 wh., cr. pd. 4H 2 O, 120 6H 2 O, 250 i. sl. s. hydroxide Al(OH) 3 77.99 wh., mn. 2.42 2H 2 O, 300 0.000104 18 i. s. a., alk.; i. a. nitrate Al(NO 3 ) 3 9H 2 O 375.14 rhb., delq. 73 d. 134 v. s. v. s. d. s. al., CS 2 nitride Al 2 N 2 81.96 yel., hex. 3.05 25 4 2150 4atm. d. >1400 d. slowly s. alk. d. oxide Al 2 O 3 101.94 col., hex., 1.67 8 3.99 1999 to 2032 i. i. v. sl. s. a., alk. oxide (corundum) Al 2 O 3 101.94 wh., trig., 1.768 4.00 1999 to 2032 2210 i. i. v. sl. s. a., alk. phosphate AlPO 4 121.95 col., hex. 2.59 i. i. s. a., alk.; i. ac. *By N. A. Lange, Ph.D., Handbook Publishers, Inc., Sandusky, Ohio. Abridged from table of Physical Constants of Inorganic Compounds in Lange, Handbook of Chemistry. 2-7