Formaldehyde
- Formula: CH2O
- Molecular weight: 30.0260
- IUPAC Standard InChIKey: WSFSSNUMVMOOMR-UHFFFAOYSA-N
- CAS Registry Number: 50-00-0
- 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:
- Other names: Methanal; BFV; Fannoform; Formaldehyde, gas; Formalin; Formalith; Formic aldehyde; Formol; Fyde; Lysoform; Methyl aldehyde; Methylene oxide; Morbicid; Oxomethane; Oxymethylene; Paraform; Superlysoform; Karsan; Methaldehyde; Aldehyde formique; Aldeide formica; Formaldehyd; Formalin-loesungen; Formalina; Formaline; NCI-C02799; Oplossingen; Aldehyd mravenci; Formalin 40; Rcra waste number U122; UN 1198; UN 2209; H2CO; Durine; Hercules 37M6-8; CH2O; NSC 298885; Fordor
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Gas phase thermochemistry data
Go To: Top, Reaction thermochemistry data, Vibrational and/or electronic energy levels, 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
GT - Glushko Thermocenter, Russian Academy of Sciences, Moscow
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔfH°gas | -115.90 | kJ/mol | Review | Chase, 1998 | Data last reviewed in March, 1961 |
ΔfH°gas | -108.6 ± 0.46 | kJ/mol | Cm | Fletcher and Pilcher, 1970 | ALS |
Quantity | Value | Units | Method | Reference | Comment |
ΔcH°gas | -570.78 ± 0.42 | kJ/mol | Cm | Fletcher and Pilcher, 1970 | Corresponding ΔfHºgas = -108.6 kJ/mol (simple calculation by NIST; no Washburn corrections); ALS |
ΔcH°gas | -561.1 | kJ/mol | Ccb | Wartenberg and Lerner-Steinberg, 1925 | Gas phase; Corresponding ΔfHºgas = -118. kJ/mol (simple calculation by NIST; no Washburn corrections); ALS |
Quantity | Value | Units | Method | Reference | Comment |
S°gas,1 bar | 218.95 | J/mol*K | Review | Chase, 1998 | Data last reviewed in March, 1961 |
Constant pressure heat capacity of gas
Cp,gas (J/mol*K) | Temperature (K) | Reference | Comment |
---|---|---|---|
33.26 | 50. | Thermodynamics Research Center, 1997 | p=1 bar. Recommended entropies and heat capacities are in good agreement with other statistically calculated values [ Thompson, 1941, Pillai M.G.K., 1961, Gurvich, Veyts, et al., 1989]. Please also see Chao J., 1980, Chao J., 1986.; GT |
33.26 | 100. | ||
33.28 | 150. | ||
33.50 | 200. | ||
34.70 | 273.15 | ||
35.39 ± 0.02 | 298.15 | ||
35.44 | 300. | ||
39.24 | 400. | ||
43.74 | 500. | ||
48.18 | 600. | ||
52.28 | 700. | ||
55.94 | 800. | ||
59.16 | 900. | ||
61.95 | 1000. | ||
64.37 | 1100. | ||
66.45 | 1200. | ||
68.25 | 1300. | ||
69.80 | 1400. | ||
71.15 | 1500. | ||
73.79 | 1750. | ||
75.68 | 2000. | ||
77.08 | 2250. | ||
78.13 | 2500. | ||
78.93 | 2750. | ||
79.56 | 3000. |
Gas Phase Heat Capacity (Shomate Equation)
Cp° = A + B*t + C*t2 + D*t3 +
E/t2
H° − H°298.15= A*t + B*t2/2 +
C*t3/3 + D*t4/4 − E/t + F − H
S° = A*ln(t) + B*t + C*t2/2 + D*t3/3 −
E/(2*t2) + G
Cp = heat capacity (J/mol*K)
H° = standard enthalpy (kJ/mol)
S° = standard entropy (J/mol*K)
t = temperature (K) / 1000.
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Temperature (K) | 298. to 1200. | 1200. to 6000. |
---|---|---|
A | 5.193767 | 71.35268 |
B | 93.23249 | 6.174497 |
C | -44.85457 | -1.191090 |
D | 7.882279 | 0.079564 |
E | 0.551175 | -15.58917 |
F | -119.3591 | -170.6327 |
G | 202.4663 | 262.3180 |
H | -115.8972 | -115.8972 |
Reference | Chase, 1998 | Chase, 1998 |
Comment | Data last reviewed in March, 1961 | Data last reviewed in March, 1961 |
Reaction thermochemistry data
Go To: Top, Gas phase thermochemistry data, Vibrational and/or electronic energy levels, 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
ALS - Hussein Y. Afeefy, Joel F. Liebman, and Stephen E. Stein
RCD - Robert C. Dunbar
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: CH3O+ + CH2O = (CH3O+ • CH2O)
Bond type: Hydrogen bonds of the type OH-O between organics
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 116. | kJ/mol | ICR | Larson and McMahon, 1982 | gas phase; switching reaction(H3O+)H2O, Entropy change calculated or estimated; Cunningham, Payzant, et al., 1972, Lias, Liebman, et al., 1984, Keesee and Castleman, 1986; M |
ΔrH° | 123. | kJ/mol | FA | Fehsenfeld, Dotan, et al., 1978 | gas phase; From thermochemical cycle,switching reaction(H3O+)H2O; Lias, Liebman, et al., 1984, Meot-Ner (Mautner), 1992; M |
ΔrH° | 116. | kJ/mol | ICR | Larson, Clair, et al., 1982 | gas phase; From thermochemical cycle,switching reaction(H2O/H2CO), Entropy change calculated or estimated; Cunningham, Payzant, et al., 1972, Lias, Liebman, et al., 1984; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 111. | J/mol*K | N/A | Larson and McMahon, 1982 | gas phase; switching reaction(H3O+)H2O, Entropy change calculated or estimated; Cunningham, Payzant, et al., 1972, Lias, Liebman, et al., 1984, Keesee and Castleman, 1986; M |
ΔrS° | 115. | J/mol*K | FA | Fehsenfeld, Dotan, et al., 1978 | gas phase; From thermochemical cycle,switching reaction(H3O+)H2O; Lias, Liebman, et al., 1984, Meot-Ner (Mautner), 1992; M |
ΔrS° | 111. | J/mol*K | N/A | Larson, Clair, et al., 1982 | gas phase; From thermochemical cycle,switching reaction(H2O/H2CO), Entropy change calculated or estimated; Cunningham, Payzant, et al., 1972, Lias, Liebman, et al., 1984; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 82.8 | kJ/mol | ICR | Larson and McMahon, 1982 | gas phase; switching reaction(H3O+)H2O, Entropy change calculated or estimated; Cunningham, Payzant, et al., 1972, Lias, Liebman, et al., 1984, Keesee and Castleman, 1986; M |
ΔrG° | 82.8 | kJ/mol | ICR | Larson, Clair, et al., 1982 | gas phase; From thermochemical cycle,switching reaction(H2O/H2CO), Entropy change calculated or estimated; Cunningham, Payzant, et al., 1972, Lias, Liebman, et al., 1984; M |
By formula: Li+ + CH2O = (Li+ • CH2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 151. | kJ/mol | ICR | Woodin and Beauchamp, 1978 | gas phase; switching reaction(Li+)H2O, Entropy change calculated or estimated; Dzidic and Kebarle, 1970 interpolated; M |
ΔrH° | 150. | kJ/mol | ICR | Staley and Beauchamp, 1975 | gas phase; switching reaction(Li+)H2O, from graph; Dzidic and Kebarle, 1970 extrapolated; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 110. | J/mol*K | N/A | Woodin and Beauchamp, 1978 | gas phase; switching reaction(Li+)H2O, Entropy change calculated or estimated; Dzidic and Kebarle, 1970 interpolated; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 118. | kJ/mol | ICR | Woodin and Beauchamp, 1978 | gas phase; switching reaction(Li+)H2O, Entropy change calculated or estimated; Dzidic and Kebarle, 1970 interpolated; M |
(CH3O- • 4294967295) + = CH3O-
By formula: (CH3O- • 4294967295CH2O) + CH2O = CH3O-
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 166.9 ± 2.1 | kJ/mol | N/A | Nee, Osterwalder, et al., 2006 | gas phase; B |
ΔrH° | 171. ± 4.6 | kJ/mol | Ther | Osborn, Leahy, et al., 1998 | gas phase; B |
ΔrH° | 175. ± 9.2 | kJ/mol | Ther | Bartmess, Scott, et al., 1979 | gas phase; The acidity is 1.2 kcal/mol stronger than that from the D-EA cycle, due to the multi-compound fit for the acidity scale.; value altered from reference due to change in acidity scale; B |
CHO- + =
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1650.7 ± 0.96 | kJ/mol | D-EA | Murray, Miller, et al., 1986 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 1617.7 ± 1.7 | kJ/mol | H-TS | Murray, Miller, et al., 1986 | gas phase; B |
ΔrG° | 1648. ± 19. | kJ/mol | IMRB | Karpas and Klein, 1975 | gas phase; B |
By formula: CH2N+ + CH2O = (CH2N+ • CH2O)
Bond type: Hydrogen bonds of the type NH+-O between organics
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrG° | 91.2 | kJ/mol | FA | Tanaka, Mackay, et al., 1978 | gas phase; switching reaction(HCNH+)HCN; Meot-Ner (Mautner), 1978; M |
By formula: C3H9NO = C2H7N + CH2O
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 126. ± 0.8 | kJ/mol | Cm | Rogers and Rapiejko, 1974 | liquid phase; Heat of formation derived by 77PED/RYL; ALS |
By formula: C3H8O2 + H2O = CH2O + 2CH4O
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 77.19 ± 0.50 | kJ/mol | Cm | Birley and Skinner, 1970 | liquid phase; Heat of hydrolysis; ALS |
By formula: CH2O + C3H8N2O = C4H10N2O2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -20. ± 0.8 | kJ/mol | Kin | Perepelkova, Igranova, et al., 1981 | liquid phase; solvent: Phosphate buffer; ALS |
By formula: 2C2H7N + CH2O = C5H14N2 + H2O
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -191. ± 3. | kJ/mol | Cm | Rogers and Rapiejko, 1974 | gas phase; ALS |
By formula: (Fe+ • 2CH2O) + CH2O = (Fe+ • 3CH2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 76.1 ± 4.2 | kJ/mol | CIDT | Rodgers and Armentrout, 2000 | RCD |
By formula: (Fe+ • 3CH2O) + CH2O = (Fe+ • 4CH2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 50.2 ± 7.1 | kJ/mol | CIDT | Rodgers and Armentrout, 2000 | RCD |
By formula: (Fe+ • CH2O) + CH2O = (Fe+ • 2CH2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 164. ± 4.2 | kJ/mol | CIDT | Rodgers and Armentrout, 2000 | RCD |
By formula: C2H7N + CH2O = C3H9NO
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -126. ± 0.8 | kJ/mol | Cm | Rogers and Rapiejko, 1974 | gas phase; ALS |
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -12.1 | kJ/mol | Eqk | Newton and Dodge, 1933 | gas phase; ALS |
By formula: Fe+ + CH2O = (Fe+ • CH2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 138. ± 7.1 | kJ/mol | CIDT | Rodgers and Armentrout, 2000 | RCD |
By formula: Al+ + CH2O = (Al+ • CH2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 115. ± 10. | kJ/mol | EqG | Bouchard, Brenner, et al., 1997 | RCD |
By formula: C3H6O3 = 3CH2O
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 194.0 ± 2.5 | kJ/mol | Eqk | Busfield and Merigold, 1969 | solid phase; ALS |
By formula: 3CH2O = C3H6O3
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -139.2 ± 2.1 | kJ/mol | Eqk | Busfield and Merigold, 1969 | gas phase; ALS |
Vibrational and/or electronic energy levels
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 by: Takehiko Shimanouchi
Symmetry: C2ν Symmetry Number σ = 2
Sym. | No | Approximate | Selected Freq. | Infrared | Raman | Comments | ||||
---|---|---|---|---|---|---|---|---|---|---|
Species | type of mode | Value | Rating | Value | Phase | Value | Phase | |||
a1 | 1 | CH2 s-str | 2783 | A | 2782.5 S | gas | 2781.6 S | liq. | ||
a1 | 2 | CO str | 1746 | A | 1746.1 VS | gas | 1742.3 W | liq. | ||
a1 | 3 | CH2 scis | 1500 | A | 1500.1 S | gas | 1499.7 M | liq. | ||
b1 | 4 | CH2 a-str | 2843 | A | 2843.1 VS | gas | 2866 W | liq. | ||
b1 | 5 | CH2 rock | 1249 | A | 1249.1 S | gas | ||||
b2 | 6 | CH2 wag | 1167 | A | 1167.3 S | gas | ||||
Source: Shimanouchi, 1972
Notes
VS | Very strong |
S | Strong |
M | Medium |
W | Weak |
A | 0~1 cm-1 uncertainty |
References
Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Vibrational and/or electronic energy levels, Notes
Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.
Chase, 1998
Chase, M.W., Jr.,
NIST-JANAF Themochemical Tables, Fourth Edition,
J. Phys. Chem. Ref. Data, Monograph 9, 1998, 1-1951. [all data]
Fletcher and Pilcher, 1970
Fletcher, R.A.; Pilcher, G.,
Measurements of heats of combustion by flame calorimetry,
Trans. Faraday Soc., 1970, 66, 794-799. [all data]
Wartenberg and Lerner-Steinberg, 1925
Wartenberg, H.; Lerner-Steinberg,
Heat of formation of formaldehyde,
Z. Angew. Chem., 1925, 38, 591-592. [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]
Thompson, 1941
Thompson, H.W.,
Thermodynamic functions and equilibria of formaldehyde, deuteroformaldehyde, phosgene and thiophosgene,
Trans. Faraday Soc., 1941, 37, 251-260. [all data]
Pillai M.G.K., 1961
Pillai M.G.K.,
Potential energy constants, rotational distortion constants, and calculated thermodynamic properties for some planar XYZ2 molecules,
J. Mol. Spectrosc., 1961, 6, 465-471. [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., 1980
Chao J.,
Perfect gas thermodynamic properties of methanal, ethanal and their deuterated species,
Thermochim. Acta, 1980, 41, 41-54. [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]
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]
Cunningham, Payzant, et al., 1972
Cunningham, A.J.; Payzant, J.D.; Kebarle, P.,
A Kinetic Study of the Proton Hydrate H+(H2O)n Equilibria in the Gas Phase,
J. Am. Chem. Soc., 1972, 94, 22, 7627, https://doi.org/10.1021/ja00777a003
. [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]
Fehsenfeld, Dotan, et al., 1978
Fehsenfeld, F.C.; Dotan, I.; Albritton, D.L.; Howard, C.J.; Ferguson, E.E.,
Stratospheric Positive Ion Chemistry of Formaldehyde and Methanol,
J. Geophys. Res., 1978, 83, C3, 1333, https://doi.org/10.1029/JC083iC03p01333
. [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, Clair, et al., 1982
Larson, J.W.; Clair, R.L.; McMahon, T.B.,
Bimolecular Production of Proton Bound Dimers in the Gas Phase. A Low Pressure Ion Cyclotron Resonance Technique for Examination of Solvent Exchange Equilibria and Determination of Single Molecule Solvation Energetics,
Can. J. Chem., 1982, 60, 4, 542, https://doi.org/10.1139/v82-079
. [all data]
Woodin and Beauchamp, 1978
Woodin, R.L.; Beauchamp, J.L.,
Bonding of Li+ to Lewis Bases in the Gas Phase. Reversals in Methyl Substituent Effects for Different Reference Acids,
J. Am. Chem. Soc., 1978, 100, 2, 501, https://doi.org/10.1021/ja00470a024
. [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]
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]
Nee, Osterwalder, et al., 2006
Nee, M.J.; Osterwalder, A.; Zhou, J.; Neumark, D.M.,
Slow electron velocity-map imaging photoelectron spectra of the methoxide anion,
J. Chem. Phys., 2006, 125, 1, 014306, https://doi.org/10.1063/1.2212411
. [all data]
Osborn, Leahy, et al., 1998
Osborn, D.L.; Leahy, D.J.; Kim, E.H.; deBeer, E.; Neumark, D.M.,
Photoelectron spectroscopy of CH3O- and CD3O-,
Chem. Phys. Lett., 1998, 292, 4-6, 651-655, https://doi.org/10.1016/S0009-2614(98)00717-9
. [all data]
Bartmess, Scott, et al., 1979
Bartmess, J.E.; Scott, J.A.; McIver, R.T., Jr.,
The gas phase acidity scale from methanol to phenol,
J. Am. Chem. Soc., 1979, 101, 6047. [all data]
Murray, Miller, et al., 1986
Murray, K.K.; Miller, T.M.; Leopold, D.G.; Lineberger, W.C.,
Laser photoelectron spectroscopy of the Formylf anion,
J. Chem. Phys., 1986, 84, 2520. [all data]
Karpas and Klein, 1975
Karpas, Z.; Klein, F.S.,
Negative ion-molecule reactions in a mixture of ammonia-formaldehyde - an ICR mass spectrometry study,
Int. J. Mass Spectrom. Ion Phys., 1975, 18, 65. [all data]
Tanaka, Mackay, et al., 1978
Tanaka, K.; Mackay, G.I.; Bohme, D.K.,
Rate and Equilibrium Constant Measurements for Gas-Phase Proton-Transfer Reactions Involving H2O, H2S, HCN, and H2CO,
Can. J. Chem., 1978, 56, 2, 193, https://doi.org/10.1139/v78-031
. [all data]
Meot-Ner (Mautner), 1978
Meot-Ner (Mautner), M.,
Solvation of the Proton by HCN and CH3CN. Condensation of HCN with Ions in the Gas Phase.,
J. Am. Chem. Soc., 1978, 100, 15, 4694, https://doi.org/10.1021/ja00483a012
. [all data]
Rogers and Rapiejko, 1974
Rogers, F.E.; Rapiejko, R.J.,
Thermochemistry of carbonyl addition reactions. II. Enthalpy of addition of dimethylamine to formaldehyde,
J. Phys. Chem., 1974, 78, 599-603. [all data]
Birley and Skinner, 1970
Birley, G.I.; Skinner, H.A.,
Enthalpies of hydrolysis of dimethoxymethane and 1,1-dimethoxyethane,
Trans. Faraday Soc., 1970, 66, 791-793. [all data]
Perepelkova, Igranova, et al., 1981
Perepelkova, T.I.; Igranova, E.G.; Moiseev, V.D.; Demchenko, L.Ya.; Zhuravleva, I.I.,
Calorimetric study of the methylolation of 1,1-dimethylurea,
Khim. Promst. Ser. Proizvod. Pererab. Plastmass Sint. Smol, 1981, 15-18. [all data]
Rodgers and Armentrout, 2000
Rodgers, M.T.; Armentrout, P.B.,
Noncovalent Metal-Ligand Bond Energies as Studied by Threshold Collision-Induced Dissociation,
Mass Spectrom. Rev., 2000, 19, 4, 215, https://doi.org/10.1002/1098-2787(200007)19:4<215::AID-MAS2>3.0.CO;2-X
. [all data]
Newton and Dodge, 1933
Newton, R.H.; Dodge, B.F.,
The equilibrium between carbon monoxide, hydrogen, formaldehyde and methanol. I. The reactions CO + H2 = HCOH and H2 + HCOH = CH3OH,
J. Am. Chem. Soc., 1933, 55, 4747-4759. [all data]
Bouchard, Brenner, et al., 1997
Bouchard, F.; Brenner, V.; Carra, C.; Hepburn, J.W.; Koyanagi, G.K.; McMahon, T.B.; Ohanessian, G.; Peschke, M.,
Energetics and Structure of Complexes of Al+ with Small Organic Molecules in the Gas Phase,
J. Phys. Chem. A, 1997, 101, 33, 5885, https://doi.org/10.1021/jp9703465
. [all data]
Busfield and Merigold, 1969
Busfield, W.K.; Merigold, D.,
The gas-phase equilibrium between trioxan and formaldehyde: The standard enthalpy and entropy of the trimerisation of formaldehyde,
J. Chem. Soc. A, 1969, 19, 2975-2977. [all data]
Shimanouchi, 1972
Shimanouchi, T.,
Tables of Molecular Vibrational Frequencies Consolidated Volume I, National Bureau of Standards, 1972, 1-160. [all data]
Notes
Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Vibrational and/or electronic energy levels, References
- Symbols used in this document:
Cp,gas Constant pressure heat capacity of gas S°gas,1 bar Entropy of gas at standard conditions (1 bar) ΔcH°gas Enthalpy of combustion of gas at standard conditions ΔfH°gas Enthalpy of formation of gas 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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