Bromine - The NIST WebBook

Bromine

• Formula: Br2
• Molecular weight: 159.808
• IUPAC Standard InChI: InChI=1S/Br2/c1-2 Copy
• IUPAC Standard InChIKey: GDTBXPJZTBHREO-UHFFFAOYSA-N Copy
• CAS Registry Number: 7726-95-6
• Chemical structure: This structure is also available as a 2d Mol file or as a computed 3d SD file View 3d structure (requires JavaScript / HTML 5)
• Other names: Br2; Brom; Brome; Bromo; Broom; UN 1744; Dibromine
• Permanent link for this species. Use this link for bookmarking this species for future reference.
• Information on this page:
  • Reaction thermochemistry data (reactions 1 to 50)
  • References
  • Notes
• Other data available:
  • Gas phase thermochemistry data
  • Condensed phase thermochemistry data
  • Phase change data
  • Reaction thermochemistry data: reactions 51 to 55
  • Gas phase ion energetics data
  • Ion clustering data
  • Mass spectrum (electron ionization)
  • Constants of diatomic molecules
• Data at other public NIST sites:
  • Gas Phase Kinetics Database
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Reaction thermochemistry data

Go To: Top, References, Notes

Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Data compiled as indicated in comments: MS - José A. Martinho Simões B - John E. Bartmess ALS - Hussein Y. Afeefy, Joel F. Liebman, and Stephen E. Stein

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

Reactions 1 to 50

C8H6MoO3 (cr) + (solution) = (solution) + (cr)

By formula: C8H6MoO3 (cr) + Br2 (solution) = HBr (solution) + C8H5BrMoO3 (cr)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-150. ± 12.	kJ/mol	N/A	Nolan, López de la Vega, et al., 1986	solvent: Carbon tetrachloride; The reaction enthalpy was calculated Nolan, López de la Vega, et al., 1986 from the experimental values for the enthalpies of the following reactions: Mo(Cp)(CO)3(H)(cr) + 2Br2(solution) = Mo(Cp)(CO)2(Br)3(solution) + HBr(solution) + CO(solution), -254.0 ± 8.4 kJ/mol, and Mo(Cp)(CO)3(Br)(cr) + Br2(solution) = Mo(Cp)(CO)2(Br)3(solution) + CO(solution), -104.2 ± 8.4 kJ/mol; MS

C16H10Mo2O6 (cr) + (solution) = 2 (cr)

By formula: C16H10Mo2O6 (cr) + Br2 (solution) = 2C8H5BrMoO3 (cr)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-177. ± 17.	kJ/mol	N/A	Nolan, López de la Vega, et al., 1986	solvent: Carbon tetrachloride; The reaction enthalpy was calculated Nolan, López de la Vega, et al., 1986 from the experimental values for the enthalpies of the following reactions: [Mo(Cp)(CO)3]2(cr) + 3Br2(solution) = 2Mo(Cp)(CO)2(Br)3(solution) + 2CO(solution), -384.9 ± 4.2 kJ/mol, and Mo(Cp)(CO)3(Br)(cr) + Br2(solution) = Mo(Cp)(CO)2(Br)3(solution) + CO(solution), -104.2 ± 8.4 kJ/mol; MS

+ = ( • )

By formula: Br- + Br2 = (Br- • Br2)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	127. ± 7.1	kJ/mol	CIDT	Nizzi, Pommerening, et al., 1998	gas phase; B
ΔrH°	141.0	kJ/mol	N/A	Check, Faust, et al., 2001	gas phase; Fe-; ; ΔS(EA)=5.8; B
Quantity	Value	Units	Method	Reference	Comment
ΔrG°	94.14	kJ/mol	N/A	Check, Faust, et al., 2001	gas phase; Fe-; ; ΔS(EA)=5.8; B

+ =

By formula: C4H8 + Br2 = C4H8Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-120.9	kJ/mol	Cm	Lister, 1941	gas phase; Heat of bromination at 300 K; ALS
ΔrH°	-123.2 ± 0.84	kJ/mol	Cm	Conn, Kistiakowsky, et al., 1938	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -123.8 ± 0.84 kJ/mol; At 355 °K; ALS

+ =

By formula: C4H8 + Br2 = C4H8Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-121.1 ± 0.84	kJ/mol	Cm	Conn, Kistiakowsky, et al., 1938	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -121.7 ± 0.84 kJ/mol; At 355 °K; ALS

+ =

By formula: C2H4 + Br2 = C2H4Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-120.9 ± 1.3	kJ/mol	Cm	Conn, Kistiakowsky, et al., 1938	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -121.6 ± 1.3 kJ/mol; At 355 °K; ALS

+ =

By formula: C3H6 + Br2 = C3H6Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-122.5 ± 0.84	kJ/mol	Cm	Conn, Kistiakowsky, et al., 1938	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = -123.1 ± 0.84 kJ/mol; At 355 °K; ALS

+ = +

By formula: HBr + C7H7Br = C7H8 + Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	33.9 ± 4.2	kJ/mol	Eqk	Benson and Buss, 1957	gas phase; Reanalyzed by Cox and Pilcher, 1970, Original value = 33. ± 4. kJ/mol; ALS

= +

By formula: CBr2O = CO + Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	33.9 ± 0.42	kJ/mol	Eqk	Dunning and Pritchard, 1972	gas phase; ALS
ΔrH°	4.3 ± 0.4	kJ/mol	Eqk	Schumacher and Bergmann, 1931	gas phase; ALS

(l) + 3 (l) = Br3In (cr) + 3 (g)

By formula: C3H9In (l) + 3Br2 (l) = Br3In (cr) + 3CH3Br (g)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-665.3 ± 4.2	kJ/mol	RSC	Clarke and Price, 1968	Please also see Pedley and Rylance, 1977 and Cox and Pilcher, 1970, 2.; MS

(l) + 2 (l) = 2 (g) + (cr)

By formula: C2H6Hg (l) + 2Br2 (l) = 2CH3Br (g) + Br2Hg (cr)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-302.1 ± 2.5	kJ/mol	RSC	Hartley, Pritchard, et al., 1950	Please also see Pedley and Rylance, 1977 and Cox and Pilcher, 1970, 2.; MS

(l) + (g) = (l) + C3H9BrSn (l)

By formula: C10H16Sn (l) + Br2 (g) = C7H7Br (l) + C3H9BrSn (l)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-226.6 ± 0.9	kJ/mol	RSC	Pedley and Skinner, 1959	Please also see Pedley and Rylance, 1977 and Cox and Pilcher, 1970, 2.; MS

(l) + (g) = C3H9BrSn (l) + (g)

By formula: C4H12Sn (l) + Br2 (g) = C3H9BrSn (l) + CH3Br (g)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-202.1 ± 2.9	kJ/mol	RSC	Pedley, Skinner, et al., 1957	Please also see Pedley and Rylance, 1977 and Cox and Pilcher, 1970, 2.; MS

C8H6MoO3 (cr) + 2 (solution) = C7H5Br3MoO2 (solution) + (solution) + (solution)

By formula: C8H6MoO3 (cr) + 2Br2 (solution) = C7H5Br3MoO2 (solution) + HBr (solution) + CO (solution)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-254.0 ± 8.4	kJ/mol	RSC	Nolan, López de la Vega, et al., 1986	solvent: Carbon tetrachloride; MS

+ = +

By formula: C3H4O4 + Br2 = HBr + C3H3BrO4

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-66.0 ± 2.9	kJ/mol	Cm	Koros, Orban, et al., 1979	liquid phase; solvent: Sulfuric acid (1M); Bromination; ALS

(l) + (l) = 2C3H9BrSn (l)

By formula: C6H18Sn2 (l) + Br2 (l) = 2C3H9BrSn (l)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-293.9 ± 2.1	kJ/mol	RSC	Pedley, Skinner, et al., 1957	Please also see Pedley and Rylance, 1977 and Cox and Pilcher, 1970, 2.; MS

C16H10Mo2O6 (cr) + 3 (solution) = 2C7H5Br3MoO2 (solution) + 2 (solution)

By formula: C16H10Mo2O6 (cr) + 3Br2 (solution) = 2C7H5Br3MoO2 (solution) + 2CO (solution)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-384.9 ± 4.2	kJ/mol	RSC	Nolan, López de la Vega, et al., 1986	solvent: Carbon tetrachloride; MS

+ = +

By formula: HBr + C3H5BrO = C3H6O + Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	31.1 ± 8.4	kJ/mol	Eqk	King, Golden, et al., 1971	gas phase; Heat of bromination at 516-618 K; ALS

(cr) + (solution) = C7H5Br3MoO2 (solution) + (solution)

By formula: C8H5BrMoO3 (cr) + Br2 (solution) = C7H5Br3MoO2 (solution) + CO (solution)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-104.2 ± 8.4	kJ/mol	RSC	Nolan, López de la Vega, et al., 1986	solvent: Carbon tetrachloride; MS

C12H7MnO5 (cr) + 1.5 (g) = (g) + (cr) + 5 (g)

By formula: C12H7MnO5 (cr) + 1.5Br2 (g) = C7H7Br (g) + Br2Mn (cr) + 5CO (g)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-194.5 ± 7.8	kJ/mol	HAL-HFC	Connor, Zafarani-Moattar, et al., 1982	MS

+ =

By formula: Br2 + C8H14 = C8H14Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-122.63	kJ/mol	Cm	Lister, 1941	gas phase; Heat of bromination at 300 K; ALS

C6F3MnO5 (cr) + 1.5 (g) = (cr) + 5 (g) + (g)

By formula: C6F3MnO5 (cr) + 1.5Br2 (g) = Br2Mn (cr) + 5CO (g) + CBrF3 (g)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-173. ± 3.	kJ/mol	HAL-HFC	Connor, Zafarani-Moattar, et al., 1982	MS

C7F3MnO6 (cr) + 1.5 (g) = (cr) + 6 (g) + (g)

By formula: C7F3MnO6 (cr) + 1.5Br2 (g) = Br2Mn (cr) + 6CO (g) + CBrF3 (g)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-161. ± 2.	kJ/mol	HAL-HFC	Connor, Zafarani-Moattar, et al., 1982	MS

+ =

By formula: C6H10 + Br2 = C6H10Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-140.71	kJ/mol	Cm	Lister, 1941	gas phase; Heat of bromination at 300 K; ALS

+ =

By formula: C7H12 + Br2 = C7H12Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-127.4	kJ/mol	Cm	Lister, 1941	gas phase; Heat of bromination at 300 K; ALS

+ = C7H14Br2

By formula: C7H14 + Br2 = C7H14Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-126.5	kJ/mol	Cm	Lister, 1941	gas phase; Heat of bromination at 300 K; ALS

+ =

By formula: C5H8 + Br2 = C5H8Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-119.7 ± 2.5	kJ/mol	Cm	Lister, 1941	gas phase; Halogenation at 27 C; ALS

(cr) + 1.5 (g) = (cr) + 5 (g) + (g)

By formula: C6H3MnO5 (cr) + 1.5Br2 (g) = Br2Mn (cr) + 5CO (g) + CH3Br (g)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-209. ± 3.	kJ/mol	HAL-HFC	Connor, Zafarani-Moattar, et al., 1982	MS

(cr) + 1.5 (g) = (cr) + 6 (g) + (g)

By formula: C7H3MnO6 (cr) + 1.5Br2 (g) = Br2Mn (cr) + 6CO (g) + CH3Br (g)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-161. ± 5.	kJ/mol	HAL-HFC	Connor, Zafarani-Moattar, et al., 1982	MS

+ 0.5 = + 0.5

By formula: C7H7Br + 0.5H2 = C7H8 + 0.5Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-4. ± 2.	kJ/mol	Chyd	Ashcroft, Carson, et al., 1963	liquid phase; ALS

C10H22Mg (cr) + (g) + (l) = 2 (l) + Br2Mg (cr)

By formula: C10H22Mg (cr) + H2 (g) + Br2 (l) = 2C5H12 (l) + Br2Mg (cr)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-669.6 ± 6.6	kJ/mol	RSC	Akkerman, Schat, et al., 1983	MS

+ =

By formula: C2F4 + Br2 = C2Br2F4

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-161.0	kJ/mol	Cm	Lacher, Casali, et al., 1956	gas phase; Heat of bromination; ALS

2 + = + 2

By formula: 2C6H5Br + Br2Hg = C12H10Hg + 2Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	328.6 ± 3.3	kJ/mol	Cm	Chernick, Skinner, et al., 1956	liquid phase; ALS

(cr) + 2 (g) = 2 (cr) + 10 (g)

By formula: C10Mn2O10 (cr) + 2Br2 (g) = 2Br2Mn (cr) + 10CO (g)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-263.6 ± 8.2	kJ/mol	HAL-HFC	Connor, Zafarani-Moattar, et al., 1982	MS

+ 2 = 2 +

By formula: H2 + 2CH3Br = 2CH4 + Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-28. ± 3.	kJ/mol	Chyd	Adams, Carson, et al., 1966	liquid phase; ALS

+ =

By formula: C4H8 + Br2 = C4H8Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-126.3 ± 0.84	kJ/mol	Cm	Conn, Kistiakowsky, et al., 1938	gas phase; At 355 °K; ALS

+ =

By formula: C5H10 + Br2 = C5H10Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-127.2 ± 0.84	kJ/mol	Cm	Conn, Kistiakowsky, et al., 1938	gas phase; At 355 °K; ALS

+ = +

By formula: C5H6O4 + Br2 = C5H6O4 + Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-5.1 ± 0.7	kJ/mol	Eqk	Jwo, Huang, et al., 1987	solid phase; HPLC; ALS

+ =

By formula: Br2 + C2ClF3 = C2Br2ClF3

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-132.3	kJ/mol	Cm	Lacher, Casali, et al., 1956	gas phase; Heat of bromination; ALS

Br3- + = (Br3- • )

By formula: Br3- + Br2 = (Br3- • Br2)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	38. ± 7.1	kJ/mol	CIDT	Nizzi, Pommerening, et al., 1998	gas phase; B

(cr) + 0.5 (g) = (cr) + 5 (g)

By formula: C5BrMnO5 (cr) + 0.5Br2 (g) = Br2Mn (cr) + 5CO (g)

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	9.9 ± 1.8	kJ/mol	HAL-HFC	Connor, Zafarani-Moattar, et al., 1982	MS

+ 2 = 2 +

By formula: H2 + 2C2H5Br = 2C2H6 + Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	23. ± 13.	kJ/mol	Chyd	Ashcroft, Carson, et al., 1965	liquid phase; ALS

+ = +

By formula: CHCl3 + Br2 = HBr + CBrCl3

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-5.9 ± 0.4	kJ/mol	Eqk	Mendenhall, Golden, et al., 1973	gas phase; ALS

+ = +

By formula: CH2F2 + Br2 = HBr + CHBrF2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-39.9 ± 0.3	kJ/mol	Eqk	Okafo and Whittle, 1974	gas phase; ALS

+ = +

By formula: CCl4 + Br2 = BrCl + CBrCl3

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	37. ± 1.	kJ/mol	Eqk	Mendenhall, Golden, et al., 1973	gas phase; ALS

+ = +

By formula: CHF3 + Br2 = HBr + CBrF3

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-14.	kJ/mol	Eqk	Corbett, Tarr, et al., 1963	gas phase; At 298 K; ALS

+ = +

By formula: CHBr3 + Br2 = HBr + CBr4

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-7. ± 3.	kJ/mol	Eqk	King, Golden, et al., 1971, 2	gas phase; ALS

+ = +

By formula: HBr + CBrF3 = CHF3 + Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	19.2 ± 1.0	kJ/mol	Eqk	Coomber and Whittle, 1967	gas phase; ALS

+ = +

By formula: CH4 + Br2 = HBr + CH3Br

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	-26.4 ± 0.7	kJ/mol	Eqk	Ferguson, Okafo, et al., 1973	gas phase; ALS

= +

By formula: C4H8Br2 = C4H8 + Br2

Quantity	Value	Units	Method	Reference	Comment
ΔrH°	139.7 ± 0.46	kJ/mol	Cm	Sunner and Wulff, 1974	liquid phase; ALS

References

Go To: Top, Reaction thermochemistry data, Notes

Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Nolan, López de la Vega, et al., 1986 Nolan, S.P.; López de la Vega, R.; Hoff, C.D., J. Organometal. Chem., 1986, 315, 187. [all data]

Nizzi, Pommerening, et al., 1998 Nizzi, K.E.; Pommerening, C.A.; Sunderlin, L.S., Gas-phase thermochemistry of polyhalide anions, J. Phys. Chem. A, 1998, 102, 39, 7674-7679, https://doi.org/10.1021/jp9824508 . [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]

Lister, 1941 Lister, M.W., Heats of organic reactions. X. Heats of bromination of cyclic olefins, J. Am. Chem. Soc., 1941, 63, 143-149. [all data]

Conn, Kistiakowsky, et al., 1938 Conn, J.B.; Kistiakowsky, G.B.; Smith, E.A., Heats of organic reactions. VII. Addition of halogens to olefins, J. Am. Chem. Soc., 1938, 60, 2764-2771. [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]

Benson and Buss, 1957 Benson, S.W.; Buss, J.H., The thermodynamics of bromination of toluene and the heat of formation of the benzyl radical, J. Phys. Chem., 1957, 61, 104-109. [all data]

Dunning and Pritchard, 1972 Dunning, B.K.; Pritchard, H.O., The enthalpy of formation of bromophosgene, J. Chem. Thermodyn., 1972, 4, 213-218. [all data]

Schumacher and Bergmann, 1931 Schumacher, H.-J.; Bergmann, P., Die kinetik und photochemie des bromphosgens, Z. Phys. Chem., 1931, 13, 269-284. [all data]

Clarke and Price, 1968 Clarke, W.D.; Price, S.J.W., Can. J. Chem., 1968, 46, 1633. [all data]

Pedley and Rylance, 1977 Pedley, J.B.; Rylance, J., Computer Analysed Thermochemical Data: Organic and Organometallic Compounds, University of Sussex, Brigton, 1977. [all data]

Cox and Pilcher, 1970, 2 Cox, J.D.; Pilcher, G., Thermochemistry of Organic and Organometallic Compounds in Academic Press, New York, 1970. [all data]

Hartley, Pritchard, et al., 1950 Hartley, K.; Pritchard, H.O.; Skinner, H.A., Thermochemistry of metallic alkyls. III.?mercury dimethyl and mercury methyl halides, Trans. Faraday Soc., 1950, 46, 1019, https://doi.org/10.1039/tf9504601019 . [all data]

Pedley and Skinner, 1959 Pedley, J.B.; Skinner, H.A., Thermochemistry of metallic alkyls. Part 9.?Heats of bromination of some organo-tin compounds, Trans. Faraday Soc., 1959, 55, 544, https://doi.org/10.1039/tf9595500544 . [all data]

Pedley, Skinner, et al., 1957 Pedley, J.B.; Skinner, H.A.; Chernick, C.L., Thermochemistry of metallic alkyls. Part 8.?Tin tetramethyl, and hexamethyl distannane, Trans. Faraday Soc., 1957, 53, 1612, https://doi.org/10.1039/tf9575301612 . [all data]

Koros, Orban, et al., 1979 Koros, E.; Orban, M.; Nagy, Z., Calorimetric studies on the Belousov-Zhabotinsky oscillatory chemical reaction, Acta Chim. Acad. Sci. Hung., 1979, 100, 449-461. [all data]

King, Golden, et al., 1971 King, K.D.; Golden, D.M.; Benson, S.W., Thermochemistry of the gas-phase equilibrium CH3COCH3 + Br2 = CH3COCH2Br + HBr. The enthalpy of formation of bromoacetone, J. Chem. Thermodyn., 1971, 3, 129-134. [all data]

Connor, Zafarani-Moattar, et al., 1982 Connor, J.A.; Zafarani-Moattar, M.T.; Bickerton, J.; El-Saied, N.I.; Suradi, S.; Carson, R.; Al Takkhin, G.; Skinner, H.A., Organomet., 1982, 1, 1166. [all data]

Ashcroft, Carson, et al., 1963 Ashcroft, S.J.; Carson, A.S.; Pedley, J.B., Thermochemistry of reductions caused by lithium aluminium hydride. Part 2.-The heats of formation of benzyl bromide, benzyl iodide and the benzyl radical, Trans. Faraday Soc., 1963, 59, 2713-2717. [all data]

Akkerman, Schat, et al., 1983 Akkerman, O.S.; Schat, G.; Evers, E.A.I.M.; Bickelhaupt, F., Recl. Trav. Chim. Pays-Bas, 1983, 102, 109. [all data]

Lacher, Casali, et al., 1956 Lacher, J.R.; Casali, L.; Park, J.D., Reaction heats of organic halogen compounds V. The vapor phase bromination of tetrafluoroethylene and trifluorochloroethylene, J. Phys. Chem., 1956, 60, 608-610. [all data]

Chernick, Skinner, et al., 1956 Chernick, C.L.; Skinner, H.A.; Wadso, I., Thermochemistry of metallic alkyls. Part 7.-The heat of formation of mercury diphenyl, and of mercury phenyl chloride, Trans. Faraday Soc., 1956, 52, 1088-1093. [all data]

Adams, Carson, et al., 1966 Adams, G.P.; Carson, A.S.; Laye, P.G., Thermochemistry of reductions caused by lithium aluminium hydride. Part 4.-Heat of formation of methyl bromide, Trans. Faraday Soc., 1966, 62, 1447-1449. [all data]

Jwo, Huang, et al., 1987 Jwo, J-J.; Huang, C-Y.; Chang, E-F.; Wu, R.R., Kinetic study of the bromine-catalyzed isomerization of methyl- and chloro-maleic acids in aqueous Ce(IV)-Br- -H2SO4 medium, J. Chin. Chem. Soc. (Taipei), 1987, 34, 247-256. [all data]

Ashcroft, Carson, et al., 1965 Ashcroft, S.J.; Carson, A.S.; Carter, W.; Laye, P.G., Thermochemistry of reductions caused by lithium aluminium hydride. Part 3.- The C-halogen bond dissociation energies in ethyl iodine and ethyl bromide, Trans. Faraday Soc., 1965, 61, 225-229. [all data]

Mendenhall, Golden, et al., 1973 Mendenhall, G.D.; Golden, D.M.; Benson, S.W., Thermochemistry of the bromination of carbon tetrachloride and the heat of formation of carbon tetrachloride, J. Phys. Chem., 1973, 77, 2707-2709. [all data]

Okafo and Whittle, 1974 Okafo, E.N.; Whittle, E., Bond dissociation energies from equilibrium studies. Part 5.-The equilibria Br2 + CH2F2 = HBr + CHF2Br and Br2 + CH3F = HBr + CH2FBr. Determination of D(CHF2-Br) and ΔH°f (CHF2Br,g), Trans. Faraday Soc., 1974, 17, 1366-1375. [all data]

Corbett, Tarr, et al., 1963 Corbett, P.; Tarr, A.M.; Whittle, E., Vapour-phase bromination of fluoroform and methane, Trans. Faraday Soc., 1963, 59, 1609. [all data]

King, Golden, et al., 1971, 2 King, K.D.; Golden, D.M.; Benson, S.W., Kinetics and thermochemistry of the gas-phase bromination of bromoform. The C-H bond dissociation energy in CHBr3 and the C-Br bond dissociation energy in CBr4, J. Phys. Chem., 1971, 75, 987-989. [all data]

Coomber and Whittle, 1967 Coomber, J.W.; Whittle, E., Bond dissociation energies from equilibrium studies. Part 1.-D(CF3-Br), D(C2F5-Br) and D(n-C3F7-Br), Trans. Faraday Soc., 1967, 63, 608-619. [all data]

Ferguson, Okafo, et al., 1973 Ferguson, K.C.; Okafo, E.N.; Whittle, E., Bond dissociation energies from equilibrium studies Part 4.-The equilibrium Br2 + CH4 = HBr + CH3Br. Determination of D(CH3-Br) and ΔHf°(CH3Br,g), J. Chem. Soc. Faraday Trans. 1, 1973, 69, 295-301. [all data]

Sunner and Wulff, 1974 Sunner, S.; Wulff, C.A., The enthalpy of formation of 1,1-dibromo-2-methylpropane, J. Chem. Thermodyn., 1974, 6, 287-292. [all data]

Notes

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• Symbols used in this document:

  ΔrG°	Free energy of reaction at standard conditions
  ΔrH°	Enthalpy of reaction at standard conditions

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