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  • 10102-43-9 Structure
  • Basic information

    1. Product Name: Nitric oxide
    2. Synonyms: Amidogen,oxo-;INOmax;INOvent;Nitric oxide (NO);Nitrogen monooxide;Nitrogen monoxide;Nitrogen(II)oxide;Nitrosyl radical;OHM 11771;
    3. CAS NO:10102-43-9
    4. Molecular Formula: NO
    5. Molecular Weight: 30.01
    6. EINECS: 233-271-0
    7. Product Categories: N/A
    8. Mol File: 10102-43-9.mol
    9. Article Data: 652
  • Chemical Properties

    1. Melting Point: N/A
    2. Boiling Point: -151.7 °C(lit.)
    3. Flash Point: N/A
    4. Appearance: colourless gas turning brown upon exposure to air
    5. Density: 1.24 g/cmsup>3</sup>
    6. Refractive Index: N/A
    7. Storage Temp.: N/A
    8. Solubility: N/A
    9. CAS DataBase Reference: Nitric oxide(CAS DataBase Reference)
    10. NIST Chemistry Reference: Nitric oxide(10102-43-9)
    11. EPA Substance Registry System: Nitric oxide(10102-43-9)
  • Safety Data

    1. Hazard Codes: N/A
    2. Statements: N/A
    3. Safety Statements: N/A
    4. WGK Germany:
    5. RTECS:
    6. HazardClass: N/A
    7. PackingGroup: N/A
    8. Hazardous Substances Data: 10102-43-9(Hazardous Substances Data)

10102-43-9 Usage

Description

Nitric oxide, often denoted as NO, is a colorless gas that is important in various biological processes. This highly reactive molecule consists of one nitrogen atom and one oxygen atom; it is a free radical due to its unpaired electron. Nitric oxide is an essential cellular signaling molecule involved in numerous physiological and pathological processes in mammals, including vasodilation, immune response, and neurotransmission.

Uses

Used in Medical Applications:
Nitric oxide is used as a vasodilator for improving blood flow and reducing blood pressure. It is also used as an immune response modulator for enhancing the body's defense against infections and diseases.
Used in Pharmaceutical Applications:
Nitric oxide is used as a therapeutic agent for treating various health problems, such as erectile dysfunction, pulmonary hypertension, and certain cardiovascular conditions.
Used in Industrial Applications:
Nitric oxide is used as a chemical intermediate for the production of various industrial chemicals, such as nitric acid and fertilizers.
Used in Environmental Applications:
Nitric oxide is used as a pollutant control agent for reducing emissions of nitrogen oxides in industrial processes, such as combustion and automotive exhaust.
Used in Research Applications:
Nitric oxide is used as a research tool for studying the molecular mechanisms underlying various physiological and pathological processes, as well as for investigating the potential therapeutic applications of nitric oxide in various diseases and conditions.

Check Digit Verification of cas no

The CAS Registry Mumber 10102-43-9 includes 8 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 5 digits, 1,0,1,0 and 2 respectively; the second part has 2 digits, 4 and 3 respectively.
Calculate Digit Verification of CAS Registry Number 10102-43:
(7*1)+(6*0)+(5*1)+(4*0)+(3*2)+(2*4)+(1*3)=29
29 % 10 = 9
So 10102-43-9 is a valid CAS Registry Number.
InChI:InChI=1/NO/c1-2/q-1

10102-43-9SDS

SAFETY DATA SHEETS

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

Version: 1.0

Creation Date: Aug 12, 2017

Revision Date: Aug 12, 2017

1.Identification

1.1 GHS Product identifier

Product name nitric oxide

1.2 Other means of identification

Product number -
Other names NITRIC OXIDE

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:10102-43-9 SDS

10102-43-9Synthetic route

sodium nitrite
7632-00-0

sodium nitrite

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
With acetic acid; potassium iodide In water Product distribution / selectivity;100%
With sulfuric acid; water at 10℃; under 375.038 Torr; for 1.38889E-05h; Reagent/catalyst; Temperature; Pressure; Time;99.99%
With maleic acid; ascorbic acid In water Product distribution / selectivity;
hydrogen

hydrogen

Nitrogen dioxide
10102-44-0

Nitrogen dioxide

A

hydroxyl
3352-57-6

hydroxyl

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In neat (no solvent) introduction of NO2 into an rapid streaming mixture of H-He;; spectrometric determination of OH concentration;;A 100%
B n/a
In gaseous matrix Kinetics; in argon carrier under 0.7 torr; followed by infrared chemiluminescence spectroscopy;
In gas crossed molecular beam experiment; Laser fluorescence spectroscopy;
ammonia
7664-41-7

ammonia

oxygen
80937-33-3

oxygen

A

nitrogen
7727-37-9

nitrogen

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

C

dinitrogen monoxide
10024-97-2

dinitrogen monoxide

Conditions
ConditionsYield
With oxygen In neat (no solvent) Fe-ZSM-5 catalyst prepared by ion exchange and heat-treated at 400, 425or 450 °C, 100 % NH3 conversion, 100 % N2 selectivity, 1000 ppm NH3 in 2 % O2-contg. He;A 100%
B 0%
C 0%
With catalyst:Fe-mordenite In neat (no solvent) Fe-mordenite catalyst prepared by ion exchange and heat-treated at 425 °C, 92 % NH3 conversion, 99 % N2 selectivity, 1000 ppm NH3 in 2 %O2-contg. He;A 92%
B n/a
C 0%
With catalyst:Fe-ZSM-5 In neat (no solvent) Fe-ZSM-5 catalyst prepared by ion exchange and heat-treated at 375 °C, 90 % NH3 conversion, 99 % N2 selectivity, 1000 ppm NH3 in 2 % O2-contg. He;A 90%
B n/a
C 0%
C10H13NOS

C10H13NOS

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
With cobaltocene In fluorobenzene for 5h; Inert atmosphere;100%
magnesium nitrite

magnesium nitrite

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
With water; nitric acid at 20℃; under 75.0075 Torr; for 2.77778E-05h;99.99%
In water decompn. in concd. soln. already at cool;
In water decompn. in concd. soln. already at cool;
potassium nitrite
7758-09-0

potassium nitrite

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
With sulfuric acid; water at 20℃; under 375.038 Torr; for 2.22222E-05h; Pressure; Reagent/catalyst; Temperature; Time;99.98%
With sulfuric acid; potassium iodide In not given byproducts: H2O, I2; washing with NaOH soln.;
above 500 °C, based on spect. results;
ammonia
7664-41-7

ammonia

A

nitrogen
7727-37-9

nitrogen

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

C

dinitrogen monoxide
10024-97-2

dinitrogen monoxide

Conditions
ConditionsYield
With oxygen In neat (no solvent) Fe-mordenite catalyst prepared by ion exchange and heat-treated at 450 °C, 99 % NH3 conversion, 100 % N2 selectivity, 1000 ppm NH3 in 2 % O2-contg. He;A 99%
B 0%
C 0%
With oxygen; platinum high excess O2,500 °C;A <1
B n/a
C n/a
With oxygen; platinum at 300 °C;A n/a
B <9
C n/a
ammonia
7664-41-7

ammonia

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
With oxygen; platinum react. with air adding O2;99%
With oxygen; platinum optimal time of contact at very high temp.:some E-6 s;97%
With oxygen; Pt(90),Rh(10) (X%) 8 atm,high temp.;96%
methyl nitrite
624-91-9

methyl nitrite

carbon monoxide
201230-82-2

carbon monoxide

A

Dimethyl oxalate
553-90-2

Dimethyl oxalate

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
With 0.5% Pd/C at 100℃; under 375.038 Torr; for 0.000555556h; Pressure; Reagent/catalyst; Temperature; Time;A 98.9%
B n/a
ammonia
7664-41-7

ammonia

oxygen
80937-33-3

oxygen

A

nitrogen
7727-37-9

nitrogen

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
Sr0.22La0.78CoO2.843 In neat (no solvent) byproducts: H2O; 800°C;A n/a
B 98.6%
Sr0.42La0.68CoO2.80 In neat (no solvent) byproducts: H2O; 800°C;A n/a
B 98.1%
Sr0.46La0.54CoO2.79 In neat (no solvent) byproducts: H2O; 800°C;A n/a
B 98%
chloro(N,N'-ethylenebis(salicylideneiminato))iron(III)
16649-19-7, 38586-93-5

chloro(N,N'-ethylenebis(salicylideneiminato))iron(III)

bis(triphenylphosphoranylidene)ammonium nitrite

bis(triphenylphosphoranylidene)ammonium nitrite

A

(μ-oxo)bis[(1,2-ethanediamino-N,N'-bis(salicylidene))iron(III)]
18601-34-8

(μ-oxo)bis[(1,2-ethanediamino-N,N'-bis(salicylidene))iron(III)]

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In acetonitrile under vac., equimolar mixt.; chromy.;A n/a
B 98%
With water In acetonitrile under vac., equimolar mixt.; chromy.;A n/a
B 63%
ammonium nitrate

ammonium nitrate

A

nitrogen
7727-37-9

nitrogen

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

C

Nitrogen dioxide
10102-44-0

Nitrogen dioxide

D

dinitrogen monoxide
10024-97-2

dinitrogen monoxide

Conditions
ConditionsYield
at 220-260°C, nearly 98% N2O, 2% N2; troces of NO and NO2 (0.001%);A 2%
B n/a
C n/a
D 98%
nitrosyl hexafluorophosphate
16921-91-8

nitrosyl hexafluorophosphate

niobocene dichloride
12793-14-5

niobocene dichloride

A

(η5-C5H5)2niobium(V)(Cl2) hexafluoroantimonate

(η5-C5H5)2niobium(V)(Cl2) hexafluoroantimonate

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In liquid sulphur dioxide Reaction of Cp2NbCl2 with NOSbF6 in 1/1 molar ratio at room temp. under Ar.; sepn. of solvent and NO under vac., recrystn. (SO2), elem. anal.;A 98%
B n/a
nitrosonium tetrafluoroborate

nitrosonium tetrafluoroborate

palladium
7440-05-3

palladium

acetonitrile
75-05-8

acetonitrile

A

tetrakis(acetonitrile)palladium(II) bis(tetrafluoroborate)

tetrakis(acetonitrile)palladium(II) bis(tetrafluoroborate)

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In acetonitrile Pd sponge (1.0 g) and NOBF4 (2.2 g) stirred in MeCN (50 mL) under vac. for 12 h with periodical removing of NO generated during the react.; filtration; anhydrous ether added to the filtrate; resulting ppt. washed (anhydrous ether) and dried (vac.); elem. anal.;A 98%
B n/a
(N,N'-ethylenebis(salicylideneiminato))iron(III) nitrate
119030-00-1, 97337-05-8, 1228763-68-5

(N,N'-ethylenebis(salicylideneiminato))iron(III) nitrate

bis(triphenylphosphoranylidene)ammonium nitrite

bis(triphenylphosphoranylidene)ammonium nitrite

A

(μ-oxo)bis[(1,2-ethanediamino-N,N'-bis(salicylidene))iron(III)]
18601-34-8

(μ-oxo)bis[(1,2-ethanediamino-N,N'-bis(salicylidene))iron(III)]

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In acetonitrile under vac., equimolar mixt.; chromy.;A n/a
B 97%
trichlorothiophosphine
3982-91-0

trichlorothiophosphine

Nitrogen dioxide
10102-44-0

Nitrogen dioxide

A

OPSCl3(1+)

OPSCl3(1+)

B

NO*PSCl3(1+)

NO*PSCl3(1+)

C

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

D

oxygen

oxygen

Conditions
ConditionsYield
In gas Kinetics; High Pressure; the reagent ions were generated in an electron impact high-pressure ion source contg. NO2; the reagent ions were selected using a quadrupole mass filter before being injected into a drift region contg. helium carriergas; at 298 K; monitoring by quadrupole mass spectrometer at the end of the flow tube;A 97%
B 3%
C n/a
D n/a
C49H66O5*NO(1+)
1012315-99-9

C49H66O5*NO(1+)

A

C49H64O5
518981-39-0

C49H64O5

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
With tert.-butylnitrite; trifluoroacetic acid In chloroform Inert atmosphere;A 95%
B 97%
tetra-n-butylammonium tetramethylaurate(III)

tetra-n-butylammonium tetramethylaurate(III)

A

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
With [NO(1+),HMB]BF4(1-) In acetonitrile byproducts: CH4, C2H6;A 96%
B n/a
niobocene dichloride
12793-14-5

niobocene dichloride

nitrosonium tetrafluoroborate

nitrosonium tetrafluoroborate

A

(η5-C5H5)2niobium(V)(Cl2) tetrafluoroborate

(η5-C5H5)2niobium(V)(Cl2) tetrafluoroborate

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In liquid sulphur dioxide Reaction of Cp2NbCl2 with NOBF4 in 1/1 molar ratio at room temp. under Ar.; sepn. of solvent and NO under vac., recrystn. (SO2), elem. anal.;A 96%
B n/a
tetra-n-butylammonium tetramethylaurate(III)

tetra-n-butylammonium tetramethylaurate(III)

triphenylphosphine
603-35-0

triphenylphosphine

trimethyl(triphenylphosphine)gold(III)

trimethyl(triphenylphosphine)gold(III)

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
With [NO(1+),HMB]BF4(1-) In acetonitrileA 94%
B 96%
silver(I) nitrite
7783-99-5

silver(I) nitrite

(N,N'-ethylenebis(salicylideneiminato))iron(III) nitrate
119030-00-1, 97337-05-8, 1228763-68-5

(N,N'-ethylenebis(salicylideneiminato))iron(III) nitrate

A

(μ-oxo)bis[(1,2-ethanediamino-N,N'-bis(salicylidene))iron(III)]
18601-34-8

(μ-oxo)bis[(1,2-ethanediamino-N,N'-bis(salicylidene))iron(III)]

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In acetonitrile under vac., equimolar mixt.; chromy.;A n/a
B 95%
[Cu(bis(6-methyl-2-pyridylmethyl)amine)(NO2)]2[((C6H5)3P)2N](PF6)

[Cu(bis(6-methyl-2-pyridylmethyl)amine)(NO2)]2[((C6H5)3P)2N](PF6)

trifluoroacetic acid
76-05-1

trifluoroacetic acid

A

[Cu(bis(6-methyl-2-pyridylmethyl)amine)](CF3COO)2

[Cu(bis(6-methyl-2-pyridylmethyl)amine)](CF3COO)2

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In dichloromethane Kinetics; CF3COOH soln. added; UV;A n/a
B 95%
(2,6-(Ph2P(o-C6H4)CH=N)2C5H3N)Cu(NO2)

(2,6-(Ph2P(o-C6H4)CH=N)2C5H3N)Cu(NO2)

acetic acid
64-19-7

acetic acid

A

(2,6-(Ph2P(o-C6H4)CH=N)2C5H3N)Cu(OAc)2

(2,6-(Ph2P(o-C6H4)CH=N)2C5H3N)Cu(OAc)2

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In dichloromethane gas chromy.;A n/a
B 95%
1-Adamantanethiol
34301-54-7

1-Adamantanethiol

[Cl2NNF6]Cu(κ2-O2N)*THF

[Cl2NNF6]Cu(κ2-O2N)*THF

A

[Cl2NNF6]Cu(AdS-SAd)

[Cl2NNF6]Cu(AdS-SAd)

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In diethyl ether at 20℃; for 0.25h; Solvent;A 95%
B n/a
ferrocenium(III) tetrafluoroborate
1282-37-7

ferrocenium(III) tetrafluoroborate

triphenylmethanethiol
3695-77-0

triphenylmethanethiol

Fe4H2N8O8S2(2-)

Fe4H2N8O8S2(2-)

A

Roussin’s black salt

Roussin’s black salt

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
With [PPN]2[S5Fe(μ-S)2FeS5] In tetrahydrofuran; acetonitrile at 20℃; for 12h; Inert atmosphere; Schlenk technique;A 92%
B n/a
vanadium
7440-62-2

vanadium

dinitrogen tetroxide
15969-55-8

dinitrogen tetroxide

A

vanadium nitrate
15053-24-4

vanadium nitrate

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In acetonitrile acceleration with acetonitrile at o°C;;A 91%
B n/a
nitric acid
7697-37-2

nitric acid

silver
7440-22-4

silver

hydrogen cation

hydrogen cation

A

silver (I) ion
14701-21-4

silver (I) ion

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In perchloric acid byproducts: H2O; nitric acid soln. addn. to Ag suspn. at 30-40°C, mixt. keeping at tis temp. for 15 min;A n/a
B 90%
(N,N'-ethylenebis(salicylideneiminato))iron(III) nitrate
119030-00-1, 97337-05-8, 1228763-68-5

(N,N'-ethylenebis(salicylideneiminato))iron(III) nitrate

sodium nitrite
7632-00-0

sodium nitrite

A

(μ-oxo)bis[(1,2-ethanediamino-N,N'-bis(salicylidene))iron(III)]
18601-34-8

(μ-oxo)bis[(1,2-ethanediamino-N,N'-bis(salicylidene))iron(III)]

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In acetonitrile under vac., equimolar mixt.; chromy.;A n/a
B 90%
bis{octakis(dodecyloxy)phthalocyaninato}lutetium
122744-29-0

bis{octakis(dodecyloxy)phthalocyaninato}lutetium

nitrosonium tetrafluoroborate

nitrosonium tetrafluoroborate

A

2(C12H25O)8C32H8N8(2-)*Lu(5+)*BF4(1-)={(C12H25O)8C32H8N8}2LuBF4
122873-81-8

2(C12H25O)8C32H8N8(2-)*Lu(5+)*BF4(1-)={(C12H25O)8C32H8N8}2LuBF4

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Conditions
ConditionsYield
In dichloromethane evapn., dissolved in heptane, filtered, recrystn. (ethyl acetate); elem. anal.;A 90%
B n/a
copper(II)-hyponitrite

copper(II)-hyponitrite

A

nitrogen
7727-37-9

nitrogen

B

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

C

copper(II) oxide

copper(II) oxide

D

dinitrogen monoxide
10024-97-2

dinitrogen monoxide

Conditions
ConditionsYield
In neat (no solvent) decompn. at 225-230°C;;A 2-6
B 3-5
C n/a
D 90%
In neat (no solvent) decompn. at 225-230°C;;A 2-6
B 3-5
C n/a
D 90%
nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

nitrogen
7727-37-9

nitrogen

Conditions
ConditionsYield
With Pd supported ZrO2-CeO2 catalyst at 175 - 400℃; for 1h; Reagent/catalyst; Temperature; Inert atmosphere;100%
With H2; O2; catalyst: 0.1 wtpercent Pt/La0.7Sr0.2Ce0.1FeO3 In neat (no solvent, gas phase) Kinetics; NO:H2:O2 = 1:0.25:5% gas mixt. with 5% H2O added in feed stream; at 140°C for 20 h; H2O as reagent; detd. by mass spectrometry, gas chromy.;93%
With (Y0.90Pr0.10)2O(3+x) at 900℃; Temperature; Inert atmosphere;79%
carbon monoxide
201230-82-2

carbon monoxide

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

cobalt(II) iodide

cobalt(II) iodide

cobalt tricarbonyl nitrosyl

cobalt tricarbonyl nitrosyl

Conditions
ConditionsYield
In neat (no solvent) 85 atm CO, 15 atm NO, 200°C;;100%
nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

cobalt(II) iodide

cobalt(II) iodide

Co(1-)*I(1-)*2NO(1+)=[CoI(NO)2]

Co(1-)*I(1-)*2NO(1+)=[CoI(NO)2]

Conditions
ConditionsYield
In neat (no solvent) 105°C, humidity as catalyst;; sublimation in N2-stream at 115°C;;100%
In neat (no solvent) 105°C, humidity as catalyst;; sublimation in N2-stream at 115°C;;100%
In ethanol
In ethanol
carbon monoxide
201230-82-2

carbon monoxide

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

cobalt(II) bromide

cobalt(II) bromide

cobalt tricarbonyl nitrosyl

cobalt tricarbonyl nitrosyl

Conditions
ConditionsYield
In neat (no solvent) 85 atm CO, 15 atm NO, 200°C;;100%
nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

barium(II) hydroxide

barium(II) hydroxide

barium nitrite monohydrate

barium nitrite monohydrate

Conditions
ConditionsYield
1.5h, 250°C; at room temp. slowly;100%
1.5h, 250°C; at room temp. slowly;100%
With oxygen In water
With oxygen In water
nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

cobalt(II) iodide

cobalt(II) iodide

dinitrosyl cobalt(-I) iodide

dinitrosyl cobalt(-I) iodide

Conditions
ConditionsYield
In neat (no solvent) 2g dried CoI2 at 105°C reacts with NO gas during 15-20 h;; sublimation in N2 stream at 115°C;;100%
In neat (no solvent) byproducts: I2; 70-80°C;;
With copper In neat (no solvent) at 140°C;;0%
With nickel In neat (no solvent)
Fe(tetraphenylporphyrinate)C6H5
70936-44-6

Fe(tetraphenylporphyrinate)C6H5

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

{(C20H8(C6H5)4N4)Fe(C6H5)(NO)}
89672-69-5

{(C20H8(C6H5)4N4)Fe(C6H5)(NO)}

Conditions
ConditionsYield
reaction of a solid complex in NO atm. or a soln. of complex in toluenesaturated with NO at -28°C;100%
In neat (no solvent) exposure of degassed solid ((C20H8(C6H5)4N4)Fe(C6H5)) to 1 atm of nitric oxide;; elem. anal.;;>99
(η5-indenyl)(η1-phenylacetylide)bis(triphenylphosphine)ruthenium

(η5-indenyl)(η1-phenylacetylide)bis(triphenylphosphine)ruthenium

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

A

((η5-indenyl)(carbonyl)bis(triphenylphosphine)ruthenium) perchlorate * 0.5CH2Cl2

((η5-indenyl)(carbonyl)bis(triphenylphosphine)ruthenium) perchlorate * 0.5CH2Cl2

B

benzonitrile
100-47-0

benzonitrile

Conditions
ConditionsYield
With NaClO4; CH2Cl2 In dichloromethane room temp., 15 min;A 80%
B 100%
With CH2Cl2 In dichloromethane room temp., 15 min;A n/a
B 73%
[UIII(2,6-Ad-4-Me-C6H2O)3]

[UIII(2,6-Ad-4-Me-C6H2O)3]

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

[(2,6-Ad-4-Me-C6H2O)3UV(O)]

[(2,6-Ad-4-Me-C6H2O)3UV(O)]

Conditions
ConditionsYield
In neat (no solvent) under 760.051 Torr; for 0.166667h;100%
[Rh(C6H(CH3)2(CH2P(tert-butyl)2)2)(NO)]•

[Rh(C6H(CH3)2(CH2P(tert-butyl)2)2)(NO)]•

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

C26H47N2O3P2Rh

C26H47N2O3P2Rh

Conditions
ConditionsYield
In benzene Inert atmosphere;100%
[(1,3-bis[(di-tert-butylphosphino)methyl)-4,6-dimethylbenzene(-1H))Rh(N2)]
277309-56-5

[(1,3-bis[(di-tert-butylphosphino)methyl)-4,6-dimethylbenzene(-1H))Rh(N2)]

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

C26H47N2O3P2Rh

C26H47N2O3P2Rh

Conditions
ConditionsYield
In tetrahydrofuran Inert atmosphere;100%
hydrogen
1333-74-0

hydrogen

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Nitrogen dioxide
10102-44-0

Nitrogen dioxide

ammonia
7664-41-7

ammonia

Conditions
ConditionsYield
With catalyst: Ni(2+)Y zeolite In neat (no solvent) reduction of very dild. mixt. of NO/NO2 in gas mixt. of N2/H2 on zeolite catalyst (300°C reaction temp.); gas chromy. (dimethylsulfolane coated diatomite);99%
With catalyst: industrial nickel methanation catalyst In neat (no solvent) reduction of very dild. mixt. of NO/NO2 in gas mixt. of N2/H2 on zeolite catalyst (300°C reaction temp.); gas chromy. (dimethylsulfolane coated diatomite);99%
With catalyst: phthalocyanineNiY zeolite In neat (no solvent) reduction of very dild. mixt. of NO/NO2 in gas mixt. of N2/H2 on zeolite catalyst (230°C reaction temp.); gas chromy. (dimethylsulfolane coated diatomite);94%
With catalyst: NiY zeolite In neat (no solvent) reduction of very dild. mixt. of NO/NO2 in gas mixt. of N2/H2 on zeolite catalyst (450°C reaction temp.); gas chromy. (dimethylsulfolane coated diatomite);84%
[(1,1',2,2'-bisdiphenylphosphinoethylene)Pt(CF3)(OOH)]

[(1,1',2,2'-bisdiphenylphosphinoethylene)Pt(CF3)(OOH)]

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

[(1,1',2,2'-bisdiphenylphosphinoethylene)Pt(CF3)(NO2)]
79299-90-4

[(1,1',2,2'-bisdiphenylphosphinoethylene)Pt(CF3)(NO2)]

Conditions
ConditionsYield
In tetrahydrofuran byproducts: HNO2;99%
In tetrahydrofuran; diethyl ether suspended in THF/Et2O mixture, evacuated and saturated with NO, stirredat 25°C for 1.5 h, N2 bubbled; filtered, washed with Et2O, dried, recrystd. from CH2Cl2/MeOH;
aquapentacyanoferrate(III)

aquapentacyanoferrate(III)

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

pentacyanonitrosylferrate(III)

pentacyanonitrosylferrate(III)

Conditions
ConditionsYield
With perchloric acid; sodium perchlorate In water Kinetics; byproducts: H2O; HClO4 was added to soln. of Fe complex in aq. NaClO4 to pH 3; soln. was deoxygenated with N2; NO was bubbled; UV monitoring;99%
With perchloric acid; sodium perchlorate; sodium thiocyanide In perchloric acid; water Kinetics; deoxygenated soln. of NaSCN in aq. HClO4 was satd. with NO and mixed with deoxygenated soln. of Fe complex in aq. NaClO4 (pH 3) at 25°C; UV monitoring;
With 1,4-pyrazine; perchloric acid; sodium perchlorate In perchloric acid; water Kinetics; deoxygenated soln. of pyrazine in aq. HClO4 was satd. with NO and mixed with deoxygenated soln. of Fe complex in aq. NaClO4 (pH 3) at 25°C; UV monitoring;
[CuI(tris(2-pyridylmethyl)amine)(CH3CN)]2+
114581-86-1

[CuI(tris(2-pyridylmethyl)amine)(CH3CN)]2+

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

A

[Cu(tris(2-pyridylmethyl)amine)(H2O)](2+)
133578-96-8

[Cu(tris(2-pyridylmethyl)amine)(H2O)](2+)

B

dinitrogen monoxide
10024-97-2

dinitrogen monoxide

Conditions
ConditionsYield
In water room temp., pH = 7.0; reaction followed by gas chromy.;A 99%
B n/a
[(1,1',2,2'-bisdiphenylphosphinoethane)Pt(CF3)(OOH)]

[(1,1',2,2'-bisdiphenylphosphinoethane)Pt(CF3)(OOH)]

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

[(1,1',2,2'-bisdiphenylphosphinoethane)Pt(CF3)(NO2)]

[(1,1',2,2'-bisdiphenylphosphinoethane)Pt(CF3)(NO2)]

Conditions
ConditionsYield
In tetrahydrofuran byproducts: HNO2;99%
trans-[(PPh2Me)2Pt(CF3)(OOH)]
79355-45-6

trans-[(PPh2Me)2Pt(CF3)(OOH)]

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

((C6H5)2PCH3)2Pt(CF3)NO2

((C6H5)2PCH3)2Pt(CF3)NO2

Conditions
ConditionsYield
In tetrahydrofuran byproducts: HNO2;99%
nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Cr(diisopropylamido)3

Cr(diisopropylamido)3

Cr(NO)(N(i)Pr2)3

Cr(NO)(N(i)Pr2)3

Conditions
ConditionsYield
In diethyl ether reaction at 25°C;99%
[(η(3)-cyclooctenyl)Co(Pr(i)2PCH2CH2PPr(i)2)](+)BF4(-)
205433-03-0

[(η(3)-cyclooctenyl)Co(Pr(i)2PCH2CH2PPr(i)2)](+)BF4(-)

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

[(η(3)-cyclooctenyl)Co(Pr(i)2PCH2CH2PPr(i)2)NO](+)BF4(-)
205446-13-5

[(η(3)-cyclooctenyl)Co(Pr(i)2PCH2CH2PPr(i)2)NO](+)BF4(-)

Conditions
ConditionsYield
In acetone Ar-atmosphere; excess NO, 4 h; collection (filtration), washing (Et2O), drying (vac.); elem. anal.;99%
[Ru2(N,N′-diphenylformamidinate)4]

[Ru2(N,N′-diphenylformamidinate)4]

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Ru2(N,N'-diphenylformamidinate)4(NO)2

Ru2(N,N'-diphenylformamidinate)4(NO)2

Conditions
ConditionsYield
In further solvent(s) NO passed for 30 min through a CH2Cl2/tetra-n-butylammonium perchlorate soln. of Ru complex; the soln. purged with N2 until dry, washed (acetone); elem. anal.;99%
Cr(N(C(C(2)H3)2CH3)(C6H3(CH3)2))3

Cr(N(C(C(2)H3)2CH3)(C6H3(CH3)2))3

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Cr(N(C(C(2)H3)2CH3)(C6H3(CH3)2))3NO

Cr(N(C(C(2)H3)2CH3)(C6H3(CH3)2))3NO

Conditions
ConditionsYield
In diethyl ether reaction at 25°C;99%
[Cr(N(C6H3FCH3)C(CH3)(C(2)H3)2)3]

[Cr(N(C6H3FCH3)C(CH3)(C(2)H3)2)3]

nitrogen(II) oxide
10102-43-9

nitrogen(II) oxide

Cr(N(C(C(2)H3)2CH3)(C6H3(CH3)F))3NO

Cr(N(C(C(2)H3)2CH3)(C6H3(CH3)F))3NO

Conditions
ConditionsYield
In diethyl ether reaction at 25°C;99%

10102-43-9Relevant articles and documents

Photodissociation of NO2 Adsorbed on LiF(001)

Dixon-Warren, St. J.,Jackson, R. C.,Polanyi, J. C.,Rieley, H.,Shapter, J. G.,Weiss, H.

, p. 10983 - 10994 (1992)

The photochemistry of NO2 physisorbed on single-crystal LiF(001) at 100 K has been studied at λ1 = 248 nm.The adsorbate was examined by polarized FTIR in both the presence and absence of λ1 radiation.In the absence of UV irradiation the adlayer is composed of dimeric (NO2)2.In the presence of UV, FTIR shows that some N2O3 is formed.Photodissociations(PDIS) giving both NO(g) and molecular NO2(g) were the predominant mechanisms as determined by time-of-flight mass spectrometry (TOF-MS) and resonantly enhanced multiphoton ioniziation (REMPI).The main objective of this work was the characterization of the photoproduct, NO, internal state distribution by 1 + 1 REMPI.Vibrational levels from v = 0 to 9 were probed with rotational resolution using a tunable laser, λ2.The rotational distributions for each vibrational level could be described by one Boltzmann temperature.The spin-orbit states of NO(g) were equally populated in all vibrational levels.The lambda doublet states, Π(A') and Π(A ), were equally populated.The principal observation was that the vibrational distribution in NO(g) was inverted and bimodal with a peak in v = 0 and a second substantial peak in v = 3-4, qualitatively resembling but qualitatively different from that for photolysis of NO2(g).Time delays between the two lasers were used to probe the translational energy of the NO(g) photofragment in specified states of internal excitation.The transational energy distributions were invariant over all vibrational levels, except v = 0 for which much slower fragments were observed.This complete determination of the energy distribution in the degrees of freedom of the NO(g) from photodissociation of adsorbate has implications for the identity of the photolyzing species and the dynamics of photodissociation.Two mechanisms for photoformation of NO2(g) were found: one at low coverages and one at higher coverages, the former giving peak translational energies ca. 1.2 kcal/mol and the latter 0.4 kcal/mol.

A laser flash photolysis study of nitrous acid in the aqueous phase

Ouyang, Bin,Dong, Wenbo,Hou, Huiqi

, p. 306 - 311 (2005)

The OH quantum yield from the photolysis of nitrous acid in the aqueous phase by the 355 nm light was measured to be 0.25 ± 0.03. OH radical thus formed reacted readily with HNO2 to produce NO2, which sequentially reacted with HNO2 to form the HNO2-NO 2 adduct. The NO2 + HNO2 reaction was reversible with a forward rate constant of 3.76 × 107 dm 3 mol-1 s-1 and a backward rate constant of 1.06 × 105 s-1. Decay of the HNO2-NO 2 adduct would most likely generate HNO3 and NO at a rate constant of 3.0 × 103 s-1.

Photolysis of the (2-) Ion in Water and Poly(vinyl alcohol) Films: Evidence for Cyano Radical, Cyanide Ion and Nitric Oxide Loss and Redox Pathways

Oliveira, Marcelo G. de,Langley, G. John,Rest, Antony J.

, p. 2013 - 2020 (1995)

Ultraviolet-visible and IR spectroscopy and mass spectrometry have been used to investigate photolysis of the (2-) ion upon irradiation with UV/VIS light in aqueous solutions and in poly(vinyl alcohol) films at 12 and 298 K.Changes in the ν(CN) and ν(NO) bands in the IR and in the d-d and charge-transfer bands in the UV/VIS region were used to monitor the appearance and disappearance of complex ions as a function of photolysis time.Mass spectrometric analysis of the gaseous products released during the irradiation of aqueous solutions revealed NO, HCN, and (CN)2.The combined results showed that the (2-) ion undergoes photoaquation and photoreduction, producing aquacyanoferrate-(III) and -(II) species.The origin of the iron(II) species was shown to be mainly due to the photoreduction of the iron(III) species produced after primary loss of the nitrosyl ligand as molecular NO and not as NO(1+).Subsequent thermal reactions between the iron-(II) and -(III) species led to the formation of mixed-valence compounds, e.g.Prussian blue.A scheme for the photochemical and thermal reactions with CN(.), CN(1-) and NO loss pathways is proposed.The possible implications of the results for the use of (2-) as a vasodilator are discussed.

Ray, P. C.

, p. 523 - 527 (1904)

Widely differing photochemical behavior in related octahedral {Ru-NO} 6 compounds: Intramolecular redox isomerism of the excited state controlling the photodelivery of NO

De Candia, Ariel G.,Marcolongo, Juan P.,Etchenique, Roberto,Slep, Leonardo D.

, p. 6925 - 6930 (2010)

trans-[(NC)Ru(py)4(μ-CN)Ru(py)4(NO)]3+ (py = pyridine) is a stable species in aqueous solution. It displays an intense absorption in the visible region of the spectrum (λmax = 518 nm; εmax = 6100 M-1 cm-1), which turns this compound into a promising agent for the photodelivery of NO. The quantum yield for the photodelivery process resulting from irradiation with 455 nm visible light was found experimentally to be (0.06 ± 0.01)×10 -3 mol einstein-1, almost 3 orders of magnitude smaller than that in the closely related cis-[RuL(NH3)4(μ-pz) Ru(bpy)2(NO)]5+ species (L = NH3 or pyridine, pz = pyrazine, bpy = 2,2′-bipyridine; φNO = 0.02-0.04 mol einstein-1 depending on L) and also much smaller than the one in the mononuclear compound trans-[ClRu(py)4(NO)]2+ (φNO = (1.63 ± 0.04)×10-3 mol einstein-1). DFT computations provide an electronic structure picture of the photoactive excited states that helps to understand this apparently abnormal behavior.

Randeniya, Lakshman K.,Zeng, Xiangkang,Smith, M. A.

, p. 346 - 352 (1988)

Scott, D. C.,Winterbottom, F.,Scholefield, M. R.,Goyal, S.,Reisler, H.

, p. 471 - 480 (1994)

State-resolved photofragmentation of [ClNO]n van der Waals clusters in a supersonic jet

Conde, Carlos,Maul, Christof,Quinones, Edwin

, p. 1929 - 1938 (1999)

The effects of the ultraviolet laser irradiation of [ClNO]2, weakly bound clusters, formed in a supersonic jet, are analyzed by considering three processes: the photofragmentation of bare ClNO, the Cl+ClNO reaction, and NO relaxation within the cluster. The photofragmentation of jet-cooled ClNO at 355 nm produces NO (υ″ = 1) with a kinetic energy of 2240 cm-1, a spin-orbit preference of F1/F2 = 1.2, and Λ-doublet state preferences of Π(A″)/Π±(A″) = 2.0 and 4.0 for the F1 and F2 manifolds, respectively. The NO distribution of rotational states was parametrized using a Gaussian function centered at N = 34, with a fwhm of 17. On the other hand, the Cl+ClNO reaction, studied at a collision energy of 2780 cm-1, gives NO(υ″ = 1) described by a Boltzmann rotational distribution with Trot = 950±100 K. The relative population of the NO spin-orbit states is F1/F2 = 2.5, with a Λ-doublet state preference of Π(A″)/Π(A′) = 1.2 and Etrans(NO) of 578 cm-1. It is found that 57% of available energy is disposed as Eint(Cl2). As a result of the irradiation of the [ClNO]n, clusters at 355 nm are observed: Boltzmann ensembles of NO(υ″ = 1) and NO(υ″ = 0) molecules described by Trot of 310±30 and 170±25 K, respectively, with no spin-orbit or Λ-doublet state preferences, overlapped with a Gaussian distribution already assigned to the NO photofragment. The relative contribution of the NO(υ″ = 1) photofragment to the spectra is drastically reduced upon increasing the backing pressure, as it undergoes translational and rotational relaxation within the clusters. Our high-resolution studies provide evidence that suggests that the reaction takes place within the [ClNO]n clusters.

Wu, Yue,Yu, Tao,Dou, Bo-Sheng,Wang, Cheng-Xian,Xie, Xiao-Fan,et al.

, p. 88 - 107 (1989)

Laser Photolysis Studies of Nitric Oxide Adducts of Cobalt(II) Porphyrins. Photoinduced Denitrosylation at the Temperature Range 160-300 K

Hoshino, Mikio,Arai, Shigeyoshi,Yamaji, Minoru,Hama, Yoshimasa

, p. 2109 - 2111 (1986)

Laser photolysis studies reveal that nitric oxide cobalt(II) porphyrins in 2-methyltetrahydrofuran solutions undergo facile photolytic dissociation to yield nitric oxide and cobalt(II) porphyrin.The quantum yields for the photodissociation of nitric oxide

Henry, L.

, p. 498 (1934)

Production of reactive oxygen and nitrogen species by light irradiation of a nitrosyl phthalocyanine ruthenium complex as a strategy for cancer treatment

Heinrich, Tassiele A.,Tedesco, Antonio Claudio,Fukuto, Jon M.,Da Silva, Roberto Santana

, p. 4021 - 4025 (2014)

Production of reactive oxygen species has been used in clinical therapy for cancer treatment in a technique known as Photodynamic Therapy (PDT). The success of this therapy depends on oxygen concentration since hypoxia limits the formation of reactive oxygen species with consequent clinical failure of PDT. Herein, a possible synergistic effect between singlet oxygen and nitric oxide (NO) is examined since this scenario may display increased tumoricidal activity. To this end, the trinuclear species [Ru(pc)(pz)2{Ru(bpy) 2(NO)}2](PF6)6(I) (pc = phthalocyanine; pz = pyrazine; bpy = bipyridine) was synthesized to be a combined NO and singlet oxygen photogenerator. Photobiological assays using (I) at 4 × 10-6 M in the B16F10 cell line result in the decrease of cell viability to 21.78 ± 0.29% of normal under light irradiation at 660 nm. However, in the dark and at the same concentration of compound (I), viability was 91.82 ± 0.37% of normal. The potential application of a system like (I) in clinical therapy against cancer may be as an upgrade to normal photodynamic therapy.

Two-photon spectroscopy of the low lying Rydberg states of NO. I. The 3p and 3d complexes

Meyer, Henning

, p. 7721 - 7731 (1997)

The rotational structure and polarization dependence of two-photon spectra of aligned ensembles of open shell diatomics is investigated in terms of the spherical tensor components of the two-photon absorption operator. The formalism allows the straightforward incorporation of state interactions and perturbations. It is applied to the two-photon spectroscopy of NO, in particular to the excitation of the Rydberg states derived from the 3p and 3d complexes. All states investigated show a nearly quadratic power dependence indicating the saturation of the ionization step. Transitions dominated by a zeroth rank tensor component (e.g., C 2Π-X 2Π or H 2Σ, H′ 2Π-X 2Π) are insensitive to a possible angular momentum alignment in the ensemble. These transitions are ideally suited to determine degeneracy averaged observables, e.g., collision cross sections in a molecular beam scattering experiment or product velocity anisotropies in a single color photodissociation experiment. Rotational alignment data must be determined using two-photon transitions which are carried by a second rank tensor component (e.g., D 2Σ-X 2Π or F 2Δ-X 2Π).

Nitric Oxide Reacts Very Fast with Hydrogen Sulfide, Alcohols, and Thiols to Produce HNO: Revised Rate Constants

Neuman, Nicolas I.,Venancio, Mateus F.,Rocha, Willian R.,Bikiel, Damian E.,Suárez, Sebastián A.,Doctorovich, Fabio

, p. 15997 - 16007 (2021)

The chemical reactivity of NO and its role in several biological processes seem well established. Despite this, the chemical reduction of ?NO toward HNO has been historically discarded, mainly because of the negative reduction potential of NO. However, this value and its implications are nowadays under revision. The last reported redox potential, E′(NO,H+/HNO), at micromolar and picomolar concentrations of ?NO and HNO, respectively, is between -0.3 and 0 V at pH 7.4. This potential implies that the one-electron-reduction process for NO is feasible under biological conditions and could be promoted by well-known biological reductants with reduction potentials of around -0.3 to -0.5 V. Moreover, the biologically compatible chemical reduction of ?NO (nonenzymatic), like direct routes to HNO by alkylamines, aromatic and pseudoaromatic alcohols, thiols, and hydrogen sulfide, has been extensively explored by our group during the past decade. The aim of this work is to use a kinetic modeling approach to analyze electrochemical HNO measurements and to report for the first-time direct reaction rate constants between ?NO and moderate reducing agents, producing HNO. These values are between 5 and 30 times higher than the previously reported keff values. On the other hand, we also showed that reaction through successive attack by two NO molecules to biologically compatible compounds could produce HNO. After over 3 decades of intense research, the ?NO chemistry is still there, ready to be discovered.

Ashmore, P. G.,Burnett, M. G.

, p. 1315 - 1324 (1961)

Kinetic Study of the Equilibrium HO2 + NO OH + NO2 and the Thermochemistry of HO2

Howard, Carleton J.

, p. 6937 - 6941 (1980)

Rate constants for the reactions HO2 + NO -> NO2 (kF) and OH + NO2 -> HO2 + NO (kR) have been measured at high temperatures by using laser magnetic resonance ddtection of HO2 and OH reactants in a flow tube reactor.The results are kF(T) = (3.51 +/- 0.35) * 10-12 exp cm3 molecule-1 s-1 for 232 R(T) = (3.03 +/- 0.60) * 10-11 exp cm3 molecule-1 s-1 for 452 = 2.5 +/- 0.6 kcal mol-1.Other measurements of this quantity and the thermochemistry of HO2 are discussed.

Divers, E.,Haga, T.

, p. 48 (1887)

Synthesis, characterization and photochemical properties of some ruthenium nitrosyl complexes

Kumar, Amit,Pandey, Rampal,Gupta, Rakesh Kumar,Ghosh, Kaushik,Pandey, Daya Shankar

, p. 837 - 843 (2013)

Synthesis of new nitrosyl complexes [RuCl3(CNPy) 2(NO)] (1), [RuCl3(AMPy)2(NO)] (2), [RuCl 3(CPI)2(NO)] (3), [RuCl3(NOPI)2(NO)] (4), and [RuCl3(HPI)2/

Black, G.,Sharpless, R. L.,Slanger, T. G.

, p. 55 - 58 (1982)

Ogai, A.,Qian, C. X. W.,Iwata,L.,Reisler, H.

, p. 367 - 374 (1988)

Selective Catalytic Reduction of Nitric Oxide with Ammonia on MFI-Type Ferrisilicate

Uddin, Md. Azhar,Komatsu, Takayuki,Yashima, Tatsuaki

, p. 3275 - 3280 (1995)

The catalytic properties of framework Fe(3+) in MFI-type H-ferrisilicate for the selective reduction of nitric oxide with ammonia in the presence of oxygen have been investigated and compared with those of Fe-exchanged ZSM-5, iron oxide supported on silicalite and HZSM-5.H-ferrisilicate exhibited a high activity and selectivity for the reduction of nitric oxide into nitrogen.A side reaction, i.e. the oxidation of ammonia with oxygen into nitrogen, occured only above 773 K.The activity and selectivity of Fe-exchanged ZSM-5 for the reduction of nitric oxide were comparable to those of H-ferrisilicate, while iron oxide supported on silicalite catalysed the oxidation of ammonia with oxygen into nitric oxide preferentially under the same reaction conditions.The catalytic activity of HZSM-5 for this reaction was much lower than that of H-ferrisilicate.Therefore, the framework Fe(3+) ions in H-ferrisilicate are the active sites for the selective catalytic reduction of nitric oxide.

Kinetics of SH with NO2, O3, O2, and H2O2

Friedl, Randall R.,Brune, William H.,Anderson, James G.

, p. 5505 - 5510 (1985)

A low pressure (1-8 torr of He) discharge flow reactor with (a) LIF detection of SH using a high repetition rate (20 kHz) metal atom laser to circumvent severe predissociation of the A2Σ+ state and (b) resonance fluorescence detection of OH has been used to examine the kinetics of the title reactions at 298 K: SH + NO2 -> HSO + NO, k1=(3.0+/-0.8)x10-11 cm3s-1; SH + O3 -> HSO + O2,k2 = (3.2+/- 1.0)x10-12cm3s-1;SH + O2 -> SO + OH,k3 -17 cm3s-1;SH + H2O2 -> H2S + HO2,k4a;SH + H2O2 -> HSOH + OH,k4b;SH + H2O2 -> HSO + H2O,k4c. k4=k4a+k4b+k4c-15 cm3s-1.Regeneration of SH in reaction 2 by HSO + O3 is observed and is used to infer a rate constant for HSO + O3 -> products of (1.0+/-0.4)x10-13cm3s-1.Absence of OH production in that reaction implies that the primary products are SH + 2O2.Isotope experiments with H2S replaced by D2S substantiate that conclusion and yield a reaction rate constant for DSO + O3 -> SD + 2O2 of 9x10-14 cm3s-1.Brief discussions of SH reactivity compared with OH and Br are offered, as well as a summary of the atmospheric chemistry of SH.

Photochemical and pharmacological aspects of nitric oxide release from some nitrosyl ruthenium complexes entrapped in sol-gel and silicone matrices

de Lima, Renata Galv?o,Sauaia, Marilia Gama,Ferezin, Camila,Pepe, Iuri Muniz,José, Nádia Mamede,Bendhack, Lusiane M.,da Rocha, Zênis Novais,da Silva, Roberto Santana

, p. 4620 - 4624 (2007)

The entrapped [Ru(terpy)(L)NO](PF6)3, where terpy = 2,2′:6′,2″-terpyridine and L = 2,2′-bipyridine (bpy) and 3,4-diiminebenzoic acid (NH · NHq) complexes into sol-gel processed polysiloxane and silicone matrices, shows NO release characteristics when submitted to light irradiation at 355 and 532 nm, as judged by NO measurement using a NO-sensor electrode. The pharmacological properties of doped matrix showed vasodilator characteristics by visible light irradiation, which is of great interest because the target delivery system can avoid the occurrence of side effects possibly by the aquo ruthenium species. All matrices obtained showed to be amorphous materials. The scanning electron micrographs of the matrices showed irregularly shaped particles, with a broad size of 1000 μm for both matrices and homogeneous distribution.

O-Atom Yields from Microwave Discharges in N2O/Ar Mixtures

Piper, Lawrence G.,Rawlins, Wilson T.

, p. 320 - 325 (1986)

We have studied the products of Ar/N2O microwave discharges to determine their fitness as sources of atomic oxygen in discharge-flow reactors.For N2O feed rates below 10 to 20 μmol s-1, the discharge converts about 75percent of the N2O to atomic oxygen and, in addition, prduces small quantities of atomic nitrogen, generally less than 10percent of the O-atom product.At higher N2O feed rates the O-atom production efficiency decreases, and some nitric oxide accompanies the O atoms out of the discharge.At intermediate N2O feed rates, only atomic oxygen is observed, and neither N nor NO leaves the discharge.The exact point at which this occurs is a function of the discharge power and the Ar/N2O mixing ratio.Adding molecular nitrogen to the discharge eliminates any NO product, but at the penalty of a slightly reduced O-atom production efficiency.Atomic oxygen flows in excess of 20 μmol s-1 are produced at pressures near 1 torr and dicharge powers of only 30 W.In kinetic modeling of the discharge chemistry, we can account for the experimental observations only if the electron-impact dissociation of the N2O in the discharge proceeds through a spin-forbidden channel to produce O(3P).In addition, the model indicates that about 10-20percent of the N2O dissociations resuts from collisions between metastable argon atoms in the discharge and N2O.

DIODE LASER KINETIC STUDIES OD RADICAL REACTIONS. 1. REACTION OF CF3 RADICALS WITH NO2

Sugawara, Ko-ichi,Nakanaga, Taisuke,Takeo, Harutoshi,Matsumura, Chi

, p. 1894 - 1898 (1989)

The reaction of CF3 radicals with NO2 has been studied over the pressure range 4-20 Torr at 300 K.CF3 radicals were produced by infrared multiphoton dissociation of CF3I.The subsequent decay of the radicals was monitored by using time-resolved diode laser

Ceria Nanoparticles as an Unexpected Catalyst to Generate Nitric Oxide from S-Nitrosoglutathione

Chandrawati, Rona,Gao, Yuan,Kumar, Priyank,Luo, Zijie,Yang, Tao,Zhou, Yingzhu

, (2022/01/24)

Ceria nanoparticles (NPs) are widely reported to scavenge nitric oxide (NO) radicals. This study reveals evidence that an opposite effect of ceria NPs exists, that is, to induce NO generation. Herein, S-nitrosoglutathione (GSNO), one of the most biologically abundant NO donors, is catalytically decomposed by ceria NPs to produce NO. Ceria NPs maintain a high NO release recovery rate and retain their crystalline structure for at least 4 weeks. Importantly, the mechanism of this newly discovered NO generation capability of ceria NPs from GSNO is deciphered to be attributed to the oxidation of Ce3+ to Ce4+ on their surface, which is supported by X-ray photoelectron spectroscopy and density functional theory analysis. The prospective therapeutic effect of NO-generating ceria NPs is evaluated by the suppression of cancer cells, displaying a significant reduction of 93% in cell viability. Overall, this report is, to the authors’ knowledge, the first study to identify the capability of ceria NPs to induce NO generation from GSNO, which overturns the conventional concept of them acting solely as a NO-scavenging agent. This study will deepen our knowledge about the therapeutic effects of ceria NPs and open a new route toward the NO-generating systems for biomedical applications.

Two-dimensional cluster catalysts with superior thermal stability and catalytic activity for AP

Guo, Yanli,Liang, Taixin,Liu, Wei,Song, Ruidong,Wang, Chao,Xiao, Fei,Zhang, Jiangbo

, (2022/01/08)

The preparation of catalysts with small particle size, large specific surface area and high atomic utilization has always been the focus of research in the field of catalysis. As for energetic materials, catalysts are always used to improve the thermal decomposition performance of ammonium perchlorate (AP) as it has significant effect on the power of engine. In this work, a two-dimensional metal clusters catalyst has been successfully prepared by solvothermal and heat treatment to improve thermal decomposition performance of AP. In detail, the transition metal ions were supported on the graphene oxide (GO) surface by organic ligands linking, followed by heat treatment to obtain two-dimensional rGO based metal clusters catalyst. The morphology and structure of the catalysts at different temperatures and their effect on AP decomposition were studied, the results show that catalyst at 300 °C has a particle size of 20 nm and uniformly distributed on rGO. The catalyst promotes the high temperature decomposition of AP by 73.7 °C with improved stability, and increases the heat release from 652.73 J/g to 1392.11 J/g. This may be attributed to good conductivity of GO and the strong gain-loss electron ability of the metal clusters. The presence of GO increased the active sites for cluster catalysis, additional, the metal clusters have a positive synergistic effect with GO. Thus, the thermal decomposition performance of AP was enhanced meanwhile thermal stability can also be improved.

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