How to get manganese dioxide with potassium permanganate

Heating to obtain potassium manganate, and oxygen, if heated a little (190 C) K2MNO4 will also decompose manganese dioxide.

The by-product K2O is also soluble.

2kmNO4 (heating) = K2mNO4 + MNO2 + O2 and then filtered with water, potassium manganate is soluble in water, its aqueous solution is green, manganese dioxide is insoluble in water, and it is definitely a powder. What's the trouble, will Taomi? Put more water each time, wash 3-4 times and wait for the manganese dioxide to sink to the bottom to deflate the water, leave some water for the last time, heat and evaporate, and filter it clean and not wasted.

It's the easiest way to do it, if it's all trouble...

I add that you can try straining with boiling water, preferably by putting the burned stuff in an Erlenmeyer flask.

Add water and put it on the electric stove to boil, don't go to it, the water on it will quickly turn green, keep changing the water on it to clean water, and it will be clean soon, or let the potassium manganate dissolve as much as possible, pour out 80% of the water at a time, potassium manganate will only be left 20%, and it will only be left after three times, it is already very easy, you must be patient when doing chemical experiments, let alone at home. Besides, manganese dioxide is a very cheap thing, so why use potassium permanganate.

What about making it? (I have been reluctant to use the test-tube potassium permanganate at home), dry battery.

The black thing inside is pure carbon (carbon black.

It's too troublesome, and it's dangerous Here are ways to make purer potassium permanganate:

1 Take a dry beaker and add distilled water to one-half of the beaker (250ml);

2 Add 1 teaspoon potassium permanganate and stir well;

3 Take another dry beaker, add hydrogen peroxide (30%, very cheap) to one-third of the beaker (250ml), dilute to one-half;

4 Carefully mix the two solutions, and you can see that there is a black precipitate formed, which is Mno2 5Filtration, no evaporation (advantages of this method: safe, high utilization) Note, there can be no H+ in the solution, because this may lead to the generation of Mn2+) I have limited knowledge, thank you for your support!

2kmNO4 = K2MNO4 + MNO2 + O2, then add water to dissolve K2MNO4, filter, wash, and dry to get.

Potassium permanganate plus hydrogen peroxide can not get manganese dioxide, and only manganese hydroxide Mn(OH)3 reaction formula is as follows: kmNO4+2H2O2===Mn(OH)3+KOH+2O2

Therefore, the following method can be used:

2kmno4+3so2+4koh===3k2so4+2mno2↓+2h2o

4kmNO4=== (heating) 2K2O+4mNO2 +3O2 10kmNO4+3C2H2+3H2O===10KoH+10mNO2 +6CO2

Of course, there are some ways!

Under standard conditions, the temperature at which potassium permanganate is decomposed into potassium manganate, manganese dioxide, and oxygen is 240. In practice, temperatures typically exceed 240 degrees and can reach 400 degrees or more. However, if the temperature is too high, the cooling time of the labware will be longer.

If there is a sudden change in temperature during the cooling process, the experimental instrument will also be damaged. Therefore, it is not recommended to heat the temperature too high.

Heating. 2kmno4=k2mno4+mno2+o2

This is also how oxygen is produced in the laboratory.

Made with potassium manganatePotassium permanganatePotassium permanganate is a strong oxidizing agent, and it is associated withReducing agentThe reaction will vary depending on the acidity of the solution. In an acidic solution, potassium permanganate reacts with potassium sulfite, and the product is manganese sulfate:

2kmNO4 5K2SO3 3H2SO42MNSO4 6K2SO4 3H2O are reacted in a neutral solution, and the product is manganese dioxide.

2kmNO4 3K2SO3 H2O2MNO2 3K2SO4 2KOH is reacted in an alkaline solution, and the product is potassium manganate:

2kmno4＋k2so3＋2koh2k2mno4＋k2so4＋h2o。

Potassium permanganateIt has strong oxidizing properties.

It is commonly used as an oxidant in laboratories and industries, and in case of ethanol.

i.e. decomposition. It will slowly decompose into manganese dioxide and potassium salts in acidic media.

and oxygen. Light has a catalytic effect on this decomposition, so it is often stored in brown bottles in the laboratory. As can be seen from the elemental potential diagram and the oxidation state diagram of the free energy, it is extremely oxidizing.

In alkaline solutions, its oxidation is not as strong as in acidic solutions. When used as an oxidant, its reduction products vary depending on the acidity and alkalinity of the medium.

Summary. Potassium perchlorate and manganese dioxide reaction to prepare potassium permanganate

Manganese dioxide first reacts with potassium chlorate to form potassium permanganate, chlorine and oxygen, 2mNO2 + 2KCLO3 = 2kmNO4 + Cl2 + O2

Potassium permanganate is then decomposed to produce potassium manganate, manganese dioxide and oxygen, 2kmNO4=K2MNO4+MNO2+O2

Potassium manganate reacts with chlorine to form potassium chloride, manganese dioxide, and oxygen.

k2mno4+cl2=2kcl+mno2+o2

The three add up.

2kClO3=2kCl+3O2 (mNO2 catalysis) (conditions include heating, gas symbol omitted).

Potassium perchlorate and manganese dioxide are reacted to produce potassium permanganate.

The process of potassium perchlorate and manganese dioxide reaction to prepare potassium permanganate: manganese dioxide first reacts with potassium chlorate to form potassium permanganate, chlorine gas and oxygen, 2mNO2 + 2KCLO3 = 2kmNO4 + Cl2 + O2 potassium permanganate and then decomposes to generate potassium manganate, manganese dioxide and oxygen, 2kmNO4 = K2mNO4 + mnO2 + O2 potassium manganate and then reacts with chlorine to generate potassium chloride, manganese dioxide and oxygen. K2mNO4 + Cl2 = 2KCl + Mno2 + O2 add up to 2Kclo3 = 2KCl + 3O2 (Mno2 catalysis) (the conditions all include heating, and the gas symbol is omitted).

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The chemical equation for the production of oxygen from potassium permanganate is: 2kmno = k mno + mno + o .

Potassium permanganate is commonly used in the laboratory to produce oxygen, and the text expression of potassium permanganate to produce oxygen is: potassium permanganate (heating) potassium manganate + manganese dioxide + oxygen.

Properties of potassium permanganate.

Potassium permanganate is a blackish-purple, elongated prismatic crystal or granule with a bluish metallic luster. In contact with some organic substances or easy oxides, it is easy to occur, soluble in water and lye, and Weishi Chunling is soluble in methanol, acetone, sulfuric acid, with a molecular formula of KMNO4 and a molecular weight. The melting point is 240 °C, which is stable, but contact with flammable materials may cause disasters.

Potassium permanganate is one of the strongest oxidizing agents, as an oxidant is greatly affected by pH, and has the strongest oxidizing ability in acidic solutions. Its corresponding acids permanganate HMNO4 and anhydride Mn2O7 are strong oxidants, which can automatically decompose and heat, and cause combustion in contact with organic matter.

Storage conditions of potassium permanganate: the warehouse is ventilated, lightly loaded and unloaded, and stored separately from organic matter, reducing agent, sulfur and phosphorus flammables.

Because the oxidation of potassium permanganate increases with the increase of acidity, potassium permanganate is reduced to Mn2+ under the condition of high acid content. It is reduced to MNO under neutral conditions; It is reduced to mnO2- under alkaline conditions, so manganese dioxide cannot exist under acidic conditions.

Potassium permanganate is a black-purple, elongated prismatic crystal or granule with a blue metallic luster; Odorless; In contact with some organic substances or easy oxides, it is easy to occur**, soluble in water, lye, slightly soluble in methanol, acetone, sulfuric acid, and the molecular weight is.

The melting point is 240 °C, which is stable, but contact with flammable materials may cause disasters. Substances to avoid include reducing agents, strong acids, organic materials, flammable materials, billowing peroxides, alcohols, and chemically reactive metals.

In the reaction of potassium permanganate to oxygen, potassium permanganate (KMNO4) undergoes a decomposition reaction to produce oxygen (O2) and other products. This reaction can be written:

2kmno4(s) →k2mno4(s) +mno2(s) +o2(g)

In this reaction, potassium permanganate (KMno4) is broken down into oxygen (O2) and other products. Specifically:

1.Two potassium permanganate molecules (2kmNO4) decompose into one subliter to make potassium permanganate molecule (K2mNO4) and one manganese dioxide molecule (mnO2). Potassium permanganate is a reducing product of potassium permanganate, while manganese dioxide is an oxidation product.

2.At the same time, this reaction also produces oxygen (O2).

Therefore, in the process of producing oxygen from potassium permanganate, potassium permanganate is decomposed into potassium permanganate, manganese dioxide and oxygen. Carbon dioxide is not involved in this reaction, but is produced by the reaction of other components of potassium permanganate, such as hydrogen and oxygen, with oxygen in the surrounding air, but this is not normally captured or collected.

The equation for the ion reaction after trimming is: 2mNO4- +5H2O2 + 6H+ =2mN2+ +5O2 + 8H2O

The trim process is as follows:

The grinding hole of the ion blind withering equation before trim is mno4- +h2o2 + h+ =mn2+ +o2 + h2o

Note that MN gets 5 electrons from +7 +2;

Since the acidic potassium permanganate is originally in the solution and does not oxidize the oxygen in the water to oxygen, it must be the oxygen of hydrogen peroxide that is oxidized, and in H2O2, the locust O rises from -1 valence to 0 valence, and a hydrogen peroxide molecule needs to get 2 electrons;

The valency of the other elements remains unchanged, so the ratio of the number of Mno4- to H2O2 is 2:5;

The coefficients of other ions or ion clusters can be found according to the conservation theorem.