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Balanced Chemical Equation for Hydrogen Peroxide Decomposition
On the Balance Chemical Equation for Hydrogen Peroxide Decomposition
The chemical formula varies greatly, and the reaction formula is clear. Now on the reaction of hydrogen peroxide decomposition, we should find its equilibrium formula.
For hydrogen peroxide, the formula is $H_ {2} O_ {2} $, and it can slowly decompose at room temperature. The products produced by this reaction are water and oxygen. The formula for water is $H_ {2} O $, and the formula for oxygen is $O_ {2} $.
The formula for the initial reaction, $H_ {2} O_ {2}\ longrightarrow H_ {2} O + O_ {2} $. However, looking at this equation, the number of left and right atoms is not equal. The hydrogen atom on the left is two, the oxygen atom is two; the hydrogen atom on the right is two, and the oxygen atom is three. To make an equilibrium, the coefficient needs to be adjusted.
Observe that the oxygen atom is two in hydrogen peroxide and is divided between water and oxygen. You can add a coefficient two before water to get $H_ {2} O_ {2}\ longrightarrow 2H_ {2} O + O_ {2} $. At this time, the hydrogen atom is two left and four right, and it is not flat. Therefore, adding a coefficient two before hydrogen peroxide gives an equilibrium formula: $2H_ {2} O_ {2}\ stackrel {catalyst }{=\!=\!=} 2H_ {2} O + O_ {2}\ uparrow $.
In this equation, the catalyst can increase the reaction rate, but its own properties and mass remain unchanged before and after the reaction. Taking manganese dioxide as an example, it is often used as a catalyst for this reaction to accelerate the decomposition of hydrogen peroxide and make oxygen escape quickly.
From this perspective, to find an equilibrium chemical equation, it is necessary to understand the reaction and the quality of the product, carefully observe the number of atoms, and adjust the coefficient, in order to form an accurate formula, so as to understand the chemical change.
The chemical formula varies greatly, and the reaction formula is clear. Now on the reaction of hydrogen peroxide decomposition, we should find its equilibrium formula.
For hydrogen peroxide, the formula is $H_ {2} O_ {2} $, and it can slowly decompose at room temperature. The products produced by this reaction are water and oxygen. The formula for water is $H_ {2} O $, and the formula for oxygen is $O_ {2} $.
The formula for the initial reaction, $H_ {2} O_ {2}\ longrightarrow H_ {2} O + O_ {2} $. However, looking at this equation, the number of left and right atoms is not equal. The hydrogen atom on the left is two, the oxygen atom is two; the hydrogen atom on the right is two, and the oxygen atom is three. To make an equilibrium, the coefficient needs to be adjusted.
Observe that the oxygen atom is two in hydrogen peroxide and is divided between water and oxygen. You can add a coefficient two before water to get $H_ {2} O_ {2}\ longrightarrow 2H_ {2} O + O_ {2} $. At this time, the hydrogen atom is two left and four right, and it is not flat. Therefore, adding a coefficient two before hydrogen peroxide gives an equilibrium formula: $2H_ {2} O_ {2}\ stackrel {catalyst }{=\!=\!=} 2H_ {2} O + O_ {2}\ uparrow $.
In this equation, the catalyst can increase the reaction rate, but its own properties and mass remain unchanged before and after the reaction. Taking manganese dioxide as an example, it is often used as a catalyst for this reaction to accelerate the decomposition of hydrogen peroxide and make oxygen escape quickly.
From this perspective, to find an equilibrium chemical equation, it is necessary to understand the reaction and the quality of the product, carefully observe the number of atoms, and adjust the coefficient, in order to form an accurate formula, so as to understand the chemical change.
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