Hydrogen chloride

Formula: ClH
Molecular weight: 36.461
IUPAC Standard InChI: InChI=1S/ClH/h1H
IUPAC Standard InChIKey: VEXZGXHMUGYJMC-UHFFFAOYSA-N
CAS Registry Number: 7647-01-0
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:
- Hydrochloric acid-d
Other names: Hydrochloric ccid; Anhydrous hydrochloric acid; Chlorohydric acid; Hydrochloric acid gas; Hydrochloride; Muriatic acid; Salzsaeure; HCl; Hydrochloric acid, anhydrous; Hydrogen-chloride-anhydrous-; Acide chlorhydrique; Acido cloridrico; Chloorwaterstof; Chlorowodor; Chlorwasserstoff; NA 1789; Spirits of salt; UN 1050; UN 1789; UN 2186; Anhydrous hydrogen chloride; Hydrogen chloride (acid); Marine acid; Soldering acid; Spirit of salt; Spirits of salts; Hydrogen chloride (HCl); NSC 77365; Hydrochloric acid
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Information on this page:
Other data available:
- Reaction thermochemistry data: reactions 51 to 100, reactions 101 to 150, reactions 151 to 158
- Ion clustering data
Data at other public NIST sites:
- Microwave spectra (on physics lab web site)
- Gas Phase Kinetics Database
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Data at NIST subscription sites:

NIST / TRC Web Thermo Tables, professional edition (thermophysical and thermochemical data)

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Gas phase thermochemistry data

Go To: Top, Phase change data, Reaction thermochemistry data, Henry's Law data, Gas phase ion energetics data, IR Spectrum, Mass spectrum (electron ionization), Constants of diatomic molecules, References, Notes

Quantity	Value	Units	Method	Reference	Comment
Δ_fH°_gas	-92.31 ± 0.10	kJ/mol	Review	Cox, Wagman, et al., 1984	CODATA Review value
Δ_fH°_gas	-92.31	kJ/mol	Review	Chase, 1998	Data last reviewed in September, 1964
Quantity	Value	Units	Method	Reference	Comment
S°_{gas,1 bar}	186.902 ± 0.005	J/mol*K	Review	Cox, Wagman, et al., 1984	CODATA Review value
S°_{gas,1 bar}	186.90	J/mol*K	Review	Chase, 1998	Data last reviewed in September, 1964

Gas Phase Heat Capacity (Shomate Equation)

C_p° = 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
C_p = heat capacity (J/mol*K)
H° = standard enthalpy (kJ/mol)
S° = standard entropy (J/mol*K)
t = temperature (K) / 1000.

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View table.

Temperature (K)	298. to 1200.	1200. to 6000.
A	32.12392	31.91923
B	-13.45805	3.203184
C	19.86852	-0.541539
D	-6.853936	0.035925
E	-0.049672	-3.438525
F	-101.6206	-108.0150
G	228.6866	218.2768
H	-92.31201	-92.31201
Reference	Chase, 1998	Chase, 1998
Comment	Data last reviewed in September, 1964	Data last reviewed in September, 1964

Phase change data

Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Henry's Law data, Gas phase ion energetics data, IR Spectrum, Mass spectrum (electron ionization), Constants of diatomic molecules, References, Notes

Data compiled as indicated in comments:
TRC - Thermodynamics Research Center, NIST Boulder Laboratories, Chris Muzny director
AC - William E. Acree, Jr., James S. Chickos

Quantity	Value	Units	Method	Reference	Comment
T_fus	161.15	K	N/A	Beckmann and Waentig, 1910	Uncertainty assigned by TRC = 2. K; TRC
Quantity	Value	Units	Method	Reference	Comment
P_triple	0.13800	bar	N/A	Henderson, Lewis, et al., 1986	Uncertainty assigned by TRC = 0.00006 bar; TRC
Quantity	Value	Units	Method	Reference	Comment
T_c	324.68	K	N/A	Henderson, Lewis, et al., 1986	Uncertainty assigned by TRC = 0.03 K; TRC
Quantity	Value	Units	Method	Reference	Comment
P_c	82.56	bar	N/A	Henderson, Lewis, et al., 1986	Uncertainty assigned by TRC = 0.0824 bar; VP measured up to 219 K and Pc determined from fitted Wagner equation; TRC

Enthalpy of vaporization

Δ_vapH (kJ/mol)	Temperature (K)	Method	Reference	Comment
16.2	188.	C	Giauque and Wiebe, 1928	AC

Antoine Equation Parameters

log₁₀(P) = A − (B / (T + C))
P = vapor pressure (bar)
T = temperature (K)

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Temperature (K)	A	B	C	Reference	Comment
122.3 to 188.3	3.60765	535.172	-39.847	Stull, 1947	Coefficents calculated by NIST from author's data.
188.3 to 309.4	4.57389	868.358	1.754	Stull, 1947	Coefficents calculated by NIST from author's data.

Enthalpy of sublimation

Δ_subH (kJ/mol)	Temperature (K)	Reference	Comment
19.7	127.	Ser and Larher, 1990	Based on data from 121. to 133. K.; AC
19.6	142.	Ser and Larher, 1990	Based on data from 134. to 150. K.; AC

In addition to the Thermodynamics Research Center (TRC) data available from this site, much more physical and chemical property data is available from the following TRC products:

Reaction thermochemistry data

Go To: Top, Gas phase thermochemistry data, Phase change data, Henry's Law data, Gas phase ion energetics data, IR Spectrum, Mass spectrum (electron ionization), Constants of diatomic molecules, References, Notes

Data compiled as indicated in comments:
B - John E. Bartmess
M - Michael M. Meot-Ner (Mautner) and Sharon G. Lias
ALS - Hussein Y. Afeefy, Joel F. Liebman, and Stephen E. Stein
MS - José A. Martinho Simões

Note: Please consider using the reaction search for this species. This page allows searching of all reactions involving this species. A general reaction search form is also available. Future versions of this site may rely on reaction search pages in place of the enumerated reaction displays seen below.

Reactions 1 to 50

+ Hydrogen chloride = ( • )

By formula: Cl^- + HCl = (Cl^- • HCl)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	124. ± 4.2	kJ/mol	N/A	Metz, Kitsopoulos, et al., 1988	gas phase; Affinity: shift in apparent EA from lesser-solvated ion. Ignores any neutral-neutral bond.; B
Δ_rH°	99.6 ± 8.4	kJ/mol	TDEq	Caldwell and Kebarle, 1985	gas phase; B,M
Δ_rH°	96.7 ± 8.4	kJ/mol	IMRE	Larson and McMahon, 1984	gas phase; B,M
Δ_rH°	99.16 ± 0.84	kJ/mol	TDAs	Yamdagni and Kebarle, 1974	gas phase; B,M
Δ_rH°	85.4	kJ/mol	HPMS	Upschulte, Evans, et al., 1986	gas phase; From thermochemical cycle(Cl-)H2O/HCl, Entropy change calculated or estimated; Keesee and Castleman, 1980; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	93.3	J/mol*K	PHPMS	Caldwell and Kebarle, 1985	gas phase; switching reaction(Cl-)SO2; M
Δ_rS°	98.3	J/mol*K	PHPMS	Yamdagni and Kebarle, 1974	gas phase; M
Δ_rS°	98.3	J/mol*K	N/A	Larson and McMahon, 1984, 2	gas phase; switching reaction(Cl-)t-C4H9OH, Entropy change calculated or estimated; French, Ikuta, et al., 1982; M
Δ_rS°	95.4	J/mol*K	N/A	Upschulte, Evans, et al., 1986	gas phase; From thermochemical cycle(Cl-)H2O/HCl, Entropy change calculated or estimated; Keesee and Castleman, 1980; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	68.2 ± 8.4	kJ/mol	IMRE	Larson and McMahon, 1987	gas phase; K = 0.60 for HCl..Cl- + DCL <=> DCl..Cl- + HCl, anchored to Larson and McMahon, 1984, 32; B
Δ_rG°	72. ± 11.	kJ/mol	TDEq	Caldwell and Kebarle, 1985	gas phase; B
Δ_rG°	66.9 ± 8.4	kJ/mol	IMRE	Larson and McMahon, 1984	gas phase; B,M
Δ_rG°	69.9 ± 1.3	kJ/mol	TDAs	Yamdagni and Kebarle, 1974	gas phase; B
Δ_rG°	56.9	kJ/mol	HPMS	Upschulte, Evans, et al., 1986	gas phase; From thermochemical cycle(Cl-)H2O/HCl, Entropy change calculated or estimated; Keesee and Castleman, 1980; M

+ = Hydrogen chloride

By formula: Cl^- + H⁺ = HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	1394.9	kJ/mol	N/A	Martin and Hepburn, 1998	gas phase; Given: ΔHacid(0K)=116288.7±0.6 cm-1, or 332.486±0.002 kcal/mol; B
Δ_rH°	1396. ± 8.8	kJ/mol	G+TS	Fujio, McIver, et al., 1981	gas phase; value altered from reference due to change in acidity scale; B
Δ_rH°	1377.0	kJ/mol	N/A	Check, Faust, et al., 2001	gas phase; FeCC-(q); ; ΔS(EA)=5.0; B
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	1372.8 ± 0.42	kJ/mol	H-TS	Martin and Hepburn, 1998	gas phase; Given: ΔHacid(0K)=116288.7±0.6 cm-1, or 332.486±0.002 kcal/mol; B
Δ_rG°	1374. ± 8.4	kJ/mol	IMRE	Fujio, McIver, et al., 1981	gas phase; value altered from reference due to change in acidity scale; B
Δ_rG°	1354.4	kJ/mol	N/A	Check, Faust, et al., 2001	gas phase; FeCC-(q); ; ΔS(EA)=5.0; B

( • Hydrogen chloride ) + = ( • 2)

By formula: (Cl^- • HCl) + HCl = (Cl^- • 2HCl)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	63.60 ± 0.84	kJ/mol	TDAs	Yamdagni and Kebarle, 1974	gas phase; B,M
Δ_rH°	58.6	kJ/mol	PHPMS	Caldwell and Kebarle, 1985	gas phase; switching reaction(Cl- HCl)SO2; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	85.4	J/mol*K	PHPMS	Caldwell and Kebarle, 1985	gas phase; switching reaction(Cl- HCl)SO2; M
Δ_rS°	102.	J/mol*K	PHPMS	Yamdagni and Kebarle, 1974	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	33.1 ± 0.84	kJ/mol	TDAs	Yamdagni and Kebarle, 1974	gas phase; B

+ Hydrogen chloride = ( • )

By formula: I^- + HCl = (I^- • HCl)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	61.9 ± 8.4	kJ/mol	TDAs	Caldwell and Kebarle, 1985	gas phase; B,M
Δ_rH°	59.4	kJ/mol	HPMS	Keesee, Lee, et al., 1980	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	83.7	J/mol*K	PHPMS	Caldwell and Kebarle, 1985	gas phase; M
Δ_rS°	95.0	J/mol*K	HPMS	Keesee, Lee, et al., 1980	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	37. ± 11.	kJ/mol	TDAs	Caldwell and Kebarle, 1985	gas phase; B

HO₄S^- + Hydrogen chloride = (HO₄S^- • )

By formula: HO₄S^- + HCl = (HO₄S^- • HCl)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	65.7 ± 4.2	kJ/mol	TDEq	Bohringer, Fahey, et al., 1984	gas phase; Relative to HOH..HSO₄^-, Bohringer, Fahey, et al., 1984; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	63.2	J/mol*K	N/A	Bohringer, Fahey, et al., 1984	gas phase; switching reaction(HSO4-)H2O, Entropy change calculated or estimated; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	46.9 ± 4.2	kJ/mol	TDEq	Bohringer, Fahey, et al., 1984	gas phase; Relative to HOH..HSO₄^-, Bohringer, Fahey, et al., 1984; B,M

( • Hydrogen chloride • ) + = ( • 2 • )

By formula: (Cl^- • HCl • H₂O) + HCl = (Cl^- • 2HCl • H₂O)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	51.5	kJ/mol	HPMS	Upschulte, Evans, et al., 1986	gas phase; From thermochemical cycle,switching reaction(Cl- H2O) HCl, deuterated; Yamdagni and Kebarle, 1974; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	87.4	J/mol*K	HPMS	Upschulte, Evans, et al., 1986	gas phase; From thermochemical cycle,switching reaction(Cl- H2O) HCl, deuterated; Yamdagni and Kebarle, 1974; M

( • 2) + Hydrogen chloride = ( • • 2)

By formula: (Cl^- • 2H₂O) + HCl = (Cl^- • HCl • 2H₂O)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	54.4	kJ/mol	HPMS	Upschulte, Evans, et al., 1986	gas phase; From thermochemical cycle(Cl- 2H2O)H2O, deuterated; Keesee and Castleman, 1980; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	90.8	J/mol*K	HPMS	Upschulte, Evans, et al., 1986	gas phase; From thermochemical cycle(Cl- 2H2O)H2O, deuterated; Keesee and Castleman, 1980; M

( • ) + Hydrogen chloride = ( • • )

By formula: (Br^- • O₂S) + HCl = (Br^- • HCl • O₂S)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	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
Δ_rS°	77.8	J/mol*K	PHPMS	Caldwell and Kebarle, 1985	gas phase; From thermochemical cycle,switching reaction(Br-)SO2; M

+ Hydrogen chloride = ( • )

By formula: Br^- + HCl = (Br^- • HCl)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	82.0 ± 8.4	kJ/mol	TDEq	Caldwell and Kebarle, 1985	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	92.0	J/mol*K	PHPMS	Caldwell and Kebarle, 1985	gas phase; switching reaction(Br-)SO2; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	54. ± 11.	kJ/mol	TDEq	Caldwell and Kebarle, 1985	gas phase; B

( • 2 Hydrogen chloride ) + = ( • 3)

By formula: (Cl^- • 2HCl) + HCl = (Cl^- • 3HCl)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	49.0 ± 1.3	kJ/mol	TDAs	Yamdagni and Kebarle, 1974	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	97.9	J/mol*K	PHPMS	Yamdagni and Kebarle, 1974	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	19.7 ± 1.3	kJ/mol	TDAs	Yamdagni and Kebarle, 1974	gas phase; B

( • 3 Hydrogen chloride ) + = ( • 4)

By formula: (Cl^- • 3HCl) + HCl = (Cl^- • 4HCl)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	43.1 ± 2.9	kJ/mol	TDAs	Yamdagni and Kebarle, 1974	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	112.	J/mol*K	PHPMS	Yamdagni and Kebarle, 1974	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	9.6 ± 4.2	kJ/mol	TDAs	Yamdagni and Kebarle, 1974	gas phase; B

( • 2 Hydrogen chloride ) + = ( • • 2)

By formula: (Cl^- • 2HCl) + H₂O = (Cl^- • H₂O • 2HCl)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	32.	kJ/mol	HPMS	Upschulte, Evans, et al., 1986	gas phase; deuterated, quoted in Keesee and Castleman, 1986; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	63.6	J/mol*K	HPMS	Upschulte, Evans, et al., 1986	gas phase; deuterated, quoted in Keesee and Castleman, 1986; M

( • Hydrogen chloride ) + = ( • • )

By formula: (Cl^- • HCl) + H₂O = (Cl^- • H₂O • HCl)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	43.9	kJ/mol	HPMS	Upschulte, Evans, et al., 1986	gas phase; deuterated, quoted in Keesee and Castleman, 1986; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	78.2	J/mol*K	HPMS	Upschulte, Evans, et al., 1986	gas phase; deuterated, quoted in Keesee and Castleman, 1986; M

+ = + Hydrogen chloride

By formula: C₂H₃ClO + H₂O = C₂H₄O₂ + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-94.47	kJ/mol	Cm	Devore and O'Neal, 1969	liquid phase; Heat of hydrolysis; ALS
Δ_rH°	-92.30	kJ/mol	Cm	Pritchard and Skinner, 1950	liquid phase; Heat of hydrolysis at 298 K, see Carson and Skinner, 1949; ALS
Δ_rH°	-92.42	kJ/mol	Cm	Carson and Skinner, 1949	liquid phase; ALS

( • • Hydrogen chloride ) + = ( • 2 • )

By formula: (Cl^- • H₂O • HCl) + H₂O = (Cl^- • 2H₂O • HCl)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	40.	kJ/mol	HPMS	Upschulte, Evans, et al., 1986	gas phase; deuterated, quoted in 86 KEE/CAS; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	85.4	J/mol*K	HPMS	Upschulte, Evans, et al., 1986	gas phase; deuterated, quoted in 86 KEE/CAS; M

( • ) + Hydrogen chloride = ( • • )

By formula: (Cl^- • O₂S) + HCl = (Cl^- • HCl • O₂S)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	58.2	kJ/mol	PHPMS	Caldwell and Kebarle, 1985	gas phase; From thermochemical cycle; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	80.3	J/mol*K	PHPMS	Caldwell and Kebarle, 1985	gas phase; From thermochemical cycle; M

= + Hydrogen chloride

By formula: C₂H₄Cl₂ = C₂H₃Cl + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	50.6 ± 4.2	kJ/mol	Cm	Buravtsev, Grigor'ev, et al., 1992	gas phase; ALS
Δ_rH°	82.0	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	liquid phase; ALS
Δ_rH°	68.2	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	gas phase; ALS
Δ_rH°	67.95	kJ/mol	Eqk	Ghosh and Guha, 1951	liquid phase; ALS

( • Hydrogen chloride ) + = ( • 2)

By formula: (Br^- • HCl) + HCl = (Br^- • 2HCl)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	52.3	kJ/mol	PHPMS	Caldwell and Kebarle, 1985	gas phase; switching reaction(Br-)SO2; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	77.0	J/mol*K	PHPMS	Caldwell and Kebarle, 1985	gas phase; switching reaction(Br-)SO2; M

= + Hydrogen chloride

By formula: C₂H₅Cl = C₂H₄ + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	92.0	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	liquid phase; ALS
Δ_rH°	71.5	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	gas phase; ALS
Δ_rH°	72.6 ± 2.1	kJ/mol	Eqk	Howlett, 1955	gas phase; ALS
Δ_rH°	71.5	kJ/mol	Eqk	Lane, Linnett, et al., 1953	gas phase; ALS

= + Hydrogen chloride

By formula: C₂H₃Cl₃ = C₂H₂Cl₂ + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	56.9	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	liquid phase; ALS
Δ_rH°	49.0	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	gas phase; ALS
Δ_rH°	56.9 ± 2.1	kJ/mol	Eqk	Levanova, Treger, et al., 1975	liquid phase; solvent: Nitrobenzene; Flow reactor at 50°C; ALS

+ = + Hydrogen chloride

By formula: H₂O + C₇H₅ClO = C₇H₆O₂ + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-34.04 ± 0.21	kJ/mol	Cm	Moselhy and Pritchard, 1975	liquid phase; solvent: Diphenyl-ether; see Carson, Pritchard, et al., 1950 and Davies, Dunning, et al., 1972; ALS
Δ_rH°	-101.9	kJ/mol	Cm	Carson, Pritchard, et al., 1950	liquid phase; Heat of hydrolysis; ALS

= + Hydrogen chloride

By formula: C₃H₇Cl = C₃H₆ + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	72.4 ± 0.8	kJ/mol	Eqk	Noren and Sunner, 1970	gas phase; ALS
Δ_rH°	73.72 ± 0.63	kJ/mol	Eqk	Kabo and Andreevskii, 1963	gas phase; At 415.5 K; ALS
Δ_rH°	73.0 ± 2.1	kJ/mol	Eqk	Howlett, 1955	gas phase; ALS

= + Hydrogen chloride

By formula: C₄H₉Cl = C₄H₈ + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	74. ± 2.	kJ/mol	Eqk	Howlett, 1955	gas phase; ALS
Δ_rH°	74.06	kJ/mol	Eqk	Howlett, 1951	gas phase; Hf-gas-(390) -44.4 kcal/mol; ALS
Δ_rH°	72. ± 2.	kJ/mol	Eqk	Kistiakowsky and Stauffer, 1937	gas phase; ALS

Hydrogen chloride + =

By formula: HCl + C₉H₁₀ = C₉H₁₁Cl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-36.8 ± 1.9	kJ/mol	Cm	Arnett and Pienta, 1980	liquid phase; solvent: Methylene chloride; Hydrochlorination; ALS
Δ_rH°	-51.9 ± 4.6	kJ/mol	Cm	Nesterova, Kovzel, et al., 1977	liquid phase; Hydrochlorination; ALS

( • ) + Hydrogen chloride = ( • • )

By formula: (Cl^- • H₂O) + HCl = (Cl^- • HCl • H₂O)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	66.9	kJ/mol	HPMS	Upschulte, Evans, et al., 1986	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	91.2	J/mol*K	HPMS	Upschulte, Evans, et al., 1986	gas phase; M

+ Hydrogen chloride = ( • )

By formula: CH₃⁺ + HCl = (CH₃⁺ • HCl)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	216.	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

= + Hydrogen chloride

By formula: C₃H₆Cl₂ = C₃H₅Cl + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	65.1	kJ/mol	Eqk	Levanova, Rodova, et al., 1983	liquid phase; Flow reactor; ALS
Δ_rH°	59.8 ± 0.8	kJ/mol	Eqk	Shevtsova, Rozhnov, et al., 1970	gas phase; Heat of Dehydrochlorination at 392 K; ALS

+ 2 = + 2 Hydrogen chloride

By formula: C₂H₄Cl₂ + 2H₂ = C₂H₆ + 2HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-143.0 ± 0.96	kJ/mol	Chyd	Lacher, Amador, et al., 1967	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -147.77 ± 0.50 kJ/mol; At 250 C; ALS

2 + = + 2 Hydrogen chloride

By formula: 2H₂ + C₃H₆Cl₂ = C₃H₈ + 2HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-126.5 ± 1.1	kJ/mol	Chyd	Lacher, Amador, et al., 1967	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -130.60 ± 0.54 kJ/mol; At 250 C; ALS

2 + = + 2 Hydrogen chloride

By formula: 2H₂ + CH₂Cl₂ = CH₄ + 2HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-163.4 ± 1.3	kJ/mol	Chyd	Lacher, Amador, et al., 1967	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -167.7 ± 1.3 kJ/mol; At 250 C; ALS

2 + = + 2 Hydrogen chloride

By formula: 2H₂ + C₂H₄Cl₂ = C₂H₆ + 2HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-140.8 ± 1.0	kJ/mol	Chyd	Lacher, Amador, et al., 1967	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -145.0 ± 0.50 kJ/mol; At 250C; ALS

= + Hydrogen chloride

By formula: C₄H₈Cl₂ = C₄H₇Cl + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-8.79 ± 0.08	kJ/mol	Eqk	Levanova, Rozhnov, et al., 1972	gas phase; At 568 K; ALS
Δ_rH°	55.2 ± 0.3	kJ/mol	Eqk	Levanova, Rozhnov, et al., 1972	gas phase; At 404.5 K; ALS

= + Hydrogen chloride

By formula: C₄H₈Cl₂ = C₄H₇Cl + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-14. ± 0.08	kJ/mol	Eqk	Levanova, Rozhnov, et al., 1972	gas phase; At 568 K; ALS
Δ_rH°	5.0 ± 0.3	kJ/mol	Eqk	Levanova, Rozhnov, et al., 1972	gas phase; At 404.5 K; ALS

2 + = + Hydrogen chloride

By formula: 2H₂ + C₂ClF₃ = C₂H₃F₃ + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-267.7 ± 2.1	kJ/mol	Chyd	Lacher, Kianpour, et al., 1956	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -271.6 kJ/mol; At 410 K; ALS

( • Hydrogen chloride ) + = ( • • )

By formula: (Cl^- • HCl) + O₂S = (Cl^- • O₂S • HCl)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	51.5	kJ/mol	PHPMS	Caldwell and Kebarle, 1985	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	77.4	J/mol*K	PHPMS	Caldwell and Kebarle, 1985	gas phase; M

( • Hydrogen chloride ) + = ( • • )

By formula: (Br^- • HCl) + O₂S = (Br^- • O₂S • HCl)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	50.6	kJ/mol	PHPMS	Caldwell and Kebarle, 1985	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	77.8	J/mol*K	PHPMS	Caldwell and Kebarle, 1985	gas phase; M

= + Hydrogen chloride

By formula: C₄H₈Cl₂ = C₄H₇Cl + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	69.0	kJ/mol	Eqk	Levanova, Rodova, et al., 1974	gas phase; ALS
Δ_rH°	66.53 ± 0.92	kJ/mol	Eqk	Rodova, Levanova, et al., 1973	gas phase; At 454 K; ALS

= + Hydrogen chloride

By formula: C₄H₉ClO = C₄H₈O + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	68.2 ± 2.1	kJ/mol	Eqk	Failes and Stimson, 1967	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = 69.0 kJ/mol; At 450 K; ALS

= Hydrogen chloride +

By formula: C₂H₂Cl₄ = HCl + C₂HCl₃

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	43.9	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	gas phase; ALS
Δ_rH°	45.40	kJ/mol	Eqk	Levanova, Bushneva, et al., 1976	liquid phase; At 333 K; ALS

= + Hydrogen chloride

By formula: C₂HCl₅ = C₂Cl₄ + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	45.1 ± 4.5	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	liquid phase; GC; ALS
Δ_rH°	39.	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	gas phase; ALS

2 Hydrogen chloride (g) + (l) = AlCl₃ (cr) + 2 (g)

By formula: 2HCl (g) + C₄H₁₀AlCl (l) = AlCl₃ (cr) + 2C₂H₆ (g)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-265.0 ± 3.3	kJ/mol	RSC	Shaulov and Shmyreva, 1968	The reaction enthalpy was derived from data in Shaulov and Shmyreva, 1968.; MS

= + Hydrogen chloride

By formula: C₅H₁₀Cl₂ = C₅H₉Cl + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	68. ± 1.	kJ/mol	Eqk	Meged, Levanova, et al., 1980	gas phase; ALS
Δ_rH°	68.2 ± 4.2	kJ/mol	Eqk	Meged, Levanova, et al., 1980	gas phase; ALS

+ Hydrogen chloride = ( • )

By formula: F^- + HCl = (F^- • HCl)

Bond type: Hydrogen bond (negative ion to hydride)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	250. ± 8.	kJ/mol	ICR	Larson and McMahon, 1985	gas phase; bracketing; M

= + Hydrogen chloride

By formula: C₄H₈Cl₂ = C₄H₇Cl + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	61.1	kJ/mol	Eqk	Levanova, Rodova, et al., 1974	gas phase; ALS
Δ_rH°	61.1 ± 0.4	kJ/mol	Eqk	Rodova, Shevtsova, et al., 1974	gas phase; ALS

+ Hydrogen chloride = ( • )

By formula: Na⁺ + HCl = (Na⁺ • HCl)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	51.0	kJ/mol	FA	Perry, Rowe, et al., 1980	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	85.4	J/mol*K	FA	Perry, Rowe, et al., 1980	gas phase; M

= + Hydrogen chloride

By formula: C₂H₄Cl₂ = C₂H₃Cl + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	74.5	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	liquid phase; ALS
Δ_rH°	61.9	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	gas phase; ALS

= + Hydrogen chloride

By formula: C₂H₃Cl₃ = C₂H₂Cl₂ + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	51.5	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	gas phase; ALS
Δ_rH°	65.3	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	liquid phase; ALS

= Hydrogen chloride +

By formula: C₂H₂Cl₄ = HCl + C₂HCl₃

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	55.2	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	liquid phase; ALS
Δ_rH°	44.8	kJ/mol	Eqk	Levanova, Bushneva, et al., 1979	gas phase; ALS

C₃₀H₂₈Fe₂Ti (cr) + 2( Hydrogen chloride • 4.40) (solution) = 2 (cr) + (cr)

By formula: C₃₀H₂₈Fe₂Ti (cr) + 2(HCl • 4.40H₂O) (solution) = 2C₁₀H₁₀Fe (cr) + C₁₀H₁₀Cl₂Ti (cr)

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-253.5 ± 4.5	kJ/mol	RSC	Dias, Salema, et al., 1982	Please also see Calhorda, Dias, et al., 1987.; MS

+ = + Hydrogen chloride

By formula: C₇H₄Cl₂O + H₂O = C₇H₅ClO₂ + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-39.8 ± 0.3	kJ/mol	Cm	Moselhy and Pritchard, 1975	liquid phase; solvent: Diphenyl-ether; Heat of hydrolysis; ALS

Henry's Law data

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Data compiled by: Rolf Sander

Henry's Law constant (water solution)

k_H(T) = k°_H exp(d(ln(k_H))/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(k_H))/d(1/T) = Temperature dependence constant (K)

k°_H (mol/(kg*bar))	d(ln(k_H))/d(1/T) (K)	Method	Reference	Comment
19.	600.	Q	N/A	Only the tabulated data between T = 273. K and T = 303. K from missing citation was used to derive k_H and -Δ k_H/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.
2.0×10⁺⁶/K_A	9000.	T	N/A	For strong acids, the solubility is often expressed as k_H = ([H⁺] * [A^-]) / p(HA). To obtain the physical solubility of HA, the value has to be divided by the acidity constant K_A. missing citation corrects erroneous data from missing citation.
2500.		Q	N/A	Several references are given in the list of Henry's law constants but not assigned to specific species.
1.1	2000.	T	N/A
20.		C	N/A
2.0×10⁺⁶/K_A	9000.	T	N/A
1500.		X	N/A	The value is taken from the compilation of solubilities by W. Asman (unpublished).
19.	9000.	X	N/A	The value is taken from the compilation of solubilities by W. Asman (unpublished).
170000./K_A		X	N/A	The value is taken from the compilation of solubilities by W. Asman (unpublished). For strong acids, the solubility is often expressed as k_H = ([H⁺] * [A^-]) / p(HA). To obtain the physical solubility of HA, the value has to be divided by the acidity constant K_A.

Gas phase ion energetics data

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Data evaluated as indicated in comments:
HL - Edward P. Hunter and Sharon G. Lias
L - Sharon G. Lias

Data compiled as indicated in comments:
B - John E. Bartmess
LBLHLM - Sharon G. Lias, John E. Bartmess, Joel F. Liebman, John L. Holmes, Rhoda D. Levin, and W. Gary Mallard
LLK - Sharon G. Lias, Rhoda D. Levin, and Sherif A. Kafafi
RDSH - Henry M. Rosenstock, Keith Draxl, Bruce W. Steiner, and John T. Herron

View reactions leading to HCl⁺ (ion structure unspecified)

Quantity	Value	Units	Method	Reference	Comment
IE (evaluated)	12.744 ± 0.009	eV	N/A	N/A	L
Quantity	Value	Units	Method	Reference	Comment
Proton affinity (review)	556.9	kJ/mol	N/A	Hunter and Lias, 1998	HL
Quantity	Value	Units	Method	Reference	Comment
Gas basicity	530.1	kJ/mol	N/A	Hunter and Lias, 1998	HL

Ionization energy determinations

IE (eV)	Method	Reference	Comment
12.790	PE	Wang, Dillon, et al., 1984	LBLHLM
12.752 ± 0.006	PE	Pennetreau, Natalis, et al., 1983	LBLHLM
12.748	PE	Von Niessen, Asbrink, et al., 1982	LBLHLM
12.747 ± 0.002	PE	Natalis, Pennetreau, et al., 1982	LBLHLM
12.75	PE	Kimura, Katsumata, et al., 1981	LLK
12.72 ± 0.03	PI	Tiedemann, Anderson, et al., 1979	LLK
12.748	EVAL	Huber and Herzberg, 1979	LLK
12.748 ± 0.005	PE	Weiss, Lawrence, et al., 1970	RDSH
12.74 ± 0.01	PE	Lempka, Passmore, et al., 1968	RDSH
12.742 ± 0.010	PI	Nicholson, 1965	RDSH
12.74 ± 0.01	PI	Watanabe, 1957	RDSH

Appearance energy determinations

Ion	AE (eV)	Other Products	Method	Reference	Comment
Cl⁺	17.34 ± 0.01	H	PI	Krauss, Walker, et al., 1968	RDSH
H⁺	14.5	Cl^-	EI	Fox, 1957	RDSH

De-protonation reactions

+ = Hydrogen chloride

By formula: Cl^- + H⁺ = HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	1394.9	kJ/mol	N/A	Martin and Hepburn, 1998	gas phase; Given: ΔHacid(0K)=116288.7±0.6 cm-1, or 332.486±0.002 kcal/mol; B
Δ_rH°	1396. ± 8.8	kJ/mol	G+TS	Fujio, McIver, et al., 1981	gas phase; value altered from reference due to change in acidity scale; B
Δ_rH°	1377.0	kJ/mol	N/A	Check, Faust, et al., 2001	gas phase; FeCC-(q); ; ΔS(EA)=5.0; B
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	1372.8 ± 0.42	kJ/mol	H-TS	Martin and Hepburn, 1998	gas phase; Given: ΔHacid(0K)=116288.7±0.6 cm-1, or 332.486±0.002 kcal/mol; B
Δ_rG°	1374. ± 8.4	kJ/mol	IMRE	Fujio, McIver, et al., 1981	gas phase; value altered from reference due to change in acidity scale; B
Δ_rG°	1354.4	kJ/mol	N/A	Check, Faust, et al., 2001	gas phase; FeCC-(q); ; ΔS(EA)=5.0; B

IR Spectrum

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Data compiled by: Coblentz Society, Inc.

Mass spectrum (electron ionization)

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Data compiled by: NIST Mass Spectrometry Data Center, William E. Wallace, director

Spectrum

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Additional Data

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NIST MS number	18847

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Constants of diatomic molecules

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Data compiled by: Klaus P. Huber and Gerhard H. Herzberg

Symbols used in the table of constants
Symbol	Meaning
State	electronic state and / or symmetry symbol
T_e	minimum electronic energy (cm^-1)
ω_e	vibrational constant – first term (cm^-1)
ω_ex_e	vibrational constant – second term (cm^-1)
ω_ey_e	vibrational constant – third term (cm^-1)
B_e	rotational constant in equilibrium position (cm^-1)
α_e	rotational constant – first term (cm^-1)
γ_e	rotation-vibration interaction constant (cm^-1)
D_e	centrifugal distortion constant (cm^-1)
β_e	rotational constant – first term, centrifugal force (cm^-1)
r_e	internuclear distance (Å)
Trans.	observed transition(s) corresponding to electronic state
ν₀₀	position of 0-0 band (units noted in table)

Diatomic constants for H³⁵Cl
State	T_e	ω_e	ω_ex_e	ω_ey_e	B_e	α_e	γ_e	D_e	β_e	r_e	Trans.	ν₀₀
Rydberg 1												200-210 eV
	↳Hayes and Brown, 1972; Schwarz, 1975
	Numerous absorption bands above 123000 cm^-1, tentatively assigned to higher members of the Rydberg series starting with L and M and converging to A ²Σ⁺ of HCl⁺.
	↳Terwilliger and Smith, 1973
M (¹Σ⁺)	(117811)	[1529] 2									M ← X	117093
M (¹Σ⁺)	↳missing citation
L (¹Σ⁺,¹Π)	111280	1531	52 3								L ← X	110555
	↳missing citation
	4
	↳Douglas and Greening, 1979
State	T_e	ω_e	ω_ex_e	ω_ey_e	B_e	α_e	γ_e	D_e	β_e	r_e	Trans.	ν₀₀
K ¹Π	(89861)	[2604.6] Z			[9.230] 5			[-12.₆E-4] 5		[1.3654]	K ← X R	89680.5 Z
K ¹Π	↳Douglas and Greening, 1979
H ¹Σ⁺	(89120)	[2093.8] Z			[8.4410]			[8.93E-4]		[1.4278]	H ← X R	88684.5 Z
H ¹Σ⁺	↳Douglas and Greening, 1979
E ¹Σ⁺	(84193)	[2138.6] Z			[6.6423]			[36.2]		[1.6096]	E ← X R	83780.2 Z
E ¹Σ⁺	↳Douglas and Greening, 1979
g (³Σ^-)1	[84329.7] 6				[10.36] 7			[17E-4] 7		[1.28₉]	g ← X	82847.4 Z
g (³Σ^-)1	↳missing citation
State	T_e	ω_e	ω_ex_e	ω_ey_e	B_e	α_e	γ_e	D_e	β_e	r_e	Trans.	ν₀₀
f₁ ³Δ₁	[84006.1] 6				[10.27₀] 8			[-13E-4] 8		[1.294]	f₁ ← X	82523.8 Z
f₁ ³Δ₁	↳missing citation
D ¹Π	[83972.0] 9				[9.79₄] 10			[20.₅E-4] 10		[1.326]	D ← X R	82489.7 Z
D ¹Π	↳missing citation
d₀ ³Π₀	[83753.6] 9				[9.40₄] 11			[-2.₂E-4] 11		[1.353]	d₀ ← X R	82271.3 Z
d₀ ³Π₀	↳missing citation
f₂ ³Δ₂	[83497.7] 6				[10.85₁] 12			[29.₅E-4] 12		[1.259]	f₂ ← X V	82015.4 Z
f₂ ³Δ₂	↳missing citation
State	T_e	ω_e	ω_ex_e	ω_ey_e	B_e	α_e	γ_e	D_e	β_e	r_e	Trans.	ν₀₀
f₃ ³Δ₃	[83308.2] 6				[9.45] 8			[-1.₃E-4] 8		[1.34₉]	f₃ ← X R	81825.9 Z
f₃ ³Δ₃	↳missing citation
d₁ ³Π₁	[83255.6] 9				[9.76₈] 13			[8E-4] 13		[1.327]	d₁ ← X R	81773.3 Z
d₁ ³Π₁	↳missing citation
d₂ ³Π₂	[83083] 9				[8.63₂] 14			[-14E-4] 14		[1.412]	d₂ ← X R	81600.7 Z
d₂ ³Π₂	↳missing citation
C ¹Π	77575 15	[2684.0] Z	16		[9.33₃]	16				[1.358]	C ← X 17 R	77485.3 Z
C ¹Π	↳missing citation; Tilford, Ginter, et al., 1970
State	T_e	ω_e	ω_ex_e	ω_ey_e	B_e	α_e	γ_e	D_e	β_e	r_e	Trans.	ν₀₀
V ¹Σ⁺	77293.₀ 18	877.16 Z	16.04 19		2.727	-0.026		1.02E-4 19	0.2₀E-4	2.512	V ↔ X 20 R	76245.3 Z
V ¹Σ⁺	↳Jacques, 1959; Jacques and Barrow, 1959; missing citation
V ¹Σ⁺ 21											V → A
V ¹Σ⁺ 21	↳Jacques and Barrow, 1959
b₀ ³Π₀	(75617) 15	[2712]			[10.36] 22					[1.289]	b₀ ← X 23	75490.4 Z
b₀ ³Π₀	↳Price, 1938; missing citation
b₁ ³Π₁	(75195) 15	(2900)	(79)		[9.87] 22					[1.320]	b₁ ← X R	75142.₆ Z
b₁ ³Π₁	↳Price, 1938; missing citation
State	T_e	ω_e	ω_ex_e	ω_ey_e	B_e	α_e	γ_e	D_e	β_e	r_e	Trans.	ν₀₀
b₂ ³Π₂	[76322.₂] 15				[9.18] 22					[1.369]	b₂ ← X 23 R	74839.₉ Z
b₂ ³Π₂	↳Price, 1938; missing citation
A (¹Π) 24 25											A ← X
A (¹Π) 24 25	↳Datta and Banerjee, 1941; Romand, 1949
X ¹Σ⁺	0	2990.946₃ 26	52.8186 27	0.2243₇	10.59341₆ 26 28	0.30718₁ 29		5.3194E-4 28 30		1.27455₂ 31 32
	↳Rank, Eastman, et al., 1962; Rank, Rao, et al., 1965
	Rotation spectrum 33 34
	↳Hansler and Oetjen, 1953; Jones and Gordy, 1964; Rosenberg, Lightman, et al., 1972
	Raman cross sections
	↳Kaiser, 1970; de Leeuw and Dymanus, 1973
	Mol. beam electric reson. 35
	↳Kaiser, 1970; de Leeuw and Dymanus, 1973
	Mol. beam magnetic reson. 36
	↳Code, Khosla, et al., 1968

Notes

Rydberg series corresponding to excitation of a 2p electron.

v=0...5 observed. Assigned as 3pσ3pπ⁴ 5sσ. 39

Assigned as 3pσ3pπ⁴ 4pσ/π. 39

Many other absorption bands in the region 83000 - 93000 cm^-1 corresponding to Rydberg states strongly perturbed by the V ¹Σ⁺ state which itself gives rise to many perturbed bands.

Average B, D values; B(R,P)-B(Q) = +0.385.

Configuration ...σ²π³ 4pπ.

Average B, D values; B(1⁺)-B(1^-) = - 0.06₀.

Refers to Δ⁺; Q branch not resolved.

Configuration ...σ²π³ 4pσ.

Average B, D values; B(Π⁺)-B(Π^-) = +0.063.

Average B, D values; B(Π⁺)-B(Π^-) = -0.04₀.

Average B, D values; B(Δ⁺)-B(Δ^-) = -0.03₀.

Average B, D values; B(Π⁺)-B(Π^-) = -0.16₀.

Average B, D values; B(Π⁺)-B(Π^-) = -0.66₇.

Configuration σ²π³ 4sσ.

v=1,2,3 are increasingly diffuse; B₁ = 9.29₆. Tilford, Ginter, et al., 1970 give ω_e = 2817.5, ω_ex_e = 66.0, B_e = 9.44, α_e = 0.15.

A1so observed in inert matrices Boursey, 1975.

Typica1 "V" state with configuration ... σπ⁴ σ*.

missing note

Very extended progression in absorption, not yet analyzed in detail. The higher vibrational levels are strongly perturbed by Rydberg states Tilford and Ginter, 1971, Douglas and Greening, 1979. The vibrational and rotational constants given were obtained from the emission spectrum with v≤3 Jacques, 1959, Jacques and Barrow, 1959 but because of the perturbations have only very limited meaning.

Continuous absorption starting at 44000 cm^-1, maximum 40 at 65500 cm^-1.

Diffuse rotational structure; 1-0 and 2-0 are increasingly diffuse.

The b₂←X and b₀←X components have only 1/50 of the intensity of b₁←X.

Configuration ...σ²π³ σ*.

Continuous aabsorption starting at 44000 cm^-1, maximum at 65500 cm^-1.

Applying the Dunham corrections Rank, Rao, et al., 1965 obtain ω_e = 2991.0904 and B_e = 10.593553. Additional corrections (adiabatic, non- adiabatic) discussed by Bunker, 1972. Vibrational levels up to v=5 have been observed in infrared absorption Rank, Birtley, et al., 1960, Rank, Eastman, et al., 1962, Rank, Rao, et al., 1965 and emission Mould, Price, et al., 1960, higher levels in the V→X bands Jacques, 1959, Jacques and Barrow, 1959. Dunham potential coefficients Ogilvie and Koo, 1976. Most recent ab initio values of the ground state molecular constants Meyer and Rosmus, 1975; charge distribution Cade, Bader, et al., 1969.

ω_ez_e = -0.0121₈ Rank, Rao, et al., 1965.

Slightly different constants in Plyler and Tidwell, 1960, Levy, Rossi, et al., 1965, Levy, Rossi, et al., 1966. These papers and Webb and Rao, 1968 give also constants for H³⁷Cl.

+0.001772₄(v+1/2)² - 0.0001201(v+1/2)³.

-7.51₀E-6(v+1/2) + 4.0₀E-7(v+1/2)²; higher order terms in Rank, Rao, et al., 1965. See also Herman and Asgharian, 1966.

Uncorrected value from the B_e(=Y₀₁) given in the table. The internuclear distance at the minimum of the Born-Oppenheimer curve is r_e = 1.2746149 Bunker, 1972, Watson, 1973.

Rot.-vibr. Bands 41 34

Absolute intensity measurements Chamberlain and Gebbie, 1965, Sanderson, 1967.

Pressure-induced shifts (by foreign gases) of rotation-vibration and rotation lines Rank, Eastman, et al., 1960, Ben-Reuven, Kimel, et al., 1961, Gebbie and Stone, 1963, Jaffe, Friedmann, et al., 1963, Jaffe, Hirshfeld, et al., 1964. For discussions of pressure-induced bands and pure rotation lines (ΔJ=2) see Atwood, Vu, et al., 1967, Weiss and Cole, 1967. Self and foreign-gas line broadening Benedict, Herman, et al., 1956, Babrov, Ameer, et al., 1959, Goldring and Benesch, 1962, Jaffe, Kimel, et al., 1962, Plyler and Thibault, 1962, Alamichel and Legay, 1966, Levy, Mariel-Piollet, et al., 1970, Toth, Hunt, et al., 1970, Rich and Welsh, 1971, Rosenberg, Lightman, et al., 1972. Infrared absorption in liquid and solid phases Katz and Ron, 1970, Khatibi and Vu, 1972.

μ_el(v=0,1,2)= 1.1085, 1.1390, 1.1685 D, respectively Kaiser, 1970. Dipole moment function Kaiser, 1970, Smith, 1973; see also Bunker, 1973, Kaiser, 1974. g^J = 0.4594, also quadrupole and other hyperfine coupling constants Kaiser, 1970, de Leeuw and Dymanus, 1973; see also Tokuhiro, 1967, Bunker, 1973.

Proton spin - rotation interaction constant Leavitt, Baker, et al., 1961, Code, Khosla, et al., 1968.

From D₀⁰(H₂), D₀⁰(Cl₂), and ΔH^o_f0(HCl)

From the photoelectron spectrum Frost, McDowell, et al., 1967, Lempka, Passmore, et al., 1968, Weiss, Lawrence, et al., 1970; photoionization measurements give similar results Watanabe, Nakayama, et al., 1962, Nicholson, 1965. A somewhat smaller I.P.(12.73₀ eV) may be derived from the second band system in the photoelectron spectrum at 16.25₄ eV corresponding to A ²Σ⁺ of HCl⁺. Higher ionization potentials at 207.1 and 208.7 eV correspond to the removal of a 2p electron Hayes and Brown, 1972.

Strongly broadened by preionization (lifetime τ= 1.1E-14 s) Terwilliger and Smith, 1973.

Absorption coefficient k=40.

Absolute intensities (cm-2atm-1) of the 1-0 band: 130 Benedict, Herman, et al., 1956 2-0 band: 2.9 Benedict, Herman, et al., 1956 3.70 Jaffe, Kimel, et al., 1962, Toth, Hunt, et al., 1970 3-0 band: 0.023 Benedict, Herman, et al., 1956

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Levy, A.; Rossi, I.; Joffrin, C.; Van Thanh, N., Spectre de vibration-rotation de l'acide chlorhydrique gazeux. Etude de la bande v_0→2 a 1,7 micron, J. Chim. Phys. Phys.-Chim. Biol., 1965, 62, 600. [all data]

Levy, Rossi, et al., 1966
Levy, A.; Rossi, I.; Haeusler, C., Constantes de vibration-rotation de l'acide chlorhydrique gazeux etude des bandes v_o→2 et v_o→3, J. Phys. (Paris), 1966, 27, 526. [all data]

Webb and Rao, 1968
Webb, D.U.; Rao, K.N., Vibration rotation bands of heated hydrogen halides, J. Mol. Spectrosc., 1968, 28, 121. [all data]

Herman and Asgharian, 1966
Herman, R.M.; Asgharian, A., Finite nuclear mass effects on the centrifugal stretching constant in H³⁵Cl, J. Chem. Phys., 1966, 45, 2433. [all data]

Watson, 1973
Watson, J.K.G., The isotope dependence of the equilibrium rotational constants in ¹Σ states of diatomic molecules, J. Mol. Spectrosc., 1973, 45, 99. [all data]

Chamberlain and Gebbie, 1965
Chamberlain, J.E.; Gebbie, H.A., Sub-millimetre dispersion and rotational line strengths of the hydrogen halides, Nature (London), 1965, 208, 480. [all data]

Sanderson, 1967
Sanderson, R.B., Measurement of rotational line strengths in HCl by asymmetric Fourier transform techniques, Appl. Opt., 1967, 6, 1527. [all data]

Rank, Eastman, et al., 1960
Rank, D.H.; Eastman, D.P.; Birtley, W.B.; Wiggins, T.A., Perturbation of molecular rotation-vibration energy levels by rare gases, J. Chem. Phys., 1960, 33, 323. [all data]

Ben-Reuven, Kimel, et al., 1961
Ben-Reuven, A.; Kimel, S.; Hirshfeld, M.A.; Jaffe, J.H., Theory and measurement of pressure-induced shifts of HCl lines due to noble gases, J. Chem. Phys., 1961, 35, 955. [all data]

Gebbie and Stone, 1963
Gebbie, H.A.; Stone, N.W.B., Measurement of widths and shifts of pure rotation lines of hydrogen chloride perturbed by rare gases, Proc. Phys. Soc. London, 1963, 82, 309. [all data]

Jaffe, Friedmann, et al., 1963
Jaffe, J.H.; Friedmann, H.; Hirshfeld, M.A.; Ben-Reuven, A., Pressure-induced shifts of molecular lines in emission and in absorption, J. Chem. Phys., 1963, 39, 1447. [all data]

Jaffe, Hirshfeld, et al., 1964
Jaffe, J.H.; Hirshfeld, M.A.; Ben-Reuven, A., Pressure-induced shifts of DCl lines due to HCl: shift oscillation, J. Chem. Phys., 1964, 40, 1705. [all data]

Atwood, Vu, et al., 1967
Atwood, M.R.; Vu, H.; Vodar, B., Forme et structures fines de la bande induite par la pression dans la bande fondamentale de vibration-rotation des molecules HF, HCl et HBr, Spectrochim. Acta, 1967, 23, 553. [all data]

Weiss and Cole, 1967
Weiss, S.; Cole, R.H., Pressure-induced rotational quadrupole spectra of HCl and HBr, J. Chem. Phys., 1967, 46, 644. [all data]

Benedict, Herman, et al., 1956
Benedict, W.S.; Herman, R.; Moore, G.E.; Silverman, S., The strengths, widths, and shapes of infrared lines. II. The HCl fundamental, Can. J. Phys., 1956, 34, 850. [all data]

Babrov, Ameer, et al., 1959
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Goldring and Benesch, 1962
Goldring, H.; Benesch, W., Widths of HCl overtone lines at various temperatures, Can. J. Phys., 1962, 40, 1801. [all data]

Jaffe, Kimel, et al., 1962
Jaffe, J.H.; Kimel, S.; Hirshfeld, M.A., Refraction spectrum of gases in the infrared intensities and widths of lines in the 2-0 band of HCl, Can. J. Phys., 1962, 40, 113. [all data]

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Plyler, E.K.; Thibault, R.J., Foreign gas broadening of the lines of hydrogen chloride and carbon monoxide, J. Res. Nat. Bur. Stand. Sect. A, 1962, 66, 435. [all data]

Alamichel and Legay, 1966
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Toth, R.A.; Hunt, R.H.; Plyler, E.K., Line strengths, line widths, and dipole moment function for HCl, J. Mol. Spectrosc., 1970, 35, 110. [all data]

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Rich, N.H.; Welsh, H.L., Measurement of the pressure broadening of the rotational Raman lines of HCl, Chem. Phys. Lett., 1971, 11, 292. [all data]

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Smith, F.G., Dipole moment function and vibration-rotation matrix elements of HCl³⁵ and DCl³⁵, J. Quant. Spectrosc. Radiat. Transfer, 1973, 13, 717. [all data]

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Bunker, P.R., The breakdown of the Born-Oppenheimer approximation for a diatomic molecule: the dipole moment and nuclear quadrupole coupling constants, J. Mol. Spectrosc., 1973, 45, 151. [all data]

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Kaiser, E.W., Note: Comment to "Dipole moment function and vibration-rotation matrix elements of HCl³⁵ and DCl³⁵", J. Quant. Spectrosc. Radiat. Transfer, 1974, 14, 317. [all data]

Tokuhiro, 1967
Tokuhiro, T., Vibrational and rotational effects on the nuclear quadrupole coupling constants in hydrogen, deuterium, and tritium halides, J. Chem. Phys., 1967, 47, 109. [all data]

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Notes

Symbols used in this document:

AE	Appearance energy
IE (evaluated)	Recommended ionization energy
P_c	Critical pressure
P_triple	Triple point pressure
S°_{gas,1 bar}	Entropy of gas at standard conditions (1 bar)
T_c	Critical temperature
T_fus	Fusion (melting) point
d(ln(k_H))/d(1/T)	Temperature dependence parameter for Henry's Law constant
k°_H	Henry's Law constant at 298.15K
Δ_fH°_gas	Enthalpy of formation of gas at standard conditions
Δ_rG°	Free energy of reaction at standard conditions
Δ_rH°	Enthalpy of reaction at standard conditions
Δ_rS°	Entropy of reaction at standard conditions
Δ_subH	Enthalpy of sublimation
Δ_vapH	Enthalpy of vaporization

Data from NIST Standard Reference Database 69: NIST Chemistry WebBook
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NIST Chemistry WebBook, SRD 69

Hydrogen chloride

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Gas phase thermochemistry data

Gas Phase Heat Capacity (Shomate Equation)

Phase change data

Enthalpy of vaporization

Antoine Equation Parameters

Enthalpy of sublimation

Reaction thermochemistry data

Reactions 1 to 50

Henry's Law data

Henry's Law constant (water solution)

Gas phase ion energetics data

Ionization energy determinations

Appearance energy determinations

De-protonation reactions

IR Spectrum

Mass spectrum (electron ionization)

Spectrum

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Constants of diatomic molecules

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