Acetic acid

Formula: C₂H₄O₂
Molecular weight: 60.0520
IUPAC Standard InChI: InChI=1S/C2H4O2/c1-2(3)4/h1H3,(H,3,4)
IUPAC Standard InChIKey: QTBSBXVTEAMEQO-UHFFFAOYSA-N
CAS Registry Number: 64-19-7
Chemical structure:
This structure is also available as a 2d Mol file or as a computed 3d SD file
The 3d structure may be viewed using Java or Javascript.
Isotopologues:
- Acetic acid-d4
Other names: Ethanoic acid; Ethylic acid; Glacial acetic acid; Methanecarboxylic acid; Vinegar acid; CH3COOH; Acetasol; Acide acetique; Acido acetico; Azijnzuur; Essigsaeure; Octowy kwas; Acetic acid, glacial; Kyselina octova; UN 2789; Aci-jel; Shotgun; Ethanoic acid monomer; NSC 132953
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Information on this page:
Other data available:
- Phase change data
- Reaction thermochemistry data: reactions 51 to 79
- Henry's Law data
- Gas phase ion energetics data
- Ion clustering data
- IR Spectrum
- Mass spectrum (electron ionization)
- UV/Visible spectrum
- Vibrational and/or electronic energy levels
- Gas Chromatography
Data at other public NIST sites:
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Gas phase thermochemistry data

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

Data compiled as indicated in comments:
DRB - Donald R. Burgess, Jr.
GT - Glushko Thermocenter, Russian Academy of Sciences, Moscow

Quantity	Value	Units	Method	Reference	Comment
Δ_fH°_gas	-433. ± 3.	kJ/mol	AVG	N/A	Average of 8 values; Individual data points
Quantity	Value	Units	Method	Reference	Comment
S°_gas	282.84	J/mol*K	N/A	Weltner W., 1955	Other third-law entropy values at 298.15 K are 284.5 [ Chao J., 1986] and 290.37(4.18) J/mol*K [ Halford J.O., 1941].; GT

Constant pressure heat capacity of gas

C_p,gas (J/mol*K)	Temperature (K)	Reference	Comment
39.54	50.	Chao J., 1986	p=1 bar. Selected entropies and heat capacities differ from other statistically calculated values [ Weltner W., 1955] by 1.0-1.3 J/molK for S(T) and 3.1-5.4 J/molK for Cp(T). Please also see Chao J., 1978.; GT
40.42	100.
42.74	150.
48.34	200.
59.38	273.15
63.44 ± 0.11	298.15
63.74	300.
79.66	400.
93.93	500.
106.18	600.
116.63	700.
125.50	800.
132.99	900.
139.26	1000.
144.46	1100.
148.76	1200.
152.30	1300.
155.22	1400.
157.63	1500.

Condensed phase thermochemistry data

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

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

Quantity	Value	Units	Method	Reference	Comment
Δ_fH°_liquid	-483.52 ± 0.36	kJ/mol	Ccb	Steele, Chirico, et al., 1997	ALS
Δ_fH°_liquid	-484.5 ± 0.2	kJ/mol	Ccb	Lebedeva, 1964	ALS
Δ_fH°_liquid	-484.1 ± 0.4	kJ/mol	Ccb	Evans and Skinner, 1959	ALS
Δ_fH°_liquid	-487.0	kJ/mol	Cm	Carson and Skinner, 1949	Unpublished result by Rossini; ALS
Quantity	Value	Units	Method	Reference	Comment
Δ_cH°_liquid	-875.16 ± 0.34	kJ/mol	Ccb	Steele, Chirico, et al., 1997	Corresponding Δ_fHº_liquid = -483.52 kJ/mol (simple calculation by NIST; no Washburn corrections); ALS
Δ_cH°_liquid	-874.2 ± 0.2	kJ/mol	Ccb	Lebedeva, 1964	Corresponding Δ_fHº_liquid = -484.47 kJ/mol (simple calculation by NIST; no Washburn corrections); ALS
Δ_cH°_liquid	-874.5 ± 0.4	kJ/mol	Ccb	Evans and Skinner, 1959	Corresponding Δ_fHº_liquid = -484.1 kJ/mol (simple calculation by NIST; no Washburn corrections); ALS
Δ_cH°_liquid	-872.4	kJ/mol	Ccb	Schjanberg, 1935	Corresponding Δ_fHº_liquid = -486.2 kJ/mol (simple calculation by NIST; no Washburn corrections); ALS
Quantity	Value	Units	Method	Reference	Comment
S°_liquid	158.0	J/mol*K	N/A	Martin and Andon, 1982	DH
S°_liquid	193.7	J/mol*K	N/A	Parks and Kelley, 1925	Extrapolation below 90 K. 76.82 J/mol*K.; DH

Constant pressure heat capacity of liquid

C_p,liquid (J/mol*K)	Temperature (K)	Reference	Comment
123.1	298.15	Martin and Andon, 1982	T = 13 to 450 K. Data also given by equation.; DH
139.7	332.	Swietoslawski and Zielenkiewicz, 1958	Mean value 22 to 96°C.; DH
120.5	298.	Radulescu and Jula, 1934	DH
121.3	297.1	Neumann, 1932	T = 23.9 to 80.5°C. Value is unsmoothed experimental datum.; DH
159.8	298.1	Parks, Kelley, et al., 1929	Extrapolation below 90 K, 42.68 J/mol*K. Revision of previous data.; DH
123.4	294.7	Parks and Kelley, 1925	T = 87 to 295 K. Value is unsmoothed experimental datum.; DH
137.	287. - 335.	Pickering, 1895	T = 260 to 335 K.; DH
123.5	298.	von Reis, 1881	T = 292 to 358 K.; DH

Reaction thermochemistry data

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

Data compiled as indicated in comments:
B - John E. Bartmess
M - Michael M. Meot-Ner (Mautner) and Sharon G. Lias
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

+ Acetic acid = ( • )

By formula: F^- + C₂H₄O₂ = (F^- • C₂H₄O₂)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	185. ± 8.4	kJ/mol	IMRE	Larson and McMahon, 1983	gas phase; These relative affinities are ca. 10 kcal/mol weaker than threshold values (see Wenthold and Squires, 1995) for donors greater than ca. 27 kcal/mol in free energy. This discrepancy has not yet been resolved, though the stronger value appears preferable.; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	107.	J/mol*K	N/A	Larson and McMahon, 1983	gas phase; switching reaction(F-)H2O, Entropy change calculated or estimated; Arshadi, Yamdagni, et al., 1970; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	153. ± 8.4	kJ/mol	IMRE	Larson and McMahon, 1983	gas phase; These relative affinities are ca. 10 kcal/mol weaker than threshold values (see Wenthold and Squires, 1995) for donors greater than ca. 27 kcal/mol in free energy. This discrepancy has not yet been resolved, though the stronger value appears preferable.; B,M

C₂H₅O⁺ + Acetic acid = (C₂H₅O⁺ • )

By formula: C₂H₅O⁺ + C₂H₄O₂ = (C₂H₅O⁺ • C₂H₄O₂)

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

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	118.	kJ/mol	PHPMS	Meot-Ner (Mautner), 1992	gas phase; M
Δ_rH°	123.	kJ/mol	ICR	Larson and McMahon, 1982	gas 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
Δ_rS°	118.	J/mol*K	PHPMS	Meot-Ner (Mautner), 1992	gas phase; M
Δ_rS°	117.	J/mol*K	N/A	Larson and McMahon, 1982	gas 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
Δ_rG°	88.7	kJ/mol	ICR	Larson and McMahon, 1982	gas 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

+ Acetic acid = ( • )

By formula: Cl^- + C₂H₄O₂ = (Cl^- • C₂H₄O₂)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	102.1 ± 0.84	kJ/mol	TDAs	Sieck, 1985	gas phase; B,M
Δ_rH°	90.4 ± 8.4	kJ/mol	TDAs	Yamdagni and Kebarle, 1971	gas phase; B,M
Δ_rH°	100. ± 8.4	kJ/mol	IMRE	Larson and McMahon, 1984	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	82.0	J/mol*K	PHPMS	Sieck, 1985	gas phase; M
Δ_rS°	100.	J/mol*K	N/A	Larson and McMahon, 1984, 2	gas phase; switching reaction(Cl-)t-C4H9OH, Entropy change calculated or estimated; French, Ikuta, et al., 1982; M
Δ_rS°	80.8	J/mol*K	PHPMS	Yamdagni and Kebarle, 1971	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	77.8 ± 1.3	kJ/mol	TDAs	Sieck, 1985	gas phase; B
Δ_rG°	66.1 ± 8.4	kJ/mol	TDAs	Yamdagni and Kebarle, 1971	gas phase; B
Δ_rG°	69.9 ± 8.4	kJ/mol	IMRE	Larson and McMahon, 1984	gas phase; B,M

+ = Acetic acid

By formula: C₂H₃O₂^- + H⁺ = C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	1457. ± 5.9	kJ/mol	CIDC	Angel and Ervin, 2006	gas phase; B
Δ_rH°	1456. ± 9.2	kJ/mol	G+TS	Taft and Topsom, 1987	gas phase; B
Δ_rH°	1459. ± 8.8	kJ/mol	G+TS	Cumming and Kebarle, 1978	gas phase; B
Δ_rH°	1459. ± 9.2	kJ/mol	G+TS	Fujio, McIver, et al., 1981	gas phase; value altered from reference due to change in acidity scale; B
Δ_rH°	1435.9 ± 2.9	kJ/mol	EIAE	Muftakhov, Vasil'ev, et al., 1999	gas phase; B
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	1427. ± 8.4	kJ/mol	IMRE	Taft and Topsom, 1987	gas phase; B
Δ_rG°	1429. ± 8.4	kJ/mol	IMRE	Cumming and Kebarle, 1978	gas phase; B
Δ_rG°	1430. ± 8.4	kJ/mol	IMRE	Fujio, McIver, et al., 1981	gas phase; value altered from reference due to change in acidity scale; B

C₂H₇O⁺ + Acetic acid = (C₂H₇O⁺ • )

By formula: C₂H₇O⁺ + C₂H₄O₂ = (C₂H₇O⁺ • C₂H₄O₂)

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

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	123.	kJ/mol	ICR	Larson and McMahon, 1982	gas 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
Δ_rS°	119.	J/mol*K	N/A	Larson and McMahon, 1982	gas 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
Δ_rG°	87.0	kJ/mol	ICR	Larson and McMahon, 1982	gas 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

CH₆N⁺ + Acetic acid = (CH₆N⁺ • )

By formula: CH₆N⁺ + C₂H₄O₂ = (CH₆N⁺ • C₂H₄O₂)

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

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	92.0	kJ/mol	PHPMS	Meot-Ner, 1984	gas phase; M
Δ_rH°	89.5	kJ/mol	PHPMS	Meot-Ner, 1984	gas phase; Entropy change calculated or estimated; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	102.	J/mol*K	PHPMS	Meot-Ner, 1984	gas phase; M
Δ_rS°	100.	J/mol*K	N/A	Meot-Ner, 1984	gas phase; Entropy change calculated or estimated; M

Free energy of reaction

Δ_rG° (kJ/mol)	T (K)	Method	Reference	Comment
43.1	459.	PHPMS	Meot-Ner, 1984	gas phase; Entropy change calculated or estimated; M

(C₂H₅O⁺ • 3 Acetic acid ) + = (C₂H₅O⁺ • 4)

By formula: (C₂H₅O⁺ • 3C₂H₄O₂) + C₂H₄O₂ = (C₂H₅O⁺ • 4C₂H₄O₂)

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

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	50.	kJ/mol	PHPMS	Meot-Ner (Mautner), 1992	gas phase; Entropy change calculated or estimated; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	100.	J/mol*K	N/A	Meot-Ner (Mautner), 1992	gas phase; Entropy change calculated or estimated; M

Free energy of reaction

Δ_rG° (kJ/mol)	T (K)	Method	Reference	Comment
26.	245.	PHPMS	Meot-Ner (Mautner), 1992	gas phase; Entropy change calculated or estimated; M

( • 2 Acetic acid • ) + = ( • 3 • )

By formula: (C₂H₃O₂^- • 2C₂H₄O₂ • H₂O) + C₂H₄O₂ = (C₂H₃O₂^- • 3C₂H₄O₂ • H₂O)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	52.3 ± 2.5	kJ/mol	N/A	Meot-ner, Elmore, et al., 1999	gas phase; B
Δ_rH°	67.8 ± 4.2	kJ/mol	TDAs	Meot-Ner and Sieck, 1986	gas phase; B
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	24.0	kJ/mol	TDAs	Meot-ner, Elmore, et al., 1999	gas phase; B
Δ_rG°	26. ± 4.2	kJ/mol	TDAs	Meot-Ner and Sieck, 1986	gas phase; B

( • Acetic acid • ) + = ( • 2 • )

By formula: (C₂H₃O₂^- • C₂H₄O₂ • H₂O) + C₂H₄O₂ = (C₂H₃O₂^- • 2C₂H₄O₂ • H₂O)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	82.4 ± 2.1	kJ/mol	N/A	Meot-ner, Elmore, et al., 1999	gas phase; B
Δ_rH°	67.8 ± 4.2	kJ/mol	TDAs	Meot-Ner and Sieck, 1986	gas phase; B
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	45.23	kJ/mol	TDAs	Meot-ner, Elmore, et al., 1999	gas phase; B
Δ_rG°	26. ± 4.2	kJ/mol	TDAs	Meot-Ner and Sieck, 1986	gas phase; B

+ = Acetic acid +

By formula: C₂H₃ClO + H₂O = C₂H₄O₂ + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-94.47	kJ/mol	Cm	Devore and O'Neal, 1969	liquid phase; Heat of hydrolysis; ALS
Δ_rH°	-92.30	kJ/mol	Cm	Pritchard and Skinner, 1950	liquid phase; Heat of hydrolysis at 298 K, see Carson and Skinner, 1949; ALS
Δ_rH°	-92.42	kJ/mol	Cm	Carson and Skinner, 1949	liquid phase; ALS

+ = 2 Acetic acid

By formula: C₄H₆O₃ + H₂O = 2C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-56.6 ± 4.0	kJ/mol	Cm	Becker and Maelicke, 1967	liquid phase; ALS
Δ_rH°	-58.6 ± 0.4	kJ/mol	Cm	Wadso, 1962	liquid phase; ALS
Δ_rH°	-58.4 ± 0.4	kJ/mol	Cm	Conn, Kistiakowsky, et al., 1942	liquid phase; Heat of hydrolysis at 303 K; ALS

+ Acetic acid = ( • )

By formula: I^- + C₂H₄O₂ = (I^- • C₂H₄O₂)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	70.7 ± 4.2	kJ/mol	TDAs	Caldwell and Kebarle, 1984	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	89.1	J/mol*K	PHPMS	Caldwell and Kebarle, 1984	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	43.9 ± 4.2	kJ/mol	TDAs	Caldwell and Kebarle, 1984	gas phase; B

C₂H₃O₂^- + = Acetic acid

By formula: C₂H₃O₂^- + H⁺ = C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	1540. ± 13.	kJ/mol	G+TS	Grabowski and Cheng, 1989	gas phase; B
Δ_rH°	1539. ± 19.	kJ/mol	EIAE	Muftakhov, Vasil'ev, et al., 1999	gas phase; B
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	1511. ± 13.	kJ/mol	IMRB	Grabowski and Cheng, 1989	gas phase; B

C₆H₅NO₂^- + Acetic acid = (C₆H₅NO₂^- • )

By formula: C₆H₅NO₂^- + C₂H₄O₂ = (C₆H₅NO₂^- • C₂H₄O₂)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	94.56 ± 0.42	kJ/mol	TDAs	Sieck, 1985	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	112.	J/mol*K	PHPMS	Sieck, 1985	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	61.09 ± 0.84	kJ/mol	TDAs	Sieck, 1985	gas phase; B

+ Acetic acid = ( • )

By formula: C₆H₅O^- + C₂H₄O₂ = (C₆H₅O^- • C₂H₄O₂)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	115.	kJ/mol	PHPMS	Meot-Ner and Sieck, 1986	gas phase; calculated from CH3COO-.C6H5OH; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	100.	J/mol*K	PHPMS	Meot-Ner and Sieck, 1986	gas phase; calculated from CH3COO-.C6H5OH; M

(C₂H₅O⁺ • 2 Acetic acid ) + = (C₂H₅O⁺ • 3)

By formula: (C₂H₅O⁺ • 2C₂H₄O₂) + C₂H₄O₂ = (C₂H₅O⁺ • 3C₂H₄O₂)

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

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	54.8	kJ/mol	PHPMS	Meot-Ner (Mautner), 1992	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	93.7	J/mol*K	PHPMS	Meot-Ner (Mautner), 1992	gas phase; M

(C₂H₅O⁺ • Acetic acid ) + = (C₂H₅O⁺ • 2)

By formula: (C₂H₅O⁺ • C₂H₄O₂) + C₂H₄O₂ = (C₂H₅O⁺ • 2C₂H₄O₂)

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

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	77.4	kJ/mol	PHPMS	Meot-Ner (Mautner), 1992	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	103.	J/mol*K	PHPMS	Meot-Ner (Mautner), 1992	gas phase; M

C₆H₁₂NO₃⁺ + Acetic acid = (C₆H₁₂NO₃⁺ • )

By formula: C₆H₁₂NO₃⁺ + C₂H₄O₂ = (C₆H₁₂NO₃⁺ • C₂H₄O₂)

Bond type: Hydrogen bonds with polydentate bonding in positive ions

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	75.7	kJ/mol	PHPMS	Meot-Ner, 1984, 2	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	114.	J/mol*K	PHPMS	Meot-Ner, 1984, 2	gas phase; M

+ = + Acetic acid

By formula: C₄H₇NO₂ + H₂O = C₂H₅NO + C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-18.1 ± 0.2	kJ/mol	Cm	Hill and Wadso, 1968	solid phase; Heat of hydrolysis; ALS
Δ_rH°	-18.1 ± 0.2	kJ/mol	Cm	Wadso, 1965	solid phase; Heat of hydrolysis; ALS

C₄H₁₀NO⁺ + Acetic acid = (C₄H₁₀NO⁺ • )

By formula: C₄H₁₀NO⁺ + C₂H₄O₂ = (C₄H₁₀NO⁺ • C₂H₄O₂)

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

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	77.0	kJ/mol	PHPMS	Meot-Ner, 1984, 2	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	103.	J/mol*K	PHPMS	Meot-Ner, 1984, 2	gas phase; M

+ = + Acetic acid

By formula: C₂H₃IO + H₂O = HI + C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-93.97	kJ/mol	Cm	Devore and O'Neal, 1969	liquid phase; Heat of hydrolysis; ALS
Δ_rH°	-90.33	kJ/mol	Cm	Carson and Skinner, 1949	liquid phase; Heat of hydrolysis; ALS

( • ) + Acetic acid = ( • • )

By formula: (C₂H₃O₂^- • H₂O) + C₂H₄O₂ = (C₂H₃O₂^- • C₂H₄O₂ • H₂O)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	123. ± 4.2	kJ/mol	TDAs	Meot-Ner and Sieck, 1986	gas phase; B
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	85.4 ± 6.7	kJ/mol	TDAs	Meot-Ner and Sieck, 1986	gas phase; B

+ = + Acetic acid

By formula: C₄H₆O₃ + C₄H₁₁N = C₆H₁₃NO + C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-113.2 ± 0.46	kJ/mol	Cm	Wadso, 1962	liquid phase; ALS
Δ_rH°	-163.7 ± 0.3	kJ/mol	Cm	Wadso, 1958	liquid phase; Heat of aminolysis; ALS

+ = + Acetic acid

By formula: C₂H₃BrO + H₂O = HBr + C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-97.53	kJ/mol	Cm	Devore and O'Neal, 1969	liquid phase; Heat of hydrolysis; ALS
Δ_rH°	-96.48	kJ/mol	Cm	Carson and Skinner, 1949	liquid phase; ALS

+ Acetic acid = C₈H₉O₂S^-

By formula: C₆H₅S^- + C₂H₄O₂ = C₈H₉O₂S^-

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	84.94 ± 0.42	kJ/mol	TDAs	Sieck and Meot-ner, 1989	gas phase; B
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	52.3 ± 1.7	kJ/mol	TDAs	Sieck and Meot-ner, 1989	gas phase; B

( • 2 Acetic acid ) + = ( • 3)

By formula: (C₂H₃O₂^- • 2C₂H₄O₂) + C₂H₄O₂ = (C₂H₃O₂^- • 3C₂H₄O₂)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	67.8	kJ/mol	PHPMS	Meot-Ner and Sieck, 1986	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	139.	J/mol*K	PHPMS	Meot-Ner and Sieck, 1986	gas phase; M

( • Acetic acid ) + = ( • 2)

By formula: (C₂H₃O₂^- • C₂H₄O₂) + C₂H₄O₂ = (C₂H₃O₂^- • 2C₂H₄O₂)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	82.0	kJ/mol	PHPMS	Meot-Ner and Sieck, 1986	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	120.	J/mol*K	PHPMS	Meot-Ner and Sieck, 1986	gas phase; M

+ Acetic acid = ( • )

By formula: C₆H₅S^- + C₂H₄O₂ = (C₆H₅S^- • C₂H₄O₂)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	84.9	kJ/mol	PHPMS	Sieck and Meot-ner, 1989	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	110.	J/mol*K	PHPMS	Sieck and Meot-ner, 1989	gas phase; M

+ Acetic acid = ( • )

By formula: Li⁺ + C₂H₄O₂ = (Li⁺ • C₂H₄O₂)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	174.	kJ/mol	ICR	Staley and Beauchamp, 1975	gas phase; switching reaction(Li+)H2O, from graph; Dzidic and Kebarle, 1970 interpolated; M

+ Acetic acid = ( • )

By formula: C₂H₃O₂^- + C₂H₄O₂ = (C₂H₃O₂^- • C₂H₄O₂)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	123.	kJ/mol	PHPMS	Meot-Ner and Sieck, 1986	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	124.	J/mol*K	PHPMS	Meot-Ner and Sieck, 1986	gas phase; M

+ 2 = + 2 Acetic acid

By formula: C₈H₁₄O₄ + 2H₂O = C₄H₁₀O₂ + 2C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-22.3 ± 2.1	kJ/mol	Cm	Shlechter, Othmer, et al., 1945	liquid phase; Heat of formation derived by Cox and Pilcher, 1970; ALS

+ = + Acetic acid

By formula: C₅H₆N₂O + H₂O = C₃H₄N₂ + C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-20.2 ± 0.2	kJ/mol	Cm	Wadso, 1960	liquid phase; solvent: Aqueous; Heat of hydrolysis; ALS

+ 2 Acetic acid = + 2

By formula: C₄H₁₀O₂ + 2C₂H₄O₂ = C₈H₁₄O₄ + 2H₂O

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	22.30	kJ/mol	Eqk	Shlechter, Othmer, et al., 1945	liquid phase; Heat of esterification at 338-453 K; ALS

+ Acetic acid = +

By formula: C₆H₁₂O₃ + C₂H₄O₂ = C₈H₁₄O₄ + H₂O

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	1.85	kJ/mol	Eqk	Shlechter, Othmer, et al., 1945	liquid phase; Heat of esterification at 338-453 K; ALS

+ 2 = + 2 Acetic acid

By formula: C₆H₉NO₃ + 2H₂O = C₂H₅NO + 2C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-103.5 ± 0.08	kJ/mol	Cm	Hill and Wadso, 1968	liquid phase; Heat of hydrolysis; ALS

2 + = Acetic acid + 2

By formula: 2H₂O + C₄H₈O₂ = C₂H₄O₂ + 2CH₄O

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-74.4 ± 3.6	kJ/mol	Cm	Guthrie and Liu, 1995	liquid phase; Heat of hydrolysis; ALS

+ Acetic acid =

By formula: C₁₀H₁₄ + C₂H₄O₂ = C₁₂H₁₈O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-182.0 ± 0.3	kJ/mol	Cac	Wiberg, Connon, et al., 1979	liquid phase; solvent: Acetic acid; ALS

+ = Acetic acid +

By formula: C₂H₄OS + H₂O = C₂H₄O₂ + H₂S

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-2.7 ± 0.3	kJ/mol	Cm	Sunner and Wadso, 1957	liquid phase; Heat of hydrolysis; ALS

+ = Acetic acid +

By formula: C₂H₅NO + H₂O = C₂H₄O₂ + H₃N

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	76.1 ± 1.4	kJ/mol	Cm	Hill and Wadso, 1968	solid phase; Heat of hydrolysis; ALS

+ Acetic acid = +

By formula: C₆H₁₃NO + C₂H₄O₂ = C₈H₁₅NO₂ + H₂O

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	40.5 ± 0.50	kJ/mol	Cm	Wadso, 1965	liquid phase; Heat of hydrolysis; ALS

+ = + Acetic acid

By formula: C₅H₁₀OS + H₂O = C₃H₈S + C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-3.9 ± 0.3	kJ/mol	Cm	Wadso, 1957	liquid phase; Heat of hydrolysis; ALS

+ Acetic acid = C₁₀H₁₁NO₂ +

By formula: C₈H₉NO + C₂H₄O₂ = C₁₀H₁₁NO₂ + H₂O

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	45.5 ± 0.3	kJ/mol	Cm	Wadso, 1965	solid phase; Heat of hydrolysis; ALS

+ = + Acetic acid

By formula: C₉H₁₀O₂ + H₂O = C₇H₈O + C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-18.4 ± 0.59	kJ/mol	Cm	Sunner, 1957	liquid phase; Heat of hydrolysis; ALS

+ = + Acetic acid

By formula: H₂O + C₆H₁₂OS = C₄H₁₀S + C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-4.6 ± 0.3	kJ/mol	Cm	Wadso, 1957	liquid phase; Heat of hydrolysis; ALS

+ = + Acetic acid

By formula: C₃H₄N₄O + H₂O = CH₂N₄ + C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-43.1 ± 0.4	kJ/mol	Cm	Wadso, 1960	solid phase; Heat of hydrolysis; ALS

+ = + Acetic acid

By formula: C₉H₈O₃S + H₂O = C₇H₆O₂S + C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-11.5 ± 0.4	kJ/mol	Cm	Nelander, 1964	solid phase; Heat of hydrolysis; ALS

+ = + Acetic acid

By formula: C₈H₉NO + H₂O = C₆H₇N + C₂H₄O₂

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-42.0 ± 0.3	kJ/mol	Cm	Wadso, 1965	solid phase; Heat of hydrolysis; ALS

Acetic acid + = +

By formula: C₂H₄O₂ + C₃H₆O = C₅H₈O₂ + H₂O

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	60.2 ± 0.3	kJ/mol	Cm	Sunner, 1957	liquid phase; Heat of hydrolysis; ALS

+ = Acetic acid +

By formula: C₄H₈OS + H₂O = C₂H₄O₂ + C₂H₆S

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-4.0 ± 0.3	kJ/mol	Cm	Wadso, 1957	liquid phase; Heat of hydrolysis; ALS

+ = Acetic acid +

By formula: H₂O + C₅H₁₀OS = C₂H₄O₂ + C₃H₈S

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-5.8 ± 0.3	kJ/mol	Cm	Wadso, 1957	liquid phase; Heat of hydrolysis; ALS

References

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

Weltner W., 1955
Weltner W., Jr., The vibrational spectrum, associative and thermodynamic properties of acetic acid vapor, J. Am. Chem. Soc., 1955, 77, 3941-3950. [all data]

Chao J., 1986
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]

Halford J.O., 1941
Halford J.O., The entropy of acetic acid, J. Chem. Phys., 1941, 9, 859-863. [all data]

Chao J., 1978
Chao J., Ideal gas thermodynamic properties of methanoic and ethanoic acids, J. Phys. Chem. Ref. Data, 1978, 7, 363-377. [all data]

Steele, Chirico, et al., 1997
Steele, W.V.; Chirico, R.D.; Cowell, A.B.; Knipmeyer, S.E.; Nguyen, A., Thermodynamic properties and ideal-gas enthalpies of formation for 2-aminoisobutyric acid (2-methylalanine), acetic acid, (4-methyl-3-penten-2-one), 4-methylpent-1-ene, 2,2'-bis(phenylthio)propane, and glycidyl phenyl ether (1,2-epoxy-3-phenoxypropane), J. Chem. Eng. Data, 1997, 42, 1052-1066. [all data]

Lebedeva, 1964
Lebedeva, N.D., Heats of combustion of monocarboxylic acids, Russ. J. Phys. Chem. (Engl. Transl.), 1964, 38, 1435-1437. [all data]

Evans and Skinner, 1959
Evans, F.W.; Skinner, H.A., The heat of combustion of acetic acid, Trans. Faraday Soc., 1959, 55, 260-261. [all data]

Carson and Skinner, 1949
Carson, A.S.; Skinner, H.A., 201. Carbon-halogen bond energies in the acetyl halides, J. Chem. Soc., 1949, 936-939. [all data]

Schjanberg, 1935
Schjanberg, E., Die Verbrennungswarmen und die Refraktionsdaten einiger chlorsubstituierter Fettsauren und Ester., Z. Phys. Chem. Abt. A, 1935, 172, 197-233. [all data]

Martin and Andon, 1982
Martin, J.F.; Andon, R.J.L., Thermodynamic properties of organic oxygen compounds. Part LII. Molar heat capacity of ethanoic, propanoic, and butanoic acids, J. Chem. Thermodynam., 1982, 14, 679-688. [all data]

Parks and Kelley, 1925
Parks, G.S.; Kelley, K.K., Thermal data on organic compounds. II. The heat capacities of five organic compounds. The entropies and free energies of some homologous series of aliphatic compounds, J. Am. Chem. Soc., 1925, 47, 2089-2097. [all data]

Swietoslawski and Zielenkiewicz, 1958
Swietoslawski, W.; Zielenkiewicz, A., Mean specific heat of some ternary azeotropes, Bull. Acad. Pol. Sci. Ser. Sci. Chim., 1958, 6, 365-366. [all data]

Radulescu and Jula, 1934
Radulescu, D.; Jula, O., Beiträge zur Bestimmung der Abstufung der Polarität des Aminstickstoffes in den organischen Verbindungen, Z. Phys. Chem., 1934, B26, 390-393. [all data]

Neumann, 1932
Neumann, M.B., Die Untersuchung der Wärmekapazität vom binären System CH₃COOH + H₂O bei verschiedenen Temperaturen, Z. Phys. Chem., 1932, A158, 258-264. [all data]

Parks, Kelley, et al., 1929
Parks, G.S.; Kelley, K.K.; Huffman, H.M., Thermal data on organic compounds. V. A revision of the entropies and free energies of nineteen organic compounds, J. Am. Chem. Soc., 1929, 51, 1969-1973. [all data]

Pickering, 1895
Pickering, S.U., A comparison of some properties of acetic acid and its chloro- and bromo-derivatives, J. Chem. Soc., 1895, 67, 664-684. [all data]

von Reis, 1881
von Reis, M.A., Die specifische Wärme flüssiger organischer Verbindungen und ihre Beziehung zu deren Moleculargewicht, Ann. Physik [3], 1881, 13, 447-464. [all data]

Larson and McMahon, 1983
Larson, J.W.; McMahon, T.B., Strong hydrogen bonding in gas-phase anions. An ion cyclotron resonance determination of fluoride binding energetics to bronsted acids from gas-phase fluoride exchange equilibria measurements, J. Am. Chem. Soc., 1983, 105, 2944. [all data]

Wenthold and Squires, 1995
Wenthold, P.G.; Squires, R.R., Bond dissociation energies of F2(-) and HF2(-). A gas-phase experimental and G2 theoretical study, J. Phys. Chem., 1995, 99, 7, 2002, https://doi.org/10.1021/j100007a034 . [all data]

Arshadi, Yamdagni, et al., 1970
Arshadi, M.; Yamdagni, R.; Kebarle, P., Hydration of Halide Negative Ions in the Gas Phase. II. Comparison of Hydration Energies for the Alkali Positive and Halide Negative Ions, J. Phys. Chem., 1970, 74, 7, 1475, https://doi.org/10.1021/j100702a014 . [all data]

Meot-Ner (Mautner), 1992
Meot-Ner (Mautner), M., Intermolecular Forces in Organic Clusters, J. Am. Chem. Soc., 1992, 114, 9, 3312, https://doi.org/10.1021/ja00035a024 . [all data]

Larson and McMahon, 1982
Larson, J.W.; McMahon, T.B., Formation, Thermochemistry, and Relative Stabilities of Proton - Bound dimers of Oxygen n - Donor Bases from Ion Cyclotron Resonance Solvent - Exchange Equilibria Measurements, J. Am. Chem. Soc., 1982, 104, 23, 6255, https://doi.org/10.1021/ja00387a016 . [all data]

Grimsrud and Kebarle, 1973
Grimsrud, E.P.; Kebarle, P., Gas Phase Ion Equilibria Studies of the Solvation of the Hydrogen Ion by Methanol, Dimethyl Ether and Water. Effect of Hydrogen Bonding, J. Am. Chem. Soc., 1973, 95, 24, 7939, https://doi.org/10.1021/ja00805a002 . [all data]

Lias, Liebman, et al., 1984
Lias, S.G.; Liebman, J.F.; Levin, R.D., Evaluated gas phase basicities and proton affinities of molecules heats of formation of protonated molecules, J. Phys. Chem. Ref. Data, 1984, 13, 695. [all data]

Keesee and Castleman, 1986
Keesee, R.G.; Castleman, A.W., Jr., Thermochemical data on Ggs-phase ion-molecule association and clustering reactions, J. Phys. Chem. Ref. Data, 1986, 15, 1011. [all data]

Sieck, 1985
Sieck, L.W., Thermochemistry of Solvation of NO₂^- and C₆H₅NO₂^- by Polar Molecules in the Vapor Phase. Comparison with Cl^- and Variation with Ligand Structure., J. Phys. Chem., 1985, 89, 25, 5552, https://doi.org/10.1021/j100271a049 . [all data]

Yamdagni and Kebarle, 1971
Yamdagni, R.; Kebarle, P., Hydrogen bonding energies to negative ions from gas phase measurements of ionic equilibria, J. Am. Chem. Soc., 1971, 93, 7139. [all data]

Larson and McMahon, 1984
Larson, J.W.; McMahon, T.B., Hydrogen bonding in gas phase anions. An experimental investigation of the interaction between chloride ion and bronsted acids from ICR chloride exchange equilibria, J. Am. Chem. Soc., 1984, 106, 517. [all data]

Larson and McMahon, 1984, 2
Larson, J.W.; McMahon, T.B., Gas phase negative ion chemistry of alkylchloroformates, Can. J. Chem., 1984, 62, 675. [all data]

French, Ikuta, et al., 1982
French, M.A.; Ikuta, S.; Kebarle, P., Hydrogen bonding of O-H and C-H hydrogen donors to Cl^-. Results from mass spectrometric measurement of the ion-molecule equilibria RH + Cl^- = RHCl^-, Can. J. Chem., 1982, 60, 1907. [all data]

Angel and Ervin, 2006
Angel, L.A.; Ervin, K.M., Gas-phase acidities and O-H bond dissociation enthalpies of phenol, 3-methylphenol, 2,4,6-trimethylphenol, and ethanoic acid, J. Phys. Chem. A, 2006, 110, 35, 10392-10403, https://doi.org/10.1021/jp0627426 . [all data]

Taft and Topsom, 1987
Taft, R.W.; Topsom, R.D., The Nature and Analysis of Substituent Effects, Prog. Phys. Org. Chem., 1987, 16, 1. [all data]

Cumming and Kebarle, 1978
Cumming, J.B.; Kebarle, P., Summary of gas phase measurements involving acids AH. Entropy changes in proton transfer reactions involving negative ions. Bond dissociation energies D(A-H) and electron affinities EA(A), Can. J. Chem., 1978, 56, 1. [all data]

Fujio, McIver, et al., 1981
Fujio, M.; McIver, R.T., Jr.; Taft, R.W., Effects on the acidities of phenols from specific substituent-solvent interactions. Inherent substituent parameters from gas phase acidities, J. Am. Chem. Soc., 1981, 103, 4017. [all data]

Muftakhov, Vasil'ev, et al., 1999
Muftakhov, M.V.; Vasil'ev, Y.V.; Mazunov, V.A., Determination of electron affinity of carbonyl radicals by means of negative ion mass spectrometry, Rapid Commun. Mass Spectrom., 1999, 13, 12, 1104-1108, https://doi.org/10.1002/(SICI)1097-0231(19990630)13:12<1104::AID-RCM619>3.0.CO;2-C . [all data]

Meot-Ner, 1984
Meot-Ner, (Mautner)M., The Ionic Hydrogen Bond and Ion Solvation. 1. -NH+ O-, -NH+ N- and -OH+ O- Bonds. Correlations with Proton Affinity. Deviations Due to Structural Effects, J. Am. Chem. Soc., 1984, 106, 5, 1257, https://doi.org/10.1021/ja00317a015 . [all data]

Meot-ner, Elmore, et al., 1999
Meot-ner, M.; Elmore, D.E.; Scheiner, S., Ionic Hydrogen Bond Effects on the Acidities, Basicities, Solvation, Solvent Bridging and Self-assembly of Carboxylic Groups, J. Am. Chem. Soc., 1999, 121, 33, 7625, https://doi.org/10.1021/ja982173i . [all data]

Meot-Ner and Sieck, 1986
Meot-Ner, M.; Sieck, L.W., The ionic hydrogen bond and ion solvation. 5. OH...O^- bonds. Gas phase solvation and clustering of alkoxide and carboxylate anions, J. Am. Chem. Soc., 1986, 108, 7525. [all data]

Devore and O'Neal, 1969
Devore, J.A.; O'Neal, H.E., Heats of formation of the acetyl halides and of the acetyl radical, J. Phys. Chem., 1969, 73, 2644-2648. [all data]

Pritchard and Skinner, 1950
Pritchard, H.O.; Skinner, H.A., The heats of hydrolysis of the chloro-substituted acetyl chlorides, J. Chem. Soc., 1950, 272-276. [all data]

Becker and Maelicke, 1967
Becker, F.; Maelicke, A., Thermokinetische Messungen nach dem Prinzip der Wärmefluβkalorimetrie, Z. Phys. Chem. (Neue Folge), 1967, 55, 280-295. [all data]

Wadso, 1962
Wadso, I., Heats of aminolysis and hydrolysis of some N-acetyl compounds and of acetic anhydride, Acta Chem. Scand., 1962, 16, 471-478. [all data]

Conn, Kistiakowsky, et al., 1942
Conn, J.B.; Kistiakowsky, G.B.; Roberts, R.M.; Smith, E.A., Heats of organic reactions. XIII. Heats of hydrolysis of some acid anhydrides, J. Am. Chem. Soc., 1942, 64, 1747-17. [all data]

Caldwell and Kebarle, 1984
Caldwell, G.; Kebarle, P., Binding energies and structural effects in halide anion-ROH and -RCOOH complexes from gas phase equilibria measurements, J. Am. Chem. Soc., 1984, 106, 967. [all data]

Grabowski and Cheng, 1989
Grabowski, J.J.; Cheng, X., Gas-Phase Formation of the Enolate Monoanion of Acetic Acid by Proton Abstraction, J. Am. Chem. Soc., 1989, 111, 8, 3106, https://doi.org/10.1021/ja00190a078 . [all data]

Meot-Ner, 1984, 2
Meot-Ner, (Mautner), The Ionic Hydrogen Bond. 4. Intramolecular and Multiple Bonds. Proton Affinities, Hydration and Complexes of Amides and Amino Acid Derivatives, J. Am. Chem. Soc., 1984, 106, 2, 278, https://doi.org/10.1021/ja00314a003 . [all data]

Hill and Wadso, 1968
Hill, J.O.; Wadso, I., Some thermochemical properties of N,N,N-triacetylammonia, Acta Chem. Scand., 1968, 22, 1590-1594. [all data]

Wadso, 1965
Wadso, I., Thermochemical properties of diacetimide, N-butyldiacetimide and N-phenyldiacetimide, Acta Chem. Scand., 1965, 19, 1079-1087. [all data]

Wadso, 1958
Wadso, I., The heats of aminolysis of n-butyl thiolacetate and acetic anhydride, Acta Chem. Scand., 1958, 12, 635-640. [all data]

Sieck and Meot-ner, 1989
Sieck, L.W.; Meot-ner, M., Ionic Hydrogen Bond and Ion Solvation. 8. RS-..HOR Bond Strengths. Correlation with Acidities., J. Phys. Chem., 1989, 93, 4, 1586, https://doi.org/10.1021/j100341a079 . [all data]

Staley and Beauchamp, 1975
Staley, R.H.; Beauchamp, J.L., Intrinsic Acid - Base Properties of Molecules. Binding Energies of Li+ to pi - and n - Donor Bases, J. Am. Chem. Soc., 1975, 97, 20, 5920, https://doi.org/10.1021/ja00853a050 . [all data]

Dzidic and Kebarle, 1970
Dzidic, I.; Kebarle, P., Hydration of the Alkali Ions in the Gas Phase. Enthalpies and Entropies of Reactions M+(H2O)n-1 + H2O = M+(H2O)n, J. Phys. Chem., 1970, 74, 7, 1466, https://doi.org/10.1021/j100702a013 . [all data]

Shlechter, Othmer, et al., 1945
Shlechter, N.; Othmer, D.F.; Marshak, S., Esterification of 2,3-butylene glycol with acetic acid, Ind. Eng. Chem., 1945, 37, 900-905. [all data]

Cox and Pilcher, 1970
Cox, J.D.; Pilcher, G., Thermochemistry of Organic and Organometallic Compounds, Academic Press, New York, 1970, 1-636. [all data]

Wadso, 1960
Wadso, I., Heats of hydrolysis of N-acetylated imidazole, 1,2,4-triazole and tetrazole, Acta Chem. Scand., 1960, 14, 903-908. [all data]

Guthrie and Liu, 1995
Guthrie, J.P.; Liu, Z., The enols of acetic acid and methyl acetate, Can. J. Chem., 1995, 73, 1395-2398. [all data]

Wiberg, Connon, et al., 1979
Wiberg, K.B.; Connon, H.A.; Pratt, W.E., Enthalpies of acetolysis of tricyclo[3.2.1.0^1,5]octane ([3.2.1]propellane) and 1,3-dehydroadamantane, J. Am. Chem. Soc., 1979, 101, 6970-6972. [all data]

Sunner and Wadso, 1957
Sunner, S.; Wadso, I., The heat of hydrolysis of thiolacetic acid, Trans. Faraday Soc., 1957, 53, 455-459. [all data]

Wadso, 1957
Wadso, I., The heats of hydrolysis of some alkyl thiolesters, Acta Chem. Scand., 1957, 11, 1745-1751. [all data]

Sunner, 1957
Sunner, S., The heat of hydrolysis of i-propenyl acetate and m-cresyl acetate and the heat of formation of acetone, Acta Chem. Scand., 1957, 11, 1757-1760. [all data]

Nelander, 1964
Nelander, L., The heats of hydrolysis of aspirin, thioaspirin, and their p-analogues, Acta Chem. Scand., 1964, 18, 973-984. [all data]

Notes

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

Symbols used in this document:

C_p,gas	Constant pressure heat capacity of gas
C_p,liquid	Constant pressure heat capacity of liquid
S°_gas	Entropy of gas at standard conditions
S°_liquid	Entropy of liquid at standard conditions
T	Temperature
Δ_cH°_liquid	Enthalpy of combustion of liquid at standard conditions
Δ_fH°_gas	Enthalpy of formation of gas at standard conditions
Δ_fH°_liquid	Enthalpy of formation of liquid at standard conditions
Δ_rG°	Free energy of reaction at standard conditions
Δ_rH°	Enthalpy of reaction at standard conditions
Δ_rS°	Entropy of reaction at standard conditions

Data from NIST Standard Reference Database 69: NIST Chemistry WebBook
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