Shanxian Chemical
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PotassiumPermanganateandHydrogenPeroxideReaction
The reaction between potassium permanganate and hydrogen peroxide
Potassium permanganate ($KMnO_ {4} $), purple-black crystals are also highly oxidizing. Hydrogen peroxide ($H_ {2} O_ {2} $), a colorless transparent liquid, commonly known as hydrogen peroxide, is both oxidizing and reducing. When the two meet, there must be a chemical reaction.
When the two are mixed, the solution is slightly turbulent at first, and there seems to be an undercurrent of hidden power. Soon, there are bubbles gurgling out and escaping from the liquid surface. In this bubble, oxygen ($O_ {2} $) is also. The severity of the reaction depends on the concentration and dosage of the two. If the concentration of potassium permanganate is high and the dosage is large, and the amount of hydrogen peroxide is also sufficient, the reaction will be rapid, the bubbles will surge like a spring, and the color of the solution will gradually change.
In the reaction of capping potassium permanganate, the manganese element decreases from + 7 valence to a low-priced state, or + 2 valence, etc. The oxygen element in hydrogen peroxide rises from -1 valence to 0 valence, generating oxygen. The chemical reaction equation is roughly as follows: $2KMnO_ {4} + 5H_ {2} O_ {2} + 3H_ {2} SO_ {4} = K_ {2} SO_ {4} + 2MnSO_ {4} + 5O_ {2}\ uparrow + 8H_ {2} O $ (if in an acidic environment). In this reaction, sulfuric acid ($H_ {2} SO_ {4} $) plays an acidifying role, which promotes the smooth progress of the reaction.
From this perspective, the reaction of potassium permanganate and hydrogen peroxide is a typical redox reaction. Both have important applications and research values in chemical experiments and industrial production.
Potassium permanganate ($KMnO_ {4} $), purple-black crystals are also highly oxidizing. Hydrogen peroxide ($H_ {2} O_ {2} $), a colorless transparent liquid, commonly known as hydrogen peroxide, is both oxidizing and reducing. When the two meet, there must be a chemical reaction.
When the two are mixed, the solution is slightly turbulent at first, and there seems to be an undercurrent of hidden power. Soon, there are bubbles gurgling out and escaping from the liquid surface. In this bubble, oxygen ($O_ {2} $) is also. The severity of the reaction depends on the concentration and dosage of the two. If the concentration of potassium permanganate is high and the dosage is large, and the amount of hydrogen peroxide is also sufficient, the reaction will be rapid, the bubbles will surge like a spring, and the color of the solution will gradually change.
In the reaction of capping potassium permanganate, the manganese element decreases from + 7 valence to a low-priced state, or + 2 valence, etc. The oxygen element in hydrogen peroxide rises from -1 valence to 0 valence, generating oxygen. The chemical reaction equation is roughly as follows: $2KMnO_ {4} + 5H_ {2} O_ {2} + 3H_ {2} SO_ {4} = K_ {2} SO_ {4} + 2MnSO_ {4} + 5O_ {2}\ uparrow + 8H_ {2} O $ (if in an acidic environment). In this reaction, sulfuric acid ($H_ {2} SO_ {4} $) plays an acidifying role, which promotes the smooth progress of the reaction.
From this perspective, the reaction of potassium permanganate and hydrogen peroxide is a typical redox reaction. Both have important applications and research values in chemical experiments and industrial production.
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