Hydrogen iodide
- Formula: HI
- Molecular weight: 127.91241
- IUPAC Standard InChIKey: XMBWDFGMSWQBCA-UHFFFAOYSA-N
- CAS Registry Number: 10034-85-2
- Chemical structure:
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Gas phase thermochemistry data
Go To: Top, Phase change 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.
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔfH°gas | 26.50 ± 0.10 | kJ/mol | Review | Cox, Wagman, et al., 1984 | CODATA Review value |
ΔfH°gas | 26.36 | kJ/mol | Review | Chase, 1998 | Data last reviewed in September, 1961 |
Quantity | Value | Units | Method | Reference | Comment |
S°gas,1 bar | 206.59 | J/mol*K | Review | Chase, 1998 | Data last reviewed in September, 1961 |
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 1400. | 1400. to 6000. |
---|---|---|
A | 26.04540 | 35.44358 |
B | 4.689678 | 1.414708 |
C | 4.911765 | -0.182088 |
D | -2.654397 | 0.011768 |
E | 0.121419 | -4.054561 |
F | 18.75499 | 7.919099 |
G | 237.2018 | 240.1097 |
H | 26.35903 | 26.35903 |
Reference | Chase, 1998 | Chase, 1998 |
Comment | Data last reviewed in September, 1961 | Data last reviewed in September, 1961 |
Phase change 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:
TRC - Thermodynamics Research Center, NIST Boulder Laboratories, Chris Muzny director
AC - William E. Acree, Jr., James S. Chickos
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
Tfus | 222.15 | K | N/A | Beckmann and Waentig, 1910 | Uncertainty assigned by TRC = 1.5 K; TRC |
Enthalpy of vaporization
ΔvapH (kJ/mol) | Temperature (K) | Method | Reference | Comment |
---|---|---|---|---|
19.8 | 238. | C | Giauque and Wiebe, 1929 | AC |
Antoine Equation Parameters
log10(P) = A − (B / (T + C))
P = vapor pressure (bar)
T = temperature (K)
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Temperature (K) | A | B | C | Reference | Comment |
---|---|---|---|---|---|
149.8 to 238.1 | 4.26854 | 939.994 | -18.012 | Stull, 1947 | Coefficents calculated by NIST from author's data. |
Reaction thermochemistry data
Go To: Top, Gas phase thermochemistry data, Phase change 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:
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
MS - José A. Martinho Simões
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: I- + HI = (I- • HI)
Bond type: Hydrogen bond (negative ion to hydride)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 71.1 ± 8.4 | kJ/mol | TDEq | Caldwell and Kebarle, 1985 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 102. | J/mol*K | PHPMS | Caldwell and Kebarle, 1985 | gas phase; switching reaction(I-)SO2; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 41. ± 11. | kJ/mol | TDEq | Caldwell and Kebarle, 1985 | gas phase; B |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
41. | 300. | PHPMS | Caldwell and Kebarle, 1985 | gas phase; switching reaction(I-)SO2; M |
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1315.24 ± 0.084 | kJ/mol | D-EA | Pelaez, Blondel, et al., 2009 | gas phase; Given: 3.0590463(38) eV; B |
ΔrH° | 1312.1 | kJ/mol | N/A | Check, Faust, et al., 2001 | gas phase; Fe(CO)2-(q); ; ΔS(EA)=5.0; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 1294.03 ± 0.25 | kJ/mol | H-TS | Pelaez, Blondel, et al., 2009 | gas phase; Given: 3.0590463(38) eV; B |
ΔrG° | 1290.8 | kJ/mol | N/A | Check, Faust, et al., 2001 | gas phase; Fe(CO)2-(q); ; ΔS(EA)=5.0; B |
By formula: HI + C3H5I = C3H6 + I2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -33.3 ± 1.4 | kJ/mol | Eqk | Rodgers, Golden, et al., 1966 | gas phase; ALS |
ΔrH° | -39.7 ± 4.2 | kJ/mol | Eqk | Rodgers, Golden, et al., 1966 | gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -34.9 ± 0.96 kJ/mol; At 527 K; ALS |
By formula: HI + CH3I = CH4 + I2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -52.55 ± 0.54 | kJ/mol | Eqk | Golden, Walsh, et al., 1965 | gas phase; ALS |
ΔrH° | -53.0 ± 0.2 | kJ/mol | Eqk | Goy and Pritchard, 1965 | gas phase; ALS |
ΔrH° | -46.2 ± 5.6 | kJ/mol | Cm | Nichol and Ubbelohde, 1952 | gas phase; ALS |
By formula: C5HMnO5 (l) + I2 (cr) = HI (g) + C5IMnO5 (cr)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -108. ± 8. | kJ/mol | RSC | Connor, Zafarani-Moattar, et al., 1982 | The reaction enthalpy relies on -25. ± 5. kJ/mol for the enthalpy of solution of HI(g) in benzene Connor, Zafarani-Moattar, et al., 1982.; MS |
By formula: C2H3IO + H2O = HI + C2H4O2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -93.97 | kJ/mol | Cm | Devore and O'Neal, 1969 | liquid phase; Heat of hydrolysis; ALS |
ΔrH° | -90.33 | kJ/mol | Cm | Carson and Skinner, 1949 | liquid phase; Heat of hydrolysis; ALS |
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -81. ± 2. | kJ/mol | Eqk | Benson and Amano, 1962 | gas phase; ALS |
ΔrH° | -80.1 ± 4.2 | kJ/mol | Eqk | Jones and Ogg, 1937 | gas phase; At 408-464 K; ALS |
By formula: HI + C6H11I = C6H12 + I2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -32.6 ± 8.4 | kJ/mol | Cm | Brennan and Ubbelohde, 1956 | gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -28. ± 4.2 kJ/mol; ALS |
By formula: C2H3F3 + I2 = HI + C2H2F3I
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -64. ± 2. | kJ/mol | Eqk | Wu and Rodgers, 1974 | gas phase; Heat of formation Unpublished results by B.J. Zwolinski; ALS |
By formula: C7H9NO + C7H5IO = HI + C14H13NO2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -185. ± 2. | kJ/mol | Cac | Kiselev, Khuzyasheva, et al., 1979 | liquid phase; solvent: Benzene; ALS |
By formula: C7H9N + C7H5IO = HI + C14H13NO
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -168. ± 2. | kJ/mol | Cac | Kiselev, Khuzyasheva, et al., 1979 | liquid phase; solvent: Benzene; ALS |
By formula: C7H5IO + C6H7N = HI + C13H11NO
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -166. ± 2. | kJ/mol | Cac | Kiselev, Khuzyasheva, et al., 1979 | liquid phase; solvent: Benzene; ALS |
(cr) +
(solution) =
(solution) + C8H5IO3W (solution)
By formula: C8H6O3W (cr) + I2 (solution) = HI (solution) + C8H5IO3W (solution)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -67.4 ± 3.8 | kJ/mol | RSC | Landrum and Hoff, 1985 | solvent: Dichloromethane; MS |
C8H6MoO3 (cr) + (solution) = C8H5IMoO3 (solution) +
(solution)
By formula: C8H6MoO3 (cr) + I2 (solution) = C8H5IMoO3 (solution) + HI (solution)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -75.3 ± 2.5 | kJ/mol | RSC | Landrum and Hoff, 1985 | solvent: Dichloromethane; MS |
By formula: 2C3H8S + I2 = 2HI + C6H14S2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -124.9 | kJ/mol | Cm | Sunner, 1955 | liquid phase; solvent: Ethanol/water(90/10); ALS |
By formula: 2C5H12S + I2 = 2HI + C10H22S2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -124.9 | kJ/mol | Cm | Sunner, 1955 | liquid phase; solvent: Ethanol/water(90/10); ALS |
By formula: C4H10S2 + I2 = 2HI + C4H8S2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -123.2 | kJ/mol | Cm | Sunner, 1955 | liquid phase; solvent: Ethanol/water(90/10); ALS |
By formula: C8H16O2S2 + I2 = 2HI + C8H14O2S2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -109.6 | kJ/mol | Cm | Sunner, 1955 | liquid phase; solvent: Ethanol/water(90/10); ALS |
By formula: C3H8S2 + I2 = 2HI + C3H6S2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -107.7 | kJ/mol | Cm | Sunner, 1955 | liquid phase; solvent: Ethanol/water(90/10); ALS |
By formula: HI + C7H7I = C7H8 + I2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -33. ± 4.6 | kJ/mol | Cm | Graham, Nichol, et al., 1955 | liquid phase; solvent: p-Xylene; ALS |
By formula: C3H5I + H2O = HI + C3H6O
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -8.79 | kJ/mol | Cm | Gellner and Skinner, 1949 | liquid phase; Heat of hydrolysis; ALS |
By formula: C7H7I + H2O = HI + C7H8O
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -12.6 | kJ/mol | Cm | Gellner and Skinner, 1949 | liquid phase; Heat of hydrolysis; ALS |
By formula: C7H5IO + H2O = HI + C7H6O2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -102.4 | kJ/mol | Cm | Carson, Pritchard, et al., 1950 | liquid phase; Heat of hydrolysis; ALS |
C3H9ISn (l) + (l) = (
• 55
) (solution) + C3H10OSn (cr)
By formula: C3H9ISn (l) + H2O (l) = (HI • 55H2O) (solution) + C3H10OSn (cr)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -17.6 ± 0.4 | kJ/mol | RSC | Baldwin, Lappert, et al., 1972 | MS |
By formula: HI + CH3IS = CH4S + I2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -12.0 ± 2.3 | kJ/mol | Eqk | Shum and Benson, 1983 | gas phase; ALS |
By formula: C3H6O + I2 = HI + C3H5IO
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 50.6 ± 5.0 | kJ/mol | Eqk | Solly, Golden, et al., 1970 | gas phase; ALS |
By formula: C2H4O + I2 = HI + C2H3IO
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3. ± 2. | kJ/mol | Eqk | Walsh and Benson, 1966 | gas phase; ALS |
By formula: HI + C7H7IO = C7H8O + I2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -29. ± 5.0 | kJ/mol | Cm | Brennan and Ubbelohde, 1956 | gas phase; ALS |
By formula: HI + C2H5IS = C2H6S + I2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -28. ± 4.6 | kJ/mol | Kin | Shum and Benson, 1985 | gas phase; ALS |
C10H12W (cr) + 2 (cr) = C10H10I2W (cr) + 2
(g)
By formula: C10H12W (cr) + 2I2 (cr) = C10H10I2W (cr) + 2HI (g)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -104.3 ± 5.5 | kJ/mol | RSC | Calado, Dias, et al., 1979 | MS |
By formula: HI + C7H5IO = C7H6O + I2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -13. ± 4.2 | kJ/mol | Eqk | Solly and Benson, 1971 | gas phase; ALS |
C10H11ClZr (cr) + (cr) = C10H10ClIZr (cr) +
(g)
By formula: C10H11ClZr (cr) + I2 (cr) = C10H10ClIZr (cr) + HI (g)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -78.1 ± 2.4 | kJ/mol | RSC | Diogo, Simoni, et al., 1993 | MS |
C10H12Mo (cr) + 2 (cr) = C10H10I2Mo (cr) + 2
(g)
By formula: C10H12Mo (cr) + 2I2 (cr) = C10H10I2Mo (cr) + 2HI (g)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -87.8 ± 5.1 | kJ/mol | RSC | Calado, Dias, et al., 1979 | MS |
By formula: C2H4F2 + I2 = HI + C2H3BrF2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 51.0 ± 0.8 | kJ/mol | Eqk | Pickard and Rodgers, 1977 | gas phase; ALS |
By formula: C7H6O + I2 = HI + C7H5IO
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 13. ± 4.2 | kJ/mol | Eqk | Solly and Benson, 1971 | gas phase; ALS |
By formula: HI + C6H5I = C6H6 + I2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -22. ± 5.9 | kJ/mol | Cm | Graham, Nichol, et al., 1955 | gas phase; ALS |
C10H11IW (cr) + (cr) = C10H10I2W (cr) +
(g)
By formula: C10H11IW (cr) + I2 (cr) = C10H10I2W (cr) + HI (g)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -84.6 ± 4.1 | kJ/mol | RSC | Calhorda, Dias, et al., 1987 | MS |
By formula: I (g) + H4Ge (g) = HI (g) + H3Ge (g)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 47.0 ± 4.1 | kJ/mol | KinG | Noble and Walsh, 1983 | MS |
By formula: C5H10 + I2 = 2HI + C5H8
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 102.1 | kJ/mol | Eqk | Furuyama, Golden, et al., 1970 | gas phase; ALS |
By formula: HI + C4H7IO = I2 + C4H8O
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -42.7 | kJ/mol | Kin | Solly, Golden, et al., 1970, 2 | gas phase; ALS |
By formula: 2HI + C5H6 = C5H8 + I2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -89.5 | kJ/mol | Eqk | Furuyama, Golden, et al., 1970 | gas phase; ALS |
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -86.27 | kJ/mol | Eqk | Furuyama, Golden, et al., 1969 | gas phase; ALS |
(g) + C3H10Ge (g) = C3H9Ge (g) +
(g)
By formula: I (g) + C3H10Ge (g) = C3H9Ge (g) + HI (g)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 42.0 ± 1.8 | kJ/mol | KinG | Doncaster and Walsh, 1979 | MS |
Henry's Law data
Go To: Top, Gas phase thermochemistry data, Phase change 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 |
---|---|---|---|---|
2.5×10+9/KA | 9800. | T | N/A | For strong acids, the solubility is often expressed as kH = ([H+] * [A-]) / p(HA). To obtain the physical solubility of HA, the value has to be divided by the acidity constant KA. missing citation corrects erroneous data from missing citation. |
2.2×10+9/KA | 9800. | T | N/A |
References
Go To: Top, Gas phase thermochemistry data, Phase change 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.
Cox, Wagman, et al., 1984
Cox, J.D.; Wagman, D.D.; Medvedev, V.A.,
CODATA Key Values for Thermodynamics, Hemisphere Publishing Corp., New York, 1984, 1. [all data]
Chase, 1998
Chase, M.W., Jr.,
NIST-JANAF Themochemical Tables, Fourth Edition,
J. Phys. Chem. Ref. Data, Monograph 9, 1998, 1-1951. [all data]
Beckmann and Waentig, 1910
Beckmann, E.; Waentig, P.,
Cryoscopic Measurements at Low Temperatures,
Z. Anorg. Chem., 1910, 67, 17. [all data]
Giauque and Wiebe, 1929
Giauque, W.F.; Wiebe, R.,
THE HEAT CAPACITY OF HYDROGEN IODIDE FROM 15°K. TO ITS BOILING POINT AND ITS HEAT OF VAPORIZATION. THE ENTROPY FROM SPECTROSCOPIC DATA,
J. Am. Chem. Soc., 1929, 51, 5, 1441-1449, https://doi.org/10.1021/ja01380a019
. [all data]
Stull, 1947
Stull, Daniel R.,
Vapor Pressure of Pure Substances. Organic and Inorganic Compounds,
Ind. Eng. Chem., 1947, 39, 4, 517-540, https://doi.org/10.1021/ie50448a022
. [all data]
Caldwell and Kebarle, 1985
Caldwell, G.; Kebarle, P.,
The hydrogen bond energies of the bihalide ions XHX- and YHX-,
Can. J. Chem., 1985, 63, 1399. [all data]
Pelaez, Blondel, et al., 2009
Pelaez, R.J.; Blondel, C.; Delsart, C.; Drag, C.,
Pulsed photodetachment microscopy and the electron affinity of iodine,
J. Phys. B: Atom. Mol. Opt. Phys., 2009, 42, 12, 125001, https://doi.org/10.1088/0953-4075/42/12/125001
. [all data]
Check, Faust, et al., 2001
Check, C.E.; Faust, T.O.; Bailey, J.M.; Wright, B.J.; Gilbert, T.M.; Sunderlin, L.S.,
Addition of Polarization and Diffuse Functions to the LANL2DZ Basis Set for P-Block Elements,
J. Phys. Chem. A,, 2001, 105, 34, 8111, https://doi.org/10.1021/jp011945l
. [all data]
Rodgers, Golden, et al., 1966
Rodgers, A.S.; Golden, D.M.; Benson, S.W.,
The thermochemistry of the gas phase equilibrium I2 + C3H6 = C3H5I + HI,
J. Am. Chem. Soc., 1966, 88, 3194-3196. [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]
Golden, Walsh, et al., 1965
Golden, D.M.; Walsh, R.; Benson, S.W.,
The thermochemistry of the gas phase equilibrium I2 + CH4 «=» CH3I + HI and the heat of formation of the methyl radical,
J. Am. Chem. Soc., 1965, 87, 4053-4057. [all data]
Goy and Pritchard, 1965
Goy, C.A.; Pritchard, H.O.,
Kinetics and thermodynamics of the reaction between iodine and methane and the heat of formation of methyl iodide,
J. Phys. Chem., 1965, 69, 3040-3041. [all data]
Nichol and Ubbelohde, 1952
Nichol, R.J.; Ubbelohde, A.R.,
A thermochemical evaluation of bond strengths in some carbon compounds. part II. Bond strengths based on the reaction CH3I + HI = CH4 + I2,
J. Am. Chem. Soc., 1952, 415-421. [all data]
Connor, Zafarani-Moattar, et al., 1982
Connor, J.A.; Zafarani-Moattar, M.T.; Bickerton, J.; El-Saied, N.I.; Suradi, S.; Carson, R.; Al Takkhin, G.; Skinner, H.A.,
Organomet., 1982, 1, 1166. [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]
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]
Benson and Amano, 1962
Benson, S.W.; Amano, A.,
Thermodynamic properties of tertiary iodides,
J. Chem. Phys., 1962, 37, 197-198. [all data]
Jones and Ogg, 1937
Jones, J.L.; Ogg, R.A., Jr.,
The equilibrium (CH3)3CI = (CH3)2C = CH2 + HI,
J. Am. Chem. Soc., 1937, 59, 1943-1945. [all data]
Brennan and Ubbelohde, 1956
Brennan, D.; Ubbelohde, A.R.,
A thermochemical evaluation of bond strengths in some carbon compounds. Part IV. Bond-strength differences based on the reaction: RI + HI = RH + I2, where R = p-methoxyphenyl and cyclohexyl,
J. Chem. Soc., 1956, 3011-3016. [all data]
Wu and Rodgers, 1974
Wu, E.; Rodgers, A.S.,
Thermochemistry of gas-phase equilibrium CF3CH3 + I2 = CF3CH2I + HI. The carbon-hydrogen bond dissociation energy in 1,1,1-trifluoroethane and the heat of formation of the 2,2,2-trifluoroethyl radical,
J. Phys. Chem., 1974, 78, 2315-2317. [all data]
Kiselev, Khuzyasheva, et al., 1979
Kiselev, V.D.; Khuzyasheva, d.G.; Konovalov, A.I.,
Thermochemical study of the acylation of para-substituted anilines,
J. Gen. Chem. USSR, 1979, 49, 2273-2276. [all data]
Landrum and Hoff, 1985
Landrum, J.T.; Hoff, C.D.,
J. Organometal. Chem., 1985, 282, 215. [all data]
Sunner, 1955
Sunner, S.,
Strain in 6,8-thioctic acid,
Nature (London), 1955, 176, 217. [all data]
Graham, Nichol, et al., 1955
Graham, W.S.; Nichol, R.J.; Ubbelohde, A.R.,
A thermochemical evaluation of bond strengths in some carbon compounds. Part III. Bond strengths based on the reactions: (a) Ph·CH2I + HI=Ph·CH3 + I2 and (b) PhI + HI=PhH + I2,
J. Chem. Soc., 1955, 115-121. [all data]
Gellner and Skinner, 1949
Gellner, O.H.; Skinner, H.A.,
Dissociation energies of carbon-halogen bonds. The bond strengths allyl-X and benzyl-X,
J. Chem. Soc., 1949, 1145-1148. [all data]
Carson, Pritchard, et al., 1950
Carson, A.S.; Pritchard, H.O.; Skinner, H.A.,
The heats of hydrolysis of the benzoyl halides,
J. Chem. Soc., 1950, 656-659. [all data]
Baldwin, Lappert, et al., 1972
Baldwin, J.C.; Lappert, M.F.; Pedley, J.B.; Poland, J.S.,
J. Chem. Soc., Dalton Trans., 1972, 1943.. [all data]
Shum and Benson, 1983
Shum, L.G.S.; Benson, S.W.,
Thermochemnistry and kinetics of the reaction of methyl mercaptan with iodine,
Int. J. Chem. Kinet., 1983, 15, 433-453. [all data]
Solly, Golden, et al., 1970
Solly, R.K.; Golden, D.M.; Benson, S.W.,
Thermochemical properties of iodoacetone. Intramolecular electrostatic interactions in polar molecules,
J. Am. Chem. Soc., 1970, 92, 4653-4656. [all data]
Walsh and Benson, 1966
Walsh, R.; Benson, S.W.,
The heats of formation of acetyl iodide and the acetyl radical,
J. Phys. Chem., 1966, 70, 3751-3753. [all data]
Shum and Benson, 1985
Shum, L.G.S.; Benson, S.W.,
Iodine catalyzed pyrolysis of dimethyl sulfide. Heats of formaton of CH3SCH2I, the CH3SCH2 radical, and the pibond energy in CH2S,
Int. J. Chem. Kinet., 1985, 17, 277-292. [all data]
Calado, Dias, et al., 1979
Calado, J.C.G.; Dias, A.R.; Martinho Simões, J.A.; Ribeiro da Silva, M.A.V.,
Rev. Port. Quím., 1979, 21, 129. [all data]
Solly and Benson, 1971
Solly, R.K.; Benson, S.W.,
Thermochemistry of the reaction of benzaldehyde with iodine. The enthalpy of formation of benzaldehyde and benzoyl iodide,
J. Chem. Thermodyn., 1971, 3, 203-209. [all data]
Diogo, Simoni, et al., 1993
Diogo, H.P.; Simoni, J.A.; Minas da Piedade, M.E.; Dias, A.R.; Martinho Simões, J.A.,
J. Am. Chem. Soc., 1993, 115, 2764. [all data]
Pickard and Rodgers, 1977
Pickard, J.M.; Rodgers, A.S.,
The kinetics and thermochemistry of the reaction of 1,1-difluoroethane with iodine. The difluoromethylene-hydrogen bond dissociation energy in 1,1-difluoroethane and the heat of formation of 1,1-difluoroethyl,
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Calhorda, Dias, et al., 1987
Calhorda, M.J.; Dias, A.R.; Minas da Piedade M.E.; Salema, M.S.; Martinho Simões J.A.,
Organometallics, 1987, 6, 734. [all data]
Noble and Walsh, 1983
Noble, P.N.; Walsh, R.,
Kinetics of the gas phase reaction between iodine and monogermane and the bond dissociation energy D(H3Ge-H),
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Furuyama, Golden, et al., 1970
Furuyama, S.; Golden, D.M.; Benson, S.W.,
Thermochemistry of cyclopentene and cyclopentadiene from studies of gas-phase equilibria,
J. Chem. Thermodyn., 1970, 2, 161-169. [all data]
Solly, Golden, et al., 1970, 2
Solly, R.K.; Golden, D.M.; Benson, S.W.,
Kinetics and thermochemistry of the gas phase reaction of methyl ethyl ketone with iodine. II. The heat of formation and unimolecular decomposition of 2-iodo-3-butanone,
Int. J. Chem. Kinet., 1970, 2, 393-407. [all data]
Furuyama, Golden, et al., 1969
Furuyama, S.; Golden, D.M.; Benson, S.W.,
Thermochemistry of the gas phase equilibria i-C3H7I = C3H6 + HI, n-C3H7I = i-C3H7I, and C3H6 + 2HI = C3H8 + I2,
J. Chem. Thermodyn., 1969, 1, 363-375. [all data]
Doncaster and Walsh, 1979
Doncaster, A.M.; Walsh, R.,
J. Phys. Chem., 1979, 83, 578. [all data]
Notes
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- Symbols used in this document:
S°gas Entropy of gas at standard conditions S°gas,1 bar Entropy of gas at standard conditions (1 bar) T Temperature Tfus Fusion (melting) point d(ln(kH))/d(1/T) Temperature dependence parameter for Henry's Law constant k°H Henry's Law constant at 298.15K 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 ΔvapH Enthalpy of vaporization - Data from NIST Standard Reference Database 69: NIST Chemistry WebBook
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