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
Permanent link for this species. Use this link for bookmarking this species for future reference.
Information on this page:
Other data available:
- Phase change data
- Reaction thermochemistry data: reactions 51 to 100, reactions 101 to 150, reactions 151 to 158
- Gas phase ion energetics data
- Ion clustering data
- IR Spectrum
- Mass spectrum (electron ionization)
Data at other public NIST sites:
- Microwave spectra (on physics lab web site)
- Gas Phase Kinetics Database
Options:
- Switch to SI units

Data at NIST subscription sites:

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

NIST subscription sites provide data under the NIST Standard Reference Data Program, but require an annual fee to access. The purpose of the fee is to recover costs associated with the development of data collections included in such sites. Your institution may already be a subscriber. Follow the links above to find out more about the data in these sites and their terms of usage.

Gas phase thermochemistry data

Go To: Top, Reaction thermochemistry data, Henry's Law data, Constants of diatomic molecules, References, Notes

Quantity	Value	Units	Method	Reference	Comment
Δ_fH°_gas	-22.06 ± 0.024	kcal/mol	Review	Cox, Wagman, et al., 1984	CODATA Review value
Δ_fH°_gas	-22.06	kcal/mol	Review	Chase, 1998	Data last reviewed in September, 1964
Quantity	Value	Units	Method	Reference	Comment
S°_{gas,1 bar}	44.671 ± 0.001	cal/mol*K	Review	Cox, Wagman, et al., 1984	CODATA Review value
S°_{gas,1 bar}	44.670	cal/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 (cal/mol*K)
H° = standard enthalpy (kcal/mol)
S° = standard entropy (cal/mol*K)
t = temperature (K) / 1000.

View plot Requires a JavaScript / HTML 5 canvas capable browser.

View table.

Temperature (K)	298. to 1200.	1200. to 6000.
A	7.677802	7.628880
B	-3.216552	0.765579
C	4.748691	-0.129431
D	-1.638131	0.008586
E	-0.011872	-0.821827
F	-24.28791	-25.81621
G	54.65741	52.16941
H	-22.06310	-22.06310
Reference	Chase, 1998	Chase, 1998
Comment	Data last reviewed in September, 1964	Data last reviewed in September, 1964

Reaction thermochemistry data

Go To: Top, Gas phase thermochemistry data, Henry's Law data, 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°	29.6 ± 1.0	kcal/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°	23.8 ± 2.0	kcal/mol	TDEq	Caldwell and Kebarle, 1985	gas phase; B,M
Δ_rH°	23.1 ± 2.0	kcal/mol	IMRE	Larson and McMahon, 1984	gas phase; B,M
Δ_rH°	23.70 ± 0.20	kcal/mol	TDAs	Yamdagni and Kebarle, 1974	gas phase; B,M
Δ_rH°	20.4	kcal/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°	22.3	cal/mol*K	PHPMS	Caldwell and Kebarle, 1985	gas phase; switching reaction(Cl-)SO2; M
Δ_rS°	23.5	cal/mol*K	PHPMS	Yamdagni and Kebarle, 1974	gas phase; M
Δ_rS°	23.5	cal/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°	22.8	cal/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°	16.3 ± 2.0	kcal/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°	17.1 ± 2.6	kcal/mol	TDEq	Caldwell and Kebarle, 1985	gas phase; B
Δ_rG°	16.0 ± 2.0	kcal/mol	IMRE	Larson and McMahon, 1984	gas phase; B,M
Δ_rG°	16.70 ± 0.30	kcal/mol	TDAs	Yamdagni and Kebarle, 1974	gas phase; B
Δ_rG°	13.6	kcal/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°	333.40	kcal/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°	333.6 ± 2.1	kcal/mol	G+TS	Fujio, McIver, et al., 1981	gas phase; value altered from reference due to change in acidity scale; B
Δ_rH°	329.10	kcal/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°	328.10 ± 0.10	kcal/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°	328.3 ± 2.0	kcal/mol	IMRE	Fujio, McIver, et al., 1981	gas phase; value altered from reference due to change in acidity scale; B
Δ_rG°	323.70	kcal/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°	15.20 ± 0.20	kcal/mol	TDAs	Yamdagni and Kebarle, 1974	gas phase; B,M
Δ_rH°	14.0	kcal/mol	PHPMS	Caldwell and Kebarle, 1985	gas phase; switching reaction(Cl- HCl)SO2; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	20.4	cal/mol*K	PHPMS	Caldwell and Kebarle, 1985	gas phase; switching reaction(Cl- HCl)SO2; M
Δ_rS°	24.4	cal/mol*K	PHPMS	Yamdagni and Kebarle, 1974	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	7.90 ± 0.20	kcal/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°	14.8 ± 2.0	kcal/mol	TDAs	Caldwell and Kebarle, 1985	gas phase; B,M
Δ_rH°	14.2	kcal/mol	HPMS	Keesee, Lee, et al., 1980	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	20.0	cal/mol*K	PHPMS	Caldwell and Kebarle, 1985	gas phase; M
Δ_rS°	22.7	cal/mol*K	HPMS	Keesee, Lee, et al., 1980	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	8.8 ± 2.6	kcal/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°	15.7 ± 1.0	kcal/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°	15.1	cal/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°	11.2 ± 1.0	kcal/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°	12.3	kcal/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°	20.9	cal/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°	13.0	kcal/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°	21.7	cal/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°	22.4	kcal/mol	PHPMS	Caldwell and Kebarle, 1985	gas phase; From thermochemical cycle,switching reaction(Br-)SO2; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	18.6	cal/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°	19.6 ± 2.0	kcal/mol	TDEq	Caldwell and Kebarle, 1985	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	22.0	cal/mol*K	PHPMS	Caldwell and Kebarle, 1985	gas phase; switching reaction(Br-)SO2; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	13.0 ± 2.6	kcal/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°	11.70 ± 0.30	kcal/mol	TDAs	Yamdagni and Kebarle, 1974	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	23.4	cal/mol*K	PHPMS	Yamdagni and Kebarle, 1974	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	4.70 ± 0.30	kcal/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°	10.30 ± 0.70	kcal/mol	TDAs	Yamdagni and Kebarle, 1974	gas phase; B,M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	26.7	cal/mol*K	PHPMS	Yamdagni and Kebarle, 1974	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rG°	2.3 ± 1.0	kcal/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°	7.6	kcal/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°	15.2	cal/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°	10.5	kcal/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°	18.7	cal/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°	-22.58	kcal/mol	Cm	Devore and O'Neal, 1969	liquid phase; Heat of hydrolysis; ALS
Δ_rH°	-22.06	kcal/mol	Cm	Pritchard and Skinner, 1950	liquid phase; Heat of hydrolysis at 298 K, see Carson and Skinner, 1949; ALS
Δ_rH°	-22.09	kcal/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°	9.6	kcal/mol	HPMS	Upschulte, Evans, et al., 1986	gas phase; deuterated, quoted in 86 KEE/CAS; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	20.4	cal/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°	13.9	kcal/mol	PHPMS	Caldwell and Kebarle, 1985	gas phase; From thermochemical cycle; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	19.2	cal/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°	12.1 ± 1.0	kcal/mol	Cm	Buravtsev, Grigor'ev, et al., 1992	gas phase; ALS
Δ_rH°	19.6	kcal/mol	Eqk	Levanova, Bushneva, et al., 1979	liquid phase; ALS
Δ_rH°	16.3	kcal/mol	Eqk	Levanova, Bushneva, et al., 1979	gas phase; ALS
Δ_rH°	16.24	kcal/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°	12.5	kcal/mol	PHPMS	Caldwell and Kebarle, 1985	gas phase; switching reaction(Br-)SO2; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	18.4	cal/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°	22.0	kcal/mol	Eqk	Levanova, Bushneva, et al., 1979	liquid phase; ALS
Δ_rH°	17.1	kcal/mol	Eqk	Levanova, Bushneva, et al., 1979	gas phase; ALS
Δ_rH°	17.35 ± 0.50	kcal/mol	Eqk	Howlett, 1955	gas phase; ALS
Δ_rH°	17.1	kcal/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°	13.6	kcal/mol	Eqk	Levanova, Bushneva, et al., 1979	liquid phase; ALS
Δ_rH°	11.7	kcal/mol	Eqk	Levanova, Bushneva, et al., 1979	gas phase; ALS
Δ_rH°	13.61 ± 0.50	kcal/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°	-8.136 ± 0.050	kcal/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°	-24.35	kcal/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°	17.3 ± 0.2	kcal/mol	Eqk	Noren and Sunner, 1970	gas phase; ALS
Δ_rH°	17.62 ± 0.15	kcal/mol	Eqk	Kabo and Andreevskii, 1963	gas phase; At 415.5 K; ALS
Δ_rH°	17.45 ± 0.50	kcal/mol	Eqk	Howlett, 1955	gas phase; ALS

= + Hydrogen chloride

By formula: C₄H₉Cl = C₄H₈ + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	17.7 ± 0.5	kcal/mol	Eqk	Howlett, 1955	gas phase; ALS
Δ_rH°	17.70	kcal/mol	Eqk	Howlett, 1951	gas phase; Hf-gas-(390) -44.4 kcal/mol; ALS
Δ_rH°	17.1 ± 0.5	kcal/mol	Eqk	Kistiakowsky and Stauffer, 1937	gas phase; ALS

Hydrogen chloride + =

By formula: HCl + C₉H₁₀ = C₉H₁₁Cl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-8.80 ± 0.45	kcal/mol	Cm	Arnett and Pienta, 1980	liquid phase; solvent: Methylene chloride; Hydrochlorination; ALS
Δ_rH°	-12.4 ± 1.1	kcal/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°	16.0	kcal/mol	HPMS	Upschulte, Evans, et al., 1986	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	21.8	cal/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°	51.7	kcal/mol	PHPMS	McMahon, Heinis, et al., 1988	gas phase; switching reaction(CH3+)N2, Entropy change calculated or estimated, uses MCA(N2) = 48.3 kcal/mol; Foster, Williamson, et al., 1974; M

= + Hydrogen chloride

By formula: C₃H₆Cl₂ = C₃H₅Cl + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	15.6	kcal/mol	Eqk	Levanova, Rodova, et al., 1983	liquid phase; Flow reactor; ALS
Δ_rH°	14.3 ± 0.2	kcal/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°	-34.18 ± 0.23	kcal/mol	Chyd	Lacher, Amador, et al., 1967	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -35.32 ± 0.12 kcal/mol; At 250 C; ALS

2 + = + 2 Hydrogen chloride

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

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-30.24 ± 0.26	kcal/mol	Chyd	Lacher, Amador, et al., 1967	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -31.21 ± 0.13 kcal/mol; At 250 C; ALS

2 + = + 2 Hydrogen chloride

By formula: 2H₂ + CH₂Cl₂ = CH₄ + 2HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-39.05 ± 0.30	kcal/mol	Chyd	Lacher, Amador, et al., 1967	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -40.07 ± 0.30 kcal/mol; At 250 C; ALS

2 + = + 2 Hydrogen chloride

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

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-33.66 ± 0.25	kcal/mol	Chyd	Lacher, Amador, et al., 1967	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -34.65 ± 0.12 kcal/mol; At 250C; ALS

= + Hydrogen chloride

By formula: C₄H₈Cl₂ = C₄H₇Cl + HCl

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	-2.10 ± 0.02	kcal/mol	Eqk	Levanova, Rozhnov, et al., 1972	gas phase; At 568 K; ALS
Δ_rH°	13.20 ± 0.06	kcal/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°	-3.3 ± 0.02	kcal/mol	Eqk	Levanova, Rozhnov, et al., 1972	gas phase; At 568 K; ALS
Δ_rH°	1.2 ± 0.06	kcal/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°	-63.98 ± 0.50	kcal/mol	Chyd	Lacher, Kianpour, et al., 1956	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -64.92 kcal/mol; At 410 K; ALS

( • Hydrogen chloride ) + = ( • • )

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

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	12.3	kcal/mol	PHPMS	Caldwell and Kebarle, 1985	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	18.5	cal/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°	12.1	kcal/mol	PHPMS	Caldwell and Kebarle, 1985	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	18.6	cal/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°	16.5	kcal/mol	Eqk	Levanova, Rodova, et al., 1974	gas phase; ALS
Δ_rH°	15.90 ± 0.22	kcal/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°	16.30 ± 0.50	kcal/mol	Eqk	Failes and Stimson, 1967	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = 16.5 kcal/mol; At 450 K; ALS

= Hydrogen chloride +

By formula: C₂H₂Cl₄ = HCl + C₂HCl₃

Quantity	Value	Units	Method	Reference	Comment
Δ_rH°	10.5	kcal/mol	Eqk	Levanova, Bushneva, et al., 1979	gas phase; ALS
Δ_rH°	10.85	kcal/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°	10.8 ± 1.1	kcal/mol	Eqk	Levanova, Bushneva, et al., 1979	liquid phase; GC; ALS
Δ_rH°	9.3	kcal/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°	-63.34 ± 0.79	kcal/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°	16.2 ± 0.3	kcal/mol	Eqk	Meged, Levanova, et al., 1980	gas phase; ALS
Δ_rH°	16.3 ± 1.0	kcal/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°	60. ± 2.	kcal/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°	14.6	kcal/mol	Eqk	Levanova, Rodova, et al., 1974	gas phase; ALS
Δ_rH°	14.61 ± 0.09	kcal/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°	12.2	kcal/mol	FA	Perry, Rowe, et al., 1980	gas phase; M
Quantity	Value	Units	Method	Reference	Comment
Δ_rS°	20.4	cal/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°	17.8	kcal/mol	Eqk	Levanova, Bushneva, et al., 1979	liquid phase; ALS
Δ_rH°	14.8	kcal/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°	12.3	kcal/mol	Eqk	Levanova, Bushneva, et al., 1979	gas phase; ALS
Δ_rH°	15.6	kcal/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°	13.2	kcal/mol	Eqk	Levanova, Bushneva, et al., 1979	liquid phase; ALS
Δ_rH°	10.7	kcal/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°	-60.6 ± 1.1	kcal/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°	-9.50 ± 0.06	kcal/mol	Cm	Moselhy and Pritchard, 1975	liquid phase; solvent: Diphenyl-ether; Heat of hydrolysis; ALS

Henry's Law data

Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Constants of diatomic molecules, References, Notes

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.

Constants of diatomic molecules

Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Henry's Law data, References, Notes

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

References

Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Henry's Law data, Constants of diatomic molecules, Notes

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]

Metz, Kitsopoulos, et al., 1988
Metz, R.B.; Kitsopoulos, T.; Weaver, A.; Neumark, D.M., Study of the Transition State Region in the Cl+HCl Reaction by Photoelectron Spectroscopy of ClHCl-, J. Chem. Phys., 1988, 88, 2, 1463, https://doi.org/10.1063/1.454218 . [all data]

Caldwell and Kebarle, 1985
Caldwell, G.; Kebarle, P., The hydrogen bond energies of the bihalide ions XHX- and YHX-, Can. J. Chem., 1985, 63, 1399. [all data]

Larson and McMahon, 1984
Larson, J.W.; McMahon, T.B., Hydrogen bonding in gas phase anions. An experimental investigation of the interaction between chloride ion and bronsted acids from ICR chloride exchange equilibria, J. Am. Chem. Soc., 1984, 106, 517. [all data]

Yamdagni and Kebarle, 1974
Yamdagni, R.; Kebarle, P., The hydrogen bond energies in ClHCl- and Cl-(HCl)n, Can. J. Chem., 1974, 52, 2449. [all data]

Upschulte, Evans, et al., 1986
Upschulte, B.L.; Evans, D.H.; Keesee, R.G.; Castleman, A.W., Unpublished results, referred to in Keesee and Castleman, 1986, 1986. [all data]

Keesee and Castleman, 1980
Keesee, R.G.; Castleman, A.W., Jr., Gas phase studies of hydration complexes of Cl- and I- and comparison to electrostatic calculations in the gas phase, Chem. Phys. Lett., 1980, 74, 139. [all data]

Larson and McMahon, 1984, 2
Larson, J.W.; McMahon, T.B., Gas phase negative ion chemistry of alkylchloroformates, Can. J. Chem., 1984, 62, 675. [all data]

French, Ikuta, et al., 1982
French, M.A.; Ikuta, S.; Kebarle, P., Hydrogen bonding of O-H and C-H hydrogen donors to Cl^-. Results from mass spectrometric measurement of the ion-molecule equilibria RH + Cl^- = RHCl^-, Can. J. Chem., 1982, 60, 1907. [all data]

Larson and McMahon, 1987
Larson, J.W.; McMahon, T.B., Isotope Effects in Proton Transfer Reactions. An Ion Cyclotron Resonance Determination of the Equilibrium Deuterium Isotope Effect in the Bichloride Ion, J. Phys. Chem., 1987, 91, 3, 554, https://doi.org/10.1021/j100287a013 . [all data]

Larson and McMahon, 1984, 3
Larson, J.W.; McMahon, T.B., Fluoride and chloride affinities of main group oxides, fluorides, oxofluorides, and alkyls. Quantitative scales of lewis acidities from ion cyclotron resonance halide-exchange equilibria, J. Phys. Chem., 1984, 88, 1083. [all data]

Martin and Hepburn, 1998
Martin, J.D.D.; Hepburn, J.W., Determination of bond dissociation energies by threshold ion-pair production spectroscopy: An improved D-0(HCl), J. Chem. Phys., 1998, 109, 19, 8139-8142, https://doi.org/10.1063/1.477476 . [all data]

Fujio, McIver, et al., 1981
Fujio, M.; McIver, R.T., Jr.; Taft, R.W., Effects on the acidities of phenols from specific substituent-solvent interactions. Inherent substituent parameters from gas phase acidities, J. Am. Chem. Soc., 1981, 103, 4017. [all data]

Check, Faust, et al., 2001
Check, C.E.; Faust, T.O.; Bailey, J.M.; Wright, B.J.; Gilbert, T.M.; Sunderlin, L.S., Addition of Polarization and Diffuse Functions to the LANL2DZ Basis Set for P-Block Elements, J. Phys. Chem. A,, 2001, 105, 34, 8111, https://doi.org/10.1021/jp011945l . [all data]

Keesee, Lee, et al., 1980
Keesee, R.G.; Lee, N.; Castleman, A.W., Jr., Properties of clusters in the gas phase: V. Complexes of neutral molecules onto negative ions, J. Chem. Phys., 1980, 73, 2195. [all data]

Bohringer, Fahey, et al., 1984
Bohringer, H.; Fahey, D.W.; Fehsenfeld, F.C.; Ferguson, E.E., Bond energies of the molecules H₂O, SO₂, H₂O₂, and HCl to various atmospheric negative ions, J. Chem. Phys., 1984, 81, 2805. [all data]

Keesee 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]

Devore and O'Neal, 1969
Devore, J.A.; O'Neal, H.E., Heats of formation of the acetyl halides and of the acetyl radical, J. Phys. Chem., 1969, 73, 2644-2648. [all data]

Pritchard and Skinner, 1950
Pritchard, H.O.; Skinner, H.A., The heats of hydrolysis of the chloro-substituted acetyl chlorides, J. Chem. Soc., 1950, 272-276. [all data]

Carson and Skinner, 1949
Carson, A.S.; Skinner, H.A., 201. Carbon-halogen bond energies in the acetyl halides, J. Chem. Soc., 1949, 936-939. [all data]

Buravtsev, Grigor'ev, et al., 1992
Buravtsev, N.N.; Grigor'ev, A.S.; Zaidman, O.A.; Kolbanovskii, Yu.A.; Markelov, M.YU.; Sadogurskii, M.N.; Treger, Yu.A., Dehydrochlorination of chloroalkanes under rigid homogeneous conditions. II. Effect of small additions of oxygen to the kinetics of high-temperature decomposition of 1,2-dichloroethane under adiabatic compression, Khim. Fiz., 1992, 11, 218-226. [all data]

Levanova, Bushneva, et al., 1979
Levanova, s.V.; Bushneva, I.I.; Rodova, R.M.; Rozhnov, A.M.; Treger, Yu.A.; Aprelkin, A.S., Thermodynamic stability of chloroethanes in dehydrochlorination reactions, J. Appl. Chem. USSR, 1979, 52, 1439-1442. [all data]

Ghosh and Guha, 1951
Ghosh, J.C.; Guha, S.R.D., Catalytic dehydrochlorination of ethylene dichloride, Petroleum (London), 1951, 14, 261-264. [all data]

Howlett, 1955
Howlett, K.E., The use of equilibrium constants to calculate thermodynamic quantities. Part II, J. Chem. Soc., 1955, 1784-17. [all data]

Lane, Linnett, et al., 1953
Lane, M.R.; Linnett, J.W.; Oswin, H.G., A study of the C₂H₄+HCl=C₂H₅Cl and C2H4+Hbr=C2H5Br equilibria, Proc. Roy. Soc. London A, 1953, 216, 361-374. [all data]

Levanova, Treger, et al., 1975
Levanova, S.V.; Treger, Yu.A.; Velichko, S.M.; Rozhnov, A.M.; Bshneva, L.I.; Talanov, A.I., Equilibrium of the vinylidene chloride-methylchloroform system, Zh. Prikl. Khim. (Leningrad), 1975, 42, 480-481. [all data]

Moselhy and Pritchard, 1975
Moselhy, G.M.; Pritchard, H.O., The thermochemistry of the chloro-benzoyl chlorides, J. Chem. Thermodyn., 1975, 7, 977-982. [all data]

Carson, Pritchard, et al., 1950
Carson, A.S.; Pritchard, H.O.; Skinner, H.A., The heats of hydrolysis of the benzoyl halides, J. Chem. Soc., 1950, 656-659. [all data]

Davies, Dunning, et al., 1972
Davies, J.V.; Dunning, B.K.; Pritchard, H.O., The enthalpy of formation of benzoyl chloride, J. Chem. Thermodyn., 1972, 4, 731-737. [all data]

Noren and Sunner, 1970
Noren, I.; Sunner, S., The enthalpy of formation of 2-chloropropane from equilibrium studies, J. Chem. Thermodyn., 1970, 2, 597-602. [all data]

Kabo and Andreevskii, 1963
Kabo, G.Ya.; Andreevskii, D.N., Equilibrium of 2-chloropropane dehydrochlorination, Neftekhimiya, 1963, 3, 764-770. [all data]

Howlett, 1951
Howlett, K.E., The use of equilibrium constants to calculate thermodynamic quantities. Part I. Equilibria in the system tert.-butyl chloride, isobutene, hydrogen chloride, J. Chem. Soc., 1951, 1409-1412. [all data]

Kistiakowsky and Stauffer, 1937
Kistiakowsky, G.B.; Stauffer, C.H., The kinetics of gaseous addition of halogen acids to isobutene, 1937, 165-170. [all data]

Arnett and Pienta, 1980
Arnett, E.M.; Pienta, N.J., Stabilities of carbonium ions in solution. 12. Heats of formation of alkyl chlorides as an entree to heats of solvation of aliphatic carbonium ions, J. Am. Chem. Soc., 1980, 102, 3329-3334. [all data]

Nesterova, Kovzel, et al., 1977
Nesterova, T.N.; Kovzel, E.N.; Karaseva, S.Ya.; Rozhnov, A.M., Heats of reaction of the hydrohalogenation of styrene and α-methylstyrene, Vses. Konf. Kalorim. Rasshir. Tezisy Dokl. 7th, 1977, 1, 132. [all data]

McMahon, Heinis, et al., 1988
McMahon, T.; Heinis, T.; Nicol, G.; Hovey, J.K.; Kebarle, P., Methyl Cation Affinities, J. Am. Chem. Soc., 1988, 110, 23, 7591, https://doi.org/10.1021/ja00231a002 . [all data]

Foster, Williamson, et al., 1974
Foster, M.S.; Williamson, A.D.; Beauchamp, J.L., Photoionization mass spectrometry of trans-azomethane, Int. J. Mass Spectrom. Ion Phys., 1974, 15, 429. [all data]

Levanova, Rodova, et al., 1983
Levanova, S.V.; Rodova, R.M.; Tereshkina, T.P.; Zabrodina, T.I., Thermocatalytic reactions of bromochloropropanes, Russ. J. Phys. Chem. (Engl. Transl.), 1983, 57, 1142-1146. [all data]

Shevtsova, Rozhnov, et al., 1970
Shevtsova, L.A.; Rozhnov, A.M.; Andreevskii, D.N., Equilibrium Dehydrochlorination of 2,2-dichloropropane, Russ. J. Phys. Chem. (Engl. Transl.), 1970, 44, 852-855. [all data]

Lacher, Amador, et al., 1967
Lacher, J.R.; Amador, A.; Park, J.D., Reaction heats of organic compounds. Part 5.-Heats of hydrogenation of dichloromethane, 1,1- and 1,2-dichloroethane and 1,2-dichloropropane, Trans. Faraday Soc., 1967, 63, 1608-1611. [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]

Levanova, Rozhnov, et al., 1972
Levanova, S.V.; Rozhnov, A.M.; Bortnik, O.K., Isomerization of dibromoethylenes, Izv. Vyssh. Uchebn. Zaved., Khim. Khim. Tekhnol., 1972, 15, 1821-1823. [all data]

Lacher, Kianpour, et al., 1956
Lacher, J.R.; Kianpour, A.; Oetting, F.; Park, J.D., Reaction calorimetry. The hydrogenation of organic fluorides and chlorides, Trans. Faraday Soc., 1956, 52, 1500-1508. [all data]

Levanova, Rodova, et al., 1974
Levanova, S.V.; Rodova, R.M.; Rozhnov, A.M.; Shevtsova, L.A., Thermodynamic calculation of the equilibrium composition of chlorobutene mixtures, Russ. J. Phys. Chem. (Engl. Transl.), 1974, 48, 1113-1114. [all data]

Rodova, Levanova, et al., 1973
Rodova, R.M.; Levanova, S.V.; Shevtsova, L.A.; Rozhnov, A.M.; Porfir'eva, E.I., Reversible reactions of 2,3-dichlorobutane, Russ. J. Phys. Chem. (Engl. Transl.), 1973, 47, 607. [all data]

Failes and Stimson, 1967
Failes, R.L.; Stimson, V.R., The thermal decomposition of 1-ethoxyethyl chloride and the reverse combination, Aust. J. Chem., 1967, 20, 1553-1560. [all data]

Levanova, Bushneva, et al., 1976
Levanova, S.V.; Bushneva, L.I.; Rodova, R.M.; Rozhnov, A.M.; Treger, Yu.A., Liquid-phase dehydrochlorination of asymmetric tetrachloroethane, Zh. Fiz. Khim., 1976, 50, 2701-2702. [all data]

Shaulov and Shmyreva, 1968
Shaulov, Yu.Kh.; Shmyreva, G.O., Russ. J. Phys. Chem., 1968, 42, 1008. [all data]

Meged, Levanova, et al., 1980
Meged, V.M.; Levanova, S.V.; Rozhnov, A.M., Dehydrohalogenation of dihalomethylbutanes. 2., Izv. Vyssh. Uchebn. Zaved., Khim. Khim. Tekhnol., 1980, 23, 149-151. [all data]

Larson and McMahon, 1985
Larson, J.W.; McMahon, T.B., Fluoride and chloride affinities of the main group oxides, fluorides, oxofluorides, and alkyls. Quantitative scales of lewis acidities from ICR halide exchange equilibria, J. Am. Chem. Soc., 1985, 107, 766. [all data]

Rodova, Shevtsova, et al., 1974
Rodova, R.M.; Shevtsova, L.A.; Levanova, S.V.; Rozhnov, A.M.; Garkushin, I.K., Dehydrochlorination of 1,1-dichlorobutane and isomerization of chlorobutenes, Izv. Vyssh. Uchebn. Zaved., Khim. Khim. Tekhnol., 1974, 17, 379-381. [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]

Dias, Salema, et al., 1982
Dias, A.R.; Salema, M.S.; Martinho Simões, J.A., Organometallics, 1982, 1, 971. [all data]

Calhorda, Dias, et al., 1987
Calhorda, M.J.; Dias, A.R.; Minas da Piedade M.E.; Salema, M.S.; Martinho Simões J.A., Organometallics, 1987, 6, 734. [all data]

Hayes and Brown, 1972
Hayes, W.; Brown, F.C., Absorption by some molecular gases in the extreme ultraviolet, Phys. Rev. A: Gen. Phys., 1972, 6, 21. [all data]

Schwarz, 1975
Schwarz, W.H.E., Interpretation of the core electron excitation spectra of hydride molecules and the properties of hydride radicals, Chem. Phys., 1975, 11, 217. [all data]

Terwilliger and Smith, 1973
Terwilliger, D.T.; Smith, A.L., Analysis of autoionizing Rydberg states in the vacuum ultraviolet absorption spectrum of HCl and DCl, J. Mol. Spectrosc., 1973, 45, 366. [all data]

Douglas and Greening, 1979
Douglas; Greening, Unpublished cited in Huber and Herzberg, 1979, 1979, 287. [all data]

Tilford, Ginter, et al., 1970
Tilford, S.G.; Ginter, M.L.; Vanderslice, J.T., Electronic spectra and structure of the hydrogen halides. The b³Π_i and C¹Π states of HCl and DCl, J. Mol. Spectrosc., 1970, 33, 505. [all data]

Jacques, 1959
Jacques, D. Phil. Thesis, Oxford, 1959, 1. [all data]

Jacques and Barrow, 1959
Jacques, J.K.; Barrow, R.F., The transition v¹Σ⁺-x¹Σ⁺ in hydrogen chloride, Proc. Phys. Soc. London, 1959, 73, 538. [all data]

Price, 1938
Price, W.C., The absorption spectra of the halogen acids in the vacuum ultra-violet, Proc. Roy. Soc. (London), 1938, A167, 216. [all data]

Datta and Banerjee, 1941
Datta, S.; Banerjee, S., The continuous absorption spectra of the hydrogen-halides. Part II. HCl, Proc. Natl. Inst. Sci. India, 1941, 7, 305. [all data]

Romand, 1949
Romand, J., Absorption ultraviolette dans la region de Schumann etude de: ClH, BrH et lH gazeux, Ann. Phys. (Paris), 1949, 4, 527. [all data]

Rank, Eastman, et al., 1962
Rank, D.H.; Eastman, D.P.; Rao, B.S.; Wiggins, T.A., Rotational and vibrational constants of the HCl³⁵ and DCl³⁵ molecules, J. Opt. Soc. Am., 1962, 52, 1. [all data]

Rank, Rao, et al., 1965
Rank, D.H.; Rao, B.S.; Wiggins, T.A., Molecular constants of HCl³⁵, J. Mol. Spectrosc., 1965, 17, 122. [all data]

Hansler and Oetjen, 1953
Hansler, R.L.; Oetjen, R.A., The infrared spectra of HCl, DCl, HBr, and NH₃ in the region from 40 to 140 microns, J. Chem. Phys., 1953, 21, 1340. [all data]

Jones and Gordy, 1964
Jones, G.; Gordy, W., Extension of submillimeter wave spectroscopy below a half-millimeter wavelength, Phys. Rev., 1964, 135, 295. [all data]

Rosenberg, Lightman, et al., 1972
Rosenberg, A.; Lightman, A.; Ben-Reuven, A., Interferometric measurements of the pure rotational spectra of HCl and DCl, J. Quant. Spectrosc. Radiat. Transfer, 1972, 12, 219. [all data]

Kaiser, 1970
Kaiser, E.W., Dipole moment and hyperfine parameters of H³⁵Cl and D³⁵Cl, J. Chem. Phys., 1970, 53, 1686. [all data]

de Leeuw and Dymanus, 1973
de Leeuw, F.H.; Dymanus, A., Magnetic properties and molecular quadrupole moment of HF and HCl by molecular-beam electric-resonance spectroscopy, J. Mol. Spectrosc., 1973, 48, 427. [all data]

Code, Khosla, et al., 1968
Code, R.F.; Khosla, A.; Ozier, I.; Ramsey, N.F.; Yi, P.N., Nuclear magnetic hyperfine spectra of H³⁵Cl and H³⁷Cl, J. Chem. Phys., 1968, 49, 1895. [all data]

Boursey, 1975
Boursey, E., Electronic excitation of HCl trapped in inert matrices, J. Chem. Phys., 1975, 62, 3353. [all data]

Tilford and Ginter, 1971
Tilford, S.G.; Ginter, M.L., Electronic spectra and structure of the hydrogen halides: states associated with the (σ²π³) cπ and (σ²π³) cσ configurations of HCl and DCl, J. Mol. Spectrosc., 1971, 40, 568. [all data]

Bunker, 1972
Bunker, P.R., On the breakdown of the Born-Oppenheimer approximation for a diatomic molecule, J. Mol. Spectrosc., 1972, 5, 478. [all data]

Rank, Birtley, et al., 1960
Rank, D.H.; Birtley, W.B.; Eastman, D.P.; Rao, B.S.; Wiggins, T.A., Precise measurements of some infrared bands of hydrogen chloride, J. Opt. Soc. Am., 1960, 50, 1275. [all data]

Mould, Price, et al., 1960
Mould, H.M.; Price, W.C.; Wilkinson, G.R., Infra-red emission from gases excited by a radio-frequency discharge, Spectrochim. Acta, 1960, 16, 479. [all data]

Ogilvie and Koo, 1976
Ogilvie, J.F.; Koo, D., Dunham potential energy coefficients of the hydrogen halides and carbon monoxide, J. Mol. Spectrosc., 1976, 61, 332-336. [all data]

Meyer and Rosmus, 1975
Meyer, W.; Rosmus, P., PNO-Cl and CEPA studies of electron correlation effects. III. Spectroscopic constants and dipole moment functions for the ground states of the first-row and second-row diatomic hydrides, J. Chem. Phys., 1975, 63, 2356. [all data]

Cade, Bader, et al., 1969
Cade, P.E.; Bader, R.F.W.; Henneker, W.H.; Keaveny, I., Molecular charge distributions and chemical binding. IV. The second-row diatomic hydrides AH, J. Chem. Phys., 1969, 50, 5313. [all data]

Plyler and Tidwell, 1960
Plyler, E.K.; Tidwell, E.D., The rotational constants of hydrogen chloride, Z. Elektrochem., 1960, 64, 717. [all data]

Levy, Rossi, et al., 1965
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
Babrov, H.; Ameer, G.; Benesch, W., Line strengths and widths in the HCl fundamental band, J. Mol. Spectrosc., 1959, 3, 185. [all data]

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]

Plyler and Thibault, 1962
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
Alamichel, C.; Legay, F., Etude de la dispersion dans le doublet isotopique R2 de la premiere bande harmonique de vibration-rotation de HCl, J. Phys. (Paris), 1966, 27, 233. [all data]

Levy, Mariel-Piollet, et al., 1970
Levy, A.; Mariel-Piollet, E.; Bouanich, J.-P.; Haeusler, C., Spectre de vibration-rotation du gaz chlorhydrique comprime. Intensites et largeurs de raies dans la bande v_0-2, J. Quant. Spectrosc. Radiat. Transfer, 1970, 10, 203. [all data]

Toth, Hunt, et al., 1970
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]

Rich and Welsh, 1971
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]

Katz and Ron, 1970
Katz, B.; Ron, A., Far infrared spectra of HCl and DCl in a nitrogen matrix, Chem. Phys. Lett., 1970, 7, 357. [all data]

Khatibi and Vu, 1972
Khatibi, P.; Vu, H., Spectres d'absorption infrarouge de HCl et de HBr en phases denses. I. Spectres dans le fondamental de vibration-rotation, J. Chim. Phys. Phys.-Chim. Biol., 1972, 69, 654. [all data]

Smith, 1973
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]

Bunker, 1973
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]

Kaiser, 1974
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]

Leavitt, Baker, et al., 1961
Leavitt, J.A.; Baker, M.R.; Nelson, H.M.; Ramsey, N.F., Proton radio-frequency spectrum of HCl³⁵, Phys. Rev., 1961, 124, 1482. [all data]

Frost, McDowell, et al., 1967
Frost, D.C.; McDowell, C.A.; Vroom, D.A., Photoelectron spectra of the halogens and the hydrogen halides, J. Chem. Phys., 1967, 46, 4255. [all data]

Lempka, Passmore, et al., 1968
Lempka, H.J.; Passmore, T.R.; Price, W.C., The photoelectron spectra and ionized states of the halogen acids, Proc. Roy. Soc. (London), 1968, A304, 53. [all data]

Weiss, Lawrence, et al., 1970
Weiss, M.J.; Lawrence, G.M.; Young, R.A., Photoelectron spectroscopy of HCI and DCI using molecular beams, J. Chem. Phys., 1970, 52, 2867. [all data]

Watanabe, Nakayama, et al., 1962
Watanabe, K.; Nakayama, T.; Mottl, J., Ionization potentials of some molecules, J. Quant. Spectry. Radiative Transfer, 1962, 2, 369. [all data]

Nicholson, 1965
Nicholson, A.J.C., Photoionization-efficiency curves. II. False and genuine structure, J. Chem. Phys., 1965, 43, 1171. [all data]

Huber and Herzberg, 1979
Huber, K.P.; Herzberg, G., Molecular Spectra and Molecular Structure. IV. Constants of Diatomic Molecules, Van Nostrand Reinhold Company, New York, 1979, 716. [all data]

Notes

Go To: Top, Gas phase thermochemistry data, Reaction thermochemistry data, Henry's Law data, Constants of diatomic molecules, References

Symbols used in this document:

S°_{gas,1 bar}	Entropy of gas at standard conditions (1 bar)
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

Data from NIST Standard Reference Database 69: NIST Chemistry WebBook
The National Institute of Standards and Technology (NIST) uses its best efforts to deliver a high quality copy of the Database and to verify that the data contained therein have been selected on the basis of sound scientific judgment. However, NIST makes no warranties to that effect, and NIST shall not be liable for any damage that may result from errors or omissions in the Database.
Customer support for NIST Standard Reference Data products.