physical properties of chemical compounds

PHYSICAL PROPERTIES OF PHYSICAL PROPERTIES OF Published on January 1, 1961 on http://pubs.acs.org | doi: 10.1021/ba-1955-0015.fw001 CHEMICAL COMPOUNDS CHEMICAL COMPOUNDS A systematic tabular presentation of accurate data A on the physical properties of 511 organic cyclic Dow compounds compiled by R R Dreisbach of the Dow Chemical Co These comprehensive and basic data were determined for specially prepared, high purity prepared, compounds In addition to the precisely measured properties the author has calculated new values for many constants based upon his new experimental values R PEPINSKY THE GROTH INSTITUT~ COLL~GE OF CHEMISTRY AND PHYSICS THE: PENNSYLVANIA STATE UNIVERSITY UNIVERSITY PARr PA • U S A Number fifteen of the Advances in Chemistry Series Number fifteen of the Advances in Chemistry Series Edited by the staff of Industrial and Engineering Chemistry Edited b y the staff of Industrial and Engineering Published June 1955 by P u b l i s h e d J u n e 1955 b y AMERICAN CHEMICAL SOCIETY A M E R I C A N C H E M I C A L SOCIETY 1155 N.W 1155 Sixteenth Street, N.W Washington, D C Washington, Published on January 1, 1961 on http://pubs.acs.org | doi: 10.1021/ba-1955-0015.fw001 Copyright 1955 by 1955 by AIIERlcAN CHEMICAL SOCIETY AMERICAN CHEMICAL SoCIETY All RightsRuerv«l AU Rightll Reserved Physical Properties Published on January 1, 1961 on http://pubs.acs.org | doi: 10.1021/ba-1955-0015.ch001 Of Chemical Compounds R R Dreisbach The Dow Chemical Co., Midland, Mich Definition of the Symbols and Parameters Used, with the Methods of Calculating the Parameters % Pur.: Mole % purity by weight F.P.! Freezing point, ° C Mol F.P 100%: Freezing point curve extrapolated to 100% purity B.P 760 mm., 100 mm., etc.: Boiling points at these pressures, ° C Pn : Pressures at 25° C., in mm P.: Pressure corresponding to temperature t in mm d 20, etc.: Density at 20° C., etc., g./ml a, b: Constants of Law of Rectilinear Diameters, dv + dL = a + bt d = density of the vapor, g./ml.; dL = density of the liquid, g./ml ng', etc.: Refractive index for the sodium line at 20° C., etc + 0.4) l)/(nfi + 2) X "c" "C": Constant of the Eykman equation, (nfi - 1)/(no X l/d = MR (obs.): Molal refraction (obs.) = (nfi (M = mol wt.) M/d = MR at 20° C MR (calc.): Molal refraction calculated from atomic refractive indices See page ADVANCES IN CHEMISTRY SERIES (nu - d/2): Refractivity intercept equals refractive index minus one half the density, both at the same temperature, 20° C D: Dielectric constant run at a frequency of 1()6 (cycles/sec.) and at 25° C unless otherwise noted When reported as data of The Dow Chemical Co., error about ±0.005 Where Reference is noted it was obtained by squaring the refractive index at 20° C Published on January 1, 1961 on http://pubs.acs.org | doi: 10.1021/ba-1955-0015.ch001 A, B, C: Constants of the Antoine vapor pressure equation for the liquid state, giving P (pressure) in mm and t (temperature) in ° C This is in the range between the temperatures as indicated These temperatures in general are the boiling point at 30 mm to a TR of 0.75 to 0.80 See method of obtaining A, B, C on page Antoine equation: log P = A - B/(t + C) A·, B*, K, c, tk, tx: Constants of the saturated vapor density equation log dy(g./ml.) = A* - B·/(t + C) to the temperature tk log dy(g./ml.) = A· - B·/(t + C) + K/(1.1 Tc - 273.2 - t) + c from temperature h to a reduced temperature, Ta, of 0.92 tk = Temperature at which it is necessary to change from the simple vapor density equation to the corrected vapor density equation in the higher ranges, ° C tk = tx + K/c and tx = (1.1 Tc - 273.2)° C A* and B· where the ls.tent heat at the atmospheric boiling point is available Vg - VL = (31381.7 X 1Hv X dt/dp)/T Where the ls.tent heat is not avails.ble use M(.1Hv)/TB = 21.0 and from this 1Hv = (TB X 21.0)/M The value 21.0 (or any other value as 21.4 say) is obtained from the nearest rels.ted compound which has a latent heat available Then proceed as in case where ls.tent heat is avails.ble for Vg value at B.P Since d = l/Vg log dY710 = A· - B·/(ta + C) at 760 mm log dY30 = A· - B·/(tao + C) at 30 mm Solve for A·, B·, since t and d at 760 mm and 30 mm and C are known A', B/, C / : Constants of the Antoine vapor pressure equation below 30 mm pressure, covering the temperature range as indicated See method of obtaining the constants on page A'·, B/*: Constants of the vapor density equation below 30 mm These two values are obtained by using the boiling point at 30 mm and the pressure at 25° C (obtained from the values A', B I, C ') and assuming that at 25 C the rels.tionship PV/RT = Then we have Vg at 25° C = RT/MP = 62,361 X (25 + 273.2)/MP Then dv = I/Vg Inserting these values of vapor density we then solve the two equations for the values of A'· and B /• as in the case of A· and B· Ac, Bc, Cc: Constants of the Antoine vapor pressure equation for the liquid state from Ta = 0.75 (or a higher Ta as indicated) to the critical temperature See method of obtaining the constants on page Cryoscopic Constants, A 0, BO: Cryoscopic constants for calculs.ting mole % purity See J Research Nall Bur Standards, 35 (1945); RP 1676 PHYSICAL PROPERTIES OF CHEMICAL COMPOUNDS t.O C.: Temperature at which a mole of the vapor occupies 22.414 liters and the vapor is in equilibrium with the liquid, in C te= B* -C (A * - log dvo) Published on January 1, 1961 on http://pubs.acs.org | doi: 10.1021/ba-1955-0015.ch001 dt/dp: Rate of change of boiling point with pressure, given by equation dt/dp = B/ [2.3026 X P X (A - log P)2Jo C./mm ~Hm: Latent heat of fusion in caL/g ~Hv: Latent heat of vaporization at the temperature designated, caL/g t.(d, e): The latent heat of vaporization at the temperature to as given by the equation ~Hv = d - et, and indicates the accuracy of thiR equation at the temperature t • ~Hv/T.: ~Iolal latent heat of vaporization at t divided by To (Equal to the molal entropy of vaporization at te.) d, e; d', e': These are parameters of the latent heat of vaporization equation, ~Hv­ (caL/g.) = d - et This is valid between the temperatures indicated It has been found that the latent heat between the boiling point at 30 mm and the boiling point at i60 mOl is almost a linear function of the temperature As seen in most cases this equation holds almost to the temperature te Above and below this the latent heat is not linear with temperature except for short intervals d.: Critical density, g./mL v.: Critical volume, ml./g to: Critical temperature, ° C See also page P mm.: Critical pressure in mill Whel'e this was not obtained from the literature it is calculated as follows (The Thomson method, private communication from George W Thomson): The critical temperature is inserted in the Antoine equation, using the A, B, and C values to calculate the critical pressure This value is too low This is then multiplied by 1.07 and is assumed to be the critical pressure In the great majority of cases, this will agree with determined values to within ±3% For high boiling compounds this value must be decreased, since in most cases there is somewhat irl'egular drift with increasing temperature, so this should be continually lowered as the boiling point becomes increasingly higher PV/RT: Compressibility at the temperature designated z = PV/RT where P = pressure in mill., V = volume in mL/mole, and R = 62361 ~Hc: Heat of combustion, kcaL/mole, gas at constant pressure, 298.16 K or 25 C ~Hf: Heat of formation, kcaL/mole, liquid at 298.16° K or 25 C ~Ff: Free energy of fOlnlation, kcal./mole, liquid at 298.16° K or 25° C ,,: Kinematic viscosity in centistokes, at temperature designated The kinematic viscosity is given by the equation log" = A" + B'/T between the temperatures indicated to an accuracy of 1% or better HoP °c., 30mm.; dt/dp; ~H,'; PV /RT: These ,'aluesat30mm are calculated from the Antoine equation using A, B, lind C It has been found that at 30 mOl in almost all Cox ChaIt Families the ratio PY /RT is negligibly different from one This, then, has been taken as olle point (the other point being the B.P at 760 mm.) from which to calculate A* and B*, always assuming the compressibility as 1.0000 at 30 mm Published on January 1, 1961 on http://pubs.acs.org | doi: 10.1021/ba-1955-0015.ch001 ADVANaS IN CHEMISTRY SHIES cp: Specific heat at constant pressure at temperature designated, cal./g K Cy: Specific heat at constant volume at temperature designated, cal./g K f, g, h, f', g', h': Parameters of the heat content equation for the liquid for the temperature ranges designated, K Cp (liquid) = f + gT + hTI m, n, 0, m', n', 0': Parameters of the heat content equation for the vapor for the temperature ranges designated, K Cp (vapor) = m + nT + oTt 'Y: Surface tension in dynes/cm., at temperature designated [PI: Parachor at the temperature designated: M('Y)'/'/(dL - dy) = [PI [PI Sugd.: Parachor from atomic and structural values &8 given by Sugden See Table The parachor value for oxygen &8 hydroxyl (alcohols) in these tables is taken &8 15 Sugden gives the values of 20 for oxygen and 30 for oxygen in esters, which does not seem to work for alcohols and phenols Exp L.l.; Exp L.u.: Explosion limits lower and upper range, % by wt Dispersion: Specific dispersion, 104(nr - nc)/d, ml./g at 25 c nr, nc = refractive index for F and Clines d = density, g./ml Flash and Fire Points, C.: Cleveland open cup (ASTM D 92-46) if not otherwise designated Closed cup (ASTM D 56-36) will be designated &8 such M Spec.: Mass Spectrograph Ultra V.: Ultraviolet X-Ray Dif.: X-Ray Diffraction Infrared: Infrared Spectrograph Solubility at 25 C., in solvents as designated Ezplanation of the methods used for calculating the variom parameter in the foregoing: A, B, C: The A, B, and C constants, except where given by the API reports, are calculated by means of the Thomson method [Chem Rev• , 38, 1-39 (1946)] using the determined boiling points at three different pressures The three formulas for this are &8 follows: (y, - YI)/(YI - YI)·(tt - tM(t - tt) =·1 - (t - tl)/(t + C) B = (Ya - YI)/(tt - tl)·(tl + C)(ta + C) and A = YI + B/(tl + C) where Yh Y2, and y, are equal to log PI, log P"~ and log Paat temperatures t l, t " and ta Unless the data for the three points are very accurate the C value can be considerably in error As a check on this method an empirical formula developed by Thomson (private communication from George W Thomson) will give a much better value of C if the data are much in error This formula is C = 239 - 0.19b The A and B values can then be readily determined from the two points given, since they are much less critical A', B', C' (for pressures below 30 mm.): Applicable when molar heats of vaporization are available at 25 C and the Antoine equation can be used to obtain the boiling point at 30 mm Let A, B, C be the constants of the usual Antoine equation valid above 30 mm and let A', B', C' be the constants of the Antoine equation 8Oughtforbelow 30 mm These two equations are taken to give the same value of the p~ure­ temperature slope at 30 mm log 30 = A - B/(tl + C) = A' - B'/(tl + C') B/(t , C)' = B'/(tl + C')2 + PHYSICAL PROPERTIES OF CHEMICAL COMPOUNDS Since PV/RT may be assumed to be 1.0000 at th the temperature corresponding to 30 mm., and is also 1.0000 at 25° C., the molar heat of vaporization at 25° C., M~Hv2, is given by M~Hv2 = 2.3026 RB' l(t2 + 273.2)/(t2 + C'»)2 where t2 = 25° C To solve for A', B', C' let g2 = M~Hv2l2.3026 R(t2 + 273.2)2 = M.1Hv2l406883 if t2 = 25 C Also g2 = B'/(t2 + C')2 Published on January 1, 1961 on http://pubs.acs.org | doi: 10.1021/ba-1955-0015.ch001 Since th t2 and all values on left hand side of equations above are known then B' and C' are readily obtained as follows: [B'j(t! + C')2)[(tl + C')2/B') = g2 (tl + C'>,/B' = say, h Then C' = (tl - ht2 )/(h - 1) and B' = g2(t + C')2 Also B' = B[(tl + C')/(tl + C»)2 A' = log 30 + B'/(t + C') since PI = 30 mm These formulas were developed with the aid of George Thomson When heal8 of vaporization at 25° C are not knoum: In this case the C' value is estimated and A' and B' are calculated from known data It was noticed that C' has a value approximately 18 higher than C when latent heats at 25° C are known By adding this increment to C we have C', thenB' from the relation for the first case B' = B [(t30 + C')/(t3o + C»)2 and then A' as in first case Ac, Bc, Cc: This method was developed by George Thomson [Chern Re1J8., 38, No.1, 23 (1946)] and is similar to the one for obtaining A', B', C' It is assumed that the parameters A, B, C of the Antoine equation are good to a T 0.75 or a higher reduced temperature, and this temperature corresponds to the 25° C in the case of A', B', C', and the critical point corresponds to the 30 mm point B/(tl + C)2.(t - tl)/(y - YI) = + (to - tl)/(tl + Cc) and Bc = (y - YI)/(t - t.)·(tl + Cc)(t + Cc); Ac = B/(t + Cc) + y where tl ° C = T 0.75, t C = critical temperature YI = log P at t l, y = log P The first equation is used to evaluate Cc, the lrecond, Bc, and the third, Ac As.qociation: The association in the vapor phase of organic acids seems to vary inversely as the temperature fOJ some acids, at least for part of the range In part of the range, and also apparently for some acids over the whole range, the association is fairly constant The association is given in these sheets by the formula ME = P - rt For instance, for acetic acid this formula would be ME = 2.225 - 0.004085 t from 0° C to 100° C From 100° C to a T of 0.92, ME = 1.85 That is to say, the vapor density as calculated by the A *, B* formula would have to be multiplied by this correction factor to take care of the association Further, if the reciprocal of the density is used as calculated to give vapor volume, it would be necessary to divide by 1.85 to get the actual vapor volume t.: Where the critical temperature has not been determined, it is calculated by Watson's equation: T./T, = 0.283(M/d.)o.18 where d = liquid density, g./ml at the boiling point, and M = molecular weight This is used for ull hydrocarbons and halohydrocarbons ADVANCES IN CHEMISTRY SERIES f, g, h, m, n, 0, etc.: For a short temperature range the equation Cp = f + gT + hTI reproduces almost exactly determined data The parameters were set up on the IBM machines using eight determined values where that many or more were available Published on January 1, 1961 on http://pubs.acs.org | doi: 10.1021/ba-1955-0015.ch001 The IB~I machines were used to set up the Antoine con8tants from determined data A preliminary C value was obtained from the equation C = 239 - O.19ta A and B were then obtained and new C values either side of the first C used and new A and B values found In each case above, the boiling points at the experimental pressures were calculated and compared with the determined boiling points Actually the value of C was generally obtained from C = 239 - O.19ta, since the determined values must be very very accurate to give better values of C Cox Chart Famllie Alkyl and halo benzene" Styrenes :J Thiaalkyl benzenes Thiophenes Alkyl naphthalenes Tetrahydronaphthalenes i Decahydronaphthalene~ Aromatic phenols Thiophenols Aromatic amine" 11 N itrobenzenf'll 10 12 13 14 15 16 Ii 18 19 20 21 22 Aromatic alcohols (Phenyl ethyl alcohols) Aromatic ketones Aromatic esters Cyclopentanes Cyclopentenes Thiacyclopentanes Thiacyclopropanes Cyclohexancs Cyclohexenep Thiacyclohexanes Miscellaneous PHYSICAL PROPERnES Of CHEMICAL COMPOUNDS Atomic Refractive Indices Used for Computing Molecular Refractive Index Published on January 1, 1961 on http://pubs.acs.org | doi: 10.1021/ba-1955-0015.ch001 All values are for the sodium line Carbon singly bound and alone Carbon singly bound Carbon double bond Carbon triple bond Carbon conjugated Hydrogen Oxygen-hydroxyl Oxygen-ethereal Oxygen-ketonic Oxygen-as ester 2.592 2.418 l.733 2.398 1.27 1.100 1.525 1.643 2.211 1.64 Sulfur-as SH Sulfur-as RSR Sulfur-as RCNS Sulfur-as RSSR Nitrogen as aliphatic primary amine as aromatic primary amine as aliphatic secondary amine as aromatic secondary amine as aliphatic tertiary amine as aromatic tertiary amine as hydroxylamine as hydrazine as aliphatic cyanide as aromatic cyanide as aliphatic oxime as primary amide as secondary amide as tertiary amide 7.69 7.97 7.91 8.11 NO as nitrites NO as nitrosoamine NO as alkyl nitrite NO as alkyl nitrate NO as nitro paraffin NO as nitro aromatic NO as nitramine Fluorine Chlorine Bromine Iodine 5.91 5.37 7.44 7.59 6:72 7.30 7.51 0.955.967 8.865 13.900 2.45 3.21 2.65 3.59 3.00 4.36 2.48 2.47 3.05 3.79 3.93 2.65 2.27 2.71 • This value for one fluorine atom attached to carbon The value 1.1 is to be used for each fluorine atom in polyfluorides Atomic and Structural Constants for Calculation of Parachor CH C H o (Alcohol) O.(Ester) N N (Nitrile) S F Cl Sugden 39.0 4.8 17.1 20.0 15.0 60.0 12.5 14.4 48.2 25.7 54.3 Sugden Br 68.0 I 91.0 Single bond Double bond 23 Triple bond 46.6 3-Membered ring 16.7 4-Membered ring 11.6 5-Membered ring 8.5 6-Membered ring 6.1 7-Membered ring Aliphatic alcohol subtract 6.0 Published on January 1, 1961 on http://pubs.acs.org | doi: 10.1021/ba-1955-0015.ch001 Published on January 1, 1961 on http://pubs.acs.org | doi: 10.1021/ba-1955-0015.ch001 Published on January 1, 1961 on http://pubs.acs.org | doi: 10.1021/ba-1955-0015.ch001 TABLE XXII 523 MISCELLANEOUS No o-Chlorobenzaldehyde NAME Mole % P u r 9 61 Ref STRUCTURAL CHO MolecuUr Formula c H C Ref, RefJ 12 19 12.39 F P IÇ F P TOOT Published on January 1, 1961 on http://pubs.acs.org | doi: 10.1021/ba-1955-0015.ch001 Pressure m m 25*C 211.89 140.40 108.63 84 31 53 1.24829 1.24320 1.23811 d 1.26865 - 00102 Ref n Index 20*C 25 30 1.56620 1.56384 1.56161 M R (Obs.) M R (Calc.) (nD-d/2) 30 m m 94.47 55 72.53 69.72 69.43 t (d.e) e to ^C_ to *C 99.25 1261 14 0.1067 I I j I tcT L _ K Surface tension dyne β/cm C Ϊ 30 40 # Parachor d g/ml v ml/g c 20 C 30 40 Sugd e 0.59201 A · 109 to Β l290_^C C PV/RT 25 C 30 m m BP Α · Ι ΐ to B*(246_*C_ 1.52895 1623 if' % A He k c a l / m A Hi AFf Viscosity centistokes to •C η Α · I 25 to B'|109 C C» A * 25 to Β·*109 C 1.85246 1823.9 -c 7.38896 1925.0 217 # # Acl 1.0000 1.0000 0.9405 0.9222 e 7.06216 1718.10 199 I to •C (B )| to (A )| v c Cryos A* consts B* SOURCE: PURIFICATION: LITERATURE 1-Dow M Spec Ultra V X-Ray Dif Infrared Solubility i n Acetone C a r b o n tet Bensene Ether n-Heptane Ethanol Water Water i n *K vap p * p u r i t y 9 39 m o l e % REFERENCES: Flash Point C F i r e Point ·Κ vap c 236.44 liq c 0.01986 269 E x p L 1.%/wt u Dispersion •c v to 31.70 30 68 68 tP] c Dielectric Ref to 19.37 e d I 109 l e l_23_6_ d'"~| 25 e» ! 109 » h' i m e AHv/T f h 0.7974 22.67 ΔΗν cal/g 25 C 30 m m BP 37.005 37.073 0.94206 n u 48.61 05615 03665 A H m cal/g 0.2718 1307.6 Density g / m l 2