Formic acid
- Formula: CH2O2
- Molecular weight: 46.0254
- IUPAC Standard InChIKey: BDAGIHXWWSANSR-UHFFFAOYSA-N
- CAS Registry Number: 64-18-6
- 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. - Other names: Methanoic acid; Aminic acid; Bilorin; Collo-Bueglatt; Collo-Didax; Formisoton; Formylic acid; Hydrogen carboxylic acid; Myrmicyl; HCOOH; Acide formique; Acido formico; Ameisensaeure; Kwas metaniowy; Kyselina mravenci; Mierenzuur; Rcra waste number U123; UN 1779; Formira; Add-F; Amasil
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Gas phase thermochemistry data
Go To: Top, 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 as indicated in comments:
ALS - Hussein Y. Afeefy, Joel F. Liebman, and Stephen E. Stein
DRB - Donald R. Burgess, Jr.
GT - Glushko Thermocenter, Russian Academy of Sciences, Moscow
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔfH°gas | -378.6 | kJ/mol | Cm | Guthrie, 1974 | Heat of hydrolysis; ALS |
ΔfH°gas | -379.0 | kJ/mol | N/A | Lebedeva, 1964 | Value computed using ΔfHliquid° value of -425.5±0.3 kj/mol from Lebedeva, 1964 and ΔvapH° value of 46.5 kj/mol from Guthrie, 1974.; DRB |
ΔfH°gas | -379.2 ± 0.6 | kJ/mol | Ccb | Lebedeva, 1964 | Value computed using ΔfHliquid° from Lebedeva, 1964 and ΔvapH° value of 46.3 kJ/mol from Konicek and Wadso, 1970.; DRB |
ΔfH°gas | -378.3 | kJ/mol | N/A | Sinke, 1959 | Value computed using ΔfHliquid° value of -424.8±0.3 kj/mol from Sinke, 1959 and ΔvapH° value of 46.5 kj/mol from Guthrie, 1974.; DRB |
ΔfH°gas | -378.5 ± 0.6 | kJ/mol | Ccb | Sinke, 1959 | Value computed using ΔfHliquid° from Sinke, 1959 and ΔvapH° value of 46.3 kJ/mol from Konicek and Wadso, 1970.; DRB |
Quantity | Value | Units | Method | Reference | Comment |
S°gas | 248.70 ± 0.42 | J/mol*K | N/A | Millikan R.C., 1957 | Other third-law S(298.15 K) value is 248.11(1.26) J/mol*K [ Halford J.O., 1942, Millikan R.C., 1957]. Please also see Waring W., 1952.; GT |
Constant pressure heat capacity of gas
Cp,gas (J/mol*K) | Temperature (K) | Reference | Comment |
---|---|---|---|
33.26 | 50. | Chao J., 1986 | p=1 bar. Selected entropies and heat capacities are in close agreement with statistically calculated values [ Fukushima K., 1971] and value of S(298.15 K) calculated by ab initio method [ East A.L.L., 1997]. Maximum discrepancies with other statistical calculations [ Waring W., 1952, Green J.H.S., 1961, Gurvich, Veyts, et al., 1989] amount to 1.1-3.9 J/mol*K for S(T) and 3.0-5.9 J/mol*K for Cp(T). Please also see Chao J., 1978.; GT |
33.44 | 100. | ||
34.91 | 150. | ||
37.83 | 200. | ||
43.54 | 273.15 | ||
45.68 ± 0.07 | 298.15 | ||
45.84 | 300. | ||
54.52 | 400. | ||
62.63 | 500. | ||
69.81 | 600. | ||
76.04 | 700. | ||
81.34 | 800. | ||
85.77 | 900. | ||
89.40 | 1000. | ||
92.33 | 1100. | ||
94.65 | 1200. | ||
96.48 | 1300. | ||
97.91 | 1400. | ||
99.02 | 1500. |
Condensed phase thermochemistry data
Go To: Top, Gas 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 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 |
---|---|---|---|---|---|
ΔfH°liquid | -425.09 | kJ/mol | Cm | Guthrie, 1974 | Heat of hydrolysis; ALS |
ΔfH°liquid | -425.5 ± 0.3 | kJ/mol | Ccb | Lebedeva, 1964 | ALS |
ΔfH°liquid | -424.8 ± 0.3 | kJ/mol | Ccb | Sinke, 1959 | ALS |
Quantity | Value | Units | Method | Reference | Comment |
ΔcH°liquid | -253.8 ± 0.3 | kJ/mol | Ccb | Lebedeva, 1964 | Corresponding ΔfHºliquid = -425.51 kJ/mol (simple calculation by NIST; no Washburn corrections); ALS |
ΔcH°liquid | -254.6 ± 0.3 | kJ/mol | Ccb | Sinke, 1959 | Corresponding ΔfHºliquid = -424.72 kJ/mol (simple calculation by NIST; no Washburn corrections); ALS |
Quantity | Value | Units | Method | Reference | Comment |
S°liquid | 131.84 | J/mol*K | N/A | Stout and Fisher, 1941 | Includes 2.89 J/mol*K for zero-point entropy.; DH |
S°liquid | 128.4 | J/mol*K | N/A | Parks, Kelley, et al., 1929 | Extrapolation below 90 K, 29.7 J/mol*K. Revision of previous data.; DH |
S°liquid | 143.1 | J/mol*K | N/A | Gibson, Latimer, et al., 1920 | Used Berthelot's value, 10125 J/mol for H fusion. Extrapolation below 70 K, no details.; DH |
Constant pressure heat capacity of liquid
Cp,liquid (J/mol*K) | Temperature (K) | Reference | Comment |
---|---|---|---|
99.04 | 298.15 | Stout and Fisher, 1941 | T = 15 to 300 K.; DH |
98.10 | 298.15 | Glagoleva and Chervov, 1936 | Temperature range: 298.15, 333.15, 353.15 K.; DH |
100.0 | 290. | Radulescu and Jula, 1934 | DH |
98.3 | 291.5 | Gibson, Latimer, et al., 1920 | T = 71 to 292 K. Value is unsmoothed experimental datum.; DH |
95.4 | 298. | von Reis, 1881 | T = 291 to 385 K.; DH |
Reaction thermochemistry data
Go To: Top, Gas phase thermochemistry data, Condensed phase 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 as indicated in comments:
B - John E. Bartmess
M - Michael M. Meot-Ner (Mautner) and Sharon G. Lias
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.
Individual Reactions
By formula: Cl- + CH2O2 = (Cl- • CH2O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 115. ± 8.4 | kJ/mol | TDAs | French, Ikuta, et al., 1982 | gas phase; B,M |
ΔrH° | 116. ± 8.8 | kJ/mol | CIDT | Walker and Sunderlin, 1999 | gas phase; B |
ΔrH° | 107. ± 8.4 | kJ/mol | IMRE | Larson and McMahon, 1984 | gas phase; B,M |
ΔrH° | 156. ± 8.4 | kJ/mol | TDAs | Yamdagni and Kebarle, 1971 | gas phase; In serious disagreement with other's values. Source of error not obvious.; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 103. | J/mol*K | PHPMS | French, Ikuta, et al., 1982 | gas phase; M |
ΔrS° | 101. | 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 |
ΔrS° | 166. | J/mol*K | PHPMS | Yamdagni and Kebarle, 1971 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 84.1 ± 8.4 | kJ/mol | TDAs | French, Ikuta, et al., 1982 | gas phase; B |
ΔrG° | 77.0 ± 8.4 | kJ/mol | IMRE | Larson and McMahon, 1984 | gas phase; B,M |
ΔrG° | 106. ± 8.4 | kJ/mol | TDAs | Yamdagni and Kebarle, 1971 | gas phase; In serious disagreement with other's values. Source of error not obvious.; B |
By formula: CHO2- + H+ = CH2O2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1449. ± 5.0 | kJ/mol | D-EA | Kim, Bradforth, et al., 1995 | gas phase; dHacid(0K) = 344.67±0.62 kcal/mol; B |
ΔrH° | 1445. ± 9.2 | kJ/mol | G+TS | Caldwell, Renneboog, et al., 1989 | gas phase; B |
ΔrH° | 1445. ± 9.2 | kJ/mol | G+TS | Fujio, McIver, et al., 1981 | gas phase; value altered from reference due to change in acidity scale; B |
ΔrH° | 1444. ± 12. | kJ/mol | G+TS | Cumming and Kebarle, 1978 | gas phase; B |
ΔrH° | 1423. ± 19. | kJ/mol | EIAE | Muftakhov, Vasil'ev, et al., 1999 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 1419. ± 6.3 | kJ/mol | H-TS | Kim, Bradforth, et al., 1995 | gas phase; dHacid(0K) = 344.67±0.62 kcal/mol; B |
ΔrG° | 1415. ± 8.4 | kJ/mol | IMRE | Caldwell, Renneboog, et al., 1989 | gas phase; B |
ΔrG° | 1416. ± 8.4 | kJ/mol | IMRE | Fujio, McIver, et al., 1981 | gas phase; value altered from reference due to change in acidity scale; B |
ΔrG° | 1415. ± 8.4 | kJ/mol | IMRE | Cumming and Kebarle, 1978 | gas phase; B |
By formula: F- + CH2O2 = (F- • CH2O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 190. ± 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 |
ΔrS° | 101. | 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 |
ΔrG° | 159. ± 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 |
By formula: CH5O+ + CH2O2 = (CH5O+ • CH2O2)
Bond type: Hydrogen bonds of the type OH-O between organics
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 134. | 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 |
ΔrS° | 116. | 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 |
ΔrG° | 99.6 | 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 |
By formula: I- + CH2O2 = (I- • CH2O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 79.1 ± 4.2 | kJ/mol | TDAs | Caldwell and Kebarle, 1984 | gas phase; B,M |
ΔrH° | 54.0 ± 8.8 | kJ/mol | CIDT | Walker and Sunderlin, 1999 | gas phase; Authors suggest real value somewhere between this and Caldwell and Kebarle, 1984; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 86.6 | J/mol*K | PHPMS | Caldwell and Kebarle, 1984 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 53.1 ± 4.2 | kJ/mol | TDAs | Caldwell and Kebarle, 1984 | gas phase; B |
By formula: (Cl- • CH2O2) + CH2O2 = (Cl- • 2CH2O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 46.9 ± 8.8 | kJ/mol | CIDT | Walker and Sunderlin, 1999 | gas phase; B |
ΔrH° | 143. ± 13. | kJ/mol | N/A | Luczynski, Wlodek, et al., 1978 | gas phase; Buffer gas: H2. Value too bound based on French, Ikuta, et al., 1982, by Grimsrud fractionation factor ( Williamson, Knighton, et al., 1996).; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 230. | J/mol*K | HPMS | Luczynski, Wlodek, et al., 1978 | gas phase; Entropy change is questionable; M |
By formula: (Cl- • 4CH2O2) + CH2O2 = (Cl- • 5CH2O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 42.3 ± 8.4 | kJ/mol | N/A | Luczynski, Wlodek, et al., 1978 | gas phase; Buffer gas: H2. Value too bound based on French, Ikuta, et al., 1982, by Grimsrud fractionation factor ( Williamson, Knighton, et al., 1996).; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 48.1 | J/mol*K | HPMS | Luczynski, Wlodek, et al., 1978 | gas phase; Entropy change is questionable; M |
By formula: (Cl- • 2CH2O2) + CH2O2 = (Cl- • 3CH2O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 93. ± 11. | kJ/mol | N/A | Luczynski, Wlodek, et al., 1978 | gas phase; Buffer gas: H2. Value too bound based on French, Ikuta, et al., 1982, by Grimsrud fractionation factor ( Williamson, Knighton, et al., 1996).; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 150. | J/mol*K | HPMS | Luczynski, Wlodek, et al., 1978 | gas phase; Entropy change is questionable; M |
By formula: CHO2- + CH2O2 = (CHO2- • CH2O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 154. ± 4.2 | kJ/mol | N/A | Meot-Ner and Sieck, 1986 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 164. | J/mol*K | PHPMS | Meot-Ner and Sieck, 1986 | gas phase; large ΔrH, ΔrS,; cyclic structure? pyrolysis?; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 105. ± 6.7 | kJ/mol | TDAs | Meot-Ner and Sieck, 1986 | gas phase; B |
By formula: (CHO2- • 4CH2O2) + CH2O2 = (CHO2- • 5CH2O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 42.3 ± 8.4 | kJ/mol | N/A | Luczynski, Wlodek, et al., 1978 | gas phase; Buffer gas H2. There may be appreciable fractionation of neutral gases: Williamson, Knighton, et al., 1996; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 50. | J/mol*K | HPMS | Luczynski, Wlodek, et al., 1978 | gas phase; Entropy change is questionable; M |
By formula: (Cl- • 3CH2O2) + CH2O2 = (Cl- • 4CH2O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 59.0 ± 9.2 | kJ/mol | N/A | Luczynski, Wlodek, et al., 1978 | gas phase; Buffer gas: H2. Value too bound based on French, Ikuta, et al., 1982, by Grimsrud fractionation factor ( Williamson, Knighton, et al., 1996).; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 84. | J/mol*K | HPMS | Luczynski, Wlodek, et al., 1978 | gas phase; M |
By formula: (CHO2- • 3CH2O2) + CH2O2 = (CHO2- • 4CH2O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 59.4 ± 8.8 | kJ/mol | N/A | Luczynski, Wlodek, et al., 1978 | gas phase; Buffer gas H2. There may be appreciable fractionation of neutral gases: Williamson, Knighton, et al., 1996; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 90.0 | J/mol*K | HPMS | Luczynski, Wlodek, et al., 1978 | gas phase; M |
By formula: (CHO2- • 2CH2O2) + CH2O2 = (CHO2- • 3CH2O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 84. ± 11. | kJ/mol | N/A | Luczynski, Wlodek, et al., 1978 | gas phase; Buffer gas H2. There may be appreciable fractionation of neutral gases: Williamson, Knighton, et al., 1996; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 130. | J/mol*K | HPMS | Luczynski, Wlodek, et al., 1978 | gas phase; M |
By formula: (CHO2- • CH2O2) + CH2O2 = (CHO2- • 2CH2O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 109. ± 13. | kJ/mol | N/A | Luczynski, Wlodek, et al., 1978 | gas phase; Buffer gas H2. There may be appreciable fractionation of neutral gases: Williamson, Knighton, et al., 1996; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 140. | J/mol*K | HPMS | Luczynski, Wlodek, et al., 1978 | gas phase; M |
By formula: CH6N+ + CH2O2 = (CH6N+ • CH2O2)
Bond type: Hydrogen bonds of the type NH+-O between organics
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 79.5 | kJ/mol | PHPMS | Meot-Ner, 1984 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 101. | J/mol*K | PHPMS | Meot-Ner, 1984 | gas phase; M |
By formula: CH2NO5- + H2O + CH2O2 = CH4NO6-
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrG° | 18.4 ± 0.84 | kJ/mol | IMRE | Viidanoja, Reiner, et al., 2000 | gas phase; B |
+
= CH2BrO2-
By formula: Br- + CH2O2 = CH2BrO2-
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 72.0 ± 7.1 | kJ/mol | CIDT | Walker and Sunderlin, 1999 | gas phase; B |
By formula: CH2IO2- + 2CH2O2 = C2H4IO4-
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 41.8 ± 8.8 | kJ/mol | CIDT | Walker and Sunderlin, 1999 | gas phase; B |
+
= CH2NO5-
By formula: NO3- + CH2O2 = CH2NO5-
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrG° | 47.70 ± 0.84 | kJ/mol | IMRE | Viidanoja, Reiner, et al., 1998 | gas phase; B |
By formula: CH2BrO2- + 2CH2O2 = C2H4BrO4-
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 40. ± 7.1 | kJ/mol | CIDT | Walker and Sunderlin, 1999 | gas phase; B |
References
Go To: Top, Gas phase thermochemistry data, Condensed phase thermochemistry data, Reaction thermochemistry data, Notes
Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.
Guthrie, 1974
Guthrie, J.P.,
Hydration of carboxamides. Evaluation of the free energy change for addition of water to acetamide and formamide derivatives,
J. Am. Chem. Soc., 1974, 96, 3608-3615. [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]
Konicek and Wadso, 1970
Konicek, J.; Wadso, I.,
Enthalpies of vaporization of organic compounds. VII. Some carboxylic acids,
Acta Chem. Scand., 1970, 24, 2612-26. [all data]
Sinke, 1959
Sinke, G.C.,
The heat of formation of formic acid,
J. Phys. Chem., 1959, 63, 2063. [all data]
Millikan R.C., 1957
Millikan R.C.,
Infrared spectra and vibrational assignment of monomeric formic acid,
J. Chem. Phys., 1957, 27, 1305-1308. [all data]
Halford J.O., 1942
Halford J.O.,
Entropy of the monomeric forms of formic acid and acetic acid,
J. Chem. Phys., 1942, 10, 582-584. [all data]
Waring W., 1952
Waring W.,
Some thermodynamic properties of formic acid,
Chem. Rev., 1952, 51, 171-183. [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]
Fukushima K., 1971
Fukushima K.,
Normal coordinate treatment and thermodynamic properties of the cis-trans isomers of formic acid and its deutero-analog,
J. Chem. Thermodyn., 1971, 3, 553-562. [all data]
East A.L.L., 1997
East A.L.L.,
Ab initio statistical thermodynamical models for the computation of third-law entropies,
J. Chem. Phys., 1997, 106, 6655-6674. [all data]
Green J.H.S., 1961
Green J.H.S.,
Thermodynamic properties of organic oxygen compounds. Part III. Formic acid,
J. Chem. Soc., 1961, 2241-2242. [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., 1978
Chao J.,
Ideal gas thermodynamic properties of methanoic and ethanoic acids,
J. Phys. Chem. Ref. Data, 1978, 7, 363-377. [all data]
Stout and Fisher, 1941
Stout, J.W.; Fisher, L.H.,
The entropy of formic acid. The heat capacity from 15 to 300K. Heats of fusion and vaporization,
J. Chem. Phys., 1941, 9, 163-168. [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]
Gibson, Latimer, et al., 1920
Gibson, G.E.; Latimer, W.M.; Parks, G.S.,
Entropy changes at low temperatures. I. Formic acid and urea. A test of the third law of thermodynamics,
J. Am. Chem. Soc., 1920, 42, 1533-1542. [all data]
Glagoleva and Chervov, 1936
Glagoleva, A.A.; Chervov, S.I.,
Investigation of the heat capacity of formic acid and its aqueous solutions,
Zhur. Obshch. Khim., 1936, 6, 685-690. [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]
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]
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]
Walker and Sunderlin, 1999
Walker, B.W.; Sunderlin, L.S.,
The thermochemistry of formic acid halide anion clusters,
Int. J. Mass Spectrom., 1999, 184, 2-3, 183-189, https://doi.org/10.1016/S1387-3806(99)00008-1
. [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]
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, 2
Larson, J.W.; McMahon, T.B.,
Gas phase negative ion chemistry of alkylchloroformates,
Can. J. Chem., 1984, 62, 675. [all data]
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Notes
Go To: Top, Gas phase thermochemistry data, Condensed phase thermochemistry data, Reaction thermochemistry data, References
- Symbols used in this document:
Cp,gas Constant pressure heat capacity of gas Cp,liquid Constant pressure heat capacity of liquid S°gas Entropy of gas at standard conditions S°liquid Entropy of liquid at standard conditions ΔcH°liquid Enthalpy of combustion of liquid at standard conditions ΔfH°gas Enthalpy of formation of gas at standard conditions ΔfH°liquid Enthalpy of formation of liquid at standard conditions ΔrG° Free energy of reaction at standard conditions ΔrH° Enthalpy of reaction at standard conditions ΔrS° Entropy of reaction at standard conditions - Data from NIST Standard Reference Database 69: NIST Chemistry WebBook
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