Iron sulfide and ferric persulfide react with oxygen

Eventually, iron oxide and sulfur dioxide are generated, the chemical equation.

As follows: 4fes +7o = 2fe o +4so In nature, fes are mainly used in marcasite and pyrite.

Two mineral forms exist, with pyrite being the most widely distributed sulphide.

Minerals, which can be found in all types of rocks. Pyrite is the main raw material for the extraction of sulfur and the manufacture of sulphuric acid, and it is also a very cheap ancient gemstone.

With all due respect, I said that this question of yours is a bit not quite correct......I put it this way, iron sulfide, Fes, in fact, is ferrous sulfide, some people may say that I fart nonsense, iron sulfide is Fe2S3 (this substance does not exist), in fact, it is not, if you don't believe it, you can go and see:

The sulfur in Fes is minus 2 valence, and I haven't heard of iron persulfide, and I can't find the information, so if we assume that it exists, the chemical formula should be FeS2, where the persulfide refers to peroxide. The valency of iron is positive 2 and sulfur is negative 1. Let's not discuss the reading of FeS2 (although his name is ferrous sulfide), to see if they will react with each other, obviously not, because the sulfur of ferrous sulfide is negative 2 valence, FeS2 is negative 1 valence, and iron is positive 2 valence, they are all adjacent valence states so they will not react, as for why I think your chemistry teacher has said this.

Ferrous sulfide can react with oxygen.

4FeS2+11O2=2Fe2O3+8SO2 The reaction condition is high temperature.

Iron sulfide does not have this substance in nature, and the elements between them can undergo their own redox reactions, and the principle is the same as the absence of iron iodide in nature.

Fes+7O2=2Fe2O3+4So2, the reaction condition is ignition.

FeS2+11O2=2Fe2O3+8SO2, the reaction condition is high temperature.

All we know is 4FeS2+11O2=8SO2=2FE2O3

I've never heard of iron sulfide.

Ferrous disulfideReaction with oxygenEquations：4fes2+11o2=2fe2o3+8so2。

This reaction is the first step before the disarmament of industrial sulfuric acid in China.

1. In the case of insufficient oxygen, the equation is:

2fes2+o2=2feo+4s

2. The equation in the case of oxygen excess is:

2fes2+7o2=2fe2o3+4so2<>

2. The use of ferrous sulfide:It has important uses in rubber, papermaking, textile, food, matches and other industries, as well as in agriculture. In particular, it is used in the defense industry to manufacture various explosives and fumes. to pyrite.

Sulfuric acid is used as a raw material to make sulfuric acid, and its slag can be used to make iron and steel.

If the sulfur content of slag is high and the iron content is not high, it can be used as an auxiliary raw material for cement - mixture.

Upstream raw materials: diesel, industrial fuses, detonators, coal, gasoline, cement cavities, explosives.

Downstream products: sulfuric acid, chlorosulfonic acid.

Manganese sulfate, sulfur dioxide.

Sulfur, iron powder, superphosphate, phenolic resin paint, ammonia synthesis catalyst.

Iron sulfide. It reacts with oxygen to form iron oxide and sulfur dioxide.

4fes +7o₂=2fe₂o₃+4so₂。

Iron sulfide is easily oxidized in the air, so it does not exist in nature, and only slow attack can be prepared by laboratory chemical methods.

However, trivalent nonionic iron in the dry state cannot oxidize the element-2 valence sulfur, and in a strong alkaline solution, Fe3+ can react with S2- to form ferric trisulfide.

Precipitation. Because ksp(fe2s3) = 1 10-88 and ksp(fe(oh)3) = 1 10-38.

Iron oxide desulfurizer is a hydrate of activated iron oxide (Fe2O3).

It is a desulfurizer that is the main desulfurization component. At room temperature, iron oxide (Fe2O3) is divided into -hydrate and -hydrate, both of which have desulfurization effects. Non-hydrate iron oxide does not have desulfurization at room temperature.

Iron oxide desulfurizer has been rapidly promoted in recent years due to its large sulfur capacity, low sulfur capacity, and air regeneration at room temperature, and the main reason is that it can desulfurize the H2S (activated carbon) in the gas source under oxygen-free conditions.

No desulfurization under oxygen-free conditions), after the improvement in recent years, the water resistance strength and desulfurization accuracy of iron oxide have been greatly improved, and it is suitable for most industrial desulfurization and bridge disturbance projects.

Chemical-iron hunger and oxygen react with the rotten sun.

In case of oxygen deficiencyEquationsYes: 2fes2+o2=2feo+4s. The equation in case of oxygen excess is:

2fes2+7o2=2fe2o3+4so2。

Ferrous sulfide undergoes a chemical reaction with oxygen.

The reaction produces iron oxide and sulfur dioxide.

This is the chemical reaction of ironmaking in industry. The chemical reaction equation for the reaction is 4FeS2+11O2=2Fe2O3+8SO2. This chemical reaction is a redox reaction.

The oxidizing agent is oxygen, and the reducing agent is ferrous sulfide, which loses electrons in the chemical reaction and is oxidized, and a disulfide spike ridge ferrous loses 11 electrons.

Iron sulfide precautions

Ferric disulfide, ferrous sulfide, ferric trisulfide.

It is insoluble in water. Why ferrous sulfide in acid is not a precipitate, but copper sulfide.

It is precipitation: because the volume constant of copper sulfide is extremely small, hydrogen sulfide cannot be formed in solution.

gas, while ferrous sulfide cannot.

Iron sulfide is a black solid that easily turns to yellow-green at room temperature. Iron sulfide is easily oxidized in the air, so it does not exist in nature and can only be prepared by laboratory chemical methods.

The above content refers to Encyclopedia - Iron Disulfide.

The reaction phenomenon between iron oxide and dilute sulfuric acid is that the solid dissolves and the solution turns brownish-yellow.

Equation: Fe O +3H So ==Fe (SO4) +3H O

Chemical iron is the main component of rust. The main cause of rust is that iron metal will rust in the presence of impurity carbon, which reacts with moisture and oxygen in the environment.

It is used in paint, ink, rubber and other industries, can be used as a catalyst, glass, gemstones, metal polishing agent, can be used as a raw material for ironmaking.

Iron Oxide Properties:

Iron oxide is insoluble in water, soluble in hydrochloric acid and sulfuric acid, and slightly soluble in nitric acid. Strong hiding and tinting strength, no oil permeability and no water permeability. It is stable in the atmosphere and sunlight, resistant to polluting gases, high temperature and alkali.

Nitric acid reacts with iron to form ferrous nitrate, which is cooled and crystallized, dehydrated and dried, and calcined at 600 700 for 8 10h after grinding, and then washed, dried and crushed in water to obtain iron oxide red products.

The above content refers to Encyclopedia - Iron Oxide.

Iron sulfate and ferric sulfide reaction FeS2 reaction with acid:

Fes2 + H2SO4 = FeSo4 + H2S + S The H2S produced precipitates heavy metal ions in solution.

H2S + CuSO4 = Cus + H2SO4 also restores Fe3+

h2s + 4 fe2(so4)3 + 4 h2o = 8 feso4 + 5 h2so4

In an acidic environment, Mg2+ cannot be precipitated by S2-.

After filtration, the precipitate is S and Cus

The reaction is complex, and the amount of each substance is not known, so it can only be speculative and not necessarily accurate.

The chemical equation for the reaction of ferric oxide with sulfuric acid is as follows:

fe2o3+3h2so4=fe2（so4）3+3h2o

Iron and sulfur undergo a chemical reaction.

Iron powder and sulfur powder.

The mixture is heated to a red heat, and the reaction forms a black solid body, which releases a large amount of heat.

Chemistry holds this program:

Fe + S = Fes (Conditionally Heated Canvas Skin) Natural elemental sulfur is non-toxic and harmless to the human body, while dilute sulfuric acid, sulfate, sulfurous acid and sulfite are toxic, and sulfides are usually highly toxic. Concentrated sulfuric acid.

It can corrode the human body**.