Nitrogen
- Formula: N2
- Molecular weight: 28.0134
- IUPAC Standard InChIKey: IJGRMHOSHXDMSA-UHFFFAOYSA-N
- CAS Registry Number: 7727-37-9
- 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: Nitrogen gas; N2; UN 1066; UN 1977; Dinitrogen; Molecular nitrogen; Diatomic nitrogen; Nitrogen-14
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Gas phase thermochemistry data
Go To: Top, Reaction thermochemistry data, Mass spectrum (electron ionization), 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 |
---|---|---|---|---|---|
S°gas,1 bar | 45.7957 ± 0.001 | cal/mol*K | Review | Cox, Wagman, et al., 1984 | CODATA Review value |
S°gas,1 bar | 45.796 | cal/mol*K | Review | Chase, 1998 | Data last reviewed in March, 1977 |
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 (cal/mol*K)
H° = standard enthalpy (kcal/mol)
S° = standard entropy (cal/mol*K)
t = temperature (K) / 1000.
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Temperature (K) | 100. to 500. | 500. to 2000. | 2000. to 6000. |
---|---|---|---|
A | 6.927919 | 4.662006 | 8.489178 |
B | 0.443111 | 4.753120 | 0.269772 |
C | -2.305798 | -2.055099 | -0.046870 |
D | 3.975949 | 0.327386 | 0.003504 |
E | 0.000028 | 0.126100 | -1.088375 |
F | -2.072637 | -1.179542 | -4.534157 |
G | 54.11491 | 50.76243 | 53.77175 |
H | 0.0 | 0.0 | 0.0 |
Reference | Chase, 1998 | Chase, 1998 | Chase, 1998 |
Comment | Data last reviewed in March, 1977; New parameter fit January 2009 | Data last reviewed in March, 1977; New parameter fit January 2009 | Data last reviewed in March, 1977; New parameter fit January 2009 |
Reaction thermochemistry data
Go To: Top, Gas phase thermochemistry data, Mass spectrum (electron ionization), 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
MS - José A. Martinho Simões
B - John E. Bartmess
ALS - Hussein Y. Afeefy, Joel F. Liebman, and Stephen E. Stein
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: NO- + N2 = (NO- • N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 4.6 ± 0.3 | kcal/mol | PHPMS | Hiraoka and Yamabe, 1989 | gas phase; M |
ΔrH° | 4.7 | kcal/mol | DT | Gheno and Fitaire, 1987 | gas phase; ΔrS+-2.9 cal/mol*K; M |
ΔrH° | 4.4 | kcal/mol | HPMS | Speller, Fitaire, et al., 1983 | gas phase; Entropy change is questionable; M |
ΔrH° | 5.2 | kcal/mol | HPMS | Turner and Conway, 1976 | gas phase; M |
ΔrH° | 4.5 | kcal/mol | DT | Johnsen, Huang, et al., 1975 | gas phase; corrected for ln T by Keesee and Castleman, 1986; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17.0 | cal/mol*K | PHPMS | Hiraoka and Yamabe, 1989 | gas phase; M |
ΔrS° | 13.8 | cal/mol*K | DT | Gheno and Fitaire, 1987 | gas phase; ΔrS+-2.9 cal/mol*K; M |
ΔrS° | 13.3 | cal/mol*K | HPMS | Speller, Fitaire, et al., 1983 | gas phase; Entropy change is questionable; M |
ΔrS° | 18.9 | cal/mol*K | HPMS | Turner and Conway, 1976 | gas phase; M |
ΔrS° | 15.7 | cal/mol*K | DT | Johnsen, Huang, et al., 1975 | gas phase; corrected for ln T by Keesee and Castleman, 1986; M |
Free energy of reaction
ΔrG° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
0.5 | 200. | FA | Dunkin, Fehsenfeld, et al., 1971 | gas phase; M |
By formula: N2+ + N2 = (N2+ • N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 24.4 to 24.4 | kcal/mol | RNG | N/A | Range of 6 values; Individual data points |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 21.0 | cal/mol*K | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
ΔrS° | 16.2 | cal/mol*K | PHPMS | Teng and Conway, 1973 | gas phase; M |
ΔrS° | 19.5 | cal/mol*K | PHPMS | Payzant and Kebarle, 1970 | gas phase; M |
ΔrS° | 11. | cal/mol*K | DT | Varney, 1968 | gas phase; Entropy change is questionable; M |
ΔrS° | -1. | cal/mol*K | DT | Varney, 1959 | gas phase; Entropy change is questionable; M |
By formula: O2+ + N2 = (O2+ • N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 5.0 ± 0.3 | kcal/mol | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
ΔrH° | 5.2 | kcal/mol | HPMS | Speller and Fitaire, 1983 | gas phase; M |
ΔrH° | 5.7 | kcal/mol | PHPMS | Janik and Conway, 1967 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17.4 | cal/mol*K | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
ΔrS° | 15.8 | cal/mol*K | HPMS | Speller and Fitaire, 1983 | gas phase; M |
ΔrS° | 18.9 | cal/mol*K | PHPMS | Janik and Conway, 1967 | gas phase; M |
Free energy of reaction
ΔrG° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
0.0 | 296. | FA | Howard, Bierbaum, et al., 1972 | gas phase; M |
By formula: (HN2+ • 4N2) + N2 = (HN2+ • 5N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.0 ± 0.3 | kcal/mol | PHPMS | Hiraoka and Mori, 1989 | gas phase; M |
ΔrH° | 3.2 | kcal/mol | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase; Entropy change calculated or estimated; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 22.9 | cal/mol*K | PHPMS | Hiraoka and Mori, 1989 | gas phase; M |
ΔrS° | 20. | cal/mol*K | N/A | Hiraoka, Saluja, et al., 1979 | gas phase; Entropy change calculated or estimated; M |
Free energy of reaction
ΔrG° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
1.4 | 92. | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase; Entropy change calculated or estimated; M |
By formula: (O2- • 7N2 • O2) + N2 = (O2- • 8N2 • O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.6 ± 0.3 | kcal/mol | PHPMS | Hiraoka, 1988 | gas phase; M |
ΔrH° | 1.53 | kcal/mol | PHPMS | Hiraoka, 1988 | gas phase; Entropy change calculated or estimated; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17.9 | cal/mol*K | PHPMS | Hiraoka, 1988 | gas phase; M |
ΔrS° | 18.0 | cal/mol*K | N/A | Hiraoka, 1988 | gas phase; Entropy change calculated or estimated; M |
By formula: (O2+ • 2N2) + N2 = (O2+ • 3N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 4.2 ± 0.3 | kcal/mol | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
ΔrH° | 3.5 | kcal/mol | HPMS | Speller and Fitaire, 1983 | gas phase; Entropy change is questionable; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 19.6 | cal/mol*K | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
ΔrS° | 12.1 | cal/mol*K | HPMS | Speller and Fitaire, 1983 | gas phase; Entropy change is questionable; M |
By formula: (O2+ • N2) + N2 = (O2+ • 2N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 4.5 ± 0.3 | kcal/mol | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
ΔrH° | 4.3 | kcal/mol | HPMS | Speller and Fitaire, 1983 | gas phase; Entropy change is questionable; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 19.1 | cal/mol*K | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
ΔrS° | 13.8 | cal/mol*K | HPMS | Speller and Fitaire, 1983 | gas phase; Entropy change is questionable; M |
By formula: (NO- • N2) + N2 = (NO- • 2N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 4.2 ± 0.3 | kcal/mol | PHPMS | Hiraoka and Yamabe, 1989 | gas phase; M |
ΔrH° | 3.9 | kcal/mol | HPMS | Speller and Fitaire, 1983 | gas phase; Entropy change is questionable; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17.4 | cal/mol*K | PHPMS | Hiraoka and Yamabe, 1989 | gas phase; M |
ΔrS° | 12.6 | cal/mol*K | HPMS | Speller and Fitaire, 1983 | gas phase; Entropy change is questionable; M |
C3N2NiO3 (solution) = C3NiO3 (solution) + (solution)
By formula: C3N2NiO3 (solution) = C3NiO3 (solution) + N2 (solution)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 10. ± 1. | kcal/mol | KinS | Turner, Simpson, et al., 1983 | solvent: Liquid krypton; The reaction enthalpy relies on the experimental value for the activation enthalpy, 10. ± 1. kcal/mol, and on the assumption that the activation enthalpy for product recombination is negligible Turner, Simpson, et al., 1983.; MS |
By formula: N+ + N2 = (N+ • N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 59.4 | kcal/mol | N/A | National Bureau of Standards, 1968 | gas phase; from ΔrH(f); M |
ΔrH° | 60. | kcal/mol | EI | Saporoschenko, 1965 | gas phase; M |
ΔrH° | 59. | kcal/mol | EI | Franklin, Dibeler, et al., 1958 | gas phase; M |
Enthalpy of reaction
ΔrH° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
86.2 (+1.8,-0.) | CID | Haynes, Freysinger, et al., 1995 | gas phase; guided ion beam CID; M |
By formula: Cu+ + N2 = (Cu+ • N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 6.2 | kcal/mol | HPMS | El-Shall, Schriver, et al., 1989 | gas phase; Cu+ from laser desrption; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 16. | cal/mol*K | HPMS | El-Shall, Schriver, et al., 1989 | gas phase; Cu+ from laser desrption; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 1.4 | kcal/mol | HPMS | El-Shall, Schriver, et al., 1989 | gas phase; Cu+ from laser desrption; M |
By formula: (HN2+ • 2N2) + N2 = (HN2+ • 3N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.4 ± 0.3 | kcal/mol | PHPMS | Hiraoka and Mori, 1989 | gas phase; M |
ΔrH° | 3.8 | kcal/mol | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 20.1 | cal/mol*K | PHPMS | Hiraoka and Mori, 1989 | gas phase; M |
ΔrS° | 20. | cal/mol*K | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase; M |
By formula: (HN2+ • 3N2) + N2 = (HN2+ • 4N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.3 ± 0.3 | kcal/mol | PHPMS | Hiraoka and Mori, 1989 | gas phase; M |
ΔrH° | 3.5 | kcal/mol | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 21.2 | cal/mol*K | PHPMS | Hiraoka and Mori, 1989 | gas phase; M |
ΔrS° | 20. | cal/mol*K | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase; M |
By formula: (HN2+ • N2) + N2 = (HN2+ • 2N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.6 ± 0.3 | kcal/mol | PHPMS | Hiraoka and Mori, 1989 | gas phase; M |
ΔrH° | 4.0 | kcal/mol | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 19.2 | cal/mol*K | PHPMS | Hiraoka and Mori, 1989 | gas phase; M |
ΔrS° | 18. | cal/mol*K | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase; M |
By formula: Na+ + N2 = (Na+ • N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 8.0 | kcal/mol | FA | Perry, Rowe, et al., 1980 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 18.6 | cal/mol*K | FA | Perry, Rowe, et al., 1980 | gas phase; M |
Free energy of reaction
ΔrG° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
2.2 | 310. | FA | Perry, Rowe, et al., 1980 | gas phase; M |
2.0 | 310. | DT | Beyer and Keller, 1971 | gas phase; low E/N; M |
By formula: HN2+ + N2 = (HN2+ • N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 16.0 | kcal/mol | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase; M |
ΔrH° | 14.5 | kcal/mol | PHPMS | Meot-Ner (Mautner) and Field, 1974 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 24. | cal/mol*K | PHPMS | Hiraoka, Saluja, et al., 1979 | gas phase; M |
ΔrS° | 20.4 | cal/mol*K | PHPMS | Meot-Ner (Mautner) and Field, 1974 | gas phase; M |
C39H66N2O3P2W (solution) + (g) = C39H68O3P2W (solution) + (g)
By formula: C39H66N2O3P2W (solution) + H2 (g) = C39H68O3P2W (solution) + N2 (g)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 4.40 ± 0.41 | kcal/mol | EqS | Gonzalez and Hoff, 1989 | solvent: Tetrahydrofuran; Temperature range: 288-308 K; MS |
C39H66MoO3P3 (solution) + (g) = C39H66MoN2O3P2 (solution)
By formula: C39H66MoO3P3 (solution) + N2 (g) = C39H66MoN2O3P2 (solution)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -9.01 ± 0.60 | kcal/mol | EqS | Gonzalez and Hoff, 1989 | solvent: Tetrahydrofuran; Temperature range: 294-308 K; MS |
By formula: (H3O+ • 2N2 • 3H2O) + N2 = (H3O+ • 3N2 • 3H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.2 | kcal/mol | DT | Gheno and Fitaire, 1987 | gas phase; ΔrH, ΔrS approximate; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 6.4 | cal/mol*K | DT | Gheno and Fitaire, 1987 | gas phase; ΔrH, ΔrS approximate; M |
By formula: (O2+ • 4N2) + N2 = (O2+ • 5N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 2.7 ± 0.2 | kcal/mol | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 16.2 | cal/mol*K | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
Free energy of reaction
ΔrG° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
0.7 | 184. | HPMS | Speller and Fitaire, 1983 | gas phase; M |
By formula: (NO- • 2N2) + N2 = (NO- • 3N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.8 ± 0.3 | kcal/mol | PHPMS | Hiraoka and Yamabe, 1989 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 16.8 | cal/mol*K | PHPMS | Hiraoka and Yamabe, 1989 | gas phase; M |
Free energy of reaction
ΔrG° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
0.9 | 204. | HPMS | Speller, Fitaire, et al., 1983 | gas phase; M |
By formula: (NO- • 3N2) + N2 = (NO- • 4N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.4 ± 0.3 | kcal/mol | PHPMS | Hiraoka and Yamabe, 1989 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17.9 | cal/mol*K | PHPMS | Hiraoka and Yamabe, 1989 | gas phase; M |
Free energy of reaction
ΔrG° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
0.4 | 204. | HPMS | Speller, Fitaire, et al., 1983 | gas phase; M |
By formula: (O2+ • 3N2) + N2 = (O2+ • 4N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 4.0 ± 0.3 | kcal/mol | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 22.5 | cal/mol*K | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
Free energy of reaction
ΔrG° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
0.7 | 204. | HPMS | Speller and Fitaire, 1983 | gas phase; M |
By formula: (H3O+ • 3N2 • 2H2O) + N2 = (H3O+ • 4N2 • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3. | kcal/mol | DT | Gheno and Fitaire, 1987 | gas phase; ΔrH, ΔrS approximate; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 12. | cal/mol*K | DT | Gheno and Fitaire, 1987 | gas phase; ΔrH, ΔrS approximate; M |
By formula: (NO- • 9N2) + N2 = (NO- • 10N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.68 | kcal/mol | PHPMS | Hiraoka and Yamabe, 1989 | gas phase; Entropy change calculated or estimated; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 19. | cal/mol*K | N/A | Hiraoka and Yamabe, 1989 | gas phase; Entropy change calculated or estimated; M |
By formula: (HN2+ • 10N2) + N2 = (HN2+ • 11N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.72 | kcal/mol | PHPMS | Hiraoka and Mori, 1989 | gas phase; Entropy change calculated or estimated; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 22. | cal/mol*K | N/A | Hiraoka and Mori, 1989 | gas phase; Entropy change calculated or estimated; M |
By formula: O3- + N2 = (O3- • N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 2.70 ± 0.20 | kcal/mol | TDAs | Hiraoka, 1988 | gas phase; B,M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 18.4 | cal/mol*K | PHPMS | Hiraoka, 1988 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | -2.80 ± 0.50 | kcal/mol | TDAs | Hiraoka, 1988 | gas phase; B |
By formula: (C2H5+ • N2) + N2 = (C2H5+ • 2N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 4.6 | kcal/mol | HPMS | Speller, 1983 | gas phase; deuterated, Entropy change is questionable; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 10.9 | cal/mol*K | HPMS | Speller, 1983 | gas phase; deuterated, Entropy change is questionable; M |
By formula: (N2+ • N2) + N2 = (N2+ • 2N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 2.8 ± 0.2 | kcal/mol | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
ΔrH° | 1.4 | kcal/mol | PI | Linn, Ono, et al., 1981 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 15.0 | cal/mol*K | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
By formula: (O2+ • O2) + N2 = (O2+ • N2 • O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 2.9 | kcal/mol | HPMS | Speller and Fitaire, 1983 | gas phase; Entropy change is questionable; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 10.1 | cal/mol*K | HPMS | Speller and Fitaire, 1983 | gas phase; Entropy change is questionable; M |
By formula: (Na+ • N2) + N2 = (Na+ • 2N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 5.3 | kcal/mol | FA | Perry, Rowe, et al., 1980 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 16.8 | cal/mol*K | FA | Perry, Rowe, et al., 1980 | gas phase; M |
Free energy of reaction
ΔrG° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
-0.3 | 310. | FA | Perry, Rowe, et al., 1980 | gas phase; M |
By formula: (CH2N+ • 2N2) + N2 = (CH2N+ • 3N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.2 | kcal/mol | HPMS | Speller, Fitaire, et al., 1982 | gas phase; Entropy change is questionable; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 13.1 | cal/mol*K | HPMS | Speller, Fitaire, et al., 1982 | gas phase; Entropy change is questionable; M |
By formula: (CH2N+ • 3N2) + N2 = (CH2N+ • 4N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.1 | kcal/mol | HPMS | Speller, Fitaire, et al., 1982 | gas phase; Entropy change is questionable; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 13.8 | cal/mol*K | HPMS | Speller, Fitaire, et al., 1982 | gas phase; Entropy change is questionable; M |
By formula: (CH2N+ • 4N2) + N2 = (CH2N+ • 5N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.2 | kcal/mol | HPMS | Speller, Fitaire, et al., 1982 | gas phase; Entropy change is questionable; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 15.2 | cal/mol*K | HPMS | Speller, Fitaire, et al., 1982 | gas phase; Entropy change is questionable; M |
By formula: C4H4BrNO2 + 0.5H4N2 = HBr + C4H5NO2 + 0.5N2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -62.22 ± 0.11 | kcal/mol | Cm | Howard and Skinner, 1966 | solid phase; solvent: Aqueous solution; Reanalyzed by Pedley, Naylor, et al., 1986, Original value = -62.55 ± 0.11 kcal/mol; ALS |
By formula: O2- + N2 = (O2- • N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 6.0 ± 1.0 | kcal/mol | N/A | Posey and Johnson, 1988 | gas phase; B |
ΔrH° | <13.60 | kcal/mol | IMRB | Adams and Bohme, 1970 | gas phase; N2..O2- + O2 -> O4-; B |
C12H34P4Ru (solution) + (solution) = C12H32N2P4Ru (solution) + (solution)
By formula: C12H34P4Ru (solution) + N2 (solution) = C12H32N2P4Ru (solution) + H2 (solution)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 3.90 | kcal/mol | PAC | Belt, Scaiano, et al., 1993 | solvent: Cyclohexane; The reaction enthalpy relies on 0.85 for the quantum yield of H2 dissociation.; MS |
By formula: (H3O+ • 2N2 • 2H2O) + N2 = (H3O+ • 3N2 • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 9.0 ± 2.7 | kcal/mol | DT | Gheno and Fitaire, 1987 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 28.4 | cal/mol*K | DT | Gheno and Fitaire, 1987 | gas phase; M |
(solution) + (solution) = C8H5N2O3V (solution) + (solution)
By formula: C9H5O4V (solution) + N2 (solution) = C8H5N2O3V (solution) + CO (solution)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 6.5 ± 1. | kcal/mol | PAC | Johnson, Popov, et al., 1991 | solvent: Heptane; The reaction enthalpy relies on 0.80 for the quantum yield of CO dissociation.; MS |
By formula: (O2- • 2N2 • O2) + N2 = (O2- • 3N2 • O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 2.5 ± 0.2 | kcal/mol | PHPMS | Hiraoka, 1988 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 18.3 | cal/mol*K | PHPMS | Hiraoka, 1988 | gas phase; M |
By formula: (O2- • 3N2 • O2) + N2 = (O2- • 4N2 • O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 2.2 ± 0.2 | kcal/mol | PHPMS | Hiraoka, 1988 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 18.7 | cal/mol*K | PHPMS | Hiraoka, 1988 | gas phase; M |
By formula: (O2- • 4N2 • O2) + N2 = (O2- • 5N2 • O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.9 ± 0.2 | kcal/mol | PHPMS | Hiraoka, 1988 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 19.5 | cal/mol*K | PHPMS | Hiraoka, 1988 | gas phase; M |
By formula: (O2- • 5N2 • O2) + N2 = (O2- • 6N2 • O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.8 ± 0.2 | kcal/mol | PHPMS | Hiraoka, 1988 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 19.5 | cal/mol*K | PHPMS | Hiraoka, 1988 | gas phase; M |
By formula: (O2- • 6N2 • O2) + N2 = (O2- • 7N2 • O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.7 ± 0.2 | kcal/mol | PHPMS | Hiraoka, 1988 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 18.8 | cal/mol*K | PHPMS | Hiraoka, 1988 | gas phase; M |
By formula: (O2- • N2 • O2) + N2 = (O2- • 2N2 • O2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 2.8 ± 0.2 | kcal/mol | PHPMS | Hiraoka, 1988 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17.9 | cal/mol*K | PHPMS | Hiraoka, 1988 | gas phase; M |
By formula: (H3O+ • 2N2 • H2O) + N2 = (H3O+ • 3N2 • H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 8. ± 2. | kcal/mol | DT | Gheno and Fitaire, 1987 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 22. | cal/mol*K | DT | Gheno and Fitaire, 1987 | gas phase; M |
By formula: (H3O+ • N2 • 2H2O) + N2 = (H3O+ • 2N2 • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 5.2 | kcal/mol | DT | Gheno and Fitaire, 1987 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 16.6 | cal/mol*K | DT | Gheno and Fitaire, 1987 | gas phase; M |
By formula: (H3O+ • N2 • 3H2O) + N2 = (H3O+ • 2N2 • 3H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 4.4 | kcal/mol | DT | Gheno and Fitaire, 1987 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 15.7 | cal/mol*K | DT | Gheno and Fitaire, 1987 | gas phase; M |
By formula: (O2+ • 10N2) + N2 = (O2+ • 11N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.4 ± 0.3 | kcal/mol | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 20.2 | cal/mol*K | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
By formula: (N2+ • 10N2) + N2 = (N2+ • 11N2)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 1.7 ± 0.2 | kcal/mol | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 20.2 | cal/mol*K | PHPMS | Hiraoka and Nakajima, 1988 | gas phase; M |
Mass spectrum (electron ionization)
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: NIST Mass Spectrometry Data Center, William E. Wallace, director
Spectrum
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Additional Data
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Owner | NIST Mass Spectrometry Data Center Collection (C) 2014 copyright by the U.S. Secretary of Commerce on behalf of the United States of America. All rights reserved. |
---|---|
Origin | D.HENNEBERG, MAX-PLANCK INSTITUTE, MULHEIM, WEST GERMANY |
NIST MS number | 61309 |
References
Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Mass spectrum (electron ionization), 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]
Hiraoka and Yamabe, 1989
Hiraoka, K.; Yamabe, S.,
How are Nitrogen Molecules Bound to NO2+ and NO+?,
J. Chem. Phys., 1989, 90, 6, 3268, https://doi.org/10.1063/1.455880
. [all data]
Gheno and Fitaire, 1987
Gheno, F.; Fitaire, M.,
Association of N2 with NH4+ and H3O+(H2O)n, n = 1,2,3,
J. Chem. Phys., 1987, 87, 2, 953, https://doi.org/10.1063/1.453250
. [all data]
Speller, Fitaire, et al., 1983
Speller, C.V.; Fitaire, M.; Pointu, A.M.,
Three - Body Association Reactions of NO+ and O2+ with N2,
J. Chem. Phys., 1983, 79, 5, 2190, https://doi.org/10.1063/1.446067
. [all data]
Turner and Conway, 1976
Turner, D.L.; Conway, D.C.,
Stability of the NO+.N2 Ion Cluster,
J. Chem. Phys., 1976, 65, 10, 3944, https://doi.org/10.1063/1.432887
. [all data]
Johnsen, Huang, et al., 1975
Johnsen, R.; Huang, C.M.; Biondi, M.A.,
The Formation and Breakup of NO2+.N2 Clusters in N2 at Low Temperatures,
J. Chem. Phys., 1975, 63, 8, 3374, https://doi.org/10.1063/1.431751
. [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]
Dunkin, Fehsenfeld, et al., 1971
Dunkin, D.B.; Fehsenfeld, F.C.; Schelmetekopf, A.L.; Ferguson, E.E.,
Three-Body Association Reactions of NO+ with O2, N2, and CO2,
J. Chem. Phys., 1971, 54, 9, 3817, https://doi.org/10.1063/1.1675432
. [all data]
Hiraoka and Nakajima, 1988
Hiraoka, K.; Nakajima, G.,
A Determination of the Stabilities of N2+(N2)n and O2+(N2)n with n = 1 - 11 from Measurements of the Gas - Phase Ion Equilibria,
J. Chem. Phys., 1988, 88, 12, 7709, https://doi.org/10.1063/1.454285
. [all data]
Teng and Conway, 1973
Teng, H.H.; Conway, D.C.,
Ion - Molecule Equilibria in Mixtures of N2 and Ar,
J. Chem. Phys., 1973, 59, 5, 2316, https://doi.org/10.1063/1.1680338
. [all data]
Payzant and Kebarle, 1970
Payzant, J.D.; Kebarle, P.,
Clustering Equilibrium N2+ + 2N2 = N4+ + N2 and the Bond Dissociation Energy of N4+,
J. Chem. Phys., 1970, 53, 12, 4723, https://doi.org/10.1063/1.1674010
. [all data]
Varney, 1968
Varney, R.N.,
Equilibrium Constant and Rates for the Reversible Reaction N4+ -> N2+ + N2,
Phys. Rev., 1968, 174, 1, 165, https://doi.org/10.1103/PhysRev.174.165
. [all data]
Varney, 1959
Varney, R.N.,
Molecular Ions,
J. Chem. Phys., 1959, 31, 5, 1314, https://doi.org/10.1063/1.1730590
. [all data]
Speller and Fitaire, 1983
Speller, C.V.; Fitaire, M.,
Proceedings of the 16th International Conference on Phenomena of Ionized Gases, H. Boetticher, H. Wenk and E. Shulz - Gulde, ed(s)., ICPIG, Dusseldorf, 1983, 568. [all data]
Janik and Conway, 1967
Janik, G.S.; Conway, D.C.,
Bonding in Heteromolecular Ion Clusters. N2O2+,
J. Phys. Chem., 1967, 71, 4, 823, https://doi.org/10.1021/j100863a007
. [all data]
Howard, Bierbaum, et al., 1972
Howard, C.J.; Bierbaum, V.M.; Rundle, H.W.; Kaufman, F.,
Kinetics and Mechanism of Formation of Water Cluster Ions from O2+ and H2O+,
J. Chem. Phys., 1972, 57, 8, 3491, https://doi.org/10.1063/1.1678783
. [all data]
Hiraoka and Mori, 1989
Hiraoka, K.; Mori, T.,
Gas Phase Stabilities of the Cluster Ions H+(CO)2(CO)n, H+(N2)2(N2)n and H+(O2)2(O2)n with n = 1 - 14,
Chem. Phys., 1989, 137, 1-3, 345, https://doi.org/10.1016/0301-0104(89)87119-8
. [all data]
Hiraoka, Saluja, et al., 1979
Hiraoka, K.; Saluja, P.P.S.; Kebarle, P.,
Stabilities of Complexes (N2)nH+, (CO)nH+ and (O2)nH+ for n = 1 to 7 Based on Gas Phase Ion Equilibrium Measurements,
Can. J. Chem., 1979, 57, 16, 2159, https://doi.org/10.1139/v79-346
. [all data]
Hiraoka, 1988
Hiraoka, K.,
Determination of the Stabilities of O3-(N2)n, O3-(O2)n, and O4-(N2)n from Measurements of the Gas Phase Equilibria,
Chem. Phys., 1988, 125, 2-3, 439, https://doi.org/10.1016/0301-0104(88)87096-4
. [all data]
Turner, Simpson, et al., 1983
Turner, J.J.; Simpson, M.B.; Poliakoff, M.; Maier II, W.B.,
J. Am. Chem. Soc., 1983, 105, 3898. [all data]
National Bureau of Standards, 1968
National Bureau of Standards, US,
Technical Note 270 - 3
in The NBS Tables of Chemical Thermodynamic Properties, 1968. [all data]
Saporoschenko, 1965
Saporoschenko, M.,
Mobility of Mass Analyzed N+, N2+, N3+, and N4+ Ions in Nitrogen Gas,
Phys. Rev. A, 1965, 139, 352. [all data]
Franklin, Dibeler, et al., 1958
Franklin, J.L.; Dibeler, V.H.; Reese, R.M.; Krauss, M.,
Ionization and dissociation of hydrazoic acid and methyl azide by electron impact,
J. Am. Chem. Soc., 1958, 80, 298. [all data]
Haynes, Freysinger, et al., 1995
Haynes, C.L.; Freysinger, W.; Armentrout, P.B.,
Collision-induced dissociation of N3+(X3-) with Ne, Ar, Kr, and Xe,
Int. J. Mass Spectrom. Ion Processes, 1995, 149/150, 267. [all data]
El-Shall, Schriver, et al., 1989
El-Shall, M.S.; Schriver, K.E.; Whetten, R.L.; Meot-Ner (Mautner), M.,
Ion/Molecule Clustering Thermochemistry by Laser Ionization High - Pressure Mass Spectrometry,
J. Phys. Chem., 1989, 93, 24, 7969, https://doi.org/10.1021/j100361a002
. [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]
Beyer and Keller, 1971
Beyer, R.A.; Keller, G.E.,
The Clustering of Atmospheric Gases to Alkali Ions,
Trans. Am. Geophys. Union, 1971, 52, 303. [all data]
Meot-Ner (Mautner) and Field, 1974
Meot-Ner (Mautner), M.; Field, F.H.,
Kinetics and Thermodynamics of the Association of CO+ with CO and of N2+ with N2 between 120 and 650 K,
J. Chem. Phys., 1974, 61, 9, 3742, https://doi.org/10.1063/1.1682560
. [all data]
Gonzalez and Hoff, 1989
Gonzalez, A.A.; Hoff, C.D.,
Inorg. Chem., 1989, 28, 4295. [all data]
Speller, 1983
Speller, C.V.,
Ph. D. Thesis, Universite de Paris Sud, 1983. [all data]
Linn, Ono, et al., 1981
Linn, S.H.; Ono, Y.; Ng, C.Y.,
Molecular Beam Photoionization Study of CO, N2, and NO Dimers and Clusters,
J. Chem. Phys., 1981, 74, 6, 3342, https://doi.org/10.1063/1.441486
. [all data]
Speller, Fitaire, et al., 1982
Speller, C.V.; Fitaire, M.; Pointu, A.M.,
H2CN+.nN2 Clustering Formation and the Atmosphere of Titan,
Nature, 1982, 300, 5892, 507, https://doi.org/10.1038/300507a0
. [all data]
Howard and Skinner, 1966
Howard, P.B.; Skinner, H.A.,
Thermochemistry of some reactions of aqueous hydrazine with halogens, hydrogen halides and N-halogenosuccinimides,
J. Chem. Soc. A, 1966, 1536-1540. [all data]
Pedley, Naylor, et al., 1986
Pedley, J.B.; Naylor, R.D.; Kirby, S.P.,
Thermochemical Data of Organic Compounds, Chapman and Hall, New York, 1986, 1-792. [all data]
Posey and Johnson, 1988
Posey, L.A.; Johnson, M.A.,
Pulsed Photoelectron Spectroscopy of Negative Cluster Ions: Isolation of Three Distinguishable Forms of N2O2-,
J. Chem. Phys., 1988, 88, 9, 5385, https://doi.org/10.1063/1.454576
. [all data]
Adams and Bohme, 1970
Adams, N.G.; Bohme, D.,
Flowing Afterglow Studies of Formation and Reactions of Cluster Ions of O2+, O2-, and O-,
J. Chem. Phys., 1970, 52, 6, 3133, https://doi.org/10.1063/1.1673449
. [all data]
Belt, Scaiano, et al., 1993
Belt, S.T.; Scaiano, J.C.; Whittlesey, M.K.,
J. Am. Chem. Soc., 1993, 115, 1921. [all data]
Johnson, Popov, et al., 1991
Johnson, F.P.A.; Popov, V.K.; George, M.W.; Bagratashvili, V.N.; Poliakoff, M.; Turner, J.J.,
Mendeleev Commun., 1991, 145.. [all data]
Notes
Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Mass spectrum (electron ionization), References
- Symbols used in this document:
S°gas,1 bar Entropy of gas at standard conditions (1 bar) 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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