Sulfur dioxide
- Formula: O2S
- Molecular weight: 64.064
- IUPAC Standard InChIKey: RAHZWNYVWXNFOC-UHFFFAOYSA-N
- CAS Registry Number: 7446-09-5
- 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: Sulfurous acid anhydride; Fermenicide powder; Fermenticide liquid; Sulfur oxide (SO2); Sulfurous anhydride; Sulfurous oxide; SO2; Sulphur dioxide; Fermenicide liquid; Schwefeldioxyd; Siarki dwutlenek; Sulfur oxide; UN 1079; Sulfur dioxide (SO2); Sulfur superoxide
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Gas phase thermochemistry data
Go To: Top, 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 | -296.81 ± 0.20 | kJ/mol | Review | Cox, Wagman, et al., 1984 | CODATA Review value |
ΔfH°gas | -296.84 | kJ/mol | Review | Chase, 1998 | Data last reviewed in June, 1961 |
Quantity | Value | Units | Method | Reference | Comment |
S°gas,1 bar | 248.223 ± 0.050 | J/mol*K | Review | Cox, Wagman, et al., 1984 | CODATA Review value |
S°gas,1 bar | 248.21 | J/mol*K | Review | Chase, 1998 | Data last reviewed in June, 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 1200. | 1200. to 6000. |
---|---|---|
A | 21.43049 | 57.48188 |
B | 74.35094 | 1.009328 |
C | -57.75217 | -0.076290 |
D | 16.35534 | 0.005174 |
E | 0.086731 | -4.045401 |
F | -305.7688 | -324.4140 |
G | 254.8872 | 302.7798 |
H | -296.8422 | -296.8422 |
Reference | Chase, 1998 | Chase, 1998 |
Comment | Data last reviewed in June, 1961 | Data last reviewed in June, 1961 |
Reaction thermochemistry data
Go To: Top, Gas phase thermochemistry data, Henry's Law data, References, Notes
Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.
Data compiled as indicated in comments:
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.
Reactions 1 to 50
By formula: Cl- + O2S = (Cl- • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 92.9 ± 8.4 | kJ/mol | TDAs | Caldwell and Kebarle, 1985 | gas phase; B,M |
ΔrH° | 87.4 ± 8.4 | kJ/mol | IMRE | Larson and McMahon, 1985 | gas phase; B |
ΔrH° | 92.9 ± 9.2 | kJ/mol | TDEq | Bohringer, Fahey, et al., 1984 | gas phase; Relative to HOH..Cl- in Keesee, Lee, et al., 1980; B,M |
ΔrH° | 91.21 ± 0.84 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B,M |
ΔrH° | 87.4 | kJ/mol | ICR | Larson and McMahon, 1984 | gas phase; switching reaction(Cl-)t-C4H9OH, Entropy change calculated or estimated; French, Ikuta, et al., 1982; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 90.4 | J/mol*K | PHPMS | Caldwell and Kebarle, 1985 | gas phase; M |
ΔrS° | 101. | J/mol*K | N/A | Bohringer, Fahey, et al., 1984 | gas phase; switching reaction(Cl-)H2O), Entropy change calculated or estimated; Keesee and Castleman, 1980; M |
ΔrS° | 87.0 | J/mol*K | N/A | Larson and McMahon, 1984 | gas phase; switching reaction(Cl-)t-C4H9OH, Entropy change calculated or estimated; French, Ikuta, et al., 1982; M |
ΔrS° | 97.1 | J/mol*K | HPMS | Keesee, Lee, et al., 1980 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 65.7 ± 8.4 | kJ/mol | TDAs | Caldwell and Kebarle, 1985 | gas phase; B |
ΔrG° | 61.5 ± 8.4 | kJ/mol | IMRE | Larson and McMahon, 1985 | gas phase; B |
ΔrG° | 62.8 ± 6.7 | kJ/mol | TDEq | Bohringer, Fahey, et al., 1984 | gas phase; Relative to HOH..Cl- in Keesee, Lee, et al., 1980; B,M |
ΔrG° | 61.9 ± 1.3 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B |
ΔrG° | 61.5 | kJ/mol | ICR | Larson and McMahon, 1984 | gas phase; switching reaction(Cl-)t-C4H9OH, Entropy change calculated or estimated; French, Ikuta, et al., 1982; M |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
59.4 | 296. | FA | Fehsenfeld and Ferguson, 1974 | gas phase; switching reaction(Cl-)H2O; M |
By formula: F- + O2S = (F- • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 225. ± 9.2 | kJ/mol | CIDT | Lobring, Check, et al., 2003 | gas phase; B |
ΔrH° | 222. ± 10. | kJ/mol | CIDT | Squires, 1992 | gas phase; B |
ΔrH° | 183. | kJ/mol | ICR | Larson and McMahon, 1985 | gas phase; switching reaction(F-)H2O, Entropy change calculated or estimated; Arshadi, Yamdagni, et al., 1970; M |
ΔrH° | 183. ± 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 |
ΔrH° | 250. | kJ/mol | SAMS | Robbiani and Franklin, 1979 | gas phase; Cl- + CO2ClF --> SO2F- + Cl2, ΔrH>; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 100. | J/mol*K | N/A | Larson and McMahon, 1985 | gas phase; switching reaction(F-)H2O, Entropy change calculated or estimated; Arshadi, Yamdagni, et al., 1970; M |
ΔrS° | 96.2 | 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° | 153. | kJ/mol | ICR | Larson and McMahon, 1985 | gas phase; switching reaction(F-)H2O, Entropy change calculated or estimated; Arshadi, Yamdagni, et al., 1970; M |
ΔrG° | 154. ± 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: NO3- + O2S = (NO3- • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 72.0 ± 8.4 | kJ/mol | TDEq | Bohringer, Fahey, et al., 1984 | gas phase; Relative to HOH..NO3-, Keesee, Lee, et al., 1980; B,M |
ΔrH° | 76.1 ± 5.0 | kJ/mol | TDAs | Wlodek, Luczynski, et al., 1983 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 105. | J/mol*K | N/A | Bohringer, Fahey, et al., 1984 | gas phase; switching reaction(NO3-)H2O, Entropy change calculated or estimated; Lee, Keesee, et al., 1980; M |
ΔrS° | 132. | J/mol*K | HPMS | Wlodek, Luczynski, et al., 1983 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 40. ± 8.4 | kJ/mol | TDEq | Bohringer, Fahey, et al., 1984 | gas phase; Relative to HOH..NO3-, Keesee, Lee, et al., 1980; B,M |
ΔrG° | 41.84 ± 0.42 | kJ/mol | TDAs | Banic and Iribarne, 1985 | gas phase; B |
ΔrG° | 36.8 ± 3.8 | kJ/mol | TDAs | Wlodek, Luczynski, et al., 1983 | gas phase; B |
ΔrG° | 44.4 | kJ/mol | FA | Fehsenfeld and Ferguson, 1974 | gas phase; switching reaction(NO3-)SO2, Entropy change calculated or estimated; Lee, Keesee, et al., 1980; M |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
41.8 | 299. | HPMS | Banic and Iribarne, 1985 | gas phase; electric fields; M |
By formula: I- + O2S = (I- • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 59.8 ± 8.4 | kJ/mol | TDAs | Caldwell and Kebarle, 1985 | gas phase; B,M |
ΔrH° | 53.97 ± 0.42 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 73.6 | J/mol*K | PHPMS | Caldwell and Kebarle, 1985 | gas phase; M |
ΔrS° | 84.5 | J/mol*K | HPMS | Keesee, Lee, et al., 1980 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 38. ± 11. | kJ/mol | TDAs | Caldwell and Kebarle, 1985 | gas phase; B |
ΔrG° | 7.11 ± 0.42 | kJ/mol | TDAs | Banic and Iribarne, 1985 | gas phase; B |
ΔrG° | 28.5 ± 0.84 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
38. | 301. | HPMS | Banic and Iribarne, 1985 | gas phase; electric fields; M |
By formula: O2S- + O2S = (O2S- • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 100.4 ± 0.84 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B,M |
ΔrH° | 89.1 ± 5.4 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
ΔrH° | 77.40 | kJ/mol | N/A | Dresch, Kramer, et al., 1991 | gas phase; Both dissociation and electron detachment?; B |
ΔrH° | 76.57 | kJ/mol | N/A | Snodgrass, Coe, et al., 1988 | gas phase; Appears to be dissociation + electron detachment; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 141. | J/mol*K | HPMS | Keesee, Lee, et al., 1980 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 58.2 ± 1.7 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B |
ΔrG° | 43.5 ± 9.2 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
By formula: NO2- + O2S = (NO2- • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 108.4 ± 0.84 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B,M |
ΔrH° | 102. ± 4.2 | kJ/mol | TDEq | Bohringer, Fahey, et al., 1984 | gas phase; Relative to HOH..NO2-, Keesee, Lee, et al., 1980; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 154. | J/mol*K | HPMS | Keesee, Lee, et al., 1980 | gas phase; M |
ΔrS° | 132. | J/mol*K | N/A | Bohringer, Fahey, et al., 1984 | gas phase; switching reaction(NO2-)H2O, Entropy change calculated or estimated; Lee, Keesee, et al., 1980; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 62.3 ± 1.3 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B |
By formula: CO3- + O2S = (CO3- • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 59. | kJ/mol | HPMS | Keesee, Lee, et al., 1980 | gas phase; switching reaction(O-)CO2, Entropy change calculated or estimated; Fehsenfeld and Ferguson, 1974; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 84. | J/mol*K | N/A | Keesee, Lee, et al., 1980 | gas phase; switching reaction(O-)CO2, Entropy change calculated or estimated; Fehsenfeld and Ferguson, 1974; M |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
33. | 296. | HPMS | Keesee, Lee, et al., 1980 | gas phase; switching reaction(O-)CO2, Entropy change calculated or estimated; Fehsenfeld and Ferguson, 1974; M |
By formula: (Cl- • O2S) + H2O = (Cl- • H2O • O2S)
Bond type: Hydrogen bond (negative ion to hydride)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 43.51 | kJ/mol | TDAs | Upschulte, Schelling, et al., 1984 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 81.2 | J/mol*K | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 19.2 | kJ/mol | TDAs | Upschulte, Schelling, et al., 1984 | gas phase; B |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
23. | 296. | FA | Fehsenfeld and Ferguson, 1974 | gas phase; From thermochemical cycle,switching reaction(H2O/SO2); M |
By formula: (Cl- • O2S) + O2S = (Cl- • 2O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 51.5 ± 4.2 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B,M |
ΔrH° | 51.5 | kJ/mol | PHPMS | Caldwell and Kebarle, 1985 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 84.5 | J/mol*K | PHPMS | Caldwell and Kebarle, 1985 | gas phase; M |
ΔrS° | 95.0 | J/mol*K | HPMS | Keesee, Lee, et al., 1980 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 23. ± 9.2 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B |
By formula: (NO2- • O2S) + O2S = (NO2- • 2O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 37.7 ± 0.84 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B,M |
ΔrH° | 41. | kJ/mol | HPMS | Wlodek, Luczynski, et al., 1983 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 90.0 | J/mol*K | HPMS | Wlodek, Luczynski, et al., 1983 | gas phase; M |
ΔrS° | 70.3 | J/mol*K | HPMS | Keesee, Lee, et al., 1980 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 16.7 ± 1.7 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B |
By formula: (Na+ • 3O2S) + O2S = (Na+ • 4O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 51.5 | kJ/mol | HPMS | Castleman, Peterson, et al., 1983 | gas phase; Entropy change calculated or estimated; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 110. | J/mol*K | N/A | Castleman, Peterson, et al., 1983 | gas phase; Entropy change calculated or estimated; M |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
13. | 328. | HPMS | Castleman, Peterson, et al., 1983 | gas phase; Entropy change calculated or estimated; M |
By formula: (Br- • O2S) + HBr = (Br- • HBr • O2S)
Bond type: Hydrogen bond (negative ion to hydride)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 51.0 | kJ/mol | PHPMS | Caldwell and Kebarle, 1985 | gas phase; From thermochemical cycle,switching reaction(Br- HBr)SO2; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 80.3 | J/mol*K | PHPMS | Caldwell and Kebarle, 1985 | gas phase; From thermochemical cycle,switching reaction(Br- HBr)SO2; M |
By formula: (Cl- • O2S • H2O) + O2S = (Cl- • 2O2S • H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 49.4 | kJ/mol | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; From thermochemical cycle; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 109. | J/mol*K | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; From thermochemical cycle; M |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
17. | 296. | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; From thermochemical cycle; M |
By formula: Na+ + O2S = (Na+ • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 79.1 | kJ/mol | FA | Perry, Rowe, et al., 1980 | gas phase; Entropy change calculated or estimated; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 84.9 | J/mol*K | N/A | Perry, Rowe, et al., 1980 | gas phase; Entropy change calculated or estimated; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 53.6 | kJ/mol | FA | Perry, Rowe, et al., 1980 | gas phase; Entropy change calculated or estimated; M |
By formula: (Br- • O2S) + HCl = (Br- • HCl • O2S)
Bond type: Hydrogen bond (negative ion to hydride)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 93.7 | kJ/mol | PHPMS | Caldwell and Kebarle, 1985 | gas phase; From thermochemical cycle,switching reaction(Br-)SO2; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 77.8 | J/mol*K | PHPMS | Caldwell and Kebarle, 1985 | gas phase; From thermochemical cycle,switching reaction(Br-)SO2; M |
By formula: (Cl- • 2H2O) + O2S = (Cl- • O2S • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 59.0 | kJ/mol | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; From thermochemical cycle; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 81.2 | J/mol*K | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; From thermochemical cycle; M |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
35. | 296. | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; From thermochemical cycle; M |
By formula: (O2S- • O2S) + O2S = (O2S- • 2O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 33.9 ± 1.3 | kJ/mol | TDAs | Vacher, Jorda, et al., 1992 | gas phase; B |
ΔrH° | 35. | kJ/mol | HPMS | Keesee, Lee, et al., 1980 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 66.9 | J/mol*K | HPMS | Keesee, Lee, et al., 1980 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 16.3 ± 0.84 | kJ/mol | TDAs | Vacher, Jorda, et al., 1992 | gas phase; B |
By formula: (Cl- • H2O • O2S) + H2O = (Cl- • 2H2O • O2S)
Bond type: Hydrogen bond (negative ion to hydride)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 38.9 | kJ/mol | TDAs | Upschulte, Schelling, et al., 1984 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 82.4 | J/mol*K | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 14.2 | kJ/mol | TDAs | Upschulte, Schelling, et al., 1984 | gas phase; B |
By formula: (Cl- • 2O2S) + H2O = (Cl- • H2O • 2O2S)
Bond type: Hydrogen bond (negative ion to hydride)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 41.4 | kJ/mol | TDAs | Upschulte, Schelling, et al., 1984 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 95.0 | J/mol*K | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 13.0 | kJ/mol | TDAs | Upschulte, Schelling, et al., 1984 | gas phase; B |
By formula: (NO2- • 2O2S) + O2S = (NO2- • 3O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 27.6 ± 0.84 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 56.1 | J/mol*K | HPMS | Keesee, Lee, et al., 1980 | gas phase; Entropy change is questionable; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 10.9 ± 3.3 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B |
By formula: (Cl- • O2S) + HCl = (Cl- • HCl • O2S)
Bond type: Hydrogen bond (negative ion to hydride)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 58.2 | kJ/mol | PHPMS | Caldwell and Kebarle, 1985 | gas phase; From thermochemical cycle; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 80.3 | J/mol*K | PHPMS | Caldwell and Kebarle, 1985 | gas phase; From thermochemical cycle; M |
By formula: (Cl- • H2O) + O2S = (Cl- • O2S • H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 72.8 | kJ/mol | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 84.5 | J/mol*K | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; M |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
48.1 | 296. | HPMS | Fehsenfeld and Ferguson, 1974 | gas phase; switching reaction(Cl- H2O)H2O; M |
By formula: HO2S+ + O2S = (HO2S+ • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 89.1 | kJ/mol | PHPMS | Szulejko and McMahon, 1992 | gas phase; M |
ΔrH° | 97.1 | kJ/mol | PHPMS | McMahon and Kebarle, 1986 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 108. | J/mol*K | PHPMS | Szulejko and McMahon, 1992 | gas phase; M |
ΔrS° | 115. | J/mol*K | PHPMS | McMahon and Kebarle, 1986 | gas phase; M |
By formula: (Cl- • 2O2S) + O2S = (Cl- • 3O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 41.84 ± 0.42 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 96.7 | J/mol*K | HPMS | Keesee, Lee, et al., 1980 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 13.0 ± 1.3 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B |
By formula: (I- • 2O2S) + O2S = (I- • 3O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 38.5 ± 0.84 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 103. | J/mol*K | HPMS | Keesee, Lee, et al., 1980 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 7.5 ± 2.5 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B |
By formula: (I- • O2S) + O2S = (I- • 2O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 42.26 ± 0.42 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 90.4 | J/mol*K | HPMS | Keesee, Lee, et al., 1980 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 15.1 ± 1.3 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B |
By formula: (Cl- • 3O2S) + O2S = (Cl- • 4O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 36.0 ± 0.84 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 97.1 | J/mol*K | HPMS | Keesee, Lee, et al., 1980 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 6.7 ± 4.2 | kJ/mol | TDAs | Keesee, Lee, et al., 1980 | gas phase; B |
By formula: (I- • O2S) + H2O = (I- • H2O • O2S)
Bond type: Hydrogen bond (negative ion to hydride)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrG° | 14.6 ± 0.42 | kJ/mol | TDAs | Banic and Iribarne, 1985 | gas phase; B |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
15. | 300. | HPMS | Banic and Iribarne, 1985 | gas phase; electric fields; M |
By formula: HO- + O2S = (HO- • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 259. ± 12. | kJ/mol | CIDT | Squires, 1992 | gas phase; Dissociative protonation between HCl, MeCHClCO2H; B |
ΔrH° | >213. ± 13. | kJ/mol | IMRB | Hierl and Paulson, 1984 | gas phase; CO2..HO- + SO2 ->. data revised per 92SQU; B |
By formula: Br- + O2S = (Br- • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 80.8 ± 8.4 | kJ/mol | TDAs | Caldwell and Kebarle, 1985 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 92.0 | J/mol*K | PHPMS | Caldwell and Kebarle, 1985 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 53. ± 11. | kJ/mol | TDAs | Caldwell and Kebarle, 1985 | gas phase; B |
By formula: CN- + O2S = (CN- • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 90.8 ± 3.3 | kJ/mol | TDAs | Larson, Szulejko, et al., 1988 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 120. | J/mol*K | PHPMS | Larson, Szulejko, et al., 1988 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 56.07 ± 0.84 | kJ/mol | TDAs | Larson, Szulejko, et al., 1988 | gas phase; B |
By formula: Cs+ + O2S = (Cs+ • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 45.2 | kJ/mol | DT | McKnight and Sawina, 1972 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 79.1 | J/mol*K | DT | McKnight and Sawina, 1972 | gas phase; M |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
22. | 300. | HPMS | Banic and Iribarne, 1985 | gas phase; electric fields; M |
By formula: (NO2- • O2S) + C2H5NO3 = (NO2- • C2H5NO3 • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 31. | kJ/mol | HPMS | Wlodek, Luczynski, et al., 1983 | gas phase; Entropy change is questionable; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 43.5 | J/mol*K | HPMS | Wlodek, Luczynski, et al., 1983 | gas phase; Entropy change is questionable; M |
By formula: (H4N+ • 2H2O • O2S) + H2O = (H4N+ • 3H2O • O2S)
Bond type: Hydrogen bond (positive ion to hydride)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrG° | 22. | kJ/mol | HPMS | Banic and Iribarne, 1985 | gas phase; From thermochemical cycle,switching reaction, electric fields; M |
By formula: (NO3- • O2S) + O2S = (NO3- • 2O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 37. | kJ/mol | HPMS | Wlodek, Luczynski, et al., 1983 | gas phase; Entropy change is questionable; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 59.0 | J/mol*K | HPMS | Wlodek, Luczynski, et al., 1983 | gas phase; Entropy change is questionable; M |
By formula: (H4N+ • H2O • O2S) + H2O = (H4N+ • 2H2O • O2S)
Bond type: Hydrogen bond (positive ion to hydride)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrG° | 31. | kJ/mol | HPMS | Banic and Iribarne, 1985 | gas phase; From thermochemical cycle,switching reaction, electric fields; M |
(O2S- • 2 • 3
) +
= (O2S- • 3
• 3
)
By formula: (O2S- • 2H2O • 3O2S) + H2O = (O2S- • 3H2O • 3O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 27.6 ± 1.3 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 12.6 ± 0.84 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
(O2S- • 2 • 4
) +
= (O2S- • 3
• 4
)
By formula: (O2S- • 2H2O • 4O2S) + H2O = (O2S- • 3H2O • 4O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 29.7 ± 2.9 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 10.9 ± 0.84 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
(O2S- • 5 • 2
) +
= (O2S- • 6
• 2
)
By formula: (O2S- • 5O2S • 2H2O) + O2S = (O2S- • 6O2S • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 15.9 ± 3.8 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 4.60 ± 0.84 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
(O2S- • 6 • 2
) +
= (O2S- • 7
• 2
)
By formula: (O2S- • 6O2S • 2H2O) + O2S = (O2S- • 7O2S • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 15.5 ± 2.9 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 2.5 ± 0.84 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
(O2S- • • 3
) +
= (O2S- • 2
• 3
)
By formula: (O2S- • H2O • 3O2S) + H2O = (O2S- • 2H2O • 3O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 29.7 ± 1.7 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 15.9 ± 0.84 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
(O2S- • • 4
) +
= (O2S- • 2
• 4
)
By formula: (O2S- • H2O • 4O2S) + H2O = (O2S- • 2H2O • 4O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 29.7 ± 2.9 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 12.6 ± 0.84 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
By formula: (H3O+ • 4H2O) + O2S = (H3O+ • O2S • 4H2O)
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
11. | 300. | HPMS | Banic and Iribarne, 1985 | gas phase; electric fields; M |
11. | 300. | HPMS | Banic and Iribarne, 1985 | gas phase; electric fields; M |
(O2S- • 6 •
) +
= (O2S- • 7
•
)
By formula: (O2S- • 6O2S • H2O) + O2S = (O2S- • 7O2S • H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 13.4 ± 2.5 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 2.9 ± 0.84 | kJ/mol | TDAs | Vacher, Leduc, et al., 1994 | gas phase; B |
By formula: (NO3- • O2S) + H2O = (NO3- • H2O • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrG° | 18.0 ± 0.42 | kJ/mol | TDAs | Banic and Iribarne, 1985 | gas phase; B |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
18. | 299. | HPMS | Banic and Iribarne, 1985 | gas phase; electric fields; M |
By formula: (I- • H2O) + O2S = (I- • O2S • H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrG° | 37.7 ± 0.42 | kJ/mol | TDAs | Banic and Iribarne, 1985 | gas phase; B |
Free energy of reaction
ΔrG° (kJ/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
30. | 300. | HPMS | Banic and Iribarne, 1985 | gas phase; electric fields; M |
(O2S- • 2 •
) +
= (O2S- • 3
•
)
By formula: (O2S- • 2O2S • O2) + O2S = (O2S- • 3O2S • O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 15.1 ± 1.7 | kJ/mol | TDAs | Vacher, Jorda, et al., 1992 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 6. ± 13. | kJ/mol | TDAs | Vacher, Jorda, et al., 1992 | gas phase; B |
By formula: (O2S- • O2S • O2) + O2S = (O2S- • 2O2S • O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 19.2 ± 1.7 | kJ/mol | TDAs | Vacher, Jorda, et al., 1992 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 10. ± 8.4 | kJ/mol | TDAs | Vacher, Jorda, et al., 1992 | gas phase; B |
By formula: (O3S- • O2S • O2) + O2S = (O3S- • 2O2S • O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 23.8 ± 2.5 | kJ/mol | TDAs | Vacher, Jorda, et al., 1992 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 15. ± 8.8 | kJ/mol | TDAs | Vacher, Jorda, et al., 1992 | gas phase; B |
By formula: CH3+ + O2S = (CH3+ • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 254. | kJ/mol | PHPMS | McMahon, Heinis, et al., 1988 | gas phase; switching reaction(CH3+)N2, Entropy change calculated or estimated, uses MCA(N2) = 202. kJ/mol; Foster, Williamson, et al., 1974; M |
Henry's Law 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 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 |
---|---|---|---|---|
1.4 | 2900. | L | N/A | |
1.5 | 3200. | Q | N/A | Only the tabulated data between T = 273. K and T = 303. K from missing citation was used to derive kH and -Δ kH/R. Above T = 303. K the tabulated data could not be parameterized by equation (reference missing) very well. The partial pressure of water vapor (needed to convert some Henry's law constants) was calculated using the formula given by missing citation. The quantities A and α from missing citation were assumed to be identical. |
1.2 | 3100. | C | N/A | |
1.2 | 3200. | C | N/A | |
1.2 | 3100. | T | N/A | |
1.2 | 3100. | Q | N/A | missing citation refer to several references in their list of Henry's law constants but they don't assign them to specific species. |
1.3 | 3100. | N/A | N/A | |
1.2 | 3200. | X | N/A | The value is taken from the compilation of solubilities by W. Asman (unpublished). |
1.2 | X | N/A | Value given here as quoted by missing citation. | |
1.2 | C | N/A | ||
1.3 | 2800. | X | N/A | |
1.2 | 3000. | L | N/A | |
1.4 | 2800. | L | N/A | |
1.2 | 3100. | X | N/A | The value is taken from the compilation of solubilities by W. Asman (unpublished). |
1.1 | c | N/A | ||
1.2 | 3100. | c | N/A | |
1.2 | 3200. | X | N/A | The value is taken from the compilation of solubilities by W. Asman (unpublished). |
References
Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Henry's Law data, Notes
Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.
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]
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]
Larson and McMahon, 1985
Larson, J.W.; McMahon, T.B.,
Fluoride and chloride affinities of the main group oxides, fluorides, oxofluorides, and alkyls. Quantitative scales of lewis acidities from ICR halide exchange equilibria,
J. Am. Chem. Soc., 1985, 107, 766. [all data]
Bohringer, Fahey, et al., 1984
Bohringer, H.; Fahey, D.W.; Fehsenfeld, F.C.; Ferguson, E.E.,
Bond energies of the molecules H2O, SO2, H2O2, and HCl to various atmospheric negative ions,
J. Chem. Phys., 1984, 81, 2805. [all data]
Keesee, Lee, et al., 1980
Keesee, R.G.; Lee, N.; Castleman, A.W., Jr.,
Properties of clusters in the gas phase: V. Complexes of neutral molecules onto negative ions,
J. Chem. Phys., 1980, 73, 2195. [all data]
Larson and McMahon, 1984
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]
Keesee and Castleman, 1980
Keesee, R.G.; Castleman, A.W., Jr.,
Gas phase studies of hydration complexes of Cl- and I- and comparison to electrostatic calculations in the gas phase,
Chem. Phys. Lett., 1980, 74, 139. [all data]
Fehsenfeld and Ferguson, 1974
Fehsenfeld, F.C.; Ferguson, E.E.,
Laboratory studies of negative ion reactions with atmospheric trace constituents,
J. Chem. Phys., 1974, 61, 3181. [all data]
Lobring, Check, et al., 2003
Lobring, K.C.; Check, C.E.; Sunderlin, L.S.,
The fluoride affinity of SO2,
Int. J. Mass Spectrom., 2003, 222, 1-3, 221-227, https://doi.org/10.1016/S1387-3806(02)00950-8
. [all data]
Squires, 1992
Squires, R.R.,
Gas Phase Thermochemical Properties of the Bicarbonate and Bisulfate Ions,
Int. J. Mass Spectrom. Ion Proc., 1992, 117, 565, https://doi.org/10.1016/0168-1176(92)80114-G
. [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]
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]
Robbiani and Franklin, 1979
Robbiani, R.; Franklin, J.L.,
Negative ion-molecule reaction in sulfuryl halides,
J. Am. Chem. Soc., 1979, 101, 3709. [all data]
Wlodek, Luczynski, et al., 1983
Wlodek, S.; Luczynski, Z.; Wincel, H.,
Gas phase complexes of NO2- and NO3- with SO2,
Int. J. Mass Spectrom. Ion Processes, 1983, 49, 301. [all data]
Lee, Keesee, et al., 1980
Lee, N.; Keesee, R.G.; Castleman, A.W., Jr.,
The properties of clusters in the gas phase. IV. Complexes of H2O and HNOx clustering on NOx-,
J. Chem. Phys., 1980, 72, 1089. [all data]
Banic and Iribarne, 1985
Banic, C.M.; Iribarne, J.V.,
Equilibrium Constants for Clustering of Neutral Molecules about Gaseous Ions,
J. Chem. Phys., 1985, 83, 12, 6432, https://doi.org/10.1063/1.449543
. [all data]
Vacher, Leduc, et al., 1994
Vacher, J.R.; Leduc, E.; Fitaire, M.,
Stabilities of Anionic Mixed Clusters of Sulfur Dioxide and Water,
Int. J. Mass Spectrom. Ion Proc., 1994, 135, 2-3, 139, https://doi.org/10.1016/0168-1176(94)03985-2
. [all data]
Dresch, Kramer, et al., 1991
Dresch, T.; Kramer, H.; Thurner, Y.; Weber, R.,
Photoelectrons from Negative Dimers and Clusters of Sulfur Dioxide,
Chem. Phys. Lett., 1991, 177, 4-5, 383, https://doi.org/10.1016/0009-2614(91)85070-D
. [all data]
Snodgrass, Coe, et al., 1988
Snodgrass, J.T.; Coe, J.V.; Friedhoff, C.B.; McHugh, K.M.; Bowen, K.H.,
On the Photodissociation of (SO2)2-,
J. Chem. Phys., 1988, 88, 12, 8014, https://doi.org/10.1063/1.454261
. [all data]
Upschulte, Schelling, et al., 1984
Upschulte, B.L.; Schelling, F.J.; Keesee, R.G.; Castleman, A.W.,
Thermochemical Properties of Gas Phase Mixed Clusters: Water and Sulfur Dioxide with Na+ and Cl-,
Chem. Phys. Lett., 1984, 111, 4-5, 389, https://doi.org/10.1016/0009-2614(84)85526-8
. [all data]
Castleman, Peterson, et al., 1983
Castleman, A.W.; Peterson, K.I.; Upschulte, B.L.; Schelling, F.J.,
Energetics and Structure of Na+ Cluster Ions,
Int. J. Mass Spectrom. Ion Phys., 1983, 47, 203, https://doi.org/10.1016/0020-7381(83)87171-X
. [all data]
Perry, Rowe, et al., 1980
Perry, R.A.; Rowe, B.R.; Viggiano, A.A.; Albritton, D.L.; Ferguson, E.E.; Fehsenfeld, F.C.,
Laboratory Measurements of Stratospheric Sodium Ion Measurements,
Geophys. Res. Lett., 1980, 7, 9, 693, https://doi.org/10.1029/GL007i009p00693
. [all data]
Vacher, Jorda, et al., 1992
Vacher, J.R.; Jorda, M.; Leduc, E.; Fitaire, M.,
A Determination of the Stabilities of Negative Ion Clusters in SO2 and SO2-O2 Mixtures,
Int. J. Mass Spectrom. Ion Proc., 1992, 114, 3, 149, https://doi.org/10.1016/0168-1176(92)80033-W
. [all data]
Szulejko and McMahon, 1992
Szulejko, J.; McMahon, T.B.,
personal communication, 1992. [all data]
McMahon and Kebarle, 1986
McMahon, T.B.; Kebarle, P.,
Strong hydrogen bonding in gas-phase ions: A high pressure mass spectrometric study of formation and energetics of methyl fluoride proton bound dimer,
J. Am. Chem. Soc., 1986, 108, 6502. [all data]
Hierl and Paulson, 1984
Hierl, P.M.; Paulson, J.F.,
Translational energy dependence of cross sections for reactions of OH- (H2O)n with CO2 and SO2,
J. Chem. Phys., 1984, 80, 4890. [all data]
Larson, Szulejko, et al., 1988
Larson, J.W.; Szulejko, J.E.; McMahon, T.B.,
Gas Phase Lewis Acid-Base Interactions. An Experimental Determination of Cyanide Binding Energies From Ion Cyclotron Resonance and High-Pressure Mass Spectrometric Equilibrium Measurements.,
J. Am. Chem. Soc., 1988, 110, 23, 7604, https://doi.org/10.1021/ja00231a004
. [all data]
McKnight and Sawina, 1972
McKnight, L.G.; Sawina, J.M.,
Drift Velocities and Interactions of Cs+ Ions with Atmospheric Gases,
J. Chem. Phys., 1972, 57, 12, 5156, https://doi.org/10.1063/1.1678205
. [all data]
McMahon, Heinis, et al., 1988
McMahon, T.; Heinis, T.; Nicol, G.; Hovey, J.K.; Kebarle, P.,
Methyl Cation Affinities,
J. Am. Chem. Soc., 1988, 110, 23, 7591, https://doi.org/10.1021/ja00231a002
. [all data]
Foster, Williamson, et al., 1974
Foster, M.S.; Williamson, A.D.; Beauchamp, J.L.,
Photoionization mass spectrometry of trans-azomethane,
Int. J. Mass Spectrom. Ion Phys., 1974, 15, 429. [all data]
Notes
Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Henry's Law data, References
- Symbols used in this document:
S°gas,1 bar Entropy of gas at standard conditions (1 bar) T Temperature 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 - Data from NIST Standard Reference Database 69: NIST Chemistry WebBook
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