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Hydrogen Peroxide Disproportionation Reaction
"On the disproportionation reaction of hydrogen peroxide"
Hydrogen peroxide is a chemical substance, and it has the property of disproportionation. This is the principle of chemistry.
Hydrogen peroxide, the molecular formula is $H_ {2} O_ {2} $. Under appropriate conditions, it can spontaneously carry out a disproportionation reaction. The essence of the reaction is the oxygen element in the hydrogen peroxide molecule, and the valence of the hydrogen peroxide is dissimilated. The valence of some oxygen elements increases, from -1 to 0, generating oxygen; the valence of some oxygen elements decreases, from -1 to -2, generating water.
The chemical equation of the reaction is: $2H_ {2} O_ {2} = 2H_ {2} O + O_ {2}\ uparrow $. This reaction does not require an external strengthening catalyst and can occur slowly at room temperature. However, if an appropriate amount of manganese dioxide and other catalysts are added, the reaction rate will be greatly increased.
The function of the catalyst is to reduce the activation energy of the reaction, so that more hydrogen peroxide molecules can exceed the energy barrier of the reaction, thereby accelerating the progress of the reaction. Looking at this disproportionation reaction, hydrogen peroxide is both an oxidizing agent and a reducing agent. It shows unique chemical properties in chemical reactions and has important applications in many fields such as chemical industry and medical treatment. In the chemical industry, it can be used to prepare certain substances; in medicine, it is often used as a disinfectant, because the new oxygen produced by its decomposition is highly oxidizing and can kill bacteria.
This disproportionation reaction of hydrogen peroxide is like a shining star in the chemical world, illuminating the path of our exploration of the chemical reaction mechanism.
Hydrogen peroxide is a chemical substance, and it has the property of disproportionation. This is the principle of chemistry.
Hydrogen peroxide, the molecular formula is $H_ {2} O_ {2} $. Under appropriate conditions, it can spontaneously carry out a disproportionation reaction. The essence of the reaction is the oxygen element in the hydrogen peroxide molecule, and the valence of the hydrogen peroxide is dissimilated. The valence of some oxygen elements increases, from -1 to 0, generating oxygen; the valence of some oxygen elements decreases, from -1 to -2, generating water.
The chemical equation of the reaction is: $2H_ {2} O_ {2} = 2H_ {2} O + O_ {2}\ uparrow $. This reaction does not require an external strengthening catalyst and can occur slowly at room temperature. However, if an appropriate amount of manganese dioxide and other catalysts are added, the reaction rate will be greatly increased.
The function of the catalyst is to reduce the activation energy of the reaction, so that more hydrogen peroxide molecules can exceed the energy barrier of the reaction, thereby accelerating the progress of the reaction. Looking at this disproportionation reaction, hydrogen peroxide is both an oxidizing agent and a reducing agent. It shows unique chemical properties in chemical reactions and has important applications in many fields such as chemical industry and medical treatment. In the chemical industry, it can be used to prepare certain substances; in medicine, it is often used as a disinfectant, because the new oxygen produced by its decomposition is highly oxidizing and can kill bacteria.
This disproportionation reaction of hydrogen peroxide is like a shining star in the chemical world, illuminating the path of our exploration of the chemical reaction mechanism.
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