Ethanol

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Gas phase thermochemistry data

Go To: Top, Condensed phase thermochemistry data, Reaction thermochemistry data, Henry's Law data, References, Notes

Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Data compiled as indicated in comments:
DRB - Donald R. Burgess, Jr.
ALS - Hussein Y. Afeefy, Joel F. Liebman, and Stephen E. Stein
GT - Glushko Thermocenter, Russian Academy of Sciences, Moscow

Quantity Value Units Method Reference Comment
ΔfH°gas-234. ± 2.kJ/molAVGN/AAverage of 9 values; Individual data points
Quantity Value Units Method Reference Comment
ΔcH°gas-1366.3 ± 0.4kJ/molCmRossini, 1932Flame Calorimetry; Corresponding ΔfHºgas = -278.20 kJ/mol (simple calculation by NIST; no Washburn corrections); ALS

Constant pressure heat capacity of gas

Cp,gas (J/mol*K) Temperature (K) Reference Comment
37.1250.Thermodynamics Research Center, 1997p=1 bar. Recommended entropies and heat capacities are in close agreement with other statistically calculated values [ Zhuravlev E.Z., 1959, Chermin H.A.G., 1961, Green J.H.S., 1961, Green J.H.S., 1961, 2, Chao J., 1986, Gurvich, Veyts, et al., 1989]. Please also see Chao J., 1986, 2.; GT
41.70100.
46.94150.
52.02200.
61.46273.15
65.21 ± 0.14298.15
65.49300.
81.22400.
95.78500.
108.24600.
118.83700.
127.92800.
135.81900.
142.681000.
148.681100.
153.921200.
158.491300.
162.501400.
166.011500.
173.01750.
178.22000.
182.02250.
184.92500.
187.2750.
189.3000.

Constant pressure heat capacity of gas

Cp,gas (J/mol*K) Temperature (K) Reference Comment
51.38 ± 0.50200.Stromsoe E., 1970Experimental data [ Bennewitz K., 1938, Eucken A., 1948, Barrow G.M., 1952, Sinke G.C., 1953, Halford J.O., 1957] are collected in ref. [ Green J.H.S., 1961]. Ideal gas heat capacities are given by [ Stromsoe E., 1970] as a linear function Cp=f1*(a+bT). This expression approximates the experimental values with the average deviation of 1.09 J/mol*K. The accuracy of the experimental heat capacities [ Stromsoe E., 1970] is estimated as less than 0.3%. Please also see Green J.H.S., 1961, Counsell J.F., 1970.; GT
62.30 ± 0.54279.
62.09 ± 0.42280.
73.15350.01
75.7 ± 1.1356.55
74.57360.00
76.4 ± 1.1361.75
75.52367.9
76.00370.01
77.7 ± 1.1371.85
77.46380.00
79.8 ± 1.1387.25
80.0 ± 1.1388.85
80.40400.08
82.01410.16
83.39422.
84.10425.09
85.9 ± 1.1433.25
87.99437.
87.3 ± 1.1443.35
87.65450.08
91.11475.12
91.21476.
92.2 ± 1.1480.45
99.4 ± 1.1534.35
101.3 ± 1.1548.75
104.5 ± 1.1572.25
107.0 ± 1.1591.25

Condensed phase thermochemistry data

Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Henry's Law data, References, Notes

Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Data compiled as indicated in comments:
ALS - Hussein Y. Afeefy, Joel F. Liebman, and Stephen E. Stein
DRB - Donald R. Burgess, Jr.
DH - Eugene S. Domalski and Elizabeth D. Hearing

Quantity Value Units Method Reference Comment
ΔfH°liquid-276. ± 2.kJ/molAVGN/AAverage of 6 values; Individual data points
Quantity Value Units Method Reference Comment
ΔcH°liquid-1367.6 ± 0.3kJ/molCcbChao and Rossini, 1965see Rossini, 1934; Corresponding ΔfHºliquid = -276.9 kJ/mol (simple calculation by NIST; no Washburn corrections); ALS
ΔcH°liquid-1367.0 ± 0.42kJ/molCcbGreen, 1960Corresponding ΔfHºliquid = -277.6 kJ/mol (simple calculation by NIST; no Washburn corrections); ALS
ΔcH°liquid-1370.9kJ/molCcbParks, 1925Corresponding ΔfHºliquid = -273.6 kJ/mol (simple calculation by NIST; no Washburn corrections); ALS
ΔcH°liquid-1368.34kJ/molCcbRichards and Davis, 1920At 291 K; Corresponding ΔfHºliquid = -276.17 kJ/mol (simple calculation by NIST; no Washburn corrections); ALS
ΔcH°liquid-1368.6kJ/molCcbEmery and Benedict, 1911Corresponding ΔfHºliquid = -275.9 kJ/mol (simple calculation by NIST; no Washburn corrections); ALS
Quantity Value Units Method Reference Comment
S°liquid159.86J/mol*KN/AHaida, Suga, et al., 1977DH
S°liquid161.21J/mol*KN/AGreen J.H.S., 1961DH
S°liquid160.7J/mol*KN/AKelley, 1929DH
S°liquid177.0J/mol*KN/AParks, 1925Extrapolation below 90 K, 55.19 J/mol*K.; DH

Constant pressure heat capacity of liquid

Cp,liquid (J/mol*K) Temperature (K) Reference Comment
112.4298.15Petrov, Peshekhodov, et al., 1989T = 258.15, 278.15, 298.15, 318.15 K.; DH
111.53298.15Andreoli-Ball, Patterson, et al., 1988DH
112.36298.15Ogawa and Murakami, 1986DH
112.68298.15Tanaka, Toyama, et al., 1986DH
110.51298.15Ogawa and Murakami, 1985DH
115.9298.15Stephens and Olson, 1984T = 266 to 318 K. Cp given as 0.6011 cal/g*K.; DH
112.67298.15Zegers and Somsen, 1984DH
108.07288.15Benson and D'Arcy, 1982DH
113.75298.15Villamanan, Casanova, et al., 1982DH
112.15298.15Brown and Ziegler, 1979T = 159 to 306 K. Results as equation only.; DH
112.30298.15Vesely, Zabransky, et al., 1979DH
112.5298.15Haida, Suga, et al., 1977T = 14 to 300 K. Also glass, supercooled liquid, metastable crystal.; DH
112.30298.15Vesely, Svoboda, et al., 1977T = 298 to 318 K.; DH
112.33298.15Fortier, Benson, et al., 1976DH
112.094298.15Fortier and Benson, 1976DH
111.81298.15Pedersen, Kay, et al., 1975T = 298 to 348 K. Cp(liq) = 98.39 + 0.5368(T/K-273.25) J/mol*K (298 to 348 K).; DH
118.4313.2Paz Andrade, Paz, et al., 1970DH
97.53250.Nikolaev, Rabinovich, et al., 1967T = 80 to 250 K.; DH
112.056297.359Hwa and Ziegler, 1966T = 165 to 304 K. Unsmoothed experimental datum.; DH
112.26298.Rabinovich and Nikolaev, 1962T = 15 to 55°C.; DH
111.96298.15Green J.H.S., 1961T = 16 to 350 K.; DH
118.8316.Swietoslawski and Zielenkiewicz, 1960Mean value 21 to 66°C.; DH
114.7297.8Mazur, 1940T = 174 to 298 K. Unsmoothed experimental datum. Cp(liq) = 0.5437 + 0.001858t + 0.0000098t2 cal/g*K. Cp(298.15 K) = 114.9 J/mol*K, calculated from equation.; DH
111.7298.Bykov, 1939DH
103.3298.Ernst, Watkins, et al., 1936DH
118.72313.15Fiock, Ginnings, et al., 1931T = 40 to 110°C.; DH
109.87294.31Kelley, 1929T = 16 to 298 K. Value is unsmoothed experimental datum.; DH
106.3270.Mitsukuri and Hara, 1929T = 190 to 270 K.; DH
160.7298.1Parks, Kelley, et al., 1929Extrapolation below 90 K, 38.9 J/mol*K. Revision of previous data.; DH
113.4298.0Parks, 1925T = 87 to 298 K. Value is unsmoothed experimental datum.; DH
115.1303.Willams and Daniels, 1924T = 303 to 333 K. Equation only.; DH
102.4271.4Gibson, Parks, et al., 1920T = 85 to 271.4 K. Unsmoothed experimental datum. Data also given for the glassy state from 85.9 to 96.3 K.; DH
112.1298.von Reis, 1881T = 288 to 346 K.; DH

Reaction thermochemistry data

Go To: Top, Gas phase thermochemistry data, Condensed phase thermochemistry data, Henry's Law data, References, Notes

Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Data compiled as indicated in comments:
M - Michael M. Meot-Ner (Mautner) and Sharon G. Lias
B - John E. Bartmess
MS - José A. Martinho Simões
RCD - Robert C. Dunbar
ALS - Hussein Y. Afeefy, Joel F. Liebman, and Stephen E. Stein

Note: Please consider using the reaction search for this species. This page allows searching of all reactions involving this species. A general reaction search form is also available. Future versions of this site may rely on reaction search pages in place of the enumerated reaction displays seen below.

Reactions 1 to 50

C2H7O+ + Ethanol = (C2H7O+ • Ethanol)

By formula: C2H7O+ + C2H6O = (C2H7O+ • C2H6O)

Bond type: Hydrogen bonds of the type OH-O between organics

Quantity Value Units Method Reference Comment
ΔrH°134.kJ/molICRLarson and McMahon, 1982gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984, Keesee and Castleman, 1986; M
ΔrH°135.kJ/molICRBomse and Beauchamp, 1981gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984; M
Quantity Value Units Method Reference Comment
ΔrS°119.J/mol*KN/ALarson and McMahon, 1982gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984, Keesee and Castleman, 1986; M
ΔrS°119.J/mol*KN/ABomse and Beauchamp, 1981gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984; M
Quantity Value Units Method Reference Comment
ΔrG°98.3kJ/molICRLarson and McMahon, 1982gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984, Keesee and Castleman, 1986; M
ΔrG°99.2kJ/molICRBomse and Beauchamp, 1981gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984; M

C2H5O- + Ethanol = (C2H5O- • Ethanol)

By formula: C2H5O- + C2H6O = (C2H5O- • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°115. ± 4.2kJ/molTDEqMeot-Ner and Sieck, 1986gas phase; B,M
ΔrH°118. ± 10.kJ/molN/ACaldwell, Rozeboom, et al., 1984gas phase; Reanchored to average data from Paul and Kebarle, 1990 and Meot-ner and Sieck, 1986.; value altered from reference due to change in acidity scale; B,M
Quantity Value Units Method Reference Comment
ΔrS°112.J/mol*KPHPMSMeot-Ner and Sieck, 1986gas phase; M
ΔrS°123.J/mol*KN/ACaldwell, Rozeboom, et al., 1984gas phase; switching reaction(CH3O-)CH3OH; Entropy change calculated or estimated; re-evaluated using Meot-Ner(Mautner), 1986 and Paul and Kebarle, 1990; M
Quantity Value Units Method Reference Comment
ΔrG°82.0 ± 6.7kJ/molTDEqMeot-Ner and Sieck, 1986gas phase; B
ΔrG°79.5 ± 6.7kJ/molIMRECaldwell, Rozeboom, et al., 1984gas phase; Reanchored to average data from Paul and Kebarle, 1990 and Meot-ner and Sieck, 1986.; value altered from reference due to change in acidity scale; B,M
ΔrG°84.1kJ/molICRMcIver, Scott, et al., 1973gas phase; switching reaction(CH3O-)CH3OH, Entropy change calculated or estimated; Meot-Ner (Mautner), 1992; M

C2H5NaO (cr) + 0.5(Sulfuric Acid • 1100Water) (solution) = Ethanol (solution) + 0.5sodium sulphate (solution)

By formula: C2H5NaO (cr) + 0.5(H2O4S • 1100H2O) (solution) = C2H6O (solution) + 0.5Na2O4S (solution)

Quantity Value Units Method Reference Comment
ΔrH°-118.4 ± 3.8kJ/molRSCBlanchard, Joly, et al., 1974solvent: Sulphuric acid aqueous solution; The reaction enthalpy relies on -10.6 kJ/mol for the enthalpy of solution of EtOH(l) and on 9.97±0.04 for the enthalpy of solution of Na2SO4(cr) Blanchard, Joly, et al., 1974. A value of -490.8 ± 5.9 kJ/mol was derived in Blanchard, Joly, et al., 1974 for the enthalpy of formation. However, this value is affected by a calculation error. Also, the authors have not accounted for the acid dilution (this correction could not be made in the present database, due to lack of information). These problems were also noted in the data compilations Tel'noi and Rabinovich, 1980 and Wagman, Evans W.H., et al., 1982, where the values quoted for the enthalpy of formation, which rely on the experimental data reported in Blanchard, Joly, et al., 1974, are -410.0 ± 4.2 kJ/mol and -413.8 kJ/mol, respectively. See also comments in Liebman, Martinho Simões, et al., 1995; MS

Chlorine anion + Ethanol = (Chlorine anion • Ethanol)

By formula: Cl- + C2H6O = (Cl- • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°74.9 ± 1.7kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
ΔrH°73.6 ± 2.1kJ/molTDAsHiraoka, 1987gas phase; B,B,M
ΔrH°72.4 ± 8.4kJ/molIMRELarson and McMahon, 1984gas phase; B,M
Quantity Value Units Method Reference Comment
ΔrS°99.2J/mol*KPHPMSHiraoka and Mizuse, 1987gas phase; M
ΔrS°96.7J/mol*KN/ALarson and McMahon, 1984gas phase; switching reaction(Cl-)t-C4H9OH, Entropy change calculated or estimated; Larson and McMahon, 1984, 2; M
Quantity Value Units Method Reference Comment
ΔrG°44.56kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
ΔrG°43.9 ± 8.4kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B
ΔrG°43.9 ± 8.4kJ/molTDAsHiraoka, 1987gas phase; B
ΔrG°43.5 ± 8.4kJ/molIMRELarson and McMahon, 1984gas phase; B,M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
41.8295.ICRRiveros, 1974gas phase; switching reaction(Cl-)CH3OH; Riveros, Breda, et al., 1973; M

C2H5O- + Hydrogen cation = Ethanol

By formula: C2H5O- + H+ = C2H6O

Quantity Value Units Method Reference Comment
ΔrH°1587. ± 4.2kJ/molD-EARamond, Davico, et al., 2000gas phase; B
ΔrH°1582. ± 8.4kJ/molCIDCHaas and Harrison, 1993gas phase; Both metastable and 50 eV collision energy.; B
ΔrH°1579. ± 8.8kJ/molG+TSBartmess, Scott, et al., 1979gas phase; value altered from reference due to change in acidity scale; B
ΔrH°1586.2 ± 0.42kJ/molCIDTDeTuri and Ervin, 1999gas phase; B
Quantity Value Units Method Reference Comment
ΔrG°1559. ± 4.6kJ/molH-TSRamond, Davico, et al., 2000gas phase; B
ΔrG°1554. ± 8.8kJ/molH-TSHaas and Harrison, 1993gas phase; Both metastable and 50 eV collision energy.; B
ΔrG°1551. ± 8.4kJ/molIMREBartmess, Scott, et al., 1979gas phase; value altered from reference due to change in acidity scale; B

C2H5O+ + Ethanol = (C2H5O+ • Ethanol)

By formula: C2H5O+ + C2H6O = (C2H5O+ • C2H6O)

Bond type: Hydrogen bonds of the type OH-O between organics

Quantity Value Units Method Reference Comment
ΔrH°123.kJ/molICRLarson and McMahon, 1982gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984, Keesee and Castleman, 1986; M
Quantity Value Units Method Reference Comment
ΔrS°109.J/mol*KN/ALarson and McMahon, 1982gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984, Keesee and Castleman, 1986; M
Quantity Value Units Method Reference Comment
ΔrG°90.8kJ/molICRLarson and McMahon, 1982gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984, Keesee and Castleman, 1986; M

C3H9O+ + Ethanol = (C3H9O+ • Ethanol)

By formula: C3H9O+ + C2H6O = (C3H9O+ • C2H6O)

Bond type: Hydrogen bonds of the type OH-O between organics

Quantity Value Units Method Reference Comment
ΔrH°128.kJ/molICRLarson and McMahon, 1982gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984, Keesee and Castleman, 1986; M
Quantity Value Units Method Reference Comment
ΔrS°120.J/mol*KN/ALarson and McMahon, 1982gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984, Keesee and Castleman, 1986; M
Quantity Value Units Method Reference Comment
ΔrG°92.0kJ/molICRLarson and McMahon, 1982gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984, Keesee and Castleman, 1986; M

C4H9O- + Ethanol = (C4H9O- • Ethanol)

By formula: C4H9O- + C2H6O = (C4H9O- • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°111. ± 12.kJ/molN/ACaldwell, Rozeboom, et al., 1984gas phase; Reanchored to average data from Paul and Kebarle, 1990 and Meot-ner and Sieck, 1986.; value altered from reference due to change in acidity scale; B,M
Quantity Value Units Method Reference Comment
ΔrS°123.J/mol*KN/ACaldwell, Rozeboom, et al., 1984gas phase; switching reaction(CH3O-)CH3OH, Entropy change calculated or estimated; re-evaluated using Meot-Ner(Mautner), 1986 and Paul and Kebarle, 1990; M
Quantity Value Units Method Reference Comment
ΔrG°74.9 ± 8.4kJ/molIMRECaldwell, Rozeboom, et al., 1984gas phase; Reanchored to average data from Paul and Kebarle, 1990 and Meot-ner and Sieck, 1986.; value altered from reference due to change in acidity scale; B,M

C3H7O- + Ethanol = (C3H7O- • Ethanol)

By formula: C3H7O- + C2H6O = (C3H7O- • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°115. ± 12.kJ/molN/ACaldwell, Rozeboom, et al., 1984gas phase; Reanchored to average data from Paul and Kebarle, 1990 and Meot-ner and Sieck, 1986.; value altered from reference due to change in acidity scale; B,M
Quantity Value Units Method Reference Comment
ΔrS°123.J/mol*KN/ACaldwell, Rozeboom, et al., 1984gas phase; switching reaction(CH3O-)CH3OH, Entropy change calculated or estimated; re-evaluated using Meot-Ner(Mautner), 1986 and Paul and Kebarle, 1990; M
Quantity Value Units Method Reference Comment
ΔrG°78.2 ± 8.4kJ/molIMRECaldwell, Rozeboom, et al., 1984gas phase; Reanchored to average data from Paul and Kebarle, 1990 and Meot-ner and Sieck, 1986.; value altered from reference due to change in acidity scale; B,M

C3H9O+ + Ethanol = (C3H9O+ • Ethanol)

By formula: C3H9O+ + C2H6O = (C3H9O+ • C2H6O)

Bond type: Hydrogen bonds of the type OH-O between organics

Quantity Value Units Method Reference Comment
ΔrH°133.kJ/molICRBomse and Beauchamp, 1981gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984; M
Quantity Value Units Method Reference Comment
ΔrS°118.J/mol*KN/ABomse and Beauchamp, 1981gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984; M
Quantity Value Units Method Reference Comment
ΔrG°98.3kJ/molICRBomse and Beauchamp, 1981gas phase; switching reaction((CH3)2OH+)(CH3)2O, Entropy change calculated or estimated; Grimsrud and Kebarle, 1973, Lias, Liebman, et al., 1984; M

Fluorine anion + Ethanol = (Fluorine anion • Ethanol)

By formula: F- + C2H6O = (F- • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°135.6 ± 2.9kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
ΔrH°132. ± 8.4kJ/molIMRELarson and McMahon, 1983gas phase; B,M
ΔrH°136. ± 9.2kJ/molCIDTDeTuri and Ervin, 1999gas phase; B
Quantity Value Units Method Reference Comment
ΔrS°104.J/mol*KN/ALarson and McMahon, 1983gas phase; switching reaction(F-)H2O, Entropy change calculated or estimated; Arshadi, Yamdagni, et al., 1970; M
Quantity Value Units Method Reference Comment
ΔrG°103.5kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
ΔrG°101. ± 8.4kJ/molIMRELarson and McMahon, 1983gas phase; B,M

CN- + Ethanol = (CN- • Ethanol)

By formula: CN- + C2H6O = (CN- • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°72.8 ± 4.2kJ/molTDAsMeot-ner, 1988gas phase; B,M
ΔrH°73. ± 15.kJ/molIMRELarson and McMahon, 1987gas phase; B,M
Quantity Value Units Method Reference Comment
ΔrS°94.1J/mol*KPHPMSMeot-ner, 1988gas phase; M
ΔrS°103.J/mol*KN/ALarson and McMahon, 1987gas phase; switching reaction,Thermochemical ladder(CN-)H2O, Entropy change calculated or estimated; Payzant, Yamdagni, et al., 1971; M
Quantity Value Units Method Reference Comment
ΔrG°44.8 ± 4.2kJ/molTDAsMeot-ner, 1988gas phase; B
ΔrG°41.8 ± 9.6kJ/molIMRELarson and McMahon, 1987gas phase; B,M

Iodide + Ethanol = (Iodide • Ethanol)

By formula: I- + C2H6O = (I- • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°54.39 ± 0.84kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
ΔrH°50.6 ± 4.2kJ/molTDAsCaldwell and Kebarle, 1984gas phase; B,M
Quantity Value Units Method Reference Comment
ΔrS°79.1J/mol*KPHPMSCaldwell and Kebarle, 1984gas phase; M
Quantity Value Units Method Reference Comment
ΔrG°25.6kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
ΔrG°27. ± 4.2kJ/molTDAsCaldwell and Kebarle, 1984gas phase; B
ΔrG°25. ± 8.4kJ/molIMRETanabe, Morgon, et al., 1996gas phase; Anchored to H2O..I- of Caldwell and Kebarle, 1984; B

C3H9Si+ + Ethanol = (C3H9Si+ • Ethanol)

By formula: C3H9Si+ + C2H6O = (C3H9Si+ • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°176.kJ/molPHPMSWojtyniak and Stone, 1986gas phase; switching reaction,Thermochemical ladder(CH3)3Si+))H2O, Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°127.J/mol*KN/AWojtyniak and Stone, 1986gas phase; switching reaction,Thermochemical ladder(CH3)3Si+))H2O, Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
117.468.PHPMSWojtyniak and Stone, 1986gas phase; switching reaction,Thermochemical ladder(CH3)3Si+))H2O, Entropy change calculated or estimated; M

HS- + Ethanol = (HS- • Ethanol)

By formula: HS- + C2H6O = (HS- • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°68.20 ± 0.42kJ/molTDAsSieck and Meot-ner, 1989gas phase; B,M
ΔrH°67.8 ± 4.2kJ/molTDAsMeot-ner, 1988gas phase; B,M
Quantity Value Units Method Reference Comment
ΔrS°79.5J/mol*KPHPMSSieck and Meot-ner, 1989gas phase; M
ΔrS°82.8J/mol*KPHPMSMeot-ner, 1988gas phase; M
Quantity Value Units Method Reference Comment
ΔrG°44.4 ± 1.7kJ/molTDAsSieck and Meot-ner, 1989gas phase; B
ΔrG°43.1 ± 4.2kJ/molTDAsMeot-ner, 1988gas phase; B

C3H9Sn+ + Ethanol = (C3H9Sn+ • Ethanol)

By formula: C3H9Sn+ + C2H6O = (C3H9Sn+ • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°146.kJ/molPHPMSStone and Splinter, 1984gas phase; switching reaction((CH3)3Sn+)CH3OH, Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°135.J/mol*KN/AStone and Splinter, 1984gas phase; switching reaction((CH3)3Sn+)CH3OH, Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
74.9525.PHPMSStone and Splinter, 1984gas phase; switching reaction((CH3)3Sn+)CH3OH, Entropy change calculated or estimated; M

C5H11O- + Ethanol = (C5H11O- • Ethanol)

By formula: C5H11O- + C2H6O = (C5H11O- • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°110. ± 12.kJ/molN/ACaldwell, Rozeboom, et al., 1984gas phase; Reanchored to average data from Paul and Kebarle, 1990 and Meot-ner and Sieck, 1986.; value altered from reference due to change in acidity scale; B
Quantity Value Units Method Reference Comment
ΔrG°73.6 ± 8.4kJ/molIMRECaldwell, Rozeboom, et al., 1984gas phase; Reanchored to average data from Paul and Kebarle, 1990 and Meot-ner and Sieck, 1986.; value altered from reference due to change in acidity scale; B

(Chlorine anion • 2Ethanol) + Ethanol = (Chlorine anion • 3Ethanol)

By formula: (Cl- • 2C2H6O) + C2H6O = (Cl- • 3C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°58.2 ± 2.9kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
ΔrH°53.6 ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B,M
Quantity Value Units Method Reference Comment
ΔrS°108.J/mol*KPHPMSHiraoka and Mizuse, 1987gas phase; M
Quantity Value Units Method Reference Comment
ΔrG°21.6kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
ΔrG°21. ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B

(Chlorine anion • Ethanol) + Ethanol = (Chlorine anion • 2Ethanol)

By formula: (Cl- • C2H6O) + C2H6O = (Cl- • 2C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°64.02 ± 0.84kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
ΔrH°67.4 ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B,M
Quantity Value Units Method Reference Comment
ΔrS°108.J/mol*KPHPMSHiraoka and Mizuse, 1987gas phase; M
Quantity Value Units Method Reference Comment
ΔrG°30.7kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
ΔrG°35. ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B

(Chlorine anion • 9Ethanol) + Ethanol = (Chlorine anion • 10Ethanol)

By formula: (Cl- • 9C2H6O) + C2H6O = (Cl- • 10C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°37. ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; Estimated entropy; single temperature measurement; B,M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AHiraoka and Mizuse, 1987gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrG°5.9 ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; Estimated entropy; single temperature measurement; B

(Chlorine anion • 8Ethanol) + Ethanol = (Chlorine anion • 9Ethanol)

By formula: (Cl- • 8C2H6O) + C2H6O = (Cl- • 9C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°38. ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; Estimated entropy; single temperature measurement; B,M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AHiraoka and Mizuse, 1987gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrG°6.3 ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; Estimated entropy; single temperature measurement; B

CH6N+ + Ethanol = (CH6N+ • Ethanol)

By formula: CH6N+ + C2H6O = (CH6N+ • C2H6O)

Bond type: Hydrogen bonds of the type NH+-O between organics

Quantity Value Units Method Reference Comment
ΔrH°89.1kJ/molPHPMSMeot-Ner, 1984gas phase; Entropy change calculated or estimated; M
Quantity Value Units Method Reference Comment
ΔrS°100.J/mol*KN/AMeot-Ner, 1984gas phase; Entropy change calculated or estimated; M

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
37.496.PHPMSMeot-Ner, 1984gas phase; Entropy change calculated or estimated; M

Sodium ion (1+) + Ethanol = (Sodium ion (1+) • Ethanol)

By formula: Na+ + C2H6O = (Na+ • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°110. ± 5.4kJ/molCIDCAmicangelo and Armentrout, 2001Anchor NH3=24.41; RCD
ΔrH°102. ± 4.kJ/molCIDTArmentrout and Rodgers, 2000RCD
ΔrH°102. ± 4.kJ/molCIDTRodgers and Armentrout, 1999RCD

Free energy of reaction

ΔrG° (kJ/mol) T (K) Method Reference Comment
79.5298.IMREMcMahon and Ohanessian, 2000Anchor alanine=39.89; RCD
0.00.CIDTRodgers and Armentrout, 1999RCD

(Sodium ion (1+) • Ethanol) + Ethanol = (Sodium ion (1+) • 2Ethanol)

By formula: (Na+ • C2H6O) + C2H6O = (Na+ • 2C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°99.2 ± 6.7kJ/molCIDCAmicangelo and Armentrout, 2001Anchor NH3=24.41; RCD
ΔrH°96.7 ± 4.6kJ/molCIDCAmicangelo and Armentrout, 2001Anchor NH3=24.41; RCD
ΔrH°99.2 ± 6.7kJ/molCIDCAmicangelo and Armentrout, 2001Anchor NH3=24.41; RCD
ΔrH°97.5 ± 5.9kJ/molCIDCAmicangelo and Armentrout, 2001Anchor NH3=24.41; RCD

C2H5LiO (cr) + 0.5(Sulfuric Acid • 1100Water) (solution) = 0.5Li2O4S (solution) + Ethanol (solution)

By formula: C2H5LiO (cr) + 0.5(H2O4S • 1100H2O) (solution) = 0.5Li2O4S (solution) + C2H6O (solution)

Quantity Value Units Method Reference Comment
ΔrH°-113.6 ± 1.3kJ/molRSCBlanchard, Joly, et al., 1974solvent: Sulphuric acid aqueous solution; The reaction enthalpy relies on -10.6 kJ/mol for the enthalpy of solution of EtOH(l) and on -17.5±0.3 for the enthalpy of solution of Li2SO4(cr) Blanchard, Joly, et al., 1974.; MS

C2H5KO (cr) + 0.5(Sulfuric Acid • 1100Water) (solution) = Ethanol (solution) + 0.5K2O4S (solution)

By formula: C2H5KO (cr) + 0.5(H2O4S • 1100H2O) (solution) = C2H6O (solution) + 0.5K2O4S (solution)

Quantity Value Units Method Reference Comment
ΔrH°-132.3 ± 2.9kJ/molRSCBlanchard, Joly, et al., 1974solvent: Sulphuric acid aqueous solution; The reaction enthalpy relies on -10.6 kJ/mol for the enthalpy of solution of EtOH(l) and on 35.1±0.1 for the enthalpy of solution of K2SO4(cr) Blanchard, Joly, et al., 1974.; MS

Bromine anion + Ethanol = C2H6BrO-

By formula: Br- + C2H6O = C2H6BrO-

Quantity Value Units Method Reference Comment
ΔrH°58.99 ± 0.84kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
Quantity Value Units Method Reference Comment
ΔrG°34.3kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
ΔrG°37. ± 8.4kJ/molIMRETanabe, Morgon, et al., 1996gas phase; Anchored to H2O..Br- of Hiraoka, Mizure, et al., 19882; B

Hydrogen + Acetaldehyde = Ethanol

By formula: H2 + C2H4O = C2H6O

Quantity Value Units Method Reference Comment
ΔrH°-81.3 ± 1.4kJ/molChydWiberg, Crocker, et al., 1991liquid phase; solvent: Triglyme; ALS
ΔrH°-69.08 ± 0.42kJ/molChydDolliver, Gresham, et al., 1938gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -70.1 ± 0.4 kJ/mol; At 355 °K; ALS

(Chlorine anion • 3Ethanol) + Ethanol = (Chlorine anion • 4Ethanol)

By formula: (Cl- • 3C2H6O) + C2H6O = (Cl- • 4C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°50.2 ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B,M
Quantity Value Units Method Reference Comment
ΔrS°123.J/mol*KPHPMSHiraoka and Mizuse, 1987gas phase; M
Quantity Value Units Method Reference Comment
ΔrG°13. ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B

(Chlorine anion • 4Ethanol) + Ethanol = (Chlorine anion • 5Ethanol)

By formula: (Cl- • 4C2H6O) + C2H6O = (Cl- • 5C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°48.1 ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B,M
Quantity Value Units Method Reference Comment
ΔrS°128.J/mol*KPHPMSHiraoka and Mizuse, 1987gas phase; M
Quantity Value Units Method Reference Comment
ΔrG°9.6 ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B

(Chlorine anion • 5Ethanol) + Ethanol = (Chlorine anion • 6Ethanol)

By formula: (Cl- • 5C2H6O) + C2H6O = (Cl- • 6C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°46.4 ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B,M
Quantity Value Units Method Reference Comment
ΔrS°130.J/mol*KPHPMSHiraoka and Mizuse, 1987gas phase; M
Quantity Value Units Method Reference Comment
ΔrG°7.5 ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B

(Chlorine anion • 6Ethanol) + Ethanol = (Chlorine anion • 7Ethanol)

By formula: (Cl- • 6C2H6O) + C2H6O = (Cl- • 7C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°41. ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B,M
Quantity Value Units Method Reference Comment
ΔrS°113.J/mol*KPHPMSHiraoka and Mizuse, 1987gas phase; M
Quantity Value Units Method Reference Comment
ΔrG°7.1 ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B

(Chlorine anion • 7Ethanol) + Ethanol = (Chlorine anion • 8Ethanol)

By formula: (Cl- • 7C2H6O) + C2H6O = (Cl- • 8C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°38. ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B,M
Quantity Value Units Method Reference Comment
ΔrS°105.J/mol*KPHPMSHiraoka and Mizuse, 1987gas phase; M
Quantity Value Units Method Reference Comment
ΔrG°6.7 ± 4.2kJ/molTDAsHiraoka and Mizuse, 1987gas phase; B

MeCO2 anion + Ethanol = (MeCO2 anion • Ethanol)

By formula: C2H3O2- + C2H6O = (C2H3O2- • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°86.6 ± 4.2kJ/molN/AMeot-Ner and Sieck, 1986gas phase; B,M
Quantity Value Units Method Reference Comment
ΔrS°122.J/mol*KPHPMSMeot-Ner and Sieck, 1986gas phase; M
Quantity Value Units Method Reference Comment
ΔrG°49.8 ± 6.7kJ/molTDAsMeot-Ner and Sieck, 1986gas phase; B

1-Propene, 2-methyl- + Ethanol = Propane, 2-ethoxy-2-methyl-

By formula: C4H8 + C2H6O = C6H14O

Quantity Value Units Method Reference Comment
ΔrH°-32.0kJ/molCmSola, Pericas, et al., 1995liquid phase; ALS
ΔrH°-32.0kJ/molKinSola, Pericas, et al., 1995liquid phase; ALS
ΔrH°-62. ± 2.kJ/molEqkIborra, Izquierdo, et al., 1989gas phase; GC; ALS

C2H4NO2- + Ethanol = C4H10NO3-

By formula: C2H4NO2- + C2H6O = C4H10NO3-

Quantity Value Units Method Reference Comment
ΔrH°73.5 ± 2.1kJ/molTDAsNieckarz, Atkins, et al., 2008gas phase; B
Quantity Value Units Method Reference Comment
ΔrG°41. ± 4.2kJ/molTDAsNieckarz, Atkins, et al., 2008gas phase; B

Iodide + 2Ethanol = C4H12IO2-

By formula: I- + 2C2H6O = C4H12IO2-

Quantity Value Units Method Reference Comment
ΔrH°43.93 ± 0.84kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
Quantity Value Units Method Reference Comment
ΔrG°18.5kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B

Bromine anion + 2Ethanol = C4H12BrO2-

By formula: Br- + 2C2H6O = C4H12BrO2-

Quantity Value Units Method Reference Comment
ΔrH°48.1 ± 2.5kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
Quantity Value Units Method Reference Comment
ΔrG°23.9kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B

Iodide + 3Ethanol = C6H18IO3-

By formula: I- + 3C2H6O = C6H18IO3-

Quantity Value Units Method Reference Comment
ΔrH°35.1 ± 2.1kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
Quantity Value Units Method Reference Comment
ΔrG°14.7kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B

Bromine anion + 3Ethanol = C6H18BrO3-

By formula: Br- + 3C2H6O = C6H18BrO3-

Quantity Value Units Method Reference Comment
ΔrH°39.7 ± 1.3kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
Quantity Value Units Method Reference Comment
ΔrG°18.3kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B

C2H6FO- + 2Ethanol = C4H12FO2-

By formula: C2H6FO- + 2C2H6O = C4H12FO2-

Quantity Value Units Method Reference Comment
ΔrH°86.2 ± 1.3kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
Quantity Value Units Method Reference Comment
ΔrG°50.63kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B

Ethanol + Propanoic acid = Propanoic acid, ethyl ester + Water

By formula: C2H6O + C3H6O2 = C5H10O2 + H2O

Quantity Value Units Method Reference Comment
ΔrH°-22.6 ± 0.42kJ/molEqkEssex and Sandholzer, 1938liquid phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -23.54 kJ/mol; ALS

C4H12FO2- + 3Ethanol = C6H18FO3-

By formula: C4H12FO2- + 3C2H6O = C6H18FO3-

Quantity Value Units Method Reference Comment
ΔrH°65.27 ± 0.42kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B
Quantity Value Units Method Reference Comment
ΔrG°34.0kJ/molTDAsBogdanov, Peschke, et al., 1999gas phase; B

phenoxide anion + Ethanol = C8H11O2-

By formula: C6H5O- + C2H6O = C8H11O2-

Quantity Value Units Method Reference Comment
ΔrH°80.8 ± 4.2kJ/molN/AMeot-Ner and Sieck, 1986gas phase; B
Quantity Value Units Method Reference Comment
ΔrG°46.9 ± 6.7kJ/molTDAsMeot-Ner and Sieck, 1986gas phase; B

phenoxide anion + Ethanol = (phenoxide anion • Ethanol)

By formula: C6H5O- + C2H6O = (C6H5O- • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°80.8kJ/molPHPMSMeot-Ner and Sieck, 1986gas phase; M
Quantity Value Units Method Reference Comment
ΔrS°113.J/mol*KPHPMSMeot-Ner and Sieck, 1986gas phase; M

4Ethanol (l) + Titanium tetrachloride (l) = titanium(4+) ethanolate (l) + 4(Hydrogen chloride • 51.3Water) (solution)

By formula: 4C2H6O (l) + Cl4Ti (l) = C8H20O4Ti (l) + 4(HCl • 51.3H2O) (solution)

Quantity Value Units Method Reference Comment
ΔrH°-205.4 ± 4.2kJ/molRSCBradley and Hillyer, 1966Please also see Pedley and Rylance, 1977.; MS

Fluorine anion + Ethanol = C2H5D6FO-

By formula: F- + C2H6O = C2H5D6FO-

Quantity Value Units Method Reference Comment
ΔrG°99.2 ± 8.4kJ/molIMREWilkinson, Szulejko, et al., 1992gas phase; Reported relative to ROH..F-, 0.5 kcal/mol weaker.; B

Magnesium ion (1+) + Ethanol = (Magnesium ion (1+) • Ethanol)

By formula: Mg+ + C2H6O = (Mg+ • C2H6O)

Quantity Value Units Method Reference Comment
ΔrH°260. ± 20.kJ/molICROperti, Tews, et al., 1988gas phase; switching reaction,Thermochemical ladder(Mg+)CH3OH; M

3Sodium hydroxide + Carbonochloridic acid, ethyl ester = CNa2O3 + Ethanol + sodium chloride + Water

By formula: 3HNaO + C3H5ClO2 = CNa2O3 + C2H6O + ClNa + H2O

Quantity Value Units Method Reference Comment
ΔrH°-323.3 ± 1.7kJ/molCmDavies, Finch, et al., 1980liquid phase; Heat of hydrolysis; ALS

Acetylimidazole diethyl acetal + Water = Ethyl Acetate + 1H-Imidazole + Ethanol

By formula: C9H16N2O2 + H2O = C4H8O2 + C3H4N2 + C2H6O

Quantity Value Units Method Reference Comment
ΔrH°-44.69 ± 0.67kJ/molCmGuthrie and Pike, 1987liquid phase; Heat of hydrolysis; ALS

Henry's Law data

Go To: Top, Gas phase thermochemistry data, Condensed phase thermochemistry data, Reaction thermochemistry data, References, Notes

Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Data compiled by: Rolf Sander

Henry's Law constant (water solution)

kH(T) = k°H exp(d(ln(kH))/d(1/T) ((1/T) - 1/(298.15 K)))
k°H = Henry's law constant for solubility in water at 298.15 K (mol/(kg*bar))
d(ln(kH))/d(1/T) = Temperature dependence constant (K)

k°H (mol/(kg*bar)) d(ln(kH))/d(1/T) (K) Method Reference Comment
120. QN/A missing citation give several references for the Henry's law constants but don't assign them to specific species.
200. XN/A 
190.6600.MN/A 
200. XN/AValue given here as quoted by missing citation.
230. MN/A 
150.6400.XN/A 
220. MN/A 
160. M,XTimmermans, 1960Value given here as quoted by missing citation.
190. MButler, Ramchandani, et al., 1935 

References

Go To: Top, Gas phase thermochemistry data, Condensed phase thermochemistry data, Reaction thermochemistry data, Henry's Law data, Notes

Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Rossini, 1932
Rossini, F.D., The heats of combustion of methyl and ethyl alcohols, J. Res. NBS, 1932, 8, 119-139. [all data]

Thermodynamics Research Center, 1997
Thermodynamics Research Center, Selected Values of Properties of Chemical Compounds., Thermodynamics Research Center, Texas A&M University, College Station, Texas, 1997. [all data]

Zhuravlev E.Z., 1959
Zhuravlev E.Z., Isotopic effect on thermodynamic functions of some organic deuterocompounds in the ideal gas state, Tr. Khim. i Khim. Tekhnol., 1959, 2, 475-485. [all data]

Chermin H.A.G., 1961
Chermin H.A.G., Thermo data for petrochemicals. Part 28. Gaseous normal alcohols. The important thermo properties are presented for all the gaseous normal alcohols from methanol through n-decanol, Petrol. Refiner, 1961, 40 (4), 127-130. [all data]

Green J.H.S., 1961
Green J.H.S., Thermodynamic properties of organic oxygen compounds. Part 5. Ethyl alcohol, Trans. Faraday Soc., 1961, 57, 2132-2137. [all data]

Green J.H.S., 1961, 2
Green J.H.S., Thermodynamic properties of the normal alcohols C1-C12, J. Appl. Chem., 1961, 11, 397-404. [all data]

Chao J., 1986
Chao J., Ideal gas thermodynamic properties of simple alkanols, Int. J. Thermophys., 1986, 7, 431-442. [all data]

Gurvich, Veyts, et al., 1989
Gurvich, L.V.; Veyts, I.V.; Alcock, C.B., Thermodynamic Properties of Individual Substances, 4th ed.; Vols. 1 and 2, Hemisphere, New York, 1989. [all data]

Chao J., 1986, 2
Chao J., Thermodynamic properties of key organic oxygen compounds in the carbon range C1 to C4. Part 2. Ideal gas properties, J. Phys. Chem. Ref. Data, 1986, 15, 1369-1436. [all data]

Stromsoe E., 1970
Stromsoe E., Heat capacity of alcohol vapors at atmospheric pressure, J. Chem. Eng. Data, 1970, 15, 286-290. [all data]

Bennewitz K., 1938
Bennewitz K., Molar heats of vapor organic compounds, Z. Phys. Chem. (Leipzig), 1938, B39, 126-144. [all data]

Eucken A., 1948
Eucken A., Rotational hindrance in ether and alcohol molecules on the basis of heat capacity determinations, Z. Elektrochem., 1948, 52, 195-204. [all data]

Barrow G.M., 1952
Barrow G.M., Heat capacity, gas imperfection, infrared spectra, and internal rotation barriers of ethyl alcohol, J. Chem. Phys., 1952, 20, 1739-1744. [all data]

Sinke G.C., 1953
Sinke G.C., The heat capacity of organic vapors. VIII. Data for some aliphatic alcohols using an improved flow calorimeter requiring only 25 ml of sample, J. Am. Chem. Soc., 1953, 75, 1815-1818. [all data]

Halford J.O., 1957
Halford J.O., Standard heat capacities of gaseous methanol, ethanol, methane and ethane at 279 K by thermal conductivity, J. Phys. Chem., 1957, 61, 1536-1539. [all data]

Counsell J.F., 1970
Counsell J.F., Thermodynamic properties of organic oxygen compounds. 24. Vapor heat capacities and enthalpies of vaporization of ethanol, 2-methyl-1-propanol, and 1-pentanol, J. Chem. Thermodyn., 1970, 2, 367-372. [all data]

Chao and Rossini, 1965
Chao, J.; Rossini, F.D., Heats of combustion, formation, and isomerization of nineteen alkanols, J. Chem. Eng. Data, 1965, 10, 374-379. [all data]

Rossini, 1934
Rossini, F.D., Heats of combustion and of formation of the normal aliphatic alcohols in the gaseous and liquid states, and the energies of their atomic linkages, J. Res. NBS, 1934, 13, 189-197. [all data]

Green, 1960
Green, J.H.S., Revision of the values of the heats of formation of normal alcohols, Chem. Ind. (London), 1960, 1215-1216. [all data]

Parks, 1925
Parks, G.S., Thermal data on organic compounds I. The heat capacities and free energies of methyl, ethyl and normal-butyl alcohols, J. Am. Chem. Soc., 1925, 47, 338-345. [all data]

Richards and Davis, 1920
Richards, T.W.; Davis, H.S., The heats of combustion of benzene, toluene, aliphatic alcohols, cyclohexanol, and other carbon compounds, J. Am. Chem. Soc., 1920, 42, 1599-1617. [all data]

Emery and Benedict, 1911
Emery, A.G.; Benedict, F.G., The heat of combustion of compounds of physiological importance, Am. J. Physiol., 1911, 28, 301-307. [all data]

Haida, Suga, et al., 1977
Haida, O.; Suga, H.; Seki, S., Calorimetric study of the glassy state. XII. Plural glass-transition phenomena of ethanol, J. Chem. Thermodynam., 1977, 9, 1133-1148. [all data]

Kelley, 1929
Kelley, K.K., The heat capacities of ethyl and hexyl alcohols from 16°K to 298°K and the corresponding entropies and free energies, J. Am. Chem. Soc., 1929, 51, 779-786. [all data]

Petrov, Peshekhodov, et al., 1989
Petrov, A.N.; Peshekhodov, P.B.; Al'per, G.A., Heat capacity of non-aqueous solutions of non-electrolyts with N,N-dimethylformamide as a base, Sbornik Nauch. Trud., Termodin. Rast. neelect., Ivanovo, Inst. nevod. rast., 1989, Akad. [all data]

Andreoli-Ball, Patterson, et al., 1988
Andreoli-Ball, L.; Patterson, D.; Costas, M.; Caceres-Alonso, M., Heat capacity and corresponding states in alkan-1-ol-n-alkane systems, J. Chem. Soc., Faraday Trans. 1, 1988, 84(11), 3991-4012. [all data]

Ogawa and Murakami, 1986
Ogawa, H.; Murakami, S., Excess isobaric heat capacities for water + alkanol mixtures at 298.15 K, Thermochim. Acta, 1986, 109, 145-154. [all data]

Tanaka, Toyama, et al., 1986
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Notes

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