The interaction of iron with hydrogen. The use of iron: from foundation reinforcement to a magnetic drive

Brazhnikova Alla Mikhailovna,

GBOU secondary school №332

Nevsky district of St. Petersburg

This manual considers questions on the topic "Chemistry of Iron". In addition to traditional theoretical issues, issues that go beyond the basic level are considered. It contains questions for self-control, which enable students to check the level of assimilation of the relevant educational material in preparation for the exam.

CHAPTER 1. IRON IS A SIMPLE SUBSTANCE.

The structure of the iron atom .

Iron is a d-element, located in a side subgroup of group VIII of the periodic system. The most common metal in nature after aluminum. It is part of many minerals: brown iron ore (hematite) Fe 2 O 3, magnetic iron ore (magnetite) Fe 3 O 4, pyrite FeS 2.

Electronic structure : 1s 2 2s 2 2p 6 3s 2 3p 6 3d 6 4s 2 .

Valence : II, III, (IV).

Oxidation states: 0, +2, +3, +6 (only in ferrates K 2 FeO 4).

physical properties.

Iron is a shiny, silvery-white metal, m.p. - 1539 0 C.

Receipt.

Pure iron can be obtained by reducing oxides with hydrogen when heated, as well as by electrolysis of solutions of its salts. Domain process - obtaining iron in the form of alloys with carbon (cast iron and steel):

1) 3Fe 2 O 3 + CO → 2Fe 3 O 4 + CO 2

2) Fe 3 O 4 + CO → 3FeO + CO 2

3) FeO + CO → Fe + CO 2

Chemical properties.

I. Interaction with simple substances - non-metals

1) With chlorine and sulfur (when heated). With a stronger oxidizing agent, chlorine oxidizes iron to Fe 3+, with a weaker one - sulfur - to Fe 2+:

2Fe 2 + 3Cl → 2FeCl 3

2) With coal, silicon and phosphorus (at high temperature).

3) In dry air, it is oxidized by oxygen, forming scale - a mixture of iron (II) and (III) oxides:

3Fe + 2O 2 → Fe 3 O 4 (FeO Fe 2 O 3)

II. Interaction with complex substances.

1) Corrosion (rusting) of iron proceeds in moist air:

4Fe + 3O 2 + 6H 2 O → 4Fe(OH) 3

At a high temperature (700 - 900 0 C) in the absence of oxygen, iron reacts with water vapor, displacing hydrogen from it:

3Fe+ 4H 2 O → Fe 3 O 4 + 4H 2

2) Displaces hydrogen from dilute hydrochloric and sulfuric acids:

Fe + 2HCl \u003d FeCl 2 + H 2

Fe + H 2 SO 4 (razb.) \u003d FeSO 4 + H 2

Highly concentrated sulfuric and nitric acids do not react with iron at ordinary temperatures due to its passivation.

With dilute nitric acid, iron is oxidized to Fe 3+, the products of HNO 3 reduction depend on its concentration and temperature:

8Fe + 30HNO 3 (very well dec.) → 8Fe(NO 3) 3 + 3NH 4 NO 3 + 9H 2 O

Fe + 4HNO 3 (diff.) → Fe (NO 3) 3 + NO + 2H 2 O

Fe + 6HNO 3 (conc.) → (temperature) Fe(NO 3) 3 + 3NO 2 + 3H 2 O

3) Reaction with solutions of metal salts to the right of iron in the electrochemical series of metal voltages:

Fe + CuSO 4 → FeSO 4 + Cu

CHAPTER2. IRON(II) COMPOUNDS.

Iron oxide(II) .

FeO oxide is a black powder, insoluble in water.

Receipt.

Recovery from iron oxide (III) at 500 0 C by the action of carbon monoxide (II):

Fe 2 O 3 + CO → 2FeO + CO 2

Chemical properties.

The main oxide, it corresponds to Fe (OH) 2 hydroxide: it dissolves in acids, forming iron (II) salts:

FeO+ 2HCl → FeCl 2 + H 2 O

Iron hydroxide (II).

Iron hydroxide Fe(OH) 2 is a water-insoluble base.

Receipt.

The action of alkalis on iron salts () without air access:

FeSO 4 + NaOH → Fe(OH) 2 ↓+ Na 2 SO 4

Chemical properties.

Hydroxide Fe(OH) 2 exhibits basic properties, dissolves well in mineral acids, forming salts.

Fe(OH) 2 + H 2 SO 4 → FeSO 4 + 2H 2 O

When heated, it decomposes:

Fe(OH) 2 → (temperature) FeO+ H 2 O

redox properties.

Iron (II) compounds exhibit sufficiently strong reducing properties, they are stable only in an inert atmosphere; in air (slowly) or in an aqueous solution under the action of oxidizing agents (quickly) they pass into iron (III) compounds:

4 Fe(OH) 2 (precipitate) + O 2 + 2H 2 O→ 4 Fe(OH) 3 ↓

2FeCl 2 + Cl 2 → 2FeCl 3

10FeSO 4 + 2KMnO 4 + 8H 2 SO 4 → 5 Fe 2 (SO 4) 3 + 2MnSO 4 + K 2 SO 4 + 8 H 2 O

Iron (II) compounds can also act as oxidizing agents:

FeO+ CO→ (temperature) Fe+ CO

CHAPTER 3. IRON COMPOUNDS (III).

Iron oxide(III)

Fe 2 O 3 oxide is the most stable natural oxygen-containing iron compound. It is an amphoteric oxide, insoluble in water. It is formed during the firing of pyrite FeS 2 (see 20.4 "Obtaining SO 2".

Chemical properties.

1) Dissolving in acids, it forms iron (III) salts:

Fe 2 O 3 + 6HCl → 2FeCl 3 + 3H 2 O

2) When fused with potassium carbonate, it forms potassium ferrite:

Fe 2 O 3 + K 2 CO 3 → (temperature) 2KFeO 2 + CO 2

3) Under the action of reducing agents, it acts as an oxidizing agent:

Fe 2 O 3 + 3H 2 → (temperature) 2Fe + 3H 2 O

Iron hydroxide (III)

Iron hydroxide Fe (OH) 3 is a red-brown substance, insoluble in water.

Receipt.

Fe 2 (SO 4) 3 + 6NaOH → 2Fe(OH) 3 ↓ + 3Na 2 SO 4

Chemical properties.

Fe (OH) 3 hydroxide is a weaker base than iron (II) hydroxide, has a weakly pronounced amphotericity.

1) Soluble in weak acids:

2Fe(OH) 3 + 3H 2 SO 4 → Fe 2 (SO 4) 3 + 6H 2 O

2) When boiled in 50% NaOH solution, it forms

Fe(OH) 3 + 3NaOH → Na 3

Iron salts (III).

Subject to strong hydrolysis in aqueous solution:

Fe 3+ + H 2 O ↔ Fe (OH) 2+ + H +

Fe 2 (SO 4) 3 + 2H 2 O ↔ Fe (OH) SO 4 + H 2 SO 4

Under the action of strong reducing agents in an aqueous solution, they exhibit oxidizing properties, turning into iron (II) salts:

2FeCl 3 + 2KI → 2FeCl 2 + I 2 + 2KCl

Fe 2 (SO 4) 3 + Fe → 3 Fe

CHAPTER4. QUALITATIVE REACTIONS.

Qualitative reactions to Fe 2+ and Fe 3+ ions.

1. The reagent for the Fe 2+ ion is potassium hexacyanoferrate (III) (red blood salt), which gives with it an intensely blue precipitate of a mixed salt - potassium-iron (II) hexacyanoferrate (III) or turnbull blue:

FeCl 2 + K 3 → KFe 2+ ↓ + 2KCl

1. The reagent for the Fe 3+ ion is the thiocyanate ion (thiocyanate ion) CNS -, when interacting with iron (III) salts, a blood-red substance is formed - iron (III) thiocyanate:

FeCl 3 + 3KCNS → Fe(CNS) 3 + 3KCl

3) Fe 3+ ions can also be detected using potassium hexacyanoferrate (II) (yellow blood salt). In this case, a water-insoluble substance of intense blue color is formed - potassium-iron (III) hexacyanoferrate (II) or Prussian blue:

FeCl 3 + K 4 → KFe 3+ ↓ + 3KCl

CHAPTER 5. MEDICAL AND BIOLOGICAL SIGNIFICANCE OF IRON.

The role of iron in the body.

Iron participates in the formation of hemoglobin in the blood, in the synthesis of thyroid hormones, in protecting the body from bacteria. It is necessary for the formation of immune protective cells, it is required for the "work" of B vitamins.

Iron is a part of more than 70 different enzymes, including respiratory ones, which ensure the processes of respiration in cells and tissues, and are involved in the neutralization of foreign substances entering the human body.

Hematopoiesis. Hemoglobin.

Gas exchange in the lungs and tissues.

Iron-deficiency anemia.

Iron deficiency in the body leads to diseases such as anemia, anemia.

Iron deficiency anemia (IDA) is a hematological syndrome characterized by impaired hemoglobin synthesis due to iron deficiency and manifested by anemia and sideropenia. The main causes of IDA are blood loss and lack of heme-rich food and drink.

The patient may be disturbed by fatigue, shortness of breath and palpitations, especially after physical exertion, often - dizziness and headaches, tinnitus, even fainting is possible. A person becomes irritable, sleep is disturbed, concentration of attention decreases. Because blood flow to the skin is reduced, increased sensitivity to cold may develop. There are also symptoms from the gastrointestinal tract - a sharp decrease in appetite, dyspeptic disorders (nausea, changes in the nature and frequency of stools).

Iron is an integral part of vital biological complexes, such as hemoglobin (oxygen and carbon dioxide transport), myoglobin (oxygen storage in muscles), cytochromes (enzymes). The body of an adult contains 4-5 g of iron.

LIST OF USED LITERATURE:

1. K.N. Zelenin, V.P. Sergutin, O.V. Malt "We pass the exam in chemistry perfectly." Elbl-SPb LLC, 2001.
2. K.A. Makarov "Medical chemistry". Publishing house of St. Petersburg State Medical University of St. Petersburg, 1996.
3. N.L. Glinka General Chemistry. Leningrad "Chemistry", 1985.
4. V.N. Doronkin, A.G. Berezhnaya, T.V. Sazhnev, V.A. Fevraleva "Chemistry. Thematic tests for preparing for the exam. Publishing house "Legion", Rostov-on-Don, 2012.

Malleable silver-white metal with high chemical reactivity: iron corrodes quickly at high temperatures or high humidity in air. In pure oxygen, iron burns, and in a finely dispersed state, it ignites spontaneously in air. It is designated by the symbol Fe (lat. Ferrum). One of the most common metals in the earth's crust (second place after).

See also:

STRUCTURE

For iron, several polymorphic modifications have been established, of which the high-temperature modification - γ-Fe (above 906 °) forms a lattice of a face-centered cube of the Cu type (a 0 \u003d 3.63), and the low-temperature modification - α-Fe-lattice of a centered cube of the α-Fe type ( a 0 = 2.86).
Depending on the heating temperature, iron can be in three modifications, characterized by a different structure of the crystal lattice:

1. In the temperature range from the lowest to 910 ° C - a-ferrite (alpha-ferrite), having a crystal lattice structure in the form of a centered cube;
2. In the temperature range from 910 to 1390°C - austenite, the crystal lattice of which has the structure of a face-centered cube;
3. In the temperature range from 1390 to 1535 ° C (melting point) - d-ferrite (delta-ferrite). The crystal lattice of d-ferrite is the same as that of a-ferrite. The difference between them is only in other (large for d-ferrite) distances between atoms.

When liquid iron is cooled, primary crystals (crystallization centers) appear simultaneously at many points of the cooled volume. During subsequent cooling, new crystalline cells are built around each center until the entire supply of liquid metal is exhausted.
The result is a granular structure of the metal. Each grain has a crystal lattice with a certain direction of its axes.
Upon subsequent cooling of solid iron, during the transitions of d-ferrite to austenite and austenite to α-ferrite, new crystallization centers can appear with a corresponding change in grain size

PROPERTIES

In its pure form under normal conditions, it is a solid. It has a silvery-gray color and a pronounced metallic sheen. The mechanical properties of iron include the level of hardness on the Mohs scale. It is equal to four (medium). Iron has good electrical and thermal conductivity. The last feature can be felt by touching an iron object in a cold room. Since this material conducts heat quickly, it takes a lot of it out of your skin in a short amount of time, which is why you feel cold.
Touching, for example, a tree, it can be noted that its thermal conductivity is much lower. The physical properties of iron are its melting and boiling points. The first is 1539 degrees Celsius, the second is 2860 degrees Celsius. It can be concluded that the characteristic properties of iron are good ductility and fusibility. But that's not all. The physical properties of iron also include its ferromagnetism. What it is? Iron, the magnetic properties of which we can observe in practical examples every day, is the only metal that has such a unique distinguishing feature. This is due to the fact that this material is able to be magnetized under the influence of a magnetic field. And after the termination of the action of the latter, iron, the magnetic properties of which have just been formed, remains a magnet for a long time. This phenomenon can be explained by the fact that in the structure of this metal there are many free electrons that are able to move.

RESERVES AND PRODUCTION

Iron is one of the most common elements in the solar system, especially on the terrestrial planets, in particular on Earth. A significant part of the iron of the terrestrial planets is located in the cores of the planets, where its content is estimated to be about 90%. The content of iron in the earth's crust is 5%, and in the mantle about 12%.

In the earth's crust, iron is widely distributed - it accounts for about 4.1% of the mass of the earth's crust (4th place among all elements, 2nd among metals). In the mantle and the earth's crust, iron is concentrated mainly in silicates, while its content is significant in basic and ultrabasic rocks, and low in acidic and intermediate rocks.
A large number of ores and minerals containing iron are known. Of the greatest practical importance are red iron ore (hematite, Fe2O3; contains up to 70% Fe), magnetic iron ore (magnetite, FeFe 2 O 4 , Fe 3 O 4 ; contains 72.4% Fe), brown iron ore or limonite (goethite and hydrogoethite, FeOOH and FeOOH nH 2 O, respectively). Goethite and hydrogoethite are most often found in weathering crusts, forming the so-called "iron hats", whose thickness reaches several hundred meters. They can also be of sedimentary origin, falling out of colloidal solutions in lakes or coastal areas of the seas. In this case, oolitic, or legume, iron ores are formed. They often contain vivianite Fe 3 (PO 4) 2 8H 2 O, which forms black elongated crystals and radially radiant aggregates.
The content of iron in sea water is 1 10 -5 -1 10 -8%
In industry, iron is obtained from iron ore, mainly from hematite (Fe 2 O 3) and magnetite (FeO·Fe 2 O 3).
There are various ways to extract iron from ores. The most common is the domain process.
The first stage of production is the reduction of iron with carbon in a blast furnace at a temperature of 2000 °C. In a blast furnace, carbon in the form of coke, iron ore in the form of sinter or pellets, and flux (eg limestone) are fed from above and are met by a stream of injected hot air from below.
In addition to the blast furnace process, the process of direct production of iron is common. In this case, pre-crushed ore is mixed with special clay to form pellets. The pellets are roasted and treated in a shaft furnace with hot methane conversion products that contain hydrogen. Hydrogen easily reduces iron without contaminating the iron with impurities such as sulfur and phosphorus, which are common impurities in coal. Iron is obtained in solid form, and then melted down in electric furnaces. Chemically pure iron is obtained by electrolysis of solutions of its salts.

ORIGIN

The origin of telluric (terrestrial) iron is rarely found in basaltic lavas (Wifaq, Disko Island, off the western coast of Greenland, near the city of Kassel, Germany). Pyrrhotite (Fe 1-x S) and cohenite (Fe 3 C) are associated with it at both points, which explains both the reduction by carbon (including from host rocks) and the decomposition of carbonyl complexes of the Fe(CO) n type. In microscopic grains, it has been established more than once in altered (serpentinized) ultrabasic rocks, also in paragenesis with pyrrhotite, sometimes with magnetite, due to which it arises during reduction reactions. It is very rare in the zone of oxidation of ore deposits, during the formation of swamp ores. Findings in sedimentary rocks associated with the reduction of iron compounds by hydrogen and hydrocarbons have been registered.
Almost pure iron has been found in the lunar soil, which is associated with both meteorite falls and magmatic processes. Finally, two classes of meteorites, stony-iron and iron, contain natural iron alloys as a rock-forming component.

APPLICATION

Iron is one of the most used metals, accounting for up to 95% of the world's metallurgical production.
Iron is the main component of steels and cast irons - the most important structural materials.
Iron can be part of alloys based on other metals - for example, nickel.
Magnetic iron oxide (magnetite) is an important material in the manufacture of long-term computer memory devices: hard drives, floppy disks, etc.
Ultrafine magnetite powder is used in many black and white laser printers mixed with polymer granules as a toner. It uses both the black color of magnetite and its ability to adhere to a magnetized transfer roller.
The unique ferromagnetic properties of a number of iron-based alloys contribute to their widespread use in electrical engineering for the magnetic circuits of transformers and electric motors.
Iron(III) chloride (ferric chloride) is used in amateur radio practice for etching printed circuit boards.
Ferrous sulfate (iron sulfate) mixed with copper sulphate is used to control harmful fungi in gardening and construction.
Iron is used as an anode in iron-nickel batteries, iron-air batteries.
Aqueous solutions of chlorides of divalent and ferric iron, as well as its sulfates, are used as coagulants in the purification of natural and waste water in the water treatment of industrial enterprises.

Iron (English Iron) - Fe

CLASSIFICATION

Hey's CIM Ref1.57

DEFINITION

Iron- an element of the eighth group of the fourth period of the Periodic system of chemical elements of D. I. Mendeleev.

And the languid number is 26. The symbol is Fe (lat. “ferrum”). One of the most common metals in the earth's crust (second place after aluminum).

Physical properties of iron

Iron is a gray metal. In its pure form, it is quite soft, malleable and ductile. The electronic configuration of the external energy level is 3d 6 4s 2 . In its compounds, iron exhibits the oxidation states "+2" and "+3". The melting point of iron is 1539C. Iron forms two crystalline modifications: α- and γ-iron. The first of them has a cubic body-centered lattice, the second has a cubic face-centered one. α-Iron is thermodynamically stable in two temperature ranges: below 912 and from 1394C to the melting point. Between 912 and 1394C, γ-iron is stable.

The mechanical properties of iron depend on its purity - the content in it of even very small amounts of other elements. Solid iron has the ability to dissolve many elements in itself.

Chemical properties of iron

In moist air, iron quickly rusts, i.e. covered with a brown coating of hydrated iron oxide, which, due to its friability, does not protect iron from further oxidation. In water, iron corrodes intensively; with abundant access of oxygen, hydrated forms of iron oxide (III) are formed:

2Fe + 3/2O 2 + nH 2 O = Fe 2 O 3 × H 2 O.

With a lack of oxygen or with difficult access, a mixed oxide (II, III) Fe 3 O 4 is formed:

3Fe + 4H 2 O (v) ↔ Fe 3 O 4 + 4H 2.

Iron dissolves in hydrochloric acid of any concentration:

Fe + 2HCl \u003d FeCl 2 + H 2.

Similarly, dissolution occurs in dilute sulfuric acid:

Fe + H 2 SO 4 \u003d FeSO 4 + H 2.

In concentrated solutions of sulfuric acid, iron is oxidized to iron (III):

2Fe + 6H 2 SO 4 \u003d Fe 2 (SO 4) 3 + 3SO 2 + 6H 2 O.

However, in sulfuric acid, the concentration of which is close to 100%, iron becomes passive and there is practically no interaction. In dilute and moderately concentrated solutions of nitric acid, iron dissolves:

Fe + 4HNO 3 \u003d Fe (NO 3) 3 + NO + 2H 2 O.

At high concentrations of nitric acid, dissolution slows down and iron becomes passive.

Like other metals, iron reacts with simple substances. The reactions of the interaction of iron with halogens (regardless of the type of halogen) proceed when heated. The interaction of iron with bromine proceeds at an increased vapor pressure of the latter:

2Fe + 3Cl 2 \u003d 2FeCl 3;

3Fe + 4I 2 = Fe 3 I 8.

The interaction of iron with sulfur (powder), nitrogen and phosphorus also occurs when heated:

6Fe + N 2 = 2Fe 3 N;

2Fe + P = Fe 2 P;

3Fe + P = Fe 3 P.

Iron is able to react with non-metals such as carbon and silicon:

3Fe + C = Fe 3 C;

Among the reactions of the interaction of iron with complex substances, the following reactions play a special role - iron is able to reduce metals that are in the activity series to the right of it, from salt solutions (1), to reduce iron (III) compounds (2):

Fe + CuSO 4 \u003d FeSO 4 + Cu (1);

Fe + 2FeCl 3 = 3FeCl 2 (2).

Iron, at elevated pressure, reacts with a non-salt-forming oxide - CO to form substances of complex composition - carbonyls - Fe (CO) 5, Fe 2 (CO) 9 and Fe 3 (CO) 12.

Iron, in the absence of impurities, is stable in water and in dilute alkali solutions.

Getting iron

The main way to obtain iron is from iron ore (hematite, magnetite) or electrolysis of solutions of its salts (in this case, “pure” iron is obtained, i.e. iron without impurities).

Examples of problem solving

EXAMPLE 1

It has been known to people since antiquity: scientists attribute ancient household items made of this material to the 4th millennium BC.

Human life cannot be imagined without iron. It is believed that iron is used for industrial purposes more often than other metals. The most important structures are made from it. Iron is also found in small amounts in the blood. It is the content of the twenty-sixth element that colors the blood red.

Physical properties of iron

In oxygen, iron burns to form an oxide:

3Fe + 2O₂ = Fe₃O₄.

When heated, iron can react with non-metals:

Also, at a temperature of 700-900 ° C, it reacts with water vapor:

3Fe + 4H₂O = Fe₃O₄ + 4H₂.

Iron compounds

As you know, iron oxides have ions with two oxidation states: +2 and + 3. It is extremely important to know this, because completely different qualitative reactions will be carried out for different elements.

Qualitative reactions to iron

A qualitative reaction is needed in order to easily determine the presence of ions of one substance in solutions or impurities of another. Consider the qualitative reactions of ferrous and trivalent iron.

Qualitative reactions for iron (III)

The content of ferric ions in a solution can be determined using alkali. With a positive result, a base is formed - iron (III) hydroxide Fe (OH) ₃.

The resulting substance is insoluble in water and has a brown color. It is the brown precipitate that may indicate the presence of ferric ions in the solution:

FeCl₃ + 3NaOH = Fe(OH)₃↓+ 3NaCl.

Fe(III) ions can also be determined using K₃.

A solution of ferric chloride is mixed with a yellowish blood salt solution. As a result, you can see a beautiful bluish precipitate, which will indicate that ferric ions are present in the solution. you will find spectacular experiments on the study of the properties of iron.

Qualitative reactions for iron (II)

Fe²⁺ ions react with the red blood salt K₄. If a bluish precipitate forms when the salt is added, then these ions are present in the solution.

This article will talk about iron, its chemical and physical properties. They are of great importance for determining the method of transporting iron, its storage conditions, production, smelting, etc.

Iron is one of the most popular metals. But often it is called an alloy with some kind of impurity, for example, with carbon. This helps to maintain the ductility and softness of the metal itself. An indicator in this composition will be the amount of pure metal, carbon and impurities.

For steel smelting, a metallization method is used, which helps the product become more resistant to external influences, such as erosion, corrosion, and wear. In this case, the content of additional impurity can be different.

Carbon

The percentage of carbon content in the alloy can range from 0.2% to 10%. It depends on the way the iron is recovered. In this case, the amount and degree of metallization can vary very widely. In gaseous reduction processes, filamentous carbon is deposited from the gas phase onto the iron surface. But the reaction is not completed to the end, and the product that has undergone metallization has on its surface and in the pores soot formed from carbon.

Phosphorus

In the process of direct reduction of iron, the amount of phosphorus does not decrease, and the percentage of its content during metallization is equal to its amount in the feedstock. This can be reduced by the complete enrichment of the ore used for the recovery process. Moreover, the ratio of phosphorus and iron depends on the increase in the percentage of iron, which leads to a decrease in the percentage of phosphorus. In most formulations, it is 0.010-0.020%, rarely 0.030%.

Sulfur

The raw material for the direct reduction of iron is often unfluxed pellets, since they have removed most of the sulfur by oxidative roasting, and then the main source of sulfur will be the reducing agent.

With the original solid reducing agent, the amount of sulfur in the composition of the metallized material may be high. Then its lowering can be achieved by adding limestone and dolomite.

In the case of a gaseous reducing agent, the output is a product with a low percentage of sulfur, up to 0.003.

nitrogen and hydrogen

Nitrogen is contained in small amounts in the ore, which determines its small percentage in metallized materials, up to 0.003%. The amount of hydrogen reaches 150 cubic meters. see per 100 gr., and in steel its percentage is the same as in the smelting of scrap.

Non-ferrous metals

The amount of non-ferrous metals, namely nickel, chromium, lead, copper, has a composition of direct reduced iron, and is often low due to the purity of the raw materials. This indicator of sponge iron can be compared with cast iron. The only difference is that cast iron contains reduced chromium.

Titanium, chromium, vanadium are found in metallized pellets as oxides. In the process of melting, it is quite simple to organize a possibility that prevents them from being restored from slag. This gives the ability to obtain a metal, which will contain a low percentage of titanium, chromium and, possibly, manganese.

Iron, whose composition includes tin, lead, zinc and other non-ferrous metals, and in a small and stable percentage, is formed during the oxidative process of pellet roasting, direct reduction of iron and smelting. All this is due to the small amount of impurities of these metals in the ore, as well as their partial removal.

It has been determined that the removal of zinc is possible during metallization and melting. Lead evaporates during firing and reduction, but to a small extent, and the smelting process will be the main one. Tin, like antimony, is hardly removed from the composition due to their low content, or even passes into the metal. Laboratory studies have shown that what iron consists of is determined by the amount of non-ferrous metals as impurities. Their percentage ranges from less than 0.01, both in steel containing nickel, chromium and copper, to less than 0.001 in compositions with tin, lead, arsenic, antimony and zinc.