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  • 7446-11-9 Structure
  • Basic information

    1. Product Name: Sulfur trioxide
    2. Synonyms: Sulfuroxide (SO3);Sulfuric anhydride;
    3. CAS NO:7446-11-9
    4. Molecular Formula: O3S
    5. Molecular Weight: 80.06
    6. EINECS: 231-197-3
    7. Product Categories: N/A
    8. Mol File: 7446-11-9.mol
    9. Article Data: 92
  • Chemical Properties

    1. Melting Point: 16.8℃
    2. Boiling Point: 44.8 °C at 760 mmHg
    3. Flash Point: N/A
    4. Appearance: Needles or polymer
    5. Density: 2.27 g/cm3
    6. Refractive Index: N/A
    7. Storage Temp.: N/A
    8. Solubility: N/A
    9. Water Solubility: reacts violently
    10. CAS DataBase Reference: Sulfur trioxide(CAS DataBase Reference)
    11. NIST Chemistry Reference: Sulfur trioxide(7446-11-9)
    12. EPA Substance Registry System: Sulfur trioxide(7446-11-9)
  • Safety Data

    1. Hazard Codes:  C:Corrosive;
    2. Statements: R14:; R34:;
    3. Safety Statements: S25:; S36/37/39:; S45:; S8:;
    4. RIDADR: 1829
    5. WGK Germany:
    6. RTECS:
    7. HazardClass: 8
    8. PackingGroup: I
    9. Hazardous Substances Data: 7446-11-9(Hazardous Substances Data)

7446-11-9 Usage

Check Digit Verification of cas no

The CAS Registry Mumber 7446-11-9 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 7,4,4 and 6 respectively; the second part has 2 digits, 1 and 1 respectively.
Calculate Digit Verification of CAS Registry Number 7446-11:
(6*7)+(5*4)+(4*4)+(3*6)+(2*1)+(1*1)=99
99 % 10 = 9
So 7446-11-9 is a valid CAS Registry Number.
InChI:InChI=1/O3S/c1-4(2)3

7446-11-9SDS

SAFETY DATA SHEETS

According to Globally Harmonized System of Classification and Labelling of Chemicals (GHS) - Sixth revised edition

Version: 1.0

Creation Date: Aug 16, 2017

Revision Date: Aug 16, 2017

1.Identification

1.1 GHS Product identifier

Product name sulfur trioxide

1.2 Other means of identification

Product number -
Other names sulfuric acid anhydride

1.3 Recommended use of the chemical and restrictions on use

Identified uses For industry use only.
Uses advised against no data available

1.4 Supplier's details

1.5 Emergency phone number

Emergency phone number -
Service hours Monday to Friday, 9am-5pm (Standard time zone: UTC/GMT +8 hours).

More Details:7446-11-9 SDS

7446-11-9Synthetic route

calcium sulfate

calcium sulfate

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
With chlorine In neat (no solvent) at 1100 - 1150°C;;100%
With chlorine In neat (no solvent) addn. of SiO2, NaCl or Na2SO4 increase reaction temp.; react. accelerated;;
With chlorine In neat (no solvent) in presence of charcoal strong react.; addn. of NiSO4, CuSO4, MgSO4, Fe2O3 or KCl reduced yield; no influence of overheated water vapor;; react. detected at 700 - 1150°C;;
sulfur dioxide
7446-09-5

sulfur dioxide

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
manganese(IV) oxide 450°C;98%
2Na2O*3MoO3*V2O5 440°C;98.4%
two-stage catalyst contact cooled by SO2 gas, external heat exchangers, temp. in contact bed:400-411°C;98%
sulfur dioxide
7446-09-5

sulfur dioxide

oxygen
80937-33-3

oxygen

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
vanadia Kinetics; 437°C;98%
platinum Kinetics; 415°C;98%
vanadia Kinetics; 452°C;97%
pyrite

pyrite

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
3-stage contact bed;98%
no C content in pyrite;96%
no C content in pyrite;96%
pyrite

pyrite

oxygen
80937-33-3

oxygen

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
With catalyst: Fe compd. High Pressure; higher yield with increasing pressure, 600-630°C at 100 at;97%
With catalyst: Fe compd. High Pressure; higher yield with increasing pressure, 600-630°C at 100 at;97%
Kinetics; 420°C;
oxygen
80937-33-3

oxygen

sulfur
7704-34-9

sulfur

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
With hydrogenchloride; copper dichloride In neat (no solvent) Kinetics; (450°C, 1.5 s);95%
With hydrogenchloride SO3 stabilized as Lewis-addukt(HCl.SO3); O2: 30l/h, HCl: 8l/h; 60min;40%
Kinetics; 420°C;
silver sulfide

silver sulfide

A

sulfur dioxide
7446-09-5

sulfur dioxide

B

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
With oxygen In neat (no solvent) heating in a stream of O2 at 550 - 600°C (formation of SO2 from 82 % of S and of Ag2SO4), later at 980 - 1070°C (decomposition of Ag2SO4);;A 95%
B 5%
With O2 In neat (no solvent) heating in a stream of O2 at 550 - 600°C (formation of SO2 from 82 % of S and of Ag2SO4), later at 980 - 1070°C (decomposition of Ag2SO4);;A 95%
B 5%
SbCl5*SO3
25362-97-4

SbCl5*SO3

A

pyrosulfuryl chloride
7791-27-7

pyrosulfuryl chloride

B

2SbCl4(1+)*SO4(2-)=(SbCl4)2SO4

2SbCl4(1+)*SO4(2-)=(SbCl4)2SO4

C

antimonypentachloride
7647-18-9

antimonypentachloride

D

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
70°C in vac.;A n/a
B n/a
C n/a
D 95%
Hg(2+)*2(O3SC6Cl5)(1-)*2H2O=Hg(O3SC6Cl5)2*2H2O

Hg(2+)*2(O3SC6Cl5)(1-)*2H2O=Hg(O3SC6Cl5)2*2H2O

A

pentachlorobenzene
608-93-5

pentachlorobenzene

B

sulfur trioxide
7446-11-9

sulfur trioxide

C

Bis-pentachlor-phenyl-quecksilber
1043-49-8

Bis-pentachlor-phenyl-quecksilber

Conditions
ConditionsYield
130-220°C;A <1
B 80%
C 64%
Hg(O3S-p-HC6Cl4)2

Hg(O3S-p-HC6Cl4)2

A

(p-HC6Cl4)2Hg
38180-52-8

(p-HC6Cl4)2Hg

B

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
130-220°C;A 78%
B 80%
iron(II) sulfate

iron(II) sulfate

A

iron(III) oxide

iron(III) oxide

B

sulfur dioxide
7446-09-5

sulfur dioxide

C

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
With pyrographite 700°C;A n/a
B 80%
C n/a
With C 700°C;A n/a
B 80%
C n/a
700°C;A n/a
B 50%
C n/a
disulfur dioxide
126885-21-0

disulfur dioxide

A

sulfur dioxide
7446-09-5

sulfur dioxide

B

sulfur trioxide
7446-11-9

sulfur trioxide

C

sulfur
7704-34-9

sulfur

Conditions
ConditionsYield
With oxygen In neat (no solvent) oxidn. of S2O2 with an excess of O2, min. ignition pressure at 32°C 54 Torr, at 150°C 2 Torr, mechanism discussed, sometimes react. with lightening, inhibition by SO2;;A 10-25
B 15-30
C 80%
Hg(2+)*2OSO2C6F5(1-)*2H2O=Hg(OSO2C6F5)2*2H2O

Hg(2+)*2OSO2C6F5(1-)*2H2O=Hg(OSO2C6F5)2*2H2O

A

Pentafluorobenzene
363-72-4

Pentafluorobenzene

B

pentafluorobenzenesulfonic acid
313-50-8

pentafluorobenzenesulfonic acid

C

sulfur trioxide
7446-11-9

sulfur trioxide

D

bis(pentafluorophenyl)mercury(II)
973-17-1

bis(pentafluorophenyl)mercury(II)

Conditions
ConditionsYield
130-220°C;A 12%
B 9%
C 70%
D 53%
130-240°C;
130-240°C;
Hg(O3S-p-HC6F4)2*2H2O

Hg(O3S-p-HC6F4)2*2H2O

A

(p-HC6F4)2Hg
2262-05-7

(p-HC6F4)2Hg

B

1,2,4,5-Tetrafluorobenzene
327-54-8

1,2,4,5-Tetrafluorobenzene

C

2,3,5,6-tetrafluorobenzenesulfonic acid
40707-55-9

2,3,5,6-tetrafluorobenzenesulfonic acid

D

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
130-230°C;A 17%
B 17%
C 17%
D 60%
Hg(O3S-m-HC6Cl4)2*2H2O

Hg(O3S-m-HC6Cl4)2*2H2O

A

(m-HC6Cl4)2Hg
37963-59-0

(m-HC6Cl4)2Hg

B

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
130-220°C;A 44%
B 60%
bis(pentafluorosulfur) peroxide
12395-41-4

bis(pentafluorosulfur) peroxide

sulfur dioxide
7446-09-5

sulfur dioxide

A

thionyl tetrafluoride
173009-97-7, 118492-84-5, 13709-54-1

thionyl tetrafluoride

B

pentafluorosulfur fluorosulfonate
81439-35-2

pentafluorosulfur fluorosulfonate

C

sulfur trioxide
7446-11-9

sulfur trioxide

D

thionyl fluoride
7783-42-8

thionyl fluoride

E

sulfur(VI) hexafluoride
2551-62-4

sulfur(VI) hexafluoride

Conditions
ConditionsYield
byproducts: SiF4, sulfur; other Radiation; photochemical reaction with 253.7 nm radiation, 48 h;A n/a
B 45%
C n/a
D n/a
E n/a
oxygen
80937-33-3

oxygen

sulfur
7704-34-9

sulfur

A

sulfur dioxide
7446-09-5

sulfur dioxide

B

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
In gas mixt. of N2 and sulfur vapor; O2: 100l/h; 15min, tube system, products cooled;A n/a
B 41%
1000-1370°C, rapid cooling to minimize SO3 formation;
very low SO3 content;
Hg(O3S-o-HC6Cl4)2*2H2O

Hg(O3S-o-HC6Cl4)2*2H2O

A

1,2,3,4,-tetrachlorobenzene
634-66-2

1,2,3,4,-tetrachlorobenzene

B

o-HC6Cl4SO3H
40707-33-3

o-HC6Cl4SO3H

C

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
130-250°C;A 15%
B 10%
C 40%
magnesium sulfate
7487-88-9

magnesium sulfate

A

sulfur trioxide
7446-11-9

sulfur trioxide

B

magnesium oxide

magnesium oxide

Conditions
ConditionsYield
995 °C in N2; part of a Mg-S-I water splitting cycle;A 30%
B 30%
In neat (no solvent) heating at 950-1050 K (effusion orifices with A/a ratios of 10-30);
1120-1200°C; 29,1mol% in 15min; 90mol% in 2h;
900°C, in air stream;
iron(II) sulfate

iron(II) sulfate

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
In neat (no solvent) evolution of SO3 by heating FeSO4 in a glass tube by little admission of air; beginning at 590 °C, only 3% after heating 2h at 625 to 635 °C;;3%
carbon disulfide
75-15-0

carbon disulfide

oxygen

oxygen

A

sulfur trioxide
7446-11-9

sulfur trioxide

B

methylammonium carbonate
15719-64-9, 15719-76-3, 97762-63-5

methylammonium carbonate

C

sulfur dioxide

sulfur dioxide

D

sulfur

sulfur

Conditions
ConditionsYield
Bei der Explosion mit ueberschuessigem Sauerstoff;
disulfuric acid carbonylamide chloride
63549-29-1

disulfuric acid carbonylamide chloride

A

isocyanate de chlorosulfonyle
1189-71-5

isocyanate de chlorosulfonyle

B

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
at 160℃;
2,3-disulfosuccinic acid
54060-35-4

2,3-disulfosuccinic acid

A

sulfur trioxide
7446-11-9

sulfur trioxide

B

water
7732-18-5

water

C

methylammonium carbonate
15719-64-9, 15719-76-3, 97762-63-5

methylammonium carbonate

hydrogenchloride
7647-01-0

hydrogenchloride

N,N'-bis-sulfomethyl-hydrazine-N-sulfonic acid

N,N'-bis-sulfomethyl-hydrazine-N-sulfonic acid

A

formaldehyd
50-00-0

formaldehyd

B

sulfuric acid
7664-93-9

sulfuric acid

C

sulfur trioxide
7446-11-9

sulfur trioxide

D

hydrazine
302-01-2

hydrazine

[1,3,2]dioxathietane-2,2-dioxide
56639-44-2

[1,3,2]dioxathietane-2,2-dioxide

A

sulfur trioxide
7446-11-9

sulfur trioxide

B

CO

CO

C

SO2

SO2

Conditions
ConditionsYield
at 155℃; beim Schmelzen;
pyrosulfuryl chloride
7791-27-7

pyrosulfuryl chloride

hydrogen iodide
10034-85-2

hydrogen iodide

A

hydrogenchloride
7647-01-0

hydrogenchloride

B

sulfur dioxide
7446-09-5

sulfur dioxide

C

sulfur trioxide
7446-11-9

sulfur trioxide

D

iodine
7553-56-2

iodine

Conditions
ConditionsYield
In neat (no solvent) violent reaction of dry HI even at temp. of a cold mixture of ice and sodium chloride;;
fluorosulfonyl anhydride
13036-75-4

fluorosulfonyl anhydride

A

fluorosulfonyl fluoride
640723-20-2, 2699-79-8, 12769-73-2

fluorosulfonyl fluoride

B

sulfur trioxide
7446-11-9

sulfur trioxide

Conditions
ConditionsYield
500°C;
500°C;
sulfur dichloride
10545-99-0

sulfur dichloride

sulfur trioxide
7446-11-9

sulfur trioxide

A

thionyl chloride
7719-09-7

thionyl chloride

B

sulfur dioxide
7446-09-5

sulfur dioxide

Conditions
ConditionsYield
In neat (no solvent) below -10°C or under pressure;;A 100%
B n/a
lithium sulfate

lithium sulfate

sulfur trioxide
7446-11-9

sulfur trioxide

lithium pyrosulfate

lithium pyrosulfate

Conditions
ConditionsYield
SO3 in excess, 10-15 min, closed vessel 300°C;100%
In neat (no solvent) formation on heating Li2SO4 in a SO3-atmosphere to .300°C;;
In neat (no solvent) formation on heating Li2SO4 in a SO3-atmosphere to .300°C;;
In neat (no solvent) reaction of SO3-vapour with Li2SO4 at 450°C; TGA;
sulfur trioxide
7446-11-9

sulfur trioxide

sodium sulfate
7757-82-6

sodium sulfate

sodium pyrosulfate

sodium pyrosulfate

Conditions
ConditionsYield
SO3 in excess, 10-15 min, closed vessel 450°C;100%
react. of Na2SO4 with SO3 at ambient temp.;; substance with Na2S2O7 and unchanged Na2SO4 obtained;;
In neat (no solvent) react. of Na2SO4 with an excess of SO3 above 150°C;;
π-C5H5Zr(OSO3H)3*(CH3CO)2O

π-C5H5Zr(OSO3H)3*(CH3CO)2O

sulfur trioxide
7446-11-9

sulfur trioxide

π-HO3SC5H4Zr(OSO3H)3

π-HO3SC5H4Zr(OSO3H)3

Conditions
ConditionsYield
In 1,2-dichloro-ethane dry CH2ClCH2Cl/3 h/5°C;;100%
In 1,2-dichloro-ethane dry CH2ClCH2Cl/3 h/5°C;;100%
ammonium sulfate

ammonium sulfate

sulfuric acid
7664-93-9

sulfuric acid

sulfur trioxide
7446-11-9

sulfur trioxide

boric acid
11113-50-1

boric acid

3H3N*3H(1+)*B(SO4)3(3-)

3H3N*3H(1+)*B(SO4)3(3-)

Conditions
ConditionsYield
at 300℃; for 3h;100%
strontium(II) carbonate
1633-05-2

strontium(II) carbonate

sulfuric acid
7664-93-9

sulfuric acid

sulfur trioxide
7446-11-9

sulfur trioxide

boric acid
11113-50-1

boric acid

Sr(2+)*2{B(SO4)2}(1-)=Sr{B(SO4)2}2

Sr(2+)*2{B(SO4)2}(1-)=Sr{B(SO4)2}2

Conditions
ConditionsYield
at 180℃; for 24h;100%
sulfur trioxide
7446-11-9

sulfur trioxide

A

sulfur dioxide
7446-09-5

sulfur dioxide

B

oxygen
80937-33-3

oxygen

Conditions
ConditionsYield
995 °C in N2; part of a Mg-S-I water splitting cycle;A 99%
B 99%
copper(II) oxide In gas equil. react.;
platinum In gas equil. react.;
ammonium hexachloroplumbate

ammonium hexachloroplumbate

sulfuric acid
7664-93-9

sulfuric acid

sulfur trioxide
7446-11-9

sulfur trioxide

Pb(2+)*S3O10(2-)=PbS3O10

Pb(2+)*S3O10(2-)=PbS3O10

Conditions
ConditionsYield
In sulfuric acid aq. H2SO4; (NH42PbCl6 and oleum filled in glass tube; torch-sealed under vac.; heated up to 250°C; maintained for 24 h, slowly cooled (1.8 K/h); ppt. collected by decantation of mother liqour under inert condns.;99%
sulfur trioxide
7446-11-9

sulfur trioxide

mercury bis(trifluoromethanethiolate)
21259-75-6

mercury bis(trifluoromethanethiolate)

Quecksilber(II)-bis

Quecksilber(II)-bis

Conditions
ConditionsYield
In liquid sulphur dioxide Ar; 20°C;; condensation of SO2; residue washed with FCCl3; elem. anal.;;96%
sulfur trioxide
7446-11-9

sulfur trioxide

triethoxyantimony
873376-62-6

triethoxyantimony

ethoxyantimony bis(ethyl sulfate)
80398-49-8

ethoxyantimony bis(ethyl sulfate)

Conditions
ConditionsYield
In dichloromethane SO3 soln. was added to Sb compd. at -50°C (N2 or Ar); evapn., drying in vac.; elem. anal.;96%
perfluoropropylene
116-15-4

perfluoropropylene

sulfur trioxide
7446-11-9

sulfur trioxide

1,2,2-trifluoro-2-hydroxy-1-trifluoromethylethanesulfonic acid sultone
773-15-9

1,2,2-trifluoro-2-hydroxy-1-trifluoromethylethanesulfonic acid sultone

Conditions
ConditionsYield
150°C, 5 h;94%
150°C, 5 h;94%
60°C;92%
diphenyl sulphone
127-63-9

diphenyl sulphone

sulfur trioxide
7446-11-9

sulfur trioxide

benzenesulfonic acid
98-11-3

benzenesulfonic acid

Conditions
ConditionsYield
With sulfuric acid In water; benzene93%
With phosphoric acid; sulfuric acid In water; benzene87%
polytetrafluoroethylene
116-14-3

polytetrafluoroethylene

sulfur trioxide
7446-11-9

sulfur trioxide

tetrafluoroethane-β-sultone
697-18-7

tetrafluoroethane-β-sultone

Conditions
ConditionsYield
fresh distilled SO3, 2.7 atm, below 80°C, 1 h;93%
fresh distilled SO3, 2.7 atm, below 80°C, 1 h;93%
fresh distilled SO3, 2.7 atm, below 80°C, 1 h;93%
sulfur trioxide
7446-11-9

sulfur trioxide

triethoxyantimony
873376-62-6

triethoxyantimony

antimony tris(ethyl sulfate)

antimony tris(ethyl sulfate)

Conditions
ConditionsYield
In dichloromethane SO3 soln. was added to Sb compd. at -50°C (N2 or Ar); elem. anal.;93%
((CH3)3Sn)C(C6H9)CH(Sn(CH3)3)
180070-46-6, 180070-53-5

((CH3)3Sn)C(C6H9)CH(Sn(CH3)3)

sulfur trioxide
7446-11-9

sulfur trioxide

(CH3)3SnSO3C(C6H9)CHSO3Sn(CH3)3
180071-29-8

(CH3)3SnSO3C(C6H9)CHSO3Sn(CH3)3

Conditions
ConditionsYield
In dichloromethane absence of air and moisture; 2 equiv. SO2, stirring at -78°C for 4 h; evapn., distn.; elem. anal.;93%
sulfur trioxide
7446-11-9

sulfur trioxide

silver fluoride

silver fluoride

A

silver(I) fluorosulfate
33983-99-2

silver(I) fluorosulfate

B

silver sulfate

silver sulfate

Conditions
ConditionsYield
A 91%
B n/a
hexafluoro-1,3-butadiene
685-63-2

hexafluoro-1,3-butadiene

sulfur trioxide
7446-11-9

sulfur trioxide

buta-1,3-diene
106-99-0

buta-1,3-diene

4-trifluorovinyltrifluoro-1,2-oxathietane 2,2-dioxide
69740-49-4

4-trifluorovinyltrifluoro-1,2-oxathietane 2,2-dioxide

Conditions
ConditionsYield
In liquid sulphur dioxide dropping SO3 into a soln. of CF2=CFCF=CF2 in SO2 at -10°C followed by stripping SO2 and butadiene; distn.;91%
In sulfur dioxide dropping SO3 into a soln. of CF2=CFCF=CF2 in SO2 at -10°C followed by stripping SO2 and butadiene; distn.;91%
(5,7,12,14-tetramethyldibenzo[b,i][1,4,8,11]tetraazacyclotetradecinate(2-))V=O

(5,7,12,14-tetramethyldibenzo[b,i][1,4,8,11]tetraazacyclotetradecinate(2-))V=O

sulfur trioxide
7446-11-9

sulfur trioxide

(5,7,12,14-tetramethyldibenzo[b,i][1,4,8,11]tetraazacyclotetradecinate(2-))V(O2SO2)
174715-71-0

(5,7,12,14-tetramethyldibenzo[b,i][1,4,8,11]tetraazacyclotetradecinate(2-))V(O2SO2)

Conditions
ConditionsYield
In dichloromethane Ar-atmosphere; slow addn. of SO3 to V-complex at 0°C, stirring atroom temp. for 2 h; ether addn., collection (filtration), washing (CH2Cl2, ether); elem. anal.;91%
sulfuric acid
7664-93-9

sulfuric acid

phthalocyaninealuminum chloride
14154-42-8, 62905-77-5

phthalocyaninealuminum chloride

sulfur trioxide
7446-11-9

sulfur trioxide

(disulfophthalocyanine)aluminum chloride

(disulfophthalocyanine)aluminum chloride

Conditions
ConditionsYield
In sulfuric acid mixt. Al complex and oleum was stirred at room temp. for 16 h.; react. mixt. was cooled to ambient temp., poured onto ice, ppt. was filtered off, washed with 1% aq. HCl, water, dried in vac. at 90°C;91%
Chlorotrifluoroethylene
79-38-9

Chlorotrifluoroethylene

sulfur trioxide
7446-11-9

sulfur trioxide

3-chlorotrifluoro-1,2-oxathietane 2,2-dioxide
1004-47-3

3-chlorotrifluoro-1,2-oxathietane 2,2-dioxide

Conditions
ConditionsYield
at 70°C;90%
sulfur trioxide
7446-11-9

sulfur trioxide

chlorine monofluoride
7790-89-8

chlorine monofluoride

A

fluorosulfonyl fluoride
640723-20-2, 2699-79-8, 12769-73-2

fluorosulfonyl fluoride

B

ClSO3F

ClSO3F

Conditions
ConditionsYield
byproducts: Cl2; from -196 °C to room temp., excess ClF;A n/a
B 90%
sulfur trioxide
7446-11-9

sulfur trioxide

ammonia
7664-41-7

ammonia

ammonium sulfamate

ammonium sulfamate

Conditions
ConditionsYield
220-280 °C, 30 atm NH3, 30 min;90%

7446-11-9Relevant articles and documents

A study of Lux-Flood acid-base reactions in KBr melts at 800°C

Rebrova,Cherginets,Ponomarenko

, p. 1879 - 1882 (2009)

The dissociation of CO 3 2- (pK = 2.4 ± 0.2) and precipitation of MgO (pL MgO = 10.66 ± 0.1) in a KBr melt at 800°C were studied potentiometrically with the use of a Pt(O 2)|ZrO2|(Y2O3

Whittingham, G.

, p. 550 - 550 (1946)

Whittingham, G.

, p. 141 - 150 (1948)

Hill, R. A.

, p. 107 - 112 (1924)

Synthesis and structural characterization of fluorosulfate derivatives of silver(II)

Leung,Aubke

, p. 1765 - 1772 (1978)

The synthesis of silver(II) fluorosulfate, Ag(SO3F)2, by a variety of routes is described. The preparations of a mixed-valency compound of the composition Ag3(SO3F)4 and its potassium analogue K2AgII(SO3F)4, the compounds AgIIPtIV(SO3F)6 and AgIISnIV(SO3F)6, and the complex [Ag(bpy)2](SO3F)2 are also reported. Structural studies are based on vibrational, electronic mull and diffuse reflectance, and ESR spectra as well as magnetic susceptibility measurements in the temperature range of 80 to about 300 K. Both Ag3(SO3F)4 and K2Ag(SO3F)4 show antiferromagnetic coupling. All other divalent silver compounds synthesized here are magnetically dilute with the Ag2+ ion in a square-planar or tetragonally distorted (elongated) octahedral environment.

Two Ce(SO4)2·4H2O polymorphs: Crystal structure and thermal behavior

Casari, Barbara M.,Langer, Vratislav

, p. 1616 - 1622 (2007)

Syntheses, crystal structures and thermal behavior of two polymorphic forms of Ce(SO4)2·4H2O are reported. The first modification, α-Ce(SO4)2·4H2O (I), crystallizes in the orthorhombic space group Fddd, with a=5.6587(1), b=12.0469(2), c=26.7201(3) A and Z=8. The second modification, β-Ce(SO4)2·4H2O (II), crystallizes in the orthorhombic space group Pnma, with a=14.6019(2), b=11.0546(2), c=5.6340(1) A and Z=4. In both structures, the cerium atoms have eight ligands: four water molecules and four sulfate groups. The mutual position of the ligands differs in (I) and (II), resulting in geometrical isomerism. Both these structures are built up by layers of Ce(H2O)4(SO4)2 held together by a hydrogen bonding network. The dehydration of Ce(SO4)2·4H2O is a two step (I) and one step (II) process, respectively, forming Ce(SO4)2 in both cases. During the decomposition of the anhydrous form, Ce(SO4)2, into the final product CeO2, intermediate xCeO2·yCe(SO4)2 species are formed.

Synthesis, vibrational spectra, and structure of divalent metal peroxodisulfates

Skogareva,Minaeva,Filippova

, p. 1341 - 1349 (2009)

Simple strontium peroxodisulfate SrS2O8 ? 4H2O was synthesized by the reaction of solid Sr(OH)2 ? 8H2O taken in 30% excess with an aqueous solution of (NH 4)2S2O8

Kinetics of the Reaction OH + SO2 in He, N2 and O2 at Low Pressure

Lee, Yin-Yu,Kao, Wen-Chuen,Lee, Yuan-pern

, p. 4535 - 4540 (1990)

The rate constants of the gas-phase reaction of OH with SO2 for M = He, N2,and SO2 have been determined by using the discharge flow/resonance fluorescence technique.The termonuclear rate constants (all in units of cm6 molecule -2 ss

Synthesis and Crystal Structure of Tetraphenylbismuth Benzenesulfonate Hydrate and Tetraphenylbismuth 3,4-Dimethylbenzenesulfonate

Sharutin,Egorova,Ivanenko,Sharutina,Popov

, p. 468 - 473 (2003)

The reaction of pentaphenylbismuth with SO3 or with triphenylbismuth bis(benzenesulfonate) in benzene gave tetraphenylbismuth benzenesulfonate monohydrate (I). Tetraphenylbismuth 3,4- dimethylbenzenesulfonate (II) was prepared from pentaphenylbismuth and triphenylbismuth bis(3,4-dimethylbenzenesulfonate) in benzene. The structures of compounds I and II were established by X-ray diffraction. The Bi atoms have a distorted trigonal-bipyramidal coordination where the arenesulfonate group occupies an axial position. The Bi-C(average) and Bi-O distances in molecules I and II are 2.204(2), 2.695(2) A and 2.205(2), 2.728(2) A, respectively.

Discharge Flow Measurements of the Rate Constants for the Reactions OH+SO2+He and HOSO2+O2 in Relation with the Atmospheric Oxidation of SO2

Martin, D.,Jourdain, J. L.,Bras, G. Le

, p. 4143 - 4147 (1986)

The reactions OH+SO2+M (M=He, SO2)->HOSO2 (1) and HOSO2+O2 (2) have been studied by the discharge flow EPR technique at room temperature and at pressures ranging from 1 to 6.4 Torr in a halocarbon-wax-coated reactor.For He and SO2 as the third body the bimolecular rate constant can be expressed as k1(He)=(8.1+/-0.2)*10-32+(2.4+/-0.4)*10-15 (P=1-6.4 Torr) and k1(SO2)=(1.3+/-0.4)*10-30 (P0.1 Torr).Units are cubic centimeters per molecular per second.Reaction 2 was studied by adding O2 to the reacting medium and NO for the conversion of HO2 into OH.The value of k2 was found from the computer fitting of the OH profiles with and without added O2 as a function of reaction time: k2=(3.5+/-1)*10-13 cm3 molecule-1 s-1.

A molecular approach for unraveling surface phase transitions: Sulfation of BaO as a model NOx trap

Rankovic, Nikola,Chizallet, Celine,Nicolle, Andre,Da Costa, Patrick

, p. 10511 - 10514 (2012)

SO3-induced surface reconstruction: The SO3 molecule as a multidentate ligand induces remarkable surface reconstruction phenomena on alkaline earth oxide surface. By using ab initio computations, adsorption properties are derived to elucidate the thermodynamics of the SO3-BaO system. Copyright

Williams, S.

, p. 304 - 307 (1869)

Jaffe, S.,Klein, F. S.

, p. 2150 - 2157 (1966)

Magnetic structure and properties of Cu3(OH)4SO 4 made of triple chains of spins s=1/2

Vilminot,Richard-Plouet,Andre,Swierczynski,Guillot,Bouree-Vigneron,Drillon

, p. 255 - 264 (2003)

Cu3(OH)4SO4, obtained by hydrothermal synthesis from copper sulfate and soda in aqueous medium, is isostructural with the corresponding antlerite mineral, orthorhombic, space group Pnma (62), with a=8.289(1) b=6.079(1) and c=12.057(1)A, V=607.5(2) A3, Z=4. Its crystalline structure has been refined from X-ray single crystal and powder neutron diffraction data at room temperature. It consists of copper (II) triple chains, running in the b-axis direction and connected to each other by sulfate groups. The magnetic structure, solved from powder neutron diffraction data at 1.4K below the transition at 5K evidenced by susceptibility and specific measurements, reveals that, inside a triple chain, the magnetic moments of the copper ions (μB=0.88(5) at 1.4K) belonging to outer chains are oriented along the c-axis of the nuclear cell, with ferromagnetic order inside a chain and antiferromagnetic order between the two outer chains. No long-range magnetic order is obtained along the central chain with an idle spin behavior.

Structure of vanadium oxosulfato complexes in V2O5-M2S2O7-M2 SO4 (M = K, Cs) melts. A high temperature spectroscopic study

Boghosian, Soghomon,Chrissanthopoulos, Athanassios,Fehrmann, Rasmus

, p. 49 - 56 (2002)

The VV and VIV oxosulfato Complexes formed in V2O5-M2S2O7-M2 SO4 (M = K, Cs) melts under SO2(g) or O2(g) atmosphere have been studied by electronic absorption (VIS/NIR) and Raman spectroscopy at 450 ?°C. VIS/NIR spectra have been obtained at 450 ?°C for V2O5-K2S2O7 molten mixtures in SO2 atmosphere (PSO2 = 0-1.2 atm). The data are in agreement with the VV a?? VIV equilibrium: (VO)2O(SO4)44-(l) + SO2(g) a?? 2VO(SO4)22-(l) + SO3(g). SO2 does not coordinate to the VV complex but starts significantly to coordinate to VIV for PSO2 > 0.4 atm according to VO(SO4)22-(l) + SO2(g) a?? VO(SO4)2SO22-(l). The Raman spectral features and the exploitation of the relative Raman intensities indicate that the (VO)2O(SO4)44- dimeric complex unit, possessing a V-O-V bridge, is formed in the V2O5-M2S2O7 binary mixtures. The spectral changes occurring upon interaction of the binary V2O5-K2S2O7 mixtures with SO2 or addition of M2SO4 to the binary V2O5-M2S2O7 mixtures indicate a cleavage of the V-O-V bridge and formation of the VIVO(SO4)22- or VVO2(SO4)23- monomeric complex units, respectively. The most characteristic bands due to the various complexes in the melts have been assigned. The spectral data are discussed in terms of possible structures. For the first time, high-temperature vibrational spectroscopy has been used to study the structural and vibrational properties of V2O5-K2S2O7 and V2O5-K2S2O7-K2 SO4 melts. The results are valuable for the mechanistic understanding of SO2 oxidation at the molecular level.

Bell, T. N.,Robinson, P. L.,Trenwith, A. B.

, (1955)

The local structure of SO2 and SO3 on Ni(1 1 1)

Jackson,Woodruff,Chan,Jones, Robert G.,Cowie

, p. 31 - 41 (2005)

The normal incidence X-ray standing wave (NIXSW) technique, supported by X-ray photoelectron spectroscopy and near-edge X-ray absorption fine structure (NEXAFS), has been used to determine the local adsorption geometry of SO 2 and SO3 on Ni(1 1 1). Chemical-state specific NIXSW data for coadsorbed SO3 and S, formed by the disproportionation of adsorbed SO2 after heating from 140 K to 270 K, were obtained using S 1s photoemission detection. For adsorbed SO2 at 140 K the new results confirm those of an earlier study [Jackson et al., Surf. Sci. 389 (1997) 223] that the molecule is located above hollow sites with its molecular plane parallel to the surface and the S and O atoms in off-atop sites; corrections to account for the non-dipole effects in the interpretation of the NIXSW monitored by S 1s and O 1s photoemission, not included in the earlier work, remove the need for any significant adsorption-induced distortion of the SO2 in this structure. SO3, not previously investigated, is found to occupy an off-bridge site with the C3v axis slightly tilted relative to the surface normal and with one O atom in an off-atop site and the other two O atoms roughly between bridge and hollow sites. The O atoms are approximately 0.87 ? closer to the surface than the S atom. This general bonding orientation for SO3 is similar to that found on Cu(1 1 1) and Cu(1 0 0) both experimentally and theoretically, although the detailed adsorption sites differ.

Oxidation of Sulphur Dioxide using Micro- and Nanoparticles of various Iron Oxides

Reichelt, Lydia,Hippmann, Sebastian,Brichkin, Vyacheslav Nikolayevich,Bertau, Martin

, p. 1583 - 1593 (2021)

Sulphuric acid is the chemical with highest production rates in the world. At present, it is mainly synthesized using vanadium pentoxide as catalyst, which determines the applied production process particularly in terms of gas pre-treatment and heat management. For processes, which cannot be run with vanadium pentoxide, alternative catalysts are required to make different SO2 qualities accessible to sulphuric acid production. Ferric oxides are a very promising alternative, since they combine higher thermal with improved chemical stability. Within this study, various ferric oxides were examined with regard to conversion rates and structural changes during application. Effects of crystal structure, particle size as well as thermal treatment and the influence of precipitation conditions were studied. Although conversion rates are very promising, it has become apparent, though, that these materials cannot compete with vanadium pentoxide in terms of conversion rate as well as long-time stability, yet. Nevertheless, from the results of this study, it is clear that high potential lies in focused catalyst optimisation.

Catalytic properties of the thermal decomposition products of Zr(SO4)2 · 4H2o

Kotsarenko,Shmachkova

, p. 280 - 283 (2002)

The catalytic activity of the thermal decomposition products of Zr(SO4)2 · 4H2O in the reactions of 1-butene isomerization to 2-butenes, isobutanol dehydration, and n-butane skeletal isomerization was studied. Their behavi

Synthesis and characterization of molybdenum(VI) oxide sulfates and crystal structures of two polymorphs of MoO2(SO4)

Christiansen, Alexander F.,Fjellvag, Helmer,Kjekshus, Arne,Klewe, Bernt

, p. 806 - 815 (2001)

Reactions between α-MoO3 or MoO3·0.43H2O and 65-95 wt% H2SO4 were studied from room temperature up to the boiling point of the acid. Four new compounds, MoO2(SO4), (modifications I, II and III) and MoO2(SO4)·H2SO4·H 2O, have been isolated depending on the H2SO4 concentration, reaction temperature, reaction time and molybdenum source. The characterization of these phases was performed with powder X-ray diffraction, thermogravimetric analysis, differential thermal analysis, chemical analysis and density measurements. Both starting materials react with sulfuric acid and form MoO2(SO4) II at temperatures above ca. 75 °C. This compound is unstable in the reaction mixture and converts into MoO2(SO4) I or III depending on time and temperature. The three modifications of MoO2(SO4) are hygroscopic and decomposition in moist air is studied for the I and II modifications. On heating, all modifications of MoO2(SO4) decompose into α-MoO3 or a mixture of α-MoO3 and β-MoO3 depending on heating rate and sample size. The three-dimensional, open-framework structures of I and II, have been determined from single-crystal X-ray diffraction data. I crystallizes in the monoclinic space group C2/c and II in the orthorhombic space group Pna21. Both structures are made up of MoO6 octahedra and SO4 tetrahedra and contain layers of eight- and four-membered rings of alternating, corner-sharing octahedra and tetrahedra. These layers are linked (also via Mo-S bridges) to form a three-dimensional framework. The MoO6 octahedra are rather distorted, as demonstrated by large variations in the bonding Mo-O interatomic distances, which reflect the double-bond character of the binding between molybdenum and terminal oxygen atoms pointing into the eight-membered rings. The SO4 tetrahedra are quite regular. The structural relation to MoO2(SO4) III is briefly considered.

Thermal analysis for identification of E-beam nanosize ammonium sulfate

Petkova,Pelovski,Hristova

, p. 813 - 817 (2005)

Thermal decomposition of nanosize ammonium sulfate obtained as a by-product in a new electron-beam technology cleaning up waste gases from thermal power stations was studied. DTA-TG-DTG curves were used to characterize thermal properties of the new products obtained under different technological conditions. High quality of ammonium sulfate from Merck was used as a reference material. Ammonium sulfate was the main component in all the products and their thermal behavior was similar to that of the reference. Only the solid product obtained with the highest norm of ammonia contained about 3.2% ammonium nitrate. Thermoanalytical methods can successfully be applied for control the quality of the by-products from E-beam desulfurization technology. It was found that the thermal stability of the nanosize ammonium sulfate was the same as that of the reference ammonium sulfate.

Russell, E. J.,Smith, N.

, p. 340 - 352 (1900)

James, F. C.,Kerr, J. A.,Simons, J. P.

, p. 431 - 434 (1974)

Hayek, E.,Engelbrecht, A.

, (1949)

Does Tetrahydrofuran (THF) Behave like a Solvent or a Reactant in the Photolysis of Thionyl Chloride (Cl2SO) in Cyclohexane? A Transient Infrared Difference Study

Shih, Meng-Chen,Chu, Li-Kang

, p. 5401 - 5408 (2018/06/04)

The photolysis of thionyl chloride (Cl2SO) in pure cyclohexane (cHex) and in cHex with a small amount of tetrahydrofuran (THF) irradiated with 266 nm pulsed laser was investigated using time-resolved step-scan Fourier-transform spectroscopy. The density functional theory B3LYP, with the conductor-like polarizable continuum model to account for the effects of solvents, was employed to predict the molecular parameters of the relevant species. Monitoring the wavenumbers and infrared absorbances attributed to the [S,O] species and accounting for the stoichiometry revealed SO2 to be the major oxygen-containing end product for the thermal decomposition of Cl2SO. Upon successive irradiation with 266 nm pulsed laser, the major product, as detected by IR absorption, was S2O with minor SO3, which could be generated from the secondary reactions of the photolytic intermediate ClSO. The majority of the transient vibrational features upon 266 nm irradiation of the mixture of Cl2SO/cHex was attributed to ClSO, characterized at 1155 cm-1, coupled with a minor contribution of (ClSO)2 at 1212 and 1173 cm-1. For the mixture of Cl2SO/THF/cHex, the transient population of ClSO was retained, but the amount of (ClSO)2 was slightly reduced, coupled with a new upward feature at 1054 cm-1 that was plausibly attributed to the C-O-C asymmetric stretching mode of ClSO-THF complex. Upon the successive irradiation of the Cl2SO/THF/cHex mixture, the amount of S2O was also decreased. The observed complexes of THF with solutes suggested that THF should not be merely treated as a solvent but regarded as a coordination molecule in organic synthesis. The formation of the intermediate-THF complexes altered the reaction pathways, as well as the types and populations of the end products.

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