Dilute nitric acid passes through excess iron powder to form ferric or divalent iron? It s better to

Dilute nitric acid is added with excess iron powder to produce bivalent Fe2+

Although dilute nitric acid is highly oxidizing and can oxidize iron to ferric ions Fe3+, excess iron can continue to react with ferric ions Fe3+ to form bivalent Fe2+, so the final result is bivalent Fe2+

Bivalent. The amount of nitric acid is first reacted to form trivalent iron, but due to the excess iron, the trivalent is reduced to bivalent.

This problem is a tireless problem in high school chemistry, nitric acid and iron are always entangled, either one of them is excessive, or the nitric acid is dilute and concentrated, and then sulfuric acid is added...

Step 1: Fe + 4Hno3 Fe (NO3) 3 + No + 2H2O Due to the excess of Fe, the second step is carried out

2fe3+ +fe == 3fe2+

So the reaction is bivalent iron in the end.

Hope it can help you

2 valence, Mr. 3 valence, and then iron powder is excessive, 2Fe3+ + Fe = 3Fe2+ reaction occurs, and it becomes 2 valence.

The replacement reaction metals in junior high and middle schools are all 2-valent, and the valency does not change after the reaction.

Substantial Hno3 now oxidizes Fe to Fe3+, and then the remaining Fe reduces Fe3+ to Fe2+

Hno3 now oxidizes Fe to Fe3+, and then the remaining Fe reduces Fe3+ to Fe2+

Hello, I am glad to serve you and give you the following answer: The reaction between excess iron powder and a certain amount of dilute nitric acid without trivalent iron ions is because the oxidation of dilute nitric acid is too weak to oxidize iron powder into trivalent iron ions. There are two ways to solve this problem:

1.Increase the concentration of dilute nitric acid: Increasing the concentration of dilute nitric acid to a certain level can enhance its oxidation, so that iron powder can be oxidized into ferric ions.

2.Add oxidants: Some oxidants with strong oxidizing properties, such as hydrogen peroxide, chlorine peroxide, etc., can be added to enhance the oxidation of dilute nitric acid and oxidize iron powder into ferric ions.

Steps:1Increase the concentration of dilute nitric acid to a certain extent, or add some oxidants with strong oxidizing properties; 2.

Mix iron powder and dilute nitric acid and stir well; 3.heat the mixture so that it reacts; 4.Cool the mixture and do the dough to collect the ferric ion solution.

Personal tip: In the experiment, pay attention to control the reaction temperature, so as not to overheat the reaction and affect the reaction effect. In addition, attention should be paid to controlling the concentration of dilute nitric acid and the amount of oxidant added to ensure the effectiveness of the reaction.

Summary. Dilute nitric acid is added with excess iron powder to produce bivalent Fe2+Although dilute nitric acid is highly oxidizing and can oxidize iron to ferric ions Fe3+, excess iron can continue to react with ferric ions Fe3+ to form divalent Fe2+.

So what you get in the end is bivalent Fe2+.

Dilute nitric acid is added to the dust of the stove and the excess iron powder is used to produce bivalent Fe2+. Although dilute nitric acid has strong oxidation and can oxidize Tebichan to ferric ion Fe3+, excess iron can continue to react with ferric ion Fe3+ to form divalent Fe2+. So what you get in the end is bivalent Fe2+.

Can you tell us more about that?

If a small amount of Fe is added, nitric acid will oxidize the iron powder into trivalent iron, and after adding excess iron powder, 2Fe3+Fe=3Fe2+, the trivalent iron will be reduced to bivalent iron by the excess iron powder. In general, this is a redox reaction process, and there are two steps in the process.

Divalent iron reacts with dilute nitric acid to form nitrogen dioxide. Nitric acid is a strong acid with strong oxidation and corrosiveness, which belongs to the monologic inorganic strong acid, which is one of the six major inorganic strong acids, and is also an important chemical raw material. It can be used in industry to make fertilizers, pesticides, explosives, dyes, salts, etc.; In organic chemistry, the mixture of concentrated nitric acid and concentrated sulfuric acid is an important nitrification reagent, and its aqueous solution is commonly known as nitrate water or ammonia nitrogen water.

Iron is a metallic element with atomic number 26 and an elemental chemical formula for iron: Fe. Pure iron is white or silvery-white, with a metallic luster.

Melting point 1538, boiling point Nenbuhu 2750, soluble in strong acid and medium strong acid, insoluble in water. Iron has 0, +2, +3, +4, +5 and +6 valences, of which +2 and +3 are more common, and +4, +5 and +6 are rare.

Both concentrated nitric acid and dilute nitric acid are strongly oxidizing acids and neither produces H2.

FE reacts with nitric acid, whether it is trivalent iron or divalent iron mainly depends on the amount of iron and nitric acid (1) If there is too much nitric acid in the reaction, the iron is oxidized to the most **+3 valence.

Fe + 4 Hno3 (dilute) = Fe (No3)3 + No + 2 H2O

Iron reacts with dilute nitric acid to form NO).

Fe + 6 Hno3 (concentrated) = Heat = Fe (No3) 3 + 3 No2 + 3 H2O

At room temperature, Fe should be passivated in concentrated nitric acid and concentrated sulfuric acid, and heated to continue the reaction, Fe is oxidized to +3 valence, and nitric acid is reduced to NO2).

2) If there is an excess of iron, it will react with +3 ferric ions to form +2 valence ferrous nitrate Fe + 2Fe(No3)3 == 3Fe(No3)2

The reaction formula is as follows:

Fe + 4Hno (dilute) ==Fe (No) No + 2H O Excess nitric acid.

3Fe + 8Hno (dilute) == 3Fe (NO) 2O Fe excess.

The ratio of iron to nitric acid is 2:8.

Less than 1:4, nitric acid excess, the equation remains unchanged.

>1:4, iron excess, the equation changes, because ferric iron can oxidize elemental iron to form ferric.

2fe(no₃)₃fe=3fe(no₃)₂

Total reaction: 3Fe deca 8Hno = 3Fe (NO3) + 2NO + 4HO

4fe+12hno3=3fe(no3)2+fe(no3)3+3no+6h2o

Since the formation of ferrous iron is 3:8 and the formation of ferric iron is 1:4, it should be that there are both ferric iron and ferric iron in the product.