GB1114430A

GB1114430A – Manufacture of chlorine
– Google Patents

GB1114430A – Manufacture of chlorine
– Google Patents
Manufacture of chlorine

Info

Publication number
GB1114430A

GB1114430A
GB45886/65A
GB4588665A
GB1114430A
GB 1114430 A
GB1114430 A
GB 1114430A
GB 45886/65 A
GB45886/65 A
GB 45886/65A
GB 4588665 A
GB4588665 A
GB 4588665A
GB 1114430 A
GB1114430 A
GB 1114430A
Authority
GB
United Kingdom
Prior art keywords
hno3
nitric acid
reaction
nitrate
concentration
Prior art date
1964-11-07
Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)

Expired

Application number
GB45886/65A
Current Assignee (The listed assignees may be inaccurate. Google has not performed a legal analysis and makes no representation or warranty as to the accuracy of the list.)

Solvay SA

Original Assignee
Solvay SA
Priority date (The priority date is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the date listed.)
1964-11-07
Filing date
1965-10-29
Publication date
1968-05-22

1964-11-07
Priority claimed from FR997370A
external-priority
patent/FR1421608A/en

1965-10-14
Priority claimed from FR35000A
external-priority
patent/FR1460047A/en

1965-10-29
Application filed by Solvay SA
filed
Critical
Solvay SA

1968-05-22
Publication of GB1114430A
publication
Critical
patent/GB1114430A/en

Status
Expired
legal-status
Critical
Current

Links

Espacenet

Global Dossier

Discuss

Classifications

C—CHEMISTRY; METALLURGY

C01—INORGANIC CHEMISTRY

C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C

C01B21/00—Nitrogen; Compounds thereof

C01B21/20—Nitrogen oxides; Oxyacids of nitrogen; Salts thereof

C01B21/36—Nitrogen dioxide (NO2, N2O4)

C—CHEMISTRY; METALLURGY

C01—INORGANIC CHEMISTRY

C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C

C01B21/00—Nitrogen; Compounds thereof

C01B21/082—Compounds containing nitrogen and non-metals and optionally metals

C01B21/083—Compounds containing nitrogen and non-metals and optionally metals containing one or more halogen atoms

C01B21/084—Compounds containing nitrogen and non-metals and optionally metals containing one or more halogen atoms containing also one or more oxygen atoms, e.g. nitrosyl halides

C01B21/0842—Halides of nitrogen oxides

C01B21/0846—Nitrosyl chloride

C—CHEMISTRY; METALLURGY

C01—INORGANIC CHEMISTRY

C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C

C01B7/00—Halogens; Halogen acids

C01B7/01—Chlorine; Hydrogen chloride

C01B7/03—Preparation from chlorides

C—CHEMISTRY; METALLURGY

C01—INORGANIC CHEMISTRY

C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C

C01B7/00—Halogens; Halogen acids

C01B7/01—Chlorine; Hydrogen chloride

C01B7/03—Preparation from chlorides

C01B7/05—Preparation from ammonium chloride

Abstract

Chlorine and nitrogen dioxide are produced from HCl and/or NOCl or a mixture of Cl2 and NOCl by contacting the chlorine containing compound or compounds with an oxidizing reaction medium circulating countercurrentwise, the oxidizing medium comprising a liquid phase obtained by mixing a nitric acid solution of concentration of at least 60% by weight (preferably 65 to 99%), with a nearly saturated aqueous solution of one or more metal nitrates, the reaction temperature being maintained between 60 DEG and 100 DEG C. (preferably 75-90 DEG C.), the reaction medium containing sufficient nitrate to ensure equilibrium under the reaction conditions between the intial reaction medium and the vapour phase over it containing nitric acid, gaseous reactants, their oxidation products and water vapour in which the amount of nitric acid is at least 750 g. HNO3 per kg. of the vapour phase, the quantity of nitrate being also compatible with the solubility of the nitrate or nitrates in the reaction medium, the amount of water in the medium being always less than 500 g/kg. “Nearly saturated” is used to mean at least 90% saturated at at least 60 DEG C. Examples of suitable nitrates are those of Mg, Zn, Cd, Fe, Cu, Al, Ca, Li, either singly or in mixture. The minimum concentration of HNO3 in the vapour phase for the reaction to be complete is between 990 g/kg. at 60 DEG C. and 750 g/kg. at 60 DEG C. The nearly saturated aqueous solution of a metal nitrate may be an aqueous solution of Mg(NO3)2 containing 670 to 720 g/kg., the point representing the composition of the initial reaction medium, Mg(NO3)2/HNO3/H2O, on the triangular equilibrium diagram, Fig. 3a (not shown), for the system Mg(NO3)2-HNO3-H2O being situated in the solubility field of Mg(NO3)2 corresponding to the reaction temperature, the concentration of Mg(NO3)2 being preferably greater than 300 g/kg. Diagrams, e.g. Fig. 6, show curves giving minimum compositions of the reaction phase nitrate/HNO3/H2O necessary for the vapour phase to contain the concentration of HNO3 in g/kg. represented on each curve for Mg.Zn. Cd and mixed Zn and Mg nitrates. When the metal nitrate is Zn(NO3)2 or Cd(NO3)2 the point representing the intial reaction medium, Zn(NO3)2 or Cd(NO3)2/HNO3/H2O on the diagrams or Figs. 6 or 7 (not shown) respectively is situated above the curve corresponding to the reaction temperature. A solution containing about 79% by weight of mixture of 20-30% by weight Zn(NO3)2 and 80-70% by weight Mg(NO3)2 may be used, the reaction temperature preferably being about 100 DEG C. and the point representing the initial reaction medium Mg(NO3)2/Zn(NO3)2/HNO3/H2O on the diagram of Fig. 8 (not shown) being situated above the curve corresponding to the reaction temperature. If nitric acid of concentration 65% by weight or greater is used the spent solution leaving the base of the oxidation chamber may be distilled, after addition of enough 65% HNO3 to restore the reaction phase to its original acid concentration, to regenerate the initial nitric acid which is returned to the oxidation chamber, and a solution of nitrate which is returned to the oxidation chamber after having been concentrated to its initial strength. If 60% to 65% nitric acid is used the spent solution from the oxidation is separated into dilute nitric acid and a nitrate solution which after concentration is recycled. The nitrogen oxide produced may be used, preferably as a liquid mixed with HNO3, to react with HCl and/or chlorides of ammonium, alkali metals or alkaline earth metals to yield nitric acid, the nitrates, and NOCl.

GB45886/65A
1964-11-07
1965-10-29
Manufacture of chlorine

Expired

GB1114430A
(en)

Applications Claiming Priority (2)

Application Number
Priority Date
Filing Date
Title

FR997370A

FR1421608A
(en)

1964-11-07
1964-11-07

Advanced process for manufacturing chlorine

FR35000A

FR1460047A
(en)

1965-10-14
1965-10-14

Process for the production of chlorine

Publications (1)

Publication Number
Publication Date

GB1114430A
true

GB1114430A
(en)

1968-05-22

Family
ID=26166779
Family Applications (1)

Application Number
Title
Priority Date
Filing Date

GB45886/65A
Expired

GB1114430A
(en)

1964-11-07
1965-10-29
Manufacture of chlorine

Country Status (6)

Country
Link

US
(1)

US3440011A
(en)

BE
(1)

BE671818A
(en)

DE
(1)

DE1567797B2
(en)

ES
(1)

ES319299A1
(en)

GB
(1)

GB1114430A
(en)

NL
(1)

NL146124B
(en)

Families Citing this family (1)

* Cited by examiner, † Cited by third party

Publication number
Priority date
Publication date
Assignee
Title

US3661512A
(en)

*

1968-04-26
1972-05-09
Showa Denko Kk
Preparation of chlorine and alkali metal nitrate as a side reaction in the production of nitric acid

Family Cites Families (6)

* Cited by examiner, † Cited by third party

Publication number
Priority date
Publication date
Assignee
Title

US2150669A
(en)

*

1933-11-09
1939-03-14
Solvay Process Co
Process for the treatment of mixtures of nitrosyl chloride and chlorine

US2138017A
(en)

*

1937-02-19
1938-11-29
Solvay Process Co
Process for the decomposition of nitrosyl chloride

US2665195A
(en)

*

1951-03-20
1954-01-05
Allied Chem & Dye Corp
Chlorine from hci

US2793102A
(en)

*

1953-07-24
1957-05-21
Herman H Frischer
Production of pure chlorine

US3211525A
(en)

*

1959-12-24
1965-10-12
American Metal Climax Inc
Concentrating and reacting with nitric acid

DE1245922B
(en)

*

1963-06-21
1967-08-03

1965

1965-10-29
GB
GB45886/65A
patent/GB1114430A/en
not_active
Expired

1965-11-04
BE
BE671818D
patent/BE671818A/xx
unknown

1965-11-05
NL
NL656514394A
patent/NL146124B/en
unknown

1965-11-06
ES
ES0319299A
patent/ES319299A1/en
not_active
Expired

1965-11-06
DE
DE1965S0100392
patent/DE1567797B2/en
active
Granted

1965-11-08
US
US506775A
patent/US3440011A/en
not_active
Expired – Lifetime

Also Published As

Publication number
Publication date

NL6514394A
(en)

1966-05-09

US3440011A
(en)

1969-04-22

BE671818A
(en)

1966-05-04

DE1567797B2
(en)

1976-07-15

NL146124B
(en)

1975-06-16

ES319299A1
(en)

1966-05-16

DE1567797A1
(en)

1970-05-27

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