Hydrogen
- Formula: H2
- Molecular weight: 2.01588
- IUPAC Standard InChIKey: UFHFLCQGNIYNRP-UHFFFAOYSA-N
- CAS Registry Number: 1333-74-0
- 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: Dihydrogen; o-Hydrogen; p-Hydrogen; Molecular hydrogen; H2; UN 1049; UN 1966
- Permanent link for this species. Use this link for bookmarking this species for future reference.
- Information on this page:
- Other data available:
- Gas phase thermochemistry data
- Phase change data
- Reaction thermochemistry data: reactions 1 to 50, reactions 51 to 100, reactions 101 to 150, reactions 151 to 200, reactions 201 to 250, reactions 251 to 300, reactions 301 to 350, reactions 351 to 400, reactions 401 to 450, reactions 451 to 500, reactions 501 to 550, reactions 551 to 600, reactions 601 to 621
- Henry's Law data
- Gas phase ion energetics data
- Mass spectrum (electron ionization)
- Constants of diatomic molecules
- Fluid Properties
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Ion clustering data
Go To: Top, 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: 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. Searches may be limited to ion clustering reactions. A general reaction search form is also available.
Clustering reactions
By formula: Ar+ + H2 = (Ar+ • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 22.4 | kcal/mol | FA | Shul, Passarella, et al., 1987 | gas phase; switching reaction(Ar+)Ar, ΔrH>; Dehmer and Pratt, 1982 |
By formula: CHO+ + H2 = (CHO+ • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.9 | kcal/mol | PHPMS | Hiraoka and Kebarle, 1975 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 20.5 | cal/mol*K | PHPMS | Hiraoka and Kebarle, 1975 | gas phase |
By formula: CH5+ + H2 = (CH5+ • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.88 ± 0.10 | kcal/mol | PHPMS | Hiraoka, Kudaka, et al., 1991 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 12.1 | cal/mol*K | PHPMS | Hiraoka, Kudaka, et al., 1991 | gas phase |
By formula: (CH5+ • H2) + H2 = (CH5+ • 2H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.78 ± 0.10 | kcal/mol | PHPMS | Hiraoka, Kudaka, et al., 1991 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 16.2 | cal/mol*K | PHPMS | Hiraoka, Kudaka, et al., 1991 | gas phase |
By formula: (CH5+ • 2H2) + H2 = (CH5+ • 3H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.61 ± 0.10 | kcal/mol | PHPMS | Hiraoka, Kudaka, et al., 1991 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 22.6 | cal/mol*K | PHPMS | Hiraoka, Kudaka, et al., 1991 | gas phase |
By formula: (CH5+ • 3H2) + H2 = (CH5+ • 4H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.57 ± 0.10 | kcal/mol | PHPMS | Hiraoka, Kudaka, et al., 1991 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 25.7 | cal/mol*K | PHPMS | Hiraoka, Kudaka, et al., 1991 | gas phase |
By formula: C3H7+ + H2 = (C3H7+ • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 2.5 | kcal/mol | PHPMS | Hiraoka and Kebarle, 1976 | gas phase; Entropy change calculated or estimated, DG<, ΔrH< |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 20. | cal/mol*K | N/A | Hiraoka and Kebarle, 1976 | gas phase; Entropy change calculated or estimated, DG<, ΔrH< |
Free energy of reaction
ΔrG° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
0.9 | 170. | PHPMS | Hiraoka and Kebarle, 1976 | gas phase; Entropy change calculated or estimated, DG<, ΔrH< |
By formula: (Co+ • CH4) + H2 = (Co+ • H2 • CH4)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrS° | 22.9 | cal/mol*K | SIDT | Kemper, Bushnell, et al., 1993 | gas phase; switching reaction(Co+).2H2, ΔrS(440 K); Kemper, Bushnell, et al., 1993, 2 |
Enthalpy of reaction
ΔrH° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
17.4 (+0.8,-0.) | SIDT | Kemper, Bushnell, et al., 1993 | gas phase; switching reaction(Co+).2H2, ΔrS(440 K); Kemper, Bushnell, et al., 1993, 2 |
By formula: (Co+ • H2O) + H2 = (Co+ • H2 • H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrS° | 24.7 | cal/mol*K | SIDT | Kemper, Bushnell, et al., 1993 | gas phase; ΔrS(530 K) |
Enthalpy of reaction
ΔrH° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
19.8 (+0.6,-0.) | SIDT | Kemper, Bushnell, et al., 1993 | gas phase; ΔrS(530 K) |
By formula: Co+ + H2 = (Co+ • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 20. ± 1. | kcal/mol | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(O K)=18.2 kcal/mol, ΔrS(300 K)=20.6 cal/mol*K |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 22.0 | cal/mol*K | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(O K)=18.2 kcal/mol, ΔrS(300 K)=20.6 cal/mol*K |
Enthalpy of reaction
ΔrH° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
17.5 (+2.3,-0.) | CID | Haynes and Armentrout, 1996 | gas phase; guided ion beam CID |
By formula: (Co+ • H2) + H2 = (Co+ • 2H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 18.0 ± 0.6 | kcal/mol | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(0 K)=17.0 kcal/mol, ΔrS(300 K)=24.5 cal/mol*K |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 24.5 | cal/mol*K | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(0 K)=17.0 kcal/mol, ΔrS(300 K)=24.5 cal/mol*K |
By formula: (Co+ • 2H2) + H2 = (Co+ • 3H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 10.6 ± 0.4 | kcal/mol | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(0 K)=9.6 kcal/mol, ΔrS(300 K)=20.5 cal/mol*K |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 20.5 | cal/mol*K | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(0 K)=9.6 kcal/mol, ΔrS(300 K)=20.5 cal/mol*K |
By formula: (Co+ • 3H2) + H2 = (Co+ • 4H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 10.4 ± 0.6 | kcal/mol | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(0 K)=9.6 kcal/mol, ΔrS(300 K)=25.2 cal/mol*K |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 24.2 | cal/mol*K | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(0 K)=9.6 kcal/mol, ΔrS(300 K)=25.2 cal/mol*K |
By formula: (Co+ • 4H2) + H2 = (Co+ • 5H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 5.2 ± 0.6 | kcal/mol | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(0 K)=4.3 kcal/mol, ΔrS(300 K)=21.9 cal/mol*K |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 22.5 | cal/mol*K | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(0 K)=4.3 kcal/mol, ΔrS(300 K)=21.9 cal/mol*K |
By formula: (Co+ • 5H2) + H2 = (Co+ • 6H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 4.7 ± 0.6 | kcal/mol | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(0 K)=4.0 kcal/mol, ΔrS(300 K)=23.8 cal/mol*K |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 23.7 | cal/mol*K | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(0 K)=4.0 kcal/mol, ΔrS(300 K)=23.8 cal/mol*K |
By formula: (Co+ • 6H2) + H2 = (Co+ • 7H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.5 ± 0.7 | kcal/mol | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(0 K)=0.8 kcal/mol; ΔrS(300 K)=18.0 cal/mol*K |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 18.0 | cal/mol*K | SIDT | Kemper, Bushnell, et al., 1993, 2 | gas phase; ΔrH(0 K)=0.8 kcal/mol; ΔrS(300 K)=18.0 cal/mol*K |
By formula: Fe+ + H2 = (Fe+ • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 12.5 ± 0.2 | kcal/mol | SIDT | Bushnell, Kemper, et al., 1995 | gas phase; ΔrH(0K) = 10.8 kcal/mol |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 21.5 | cal/mol*K | SIDT | Bushnell, Kemper, et al., 1995 | gas phase; ΔrH(0K) = 10.8 kcal/mol |
By formula: (Fe+ • H2) + H2 = (Fe+ • 2H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 17.0 ± 0.2 | kcal/mol | SIDT | Bushnell, Kemper, et al., 1995 | gas phase; ΔrH(0K) = 15.7 kcal/mol |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 25.2 | cal/mol*K | SIDT | Bushnell, Kemper, et al., 1995 | gas phase; ΔrH(0K) = 15.7 kcal/mol |
By formula: (Fe+ • 2H2) + H2 = (Fe+ • 3H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 8.4 ± 0.1 | kcal/mol | SIDT | Bushnell, Kemper, et al., 1995 | gas phase; ΔrH(0K) = 7.5 kcal/mol |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 19.1 | cal/mol*K | SIDT | Bushnell, Kemper, et al., 1995 | gas phase; ΔrH(0K) = 7.5 kcal/mol |
By formula: (Fe+ • 3H2) + H2 = (Fe+ • 4H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 9.7 ± 0.1 | kcal/mol | SIDT | Bushnell, Kemper, et al., 1995 | gas phase; ΔrH(0K) = 8.6 kcal/mol |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 24.9 | cal/mol*K | SIDT | Bushnell, Kemper, et al., 1995 | gas phase; ΔrH(0K) = 8.6 kcal/mol |
By formula: (Fe+ • 4H2) + H2 = (Fe+ • 5H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 2.6 ± 0.1 | kcal/mol | SIDT | Bushnell, Kemper, et al., 1995 | gas phase; ΔrH(0K) = 2.2 kcal/mol |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17.9 | cal/mol*K | SIDT | Bushnell, Kemper, et al., 1995 | gas phase; ΔrH(0K) = 2.2 kcal/mol |
By formula: (Fe+ • 5H2) + H2 = (Fe+ • 6H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 2.7 ± 0.1 | kcal/mol | SIDT | Bushnell, Kemper, et al., 1995 | gas phase; ΔrH(0K) = 2.3 kcal/mol |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 18.1 | cal/mol*K | SIDT | Bushnell, Kemper, et al., 1995 | gas phase; ΔrH(0K) = 2.3 kcal/mol |
By formula: HN2+ + H2 = (HN2+ • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 7.2 | kcal/mol | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 22.6 | cal/mol*K | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase |
By formula: (HN2+ • H2) + H2 = (HN2+ • 2H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.8 | kcal/mol | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17. | cal/mol*K | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase |
By formula: HO- + H2 = (HO- • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 7. | kcal/mol | CID | Paulson and Henchman, 1984 | gas phase; approximate value |
By formula: HO2+ + H2 = (HO2+ • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 12.5 | kcal/mol | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 22. | cal/mol*K | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase |
By formula: (HO2+ • O2) + H2 = (HO2+ • H2 • O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 4.0 | kcal/mol | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17. | cal/mol*K | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase |
By formula: H3+ + H2 = (H3+ • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 6.9 ± 0.4 | kcal/mol | AVG | N/A | Average of 4 out of 11 values; Individual data points |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17.4 to 17.4 | cal/mol*K | RNG | N/A | Range of 6 values; Individual data points |
By formula: (H3+ • H2) + H2 = (H3+ • 2H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.3 ± 0.2 | kcal/mol | PHPMS | Hiraoka, 1987 | gas phase |
ΔrH° | 3.1 | kcal/mol | HPMS | Beuhler, Ehrenson, et al., 1983 | gas phase |
ΔrH° | 3.4 | kcal/mol | HPMS | Beuhler, Ehrenson, et al., 1983 | gas phase; deuterated |
ΔrH° | 4.1 | kcal/mol | PHPMS | Hiraoka and Kebarle, 1975, 2 | gas phase |
ΔrH° | 1.8 | kcal/mol | HPMS | Bennett and Field, 1972 | gas phase; Entropy change is questionable |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17.4 | cal/mol*K | PHPMS | Hiraoka, 1987 | gas phase |
ΔrS° | 16.9 | cal/mol*K | HPMS | Beuhler, Ehrenson, et al., 1983 | gas phase |
ΔrS° | 16.1 | cal/mol*K | HPMS | Beuhler, Ehrenson, et al., 1983 | gas phase; deuterated |
ΔrS° | 19.8 | cal/mol*K | PHPMS | Hiraoka and Kebarle, 1975, 2 | gas phase |
ΔrS° | 10.8 | cal/mol*K | HPMS | Bennett and Field, 1972 | gas phase; Entropy change is questionable |
By formula: (H3+ • 2H2) + H2 = (H3+ • 3H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.2 ± 0.1 | kcal/mol | PHPMS | Hiraoka, 1987 | gas phase |
ΔrH° | 3.8 | kcal/mol | PHPMS | Hiraoka and Kebarle, 1975, 2 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 18.5 | cal/mol*K | PHPMS | Hiraoka, 1987 | gas phase |
ΔrS° | 20.2 | cal/mol*K | PHPMS | Hiraoka and Kebarle, 1975, 2 | gas phase |
By formula: (H3+ • 3H2) + H2 = (H3+ • 4H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.7 ± 0.1 | kcal/mol | PHPMS | Hiraoka, 1987 | gas phase |
ΔrH° | 2.4 | kcal/mol | PHPMS | Hiraoka and Kebarle, 1975, 2 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17.9 | cal/mol*K | PHPMS | Hiraoka, 1987 | gas phase |
ΔrS° | 19.3 | cal/mol*K | PHPMS | Hiraoka and Kebarle, 1975, 2 | gas phase |
By formula: (H3+ • 4H2) + H2 = (H3+ • 5H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.6 ± 0.1 | kcal/mol | PHPMS | Hiraoka, 1987 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 18.9 | cal/mol*K | PHPMS | Hiraoka, 1987 | gas phase |
By formula: (H3+ • 5H2) + H2 = (H3+ • 6H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.5 ± 0.1 | kcal/mol | PHPMS | Hiraoka, 1987 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 20.0 | cal/mol*K | PHPMS | Hiraoka, 1987 | gas phase |
By formula: (H3+ • 6H2) + H2 = (H3+ • 7H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 0.9 ± 0.1 | kcal/mol | PHPMS | Hiraoka, 1987 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 16.5 | cal/mol*K | PHPMS | Hiraoka, 1987 | gas phase |
By formula: (H3+ • 7H2) + H2 = (H3+ • 8H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 0.8 ± 0.1 | kcal/mol | PHPMS | Hiraoka, 1987 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17.9 | cal/mol*K | PHPMS | Hiraoka, 1987 | gas phase |
By formula: (H3+ • 8H2) + H2 = (H3+ • 9H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 0.6 ± 0.1 | kcal/mol | PHPMS | Hiraoka, 1987 | gas phase |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 19.1 | cal/mol*K | PHPMS | Hiraoka, 1987 | gas phase |
By formula: H3O+ + H2 = (H3O+ • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.5 ± 0.5 | kcal/mol | SCATTERING | Okumura, Yeh, et al., 1990 | gas phase |
By formula: K+ + H2 = (K+ • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.86 | kcal/mol | SIDT | Bushnell, Kemper, et al., 1994 | gas phase; ΔrH(0K) = 1.45 kcal/mol |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 13.5 | cal/mol*K | SIDT | Bushnell, Kemper, et al., 1994 | gas phase; ΔrH(0K) = 1.45 kcal/mol |
By formula: (K+ • H2) + H2 = (K+ • 2H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.47 | kcal/mol | SIDT | Bushnell, Kemper, et al., 1994 | gas phase; ΔrH(0K) = 1.35 kcal/mol |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 11.2 | cal/mol*K | SIDT | Bushnell, Kemper, et al., 1994 | gas phase; ΔrH(0K) = 1.35 kcal/mol |
By formula: Li+ + H2 = (Li+ • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 6.5 ± 4.6 | kcal/mol | EI | Wu, 1979 | gas phase |
By formula: Na+ + H2 = (Na+ • H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 2.93 | kcal/mol | SIDT | Bushnell, Kemper, et al., 1994 | gas phase; ΔrH(0K) = 2.45 kcal/mol |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 13.2 | cal/mol*K | SIDT | Bushnell, Kemper, et al., 1994 | gas phase; ΔrH(0K) = 2.45 kcal/mol |
By formula: (Na+ • H2) + H2 = (Na+ • 2H2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 2.41 | kcal/mol | SIDT | Bushnell, Kemper, et al., 1994 | gas phase; ΔrH(0K) = 2.25 kcal/mol |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 12.4 | cal/mol*K | SIDT | Bushnell, Kemper, et al., 1994 | gas phase; ΔrH(0K) = 2.25 kcal/mol |
References
Go To: Top, Ion clustering data, Notes
Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.
Shul, Passarella, et al., 1987
Shul, R.J.; Passarella, R.; Upshulte, B.L.; Keesee, R.G.; Castleman, A.W.,
Thermal Energy Reactions Invoving Ar+ Monomer and Dimer with N2, H2, Xe, and Kr,
J. Chem. Phys., 1987, 86, 8, 4446, https://doi.org/10.1063/1.452718
. [all data]
Dehmer and Pratt, 1982
Dehmer, P.M.; Pratt, S.T.,
Photoionization of ArKr, ArXe, and KrXe and bond dissociation energies of the rare gas dimer ions,
J. Chem. Phys., 1982, 77, 4804. [all data]
Hiraoka and Kebarle, 1975
Hiraoka, K.; Kebarle, P.,
Stability and Structure of H3CO+ Formed from COH+ + H2 at Low Temperature,
J. Chem. Phys., 1975, 63, 4, 1688, https://doi.org/10.1063/1.431499
. [all data]
Hiraoka, Kudaka, et al., 1991
Hiraoka, K.; Kudaka, I.; Yamabe, S.,
Gas-Phase Solvation of CH5+ with H2,
Chem. Phys. Lett., 1991, 184, 4, 271, https://doi.org/10.1016/0009-2614(91)85122-D
. [all data]
Hiraoka and Kebarle, 1976
Hiraoka, K.; Kebarle, P.,
Stabilities and Energetics of Pentacoordinated Carbonium Ions. The Isomeric C2H7+ Ions and Some Higher Analogues: C3H9+ and C4H11+,
J. Am. Chem. Soc., 1976, 98, 20, 6119, https://doi.org/10.1021/ja00436a009
. [all data]
Kemper, Bushnell, et al., 1993
Kemper, P.R.; Bushnell, J.; Von Koppen, P.; Bowers, M.T.,
Binding Energies of Co+(H2/CH4/C2H6)1,2,3 Clusters,
J. Phys. Chem., 1993, 97, 9, 1810, https://doi.org/10.1021/j100111a016
. [all data]
Kemper, Bushnell, et al., 1993, 2
Kemper, P.R.; Bushnell, J.; Von Helden, G.; Bowers, M.T.,
Co+(H2)n Clusters: Binding Energies and Molecular Parameters,
J. Chem Phys., 1993, 97, 1, 52, https://doi.org/10.1021/j100103a012
. [all data]
Haynes and Armentrout, 1996
Haynes, C.L.; Armentrout, P.B.,
Guided Ion Beam Determination of the Co+ - H2 Bond Dissociation energy,
Chem Phys. Let., 1996, 249, 1-2, 64, https://doi.org/10.1016/0009-2614(95)01337-7
. [all data]
Bushnell, Kemper, et al., 1995
Bushnell, J.E.; Kemper, P.R.; Bowers, M.T.,
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Notes
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- Symbols used in this document:
T Temperature 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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