Water
- Formula: H2O
- Molecular weight: 18.0153
- IUPAC Standard InChIKey: XLYOFNOQVPJJNP-UHFFFAOYSA-N
- CAS Registry Number: 7732-18-5
- 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. - Isotopologues:
- Other names: Water vapor; Distilled water; Ice; H2O; Dihydrogen oxide; steam; Tritiotope
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- Information on this page:
- Other data available:
- Gas phase thermochemistry data
- Condensed 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 650, reactions 651 to 700, reactions 751 to 800, reactions 801 to 850, reactions 851 to 900, reactions 901 to 950, reactions 951 to 1000, reactions 1001 to 1050, reactions 1051 to 1100, reactions 1101 to 1150, reactions 1151 to 1200, reactions 1201 to 1250, reactions 1251 to 1300, reactions 1301 to 1350, reactions 1351 to 1360
- Gas phase ion energetics data
- Ion clustering data
- IR Spectrum
- Mass spectrum (electron ionization)
- Vibrational and/or electronic energy levels
- Gas Chromatography
- Fluid Properties
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Reaction thermochemistry 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 as indicated in comments:
ALS - Hussein Y. Afeefy, Joel F. Liebman, and Stephen E. Stein
M - Michael M. Meot-Ner (Mautner) and Sharon G. Lias
B - John E. Bartmess
MS - José A. Martinho Simões
Note: Please consider using the reaction search for this species. This page allows searching of all reactions involving this species. A general reaction search form is also available. Future versions of this site may rely on reaction search pages in place of the enumerated reaction displays seen below.
Reactions 701 to 750
By formula: C6H10 + H2O = C6H12O
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -13.34 ± 0.34 | kcal/mol | Eqk | Taft, Levy, et al., 1952 | gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -14.34 ± 0.34 kcal/mol; At 308 °K; ALS |
By formula: (CH3O- • H2O) + CH4O = (CH3O- • CH4O • H2O)
Free energy of reaction
ΔrG° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
13.7 | 296. | FA | MacKay and Bohme, 1978 | gas phase; From thermochemical cycle,switching reaction(CH3O-)2H2O; Meot-Ner(Mautner), 1986; M |
By formula: (Na+ • 2H2O) + CO2 = (Na+ • CO2 • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 10.3 | kcal/mol | HPMS | Peterson, Mark, et al., 1984 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 23.9 | cal/mol*K | HPMS | Peterson, Mark, et al., 1984 | gas phase; M |
By formula: C6H14O2 + H2O = C4H8O + 2CH4O
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 8.65 ± 0.03 | kcal/mol | Cm | Wiberg, Morgan, et al., 1994 | liquid phase; ALS |
ΔrH° | 8.732 ± 0.023 | kcal/mol | Eqk | Wiberg and Squires, 1981 | liquid phase; ALS |
By formula: H18O13S-2 + 10H2O = H20O14S-2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 10.9 ± 2.0 | kcal/mol | TDAs | Blades and Kebarle, 2005 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 5.8 ± 2.0 | kcal/mol | TDAs | Blades and Kebarle, 2005 | gas phase; B |
By formula: H20O14S-2 + 11H2O = H22O15S-2
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 10.9 ± 2.0 | kcal/mol | TDAs | Blades and Kebarle, 2005 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 5.3 ± 2.0 | kcal/mol | TDAs | Blades and Kebarle, 2005 | gas phase; B |
By formula: (Cl- • 2H2O) + CH4O = (Cl- • CH4O • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 11.4 | kcal/mol | HPMS | Evans and Keesee, 1991 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 18.1 | cal/mol*K | HPMS | Evans and Keesee, 1991 | gas phase; M |
By formula: (Na+ • O2S) + H2O = (Na+ • H2O • O2S)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 19.8 | kcal/mol | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 20.2 | cal/mol*K | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; M |
By formula: (Na+ • H2O) + CO2 = (Na+ • CO2 • H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 12.6 | kcal/mol | HPMS | Peterson, Mark, et al., 1984 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 22.5 | cal/mol*K | HPMS | Peterson, Mark, et al., 1984 | gas phase; M |
By formula: (Na+ • H2O) + O2S = (Na+ • O2S • H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 14.1 | kcal/mol | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 17.4 | cal/mol*K | HPMS | Upschulte, Schelling, et al., 1984 | gas phase; M |
By formula: (K+ • 2CH4O) + H2O = (K+ • H2O • 2CH4O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 11.3 | kcal/mol | HPMS | Evans and Keesee, 1991 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 18.0 | cal/mol*K | HPMS | Evans and Keesee, 1991 | gas phase; M |
(l) + (
• 100
) (solution) = 2
(g) + (
• 100
) (solution)
By formula: C2H6Zn (l) + (H2O4S • 100H2O) (solution) = 2CH4 (g) + (O4SZn • 100H2O) (solution)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -81.7 ± 0.2 | kcal/mol | RSC | Carson, Hartley, et al., 1949 | Please also see Pedley and Rylance, 1977 and Cox and Pilcher, 1970, 2.; MS |
(l) + (
• 100
) (solution) = 2
(g) + (
• 100
) (solution)
By formula: C4H10Zn (l) + (H2O4S • 100H2O) (solution) = 2C2H6 (g) + (O4SZn • 100H2O) (solution)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | -84.7 ± 1.0 | kcal/mol | RSC | Carson, Hartley, et al., 1949 | Please also see Pedley and Rylance, 1977 and Cox and Pilcher, 1970, 2.; MS |
By formula: (O2- • 3H2O) + H2O = (O2- • 4H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrG° | 4.4 ± 2.0 | kcal/mol | TDAs | Kebarle, Arshadi, et al., 1968 | gas phase; B,M |
ΔrG° | 3.4 | kcal/mol | PHPMS | Arshadi and Kebarle, 1970 | gas phase; M |
By formula: O4S- + H2O = (O4S- • H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrG° | 5.90 ± 0.20 | kcal/mol | IMRE | Möhler, Reiner, et al., 1992 | gas phase; B |
Free energy of reaction
ΔrG° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
5.1 | 296. | FA | Fehsenfeld and Ferguson, 1974 | gas phase; M |
By formula: O3S- + H2O = (O3S- • H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrG° | 5.60 ± 0.20 | kcal/mol | IMRE | Möhler, Reiner, et al., 1992 | gas phase; B |
Free energy of reaction
ΔrG° (kcal/mol) | T (K) | Method | Reference | Comment |
---|---|---|---|---|
5.9 | 296. | FA | Fehsenfeld and Ferguson, 1974 | gas phase; M |
By formula: (Cl- • H2O) + CH4O = (Cl- • CH4O • H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 13.2 | kcal/mol | HPMS | Evans and Keesee, 1991 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 20.9 | cal/mol*K | HPMS | Evans and Keesee, 1991 | gas phase; M |
By formula: (K+ • CH4O) + H2O = (K+ • H2O • CH4O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 15.6 | kcal/mol | HPMS | Evans and Keesee, 1991 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 22.5 | cal/mol*K | HPMS | Evans and Keesee, 1991 | gas phase; M |
By formula: (K+ • H2O) + CH4O = (K+ • CH4O • H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 19.6 | kcal/mol | HPMS | Evans and Keesee, 1991 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 32.5 | cal/mol*K | HPMS | Evans and Keesee, 1991 | gas phase; M |
+
= C6H7OS-
By formula: C6H5S- + H2O = C6H7OS-
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 11.40 ± 0.20 | kcal/mol | TDAs | Sieck and Meot-ner, 1989 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 5.60 ± 0.70 | kcal/mol | TDAs | Sieck and Meot-ner, 1989 | gas phase; B |
By formula: (H3O+ • 2H2O) + N2 = (H3O+ • N2 • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 5.0 | kcal/mol | DT | Gheno and Fitaire, 1987 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 14.3 | cal/mol*K | DT | Gheno and Fitaire, 1987 | gas phase; M |
By formula: (CH3S- • 2H2O) + H2O = (CH3S- • 3H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 11.1 | kcal/mol | PHPMS | Sieck and Meot-ner, 1989 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 20.5 | cal/mol*K | PHPMS | Sieck and Meot-ner, 1989 | gas phase; M |
By formula: (CH3S- • 3H2O) + H2O = (CH3S- • 4H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 9.6 | kcal/mol | PHPMS | Sieck and Meot-ner, 1989 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 19.2 | cal/mol*K | PHPMS | Sieck and Meot-ner, 1989 | gas phase; M |
By formula: (CH3S- • H2O) + H2O = (CH3S- • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 13.5 | kcal/mol | PHPMS | Sieck and Meot-ner, 1989 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 23.5 | cal/mol*K | PHPMS | Sieck and Meot-ner, 1989 | gas phase; M |
By formula: (H3O+ • H2O) + N2 = (H3O+ • N2 • H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 5.3 | kcal/mol | DT | Gheno and Fitaire, 1987 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 13.9 | cal/mol*K | DT | Gheno and Fitaire, 1987 | gas phase; M |
By formula: (Sr+ • 2H2O) + H2O = (Sr+ • 3H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 25.7 | kcal/mol | HPMS | Tang, Lian, et al., 1976 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 28.6 | cal/mol*K | HPMS | Tang, Lian, et al., 1976 | gas phase; M |
By formula: (Sr+ • 3H2O) + H2O = (Sr+ • 4H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 22.3 | kcal/mol | HPMS | Tang, Lian, et al., 1976 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 28.2 | cal/mol*K | HPMS | Tang, Lian, et al., 1976 | gas phase; M |
By formula: (Sr+ • 4H2O) + H2O = (Sr+ • 5H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 20.6 | kcal/mol | HPMS | Tang, Lian, et al., 1976 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 30.5 | cal/mol*K | HPMS | Tang, Lian, et al., 1976 | gas phase; M |
By formula: (Sr+ • 5H2O) + H2O = (Sr+ • 6H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 18.3 | kcal/mol | HPMS | Tang, Lian, et al., 1976 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 30.5 | cal/mol*K | HPMS | Tang, Lian, et al., 1976 | gas phase; M |
By formula: (Sr+ • 6H2O) + H2O = (Sr+ • 7H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 17.3 | kcal/mol | HPMS | Tang, Lian, et al., 1976 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 34.4 | cal/mol*K | HPMS | Tang, Lian, et al., 1976 | gas phase; M |
By formula: (Sr+ • 7H2O) + H2O = (Sr+ • 8H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 16.4 | kcal/mol | HPMS | Tang, Lian, et al., 1976 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 37.6 | cal/mol*K | HPMS | Tang, Lian, et al., 1976 | gas phase; M |
By formula: (Ag+ • 2H2O) + H2O = (Ag+ • 3H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 15.0 | kcal/mol | HPMS | Holland and Castleman, 1982 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 21.6 | cal/mol*K | HPMS | Holland and Castleman, 1982 | gas phase; M |
By formula: (Ag+ • 3H2O) + H2O = (Ag+ • 4H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 14.9 | kcal/mol | HPMS | Holland and Castleman, 1982 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 29.5 | cal/mol*K | HPMS | Holland and Castleman, 1982 | gas phase; M |
By formula: (Ag+ • 4H2O) + H2O = (Ag+ • 5H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 13.7 | kcal/mol | HPMS | Holland and Castleman, 1982 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 30.3 | cal/mol*K | HPMS | Holland and Castleman, 1982 | gas phase; M |
By formula: (Ag+ • 5H2O) + H2O = (Ag+ • 6H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 13.3 | kcal/mol | HPMS | Holland and Castleman, 1982 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 32.2 | cal/mol*K | HPMS | Holland and Castleman, 1982 | gas phase; M |
By formula: (Pb+ • 2H2O) + H2O = (Pb+ • 3H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 12.2 | kcal/mol | HPMS | Tang and Castleman, 1972 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 20.2 | cal/mol*K | HPMS | Tang and Castleman, 1972 | gas phase; M |
By formula: (Pb+ • 4H2O) + H2O = (Pb+ • 5H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 10.0 | kcal/mol | HPMS | Tang and Castleman, 1972 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 22.3 | cal/mol*K | HPMS | Tang and Castleman, 1972 | gas phase; M |
By formula: (Bi+ • 2H2O) + H2O = (Bi+ • 3H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 14.0 | kcal/mol | HPMS | Tang and Castleman, 1974 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 24.4 | cal/mol*K | HPMS | Tang and Castleman, 1974 | gas phase; M |
By formula: (Bi+ • 3H2O) + H2O = (Bi+ • 4H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 12.0 | kcal/mol | HPMS | Tang and Castleman, 1974 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 23.5 | cal/mol*K | HPMS | Tang and Castleman, 1974 | gas phase; M |
By formula: (Bi+ • 4H2O) + H2O = (Bi+ • 5H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 10.5 | kcal/mol | HPMS | Tang and Castleman, 1974 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 22.7 | cal/mol*K | HPMS | Tang and Castleman, 1974 | gas phase; M |
By formula: (CO3- • 2H2O) + H2O = (CO3- • 3H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 13.1 | kcal/mol | HPMS | Keesee, Lee, et al., 1979 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 32.5 | cal/mol*K | HPMS | Keesee, Lee, et al., 1979 | gas phase; M |
By formula: (Cu+ • 4H2O) + H2O = (Cu+ • 5H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 14.0 | kcal/mol | HPMS | Holland and Castleman, 1982 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 29.1 | cal/mol*K | HPMS | Holland and Castleman, 1982 | gas phase; M |
By formula: (Cs+ • 3H2O) + H2O = (Cs+ • 4H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 10.6 | kcal/mol | HPMS | Dzidic and Kebarle, 1970 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 25.4 | cal/mol*K | HPMS | Dzidic and Kebarle, 1970 | gas phase; M |
By formula: (K+ • 4H2O) + H2O = (K+ • 5H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 10.7 | kcal/mol | HPMS | Searles and Kebarle, 1969 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 25.2 | cal/mol*K | HPMS | Searles and Kebarle, 1969 | gas phase; M |
By formula: (K+ • 5H2O) + H2O = (K+ • 6H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 10.0 | kcal/mol | HPMS | Searles and Kebarle, 1969 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 25.7 | cal/mol*K | HPMS | Searles and Kebarle, 1969 | gas phase; M |
By formula: (C2H7S+ • H2O) + H2O = (C2H7S+ • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 11.6 | kcal/mol | PHPMS | Meot-Ner (Mautner) and Sieck, 1985 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 23.0 | cal/mol*K | PHPMS | Meot-Ner (Mautner) and Sieck, 1985 | gas phase; M |
(C3H9Si+ • ) +
= (C3H9Si+ • 2
)
By formula: (C3H9Si+ • H2O) + H2O = (C3H9Si+ • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 19.9 | kcal/mol | PHPMS | Stone and Wytenberg, 1987 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 28.1 | cal/mol*K | PHPMS | Stone and Wytenberg, 1987 | gas phase; M |
By formula: (C4H9S+ • H2O) + H2O = (C4H9S+ • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 10.4 | kcal/mol | PHPMS | Hiraoka, Takimoto, et al., 1987 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 21.0 | cal/mol*K | PHPMS | Hiraoka, Takimoto, et al., 1987 | gas phase; M |
(C6H15Ge+ • ) +
= (C6H15Ge+ • 2
)
By formula: (C6H15Ge+ • H2O) + H2O = (C6H15Ge+ • 2H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 18.4 | kcal/mol | PHPMS | Stone and Wytenberg, 1987 | gas phase; M |
Quantity | Value | Units | Method | Reference | Comment |
ΔrS° | 32.8 | cal/mol*K | PHPMS | Stone and Wytenberg, 1987 | gas phase; M |
By formula: (HO- • 3H2O) + H2O = (HO- • 4H2O)
Quantity | Value | Units | Method | Reference | Comment |
---|---|---|---|---|---|
ΔrH° | 12.00 | kcal/mol | N/A | Meot-Ner (Mautner) and Speller, 1986 | gas phase; B |
Quantity | Value | Units | Method | Reference | Comment |
ΔrG° | 5.7 ± 1.4 | kcal/mol | N/A | Meot-Ner (Mautner) and Speller, 1986 | gas phase; B |
References
Go To: Top, Reaction thermochemistry data, Notes
Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.
Taft, Levy, et al., 1952
Taft, R.W., Jr.; Levy, J.B.; Aaron, D.; Hammett, L.P.,
Rates, equilibrium and temperature coefficients in the reversible hydration of gaseous 1-methylcyclopentene-1 by dilute nitric acid,
J. Am. Chem. Soc., 1952, 74, 4735-47. [all data]
Cox and Pilcher, 1970
Cox, J.D.; Pilcher, G.,
Thermochemistry of Organic and Organometallic Compounds, Academic Press, New York, 1970, 1-636. [all data]
MacKay and Bohme, 1978
MacKay, G.I.; Bohme, D.K.,
Proton-Transfer Reactions in Nitromethane at 297K,
Int. J. Mass Spectrom. Ion Phys., 1978, 26, 4, 327, https://doi.org/10.1016/0020-7381(78)80052-7
. [all data]
Meot-Ner(Mautner), 1986
Meot-Ner(Mautner), M.,
Comparative Stabilities of Cationic and Anionic Hydrogen-Bonded Networks. Mixed Clusters of Water-Methanol,
J. Am. Chem. Soc., 1986, 108, 20, 6189, https://doi.org/10.1021/ja00280a014
. [all data]
Peterson, Mark, et al., 1984
Peterson, K.I.; Mark, T.D.; Keesee, R.G.; Castleman, A.W.,
Thermochemical Properties of Gas - Phase Mixed Clusters: H2O/CO2 with Na+,
J. Phys. Chem., 1984, 88, 13, 2880, https://doi.org/10.1021/j150657a042
. [all data]
Wiberg, Morgan, et al., 1994
Wiberg, K.B.; Morgan, K.M.; Maltz, H.,
Thermochemistry of carbonyl reactions. 6. A study of hydration equilibria,
J. Am. Chem. Soc., 1994, 116, 11067-11077. [all data]
Wiberg and Squires, 1981
Wiberg, K.B.; Squires, R.R.,
Thermochemical studies of carbonyl reactions. 2. Steric effects in acetal and ketal hydrolysis,
J. Am. Chem. Soc., 1981, 103, 4473-4478. [all data]
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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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