Nitric oxide (IV) (nitrogen dioxide), properties, preparation, chemical reactions

Nitric oxide (IV) (nitrogen dioxide), properties, preparation, chemical reactions.

 

 

Nitric oxide (IV) (nitrogen dioxide) is an inorganic substance has the chemical formula NO2.

 

Brief description of nitrogen oxide (IV)

Physical properties of nitrogen oxide (IV)

Receipt of nitrogen oxide (IV)

Chemical properties of nitrogen oxide (IV)

Chemical reactions of nitrogen oxide (IV)

The application and use of nitrogen oxide (IV)

 

Brief description of nitrogen oxide (IV):

Nitric oxide (IV) is an inorganic substance, a poisonous gas, red-brown color, with a characteristic pungent odor or yellowish liquid.

Nitric oxide (IV) contains one atom of nitrogen and two atoms of oxygen.

Chemical formula of nitrogen oxide (IV) NO2.

In the normal state NO2 exists in equilibrium with its dimer N2O4. The tendency to its formation is explained by the presence in the molecule NO2, unpaired electron.

At a temperature of 140 °C nitric oxide (IV) only consists of molecules of NO2, but very dark, almost black.

The boiling point of NO2 – +21,1 °C is a yellowish liquid containing about 0.1% NO2.

At temperatures below +21°C is a colourless liquid (or yellowish from the admixture of the monomer).

At temperatures below -12 °C white crystals consist only of molecules of N2O4.

Acidic oxide.

Nitric oxide (IV) is highly toxic. Even in small concentrations it is irritating to respiratory tract at high concentrations causes pulmonary edema.

 

Physical properties of nitrogen oxide (IV):

Parameter name:	Value:
Chemical formula	NO2
Synonyms and foreign language names	nitrogen dioxide (eng.) nitrogen(IV) oxide (eng.) nitrogen dioxide (Rus.) nitrogen dioxide (Rus.) dinitrogen tetroxide (Rus.)
The type of substance.	inorganic
Appearance	red-brown gas or yellow liquid
Color	red-brown, yellowish
Taste	—*
The smell	characteristic pungent smell
Aggregate state (at 20 °C and atmospheric pressure of 1 ATM.)	liquid
Density (state of matter – liquid, at 0 °C), kg/m3	1491
Density (state of matter – liquid, at 0 °C), g/cm3	1,491
Density (state of matter – gas), kg/m3	2,0527
Density (state of matter – gas), g/l	2,0527
Boiling point, °C	21,1
Melting point, °C	-11,2
Molar mass, g/mol	46,0055

Note:

* — no data.

 

Receipt of nitrogen oxide (IV):

Nitric oxide (IV) in the laboratory is obtained by the following chemical reactions:

1. by the action of concentrated nitric acid on copper:

Cu + 4HNO3 → Cu(NO3)2 + 2NO2 + 2H2O.

2. by thermal decomposition of the nitrate of lead:

2Pb(NO3)2 → 2PbO + 4NO2 + O2 (t = 200-470 °C).

 

Chemical properties of nitrogen oxide (IV). Chemical reactions of nitrogen oxide (IV):

Nitric oxide (IV) refers to acidic oxides.

Chemical properties of nitrogen oxide (IV) are analogous to the properties of acidic oxides other nonmetals. However, it has a high chemical activity. Reacts with nonmetals. A strong oxidizing agent. So it is characterized by the following chemical reactions:

1. the reaction of nitrogen oxide (IV) and carbon:

2NO2 + 2C → 2СО2 + N2.

The reaction form carbon dioxide and nitrogen. The carbon is combusted to nitrogen oxide (IV).

2. the reaction of nitrogen oxide (IV) and phosphorus:

10NO2 + 8P → 4P2O5 + 5N2.

In the reaction, the formed phosphorus oxide (V) and nitrogen. Phosphorus burns in nitrous oxide (IV).

3. the reaction of nitrogen oxide (IV) and sulfur:

2S + 2NO2 → 2SO2 + N2.

In the reaction of formed sulfur oxide (IV) and nitrogen. Sulfur is combusted to nitrogen oxide (IV).

4. the reaction of nitrogen oxide (IV) and fluorine:

2NO2 + 2F2 → 2NO2F.

The reaction produced a fluoride-nitrogen dioxide (V).

5. the reaction of nitrogen oxide (IV) and potassium:

NO2 + K → KNO2.

The reaction forms a salt with potassium nitrite.

6. the reaction of nitrogen oxide (IV) and copper:

2NO2 + 4Cu → 4CuO + N2 (t = 500-600 °C).

In the reaction, the formed copper oxide and nitrogen.

7. the reaction of nitrogen oxide (IV) and bismuth:

6NO2 + Bi → Bi(NO3)3 + 3NO (t = 70-110 °C).

In the reaction, the formed oxide of bismuth and oxide of nitrogen (II).

8. the reaction of nitrogen oxide (IV) and zinc:

4NO2 + Zn → 2NO + Zn(NO3)2 (t = 500-600 °C).

The reaction produces nitric oxide (II) and nitrate of zinc. At carrying out of the reaction is a liquid nitrogen oxide (IV) and zinc in powder form.

9. the reaction of nitrogen oxide (IV) and sodium:

2NO2 + Na → NO + NaNO3.

In the reaction, the formed salt is a nitrate, sodium and nitric oxide (II). At carrying out of the reaction is a liquid nitrogen oxide (IV).

10. the reaction of nitrogen oxide (IV) and hydrogen:

2NO2 + 7H2 → 4H2O + 2NH3 (kat = Pt, Ni).

The reaction produces ammonia and water.

11. the reaction of nitrogen oxide (IV) and ozone:

2NO2 + O3 → N2O5 + O2 (t = -78 OS).

The reaction produces nitric oxide (V) and oxygen.

12. the reaction of nitrogen oxide (IV) hydrogen bromide (bromoderma):

NO2 + 2HBr → NO + Br + H2O (t o).

The chemical reaction turns the nitric oxide (II) bromine and water.

13. the reaction of nitrogen oxide (IV) with yodovidona:

2HI + NO2 → I2 + NO + H2O.

The chemical reaction turns the nitric oxide (II), iodine and water.

14. the reaction of nitrogen oxide (IV) and water:

2NO2 + H2O → HNO3 + HNO2,

3NO2 + H2O → 2HNO3 + NO (t o).

As a result of chemical reactions in the first case the nitric acid and nitrous acid, in the second case, since nitrous acid is unstable, by dissolving NO2 in warm water are formed nitric acid and nitric oxide (II).

15. the reaction of nitrogen oxide (IV), oxygen and water:

4NO2 + 2H2O + O2 → 4HNO3.

As a result of chemical reaction is obtained with nitric acid.

16. the reaction of nitrogen oxide (IV) and potassium oxide:

K2O + 2NO2 → KNO2 + KNO3 (t = 150-200 oC).

The chemical reaction turns the nitrate of potassium and nitrate of potassium.

17. the reaction of nitrogen oxide (IV) and potassium hydroxide:

2NO2 + 2KOH → KNO3 + KNO2 + H2O.

As a result of chemical reaction is obtained the potassium nitrate, potassium nitrite and water.

18. the reaction of nitrogen oxide (IV) and sodium hydroxide:

2NO2 + 2NaOH → NaNO3 + NaNO2 + H2O.

As a result of chemical reaction is obtained sodium nitrate, sodium nitrite and water. Sodium hydroxide – dilute solution.

19. the reaction of nitrogen oxide (IV) and potassium chloride:

2NO2 + KCl → NOCl + KNO3.

The chemical reaction turns nitrosyl chloride and potassium nitrate. At carrying out of the reaction is a liquid nitrogen oxide (IV).

20. the reaction of nitrogen oxide (IV) and potassium bromide:

2NO2 + KBr → NOBr + KNO3.

The chemical reaction turns nitrosyl bromide and potassium nitrate. At carrying out of the reaction is a liquid nitrogen oxide (IV).

21. the reaction of nitrogen oxide (IV) and phosphorous acid:

H3PO3 + NO2 → H3PO4 + NO (t = 30-50 oC).

As a result of chemical reaction is obtained the phosphoric acid and oxide of nitrogen (II).

22. the reaction of thermal decomposition of nitrogen oxide (IV):

2NO2 → 2NO + O2 (t = 500 ºc).

The chemical reaction turns the oxygen and the nitric oxide (II).

 

The application and use of nitrogen oxide (IV):

Nitric oxide (IV) is used in the manufacture of sulfuric and nitric acids, and also as an oxidizer in liquid rocket fuel.

 

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