Iron and copper powders react with nitric acid, and iron does not react with copper nitrate

The first step of the reaction, if it is concentrated nitric acid, the chemical reaction occurs: 6Hno3 + Fe Fe(NO3)3+3NO2 +3H2O; 4Hno3+Cu Cu(NO3)2+2NO2 +2H2O or dilute nitric acid, 4HNO3+Fe Fe(NO3)3+NO+2H2O; 8hno3+3cu＝3cu(no3)2+2no↑+4h2o。At the end of the above two reactions, if there is an excess of Fe or copper, an ionic reaction will occur 2Fe3++Fe 3Fe2+ or 2Fe3++Cu 2Fe2++Cu2+, which will make the solution contain Fe2+. If Hno3 is added, the ionic reaction will occur 3Fe2++NO32-+4H+ 3Fe3++NO+2H2O, so there will be gas release.

If the first Hno3 is not excessive, then there is a high probability that Fe2+ is present in the solution after the reaction, and when HNo3 is added again, Fe2+ will be oxidized by Hno3 to Fe3+ and the gas will be released.

It is because of the ferrous ions that are generated for the first time, and the ferrous ions react with nitric acid to form no gas.

Because copper reacts with Fe(NO3)3, the product of the reaction between nitric acid and Fe, Fe2+

Nitric acid Hno3 and Fe2+ are then added to undergo a redox reaction to form gas.

Copper does not, it exists in the form of bivalent, and the divalent iron in the solution is oxidized to trivalent iron, releasing nitrogen dioxide.

The chemical equation for the reaction of copper nitrate and iron: Fe+Cu(NO) Cu+Fe(NO).

Because the acidic conditions of hydrolysis are very weak, the nitrate cannot play an oxidizing role, and this Sun Zhaochun is a displacement reaction.

Copper nitrate hydrate decomposes into copper oxide, nitrogen dioxide and oxygen at around 170°C

2cu(no₃)₂s) →2cuo(s) +4no₂(g) +o₂(g)

Nitric acid can be produced by thermal decomposition of copper nitrate and chaining the resulting gas into water. The method is similar to the last step of the Oswa-method.

2cu(no₃)₂2cuo + 4no₂+ o₂

3no₂+ h₂o → 2hno₃+ no

Thin strips of wood impregnated with copper nitrate glow emerald green under flame, while magnesium nitrate produces an orange-green light resistant.

Yes, the chemical equation for the reaction of iron with copper nitrate.

It is Fe+Cu(NO) Fe(NO) Cu, because the acidic conditions of Na shirt hydrolysis are very weak, and the nitrate collapse difference cannot play an oxidizing role, which is just a displacement reaction.

Iron and copper nitrate undergo a displacement reaction because iron is more reactive than copper.

Iron and copper sulphate.

The phenomenon of anti-hole is that the surface of the iron layer precipitates a red substance, and the solution changes from blue to light green, and finally to brown.

Iron and copper nitrate react to form ferrous nitrate and copper.

Put a smooth iron wire in the blue copper nitrate solution, take it out after a few minutes, the surface of the iron wire will be covered with a layer of red copper, this reaction is the nuclear bucket roll replacement reaction, the iron replaces the copper nitrate pin burning solution.

If the red copper wire is immersed in ferrous nitrate solution, the copper wire will not change, indicating that copper cannot replace iron from ferrous nitrate solution, indicating that the chemical properties of iron are more active than copper.

The reaction between iron and nitric acid is related to the concentration of nitric acid, whether it is heated or not, and the excess and small amount of iron.

1. Iron reacts with dilute nitric acid – the resulting gas is nitric oxide (NO).

Iron is sufficient, dilute nitric acid is insufficient.

Equation: 3Fe + 8Hno3 (dilute) = = 3Fe (NO3) 2 + 2No + 4H2O

It can be understood that dilute nitric acid first reacts with iron to form ferric nitrate, and the excess iron powder reduces ferric nitrate to ferrous nitrate.

Dilute nitric acid in sufficient amounts, iron insufficient.

Equation: Fe + 4Hno3 (dilute) ==Fe (NO3) 3 + No + 2H2O Second, iron reacts with concentrated nitric acid - the gas generated is nitrogen dioxide (NO2) At room temperature, iron and concentrated nitric acid will undergo a passivation reaction - the surface of iron forms a dense oxide film (ferric tetroxide), and the reason for the reaction is that concentrated sulfuric acid has strong oxidation.

Under heating conditions, when the iron is sufficient, and the dilute nitric acid is insufficient.

Equation: FE

Hno3 (thick).

fe(no3)2

2no2↑2h2o

Under heating conditions, there is sufficient dilute nitric acid and insufficient iron.

Reaction equation: Fe

Hno3 (thick).

fe(no3)3

no2↑h2o

Iron and concentrated nitric acid reaction equation:

Fe + 6Hno (concentrated) = Fe (No) 3 No + 3H O

Concentrated nitric acid will decompose nitrogen dioxide and turn yellow when exposed to light, so concentrated nitric acid is often placed in a brown reagent bottle and placed in a dark place. Cold concentrated nitric acid can passivate iron and aluminum. Hot concentrated nitric acid does not passivate it.

The contact between iron and concentrated nitric acid will form an oxide film on the surface of the iron, and then it will not react with dilute nitric acid

The reaction is probably like this.

Excess nitric acid: Fe

4Hno3 = Fe(NO3)3+NO+2H2OIron excess: 3Fe+8HNO3=3Fe(NO3)2+2NO+4H2O

1、fe

6h+3no3-=

fe3+3no2↑

3h2o2、fe

4h+2no3-=

fe2+2no2↑

2H2O iron and concentrated nitric acid will be passivated, so the first two chemical equations are only a short meeting, and they will not react all the time.

Iron is a valuable reaction of metals with dilute nitric acid.

Iron reacts with dilute nitric acid, in which the proportions are different, and the products are also different. The ratio of iron to nitric acid is 2 to 8, and the reaction is good. Less than 1 to 4, nitric acid excess, the equation remains the same.

Greater than 1 to 4, there is an excess of iron, and the equation changes, because trivalent iron can oxidize elemental iron to form divalent iron.

Nitric acid dissolves many metals (silver can be dissolved) and produces salts, water, and nitrogen oxides. With the decrease of the concentration of the solution, the reduction product gradually transitions from Menghu ** to low price. The reduction product is generally a mixture, the metal reacts with concentrated nitric acid to form NO2, and the reaction with dilute nitric acid forms lower valence compounds such as NO, and only the very dilute cold nitric acid will react with magnesium, manganese and calcium to form hydrogen.