Chemical equation for the dissolution of ferric oxide in HI solution

Chemical equation for the dissolution of ferric oxide in Hi solution: <>

This is not just a simple neutralization reaction between acids and basic oxides, because +3-valent iron is oxidizing and -1-valent iodine ions are reducing, so redox reactions can also occur.

Oxidation-reduction reaction is a type of reaction in which the oxidation number of an element changes before and after a chemical reaction. The essence of a redox reaction is the gain or loss of electrons or the shift of shared electron pairs. Redox reaction is one of the three basic reactions in chemical reactions (the other two are (Lewis) acid-base reaction and free radical reaction).

Combustion, respiration, photosynthesis, chemical batteries in production and life, metal smelting, rocket launches, etc. are all closely related to redox reactions in nature. The study of redox reactions is of great significance to the progress of mankind.

Before and after the redox reaction, the oxidation number of the element changes. Depending on the increase or decrease in the oxidation number, the redox reaction can be split into two half reactions: the half reaction with the increased oxidation number is called the oxidation reaction; The reaction with a decrease in oxidation number is called a reduction reaction.

Oxidation and reduction reactions are interdependent and cannot exist independently, and together they constitute redox reactions.

In the reaction, the substances that undergo oxidation reactions, called reducing agents, produce oxidation products; A substance that undergoes a reduction reaction, called an oxidant, produces a reduction product. Oxidation products are oxidizing but weaker than oxidants; The reducing product is reducing, but weaker than the reducing agent.

Whether a chemical reaction is a redox reaction can be judged according to whether the reaction has an increase in oxidation number, or whether there is electron gain, loss and transfer.

The determination of redox reactions in organic chemistry is usually based on whether the oxidation number of carbon changes: if the oxidation number of carbon increases, the reaction is an oxidation reaction; When the oxidation number of carbon decreases, this reaction is a reduction reaction. Since in the vast majority of organic matter, hydrogen always presents a positive valence state, and oxygen always presents a negative valence state, so the reaction of organic matter to obtain hydrogen and lose oxygen is generally called reduction reaction, and the reaction of oxygen loss and hydrogen loss is called oxidation reaction.

1. Strength and weakness law: oxidation: oxidant oxidation product; Reducibility: Reducing agent" reducing product.

2. Valence law: the element is in the most advanced state and only has oxidation; The element is in the lowest valence state and is only reductive; It is in the intermediate valence state, which is both oxidizing and reducing.

3. Transformation law: when the centering reaction occurs between different valence states of the same element, the oxidation number of the element is only close but not crossed, and the maximum value of the same element reaches the same valence state.

4. Priority law: For the same oxidant, when there are multiple reducing agents, it usually reacts with the most reducible reducing agent first.

5. Conservation law: The number of electrons obtained by the oxidant is equal to the number of electrons lost by the reducing agent.

Because of the valency of the iron element in ferric oxide.

is +3 valence, and the chemical valence of oxygen is -2 valence, so the chemical formula of ferric trioxide is Fe2O3

Volt trioxide Xun Qingchang iron can not get iron hydroxide in one step, and two short grip steps can.

fe2o3+6hcl=2fecl3+3h2o

fecl3+3naoh=fe(oh)3↓+3nacl

Ferric oxide is insoluble in water, and ferric oxide is a reddish-brown powder, commonly known as iron red; Chemical properties, it is an alkaline hexoxide, which can react with acids, can react with acidic oxides, and can react with reducing substances such as CO.

Iron is burned in oxygen to form Fe3O4, and red-hot iron reacts with water vapor to form Fe3O4. Iron is easily soluble in dilute inorganic acids and concentrated hydrochloric acid to form divalent iron salts and release hydrogen.

Ferric oxide is insoluble in water, and ferric oxide is a reddish-brown powder, commonly known as iron red; Chemical properties, it is an alkaline 100 oxide, which can react with acid, can react with acidic disorderly oxides, and can react with reducing substances such as CO.

Iron is burned in oxygen to form Fe3O4, and red-hot iron reacts with water vapor to form Fe3O4. Iron is easily soluble in dilute inorganic acids and concentrated hydrochloric acid to form ferric salts and release hydrogen.

Ferrous oxide reacts with hydrogen FeO+H2=Fe+H2O.

Ferric oxide reacts with hydrogen Fe2O3+3H2=2Fe+3H2O.

Ferrous oxide, one of the oxides of iron. It has a black powder in appearance with the chemical formula FeO, which is covalently bound to oxygen by iron in the oxidation state of +2 valence. Its mineral form is galena (wüstite).

Ferrous oxide is often confused with rust, but the main component of rust is hydrated iron oxide. Ferrous oxide is a non-integer compound in which the ratio of iron to oxygen varies from to.

Iron oxide, also known as ferric oxide, burnt limonite, burnt ochre, iron dan, iron red, red powder, Venetian red (the main component is iron oxide), etc. The chemical formula Fe2O3, soluble in hydrochloric acid, is a reddish-brown powder. Its reddish-brown powder is a low-grade pigment, known as iron oxide red in industry, used in paint, ink, rubber and other industries, can be used as a catalyst, glass, gemstones, metal polishing agent, can be used as ironmaking raw materials.

FeO+H2=Fe+H2O Ferrous oxide reacts with hydrogen Fe2O3+3H2=2Fe+3H2O ferric oxide reacts with hydrogen.

Red to reddish-brown powder. Odorless. Insoluble in water, organic acids and organic solvents.

Soluble in inorganic acids. There are two types: -type (positive magnetic) and -type (diamagnetic). The fineness of products produced by the dry process is generally less than 1 m.

Stable to light, heat and air. It is relatively stable to acids and alkalis. Strong tinting strength.

Relative density. If the content is low, the relative density is small. Refractive index.

The melting point is 1550, and it decomposes at about 1560[2].

Chemical properties. It has an alkaline oxide.

properties, which react with acids to form salts:[3].

fe2o3+3h2so4=fe2（so4）3+3h2o

Oxidizing:[3].

Fe2O3 + 3H2 = Heating = 2Fe + 3H2O

Fe2O3 + 3Co = High temperature = 2Fe + 3CO2

Preparation method: There are wet and dry preparation methods. Wet products have fine crystals, soft particles, easy to grind, and are easy to use as pigments. Dry products have large crystals and hard particles, and are suitable for magnetic materials and polishing and grinding materials. Bad match[1].

Wet. feso4+2naoh=fe（oh）2+na2so4

4fe（oh）2+o2+2h2o=4fe（oh）3

4feso4+4h2o+o2=2fe2o3↓+4h2so4

fe+h2so4=feso4+h2↑

Add a certain amount of 5% ferrous sulfate.

solution quickly with excess sodium hydroxide.

Solution reaction (requires an excess of alkali to be introduced into the air at room temperature to make it all turn into reddish-brown iron hydroxide colloid.

solution, as the crystal nucleus of deposited iron oxide. With the above-mentioned crystal nucleus as the carrier, ferrous sulfate as the medium, air is introduced into the 75-85, in the metal iron.

In the presence of ferrous sulfate, the ferrous sulfate reacts with oxygen in the air to form oxidized iron (i.e., iron red) and is deposited on the crystal nucleus, and the sulfate in the solution reacts with metallic iron to regenerate ferrous sulfate, which is then oxidized by the air to iron red and continues to be deposited, so that the cycle ends until the end of the whole process to generate red iron oxide [4].

Dry process. Nitric acid.

It 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 to obtain iron oxide red.

Product [4].

4fe（no3）3→2fe2o3+12no2↑+3o2↑

fe2o3·nh2o→fe2o3+nh2o

Iron oxide yellow can also be used as raw material, and iron oxide red can be obtained by calcination at 600 700 degrees [4].

Main uses: Magnetic materials.

Magnetic iron oxide.

Due to their special superparamagnetism, particles have broad application prospects in giant magnetoresistance, magnetic liquids and magnetic recording, soft magnetism, permanent magnetism, magneto-induced cooling, giant magnetoimpedance materials, magneto-optical devices, magnetic detectors, etc. Like a magnetic tape, it uses magnetic ultrafine particles of needle-like iron or iron oxide, while nano-iron oxide is a new type of magnetic recording material. Soft ferrite is widely used in radio communications, radio and television, automatic control, astronautics, radar navigation, measuring instruments, computers, printing, household appliances and biomedicine.