Shanxian Chemical
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Hydrogen Peroxide Decomposition Lab
On Hydrogen Peroxide Decomposition Experiment
I. INTRODUCTION
Learning is more valuable than practice, and the experimenter is the path to understanding the truth. There is now an experiment on the decomposition of hydrogen peroxide, which is related to the mystery of chemistry and can reveal the wonders of material changes. It is necessary to study it in detail.
II. Experimental supplies
Hydrogen peroxide solution, which is oxidizing, colorless and transparent. Also prepared manganese dioxide, which is a black-brown powder, acts as a catalyst in the reaction, which can change the rate of chemical reaction, and its own quality and chemistry remain unchanged before and after the reaction. In addition, a conical bottle is required, which is the place for the reaction; a liquid separation funnel to control the dripping rate of the hydrogen peroxide solution; a gas collection bottle to collect the generated gas; a water tank, with a drainage method to collect gas; several pipes to pass gas.
Third, experimental steps
First, put manganese dioxide in a clean conical bottle, and the dosage is appropriate, not too much or too little. More reactions will be excessive, and at least the catalytic effect will be poor. Second, fix the liquid separation funnel on the conical bottle, and ensure that the connection is well airtight to prevent gas from escaping. Slowly add hydrogen peroxide solution to the separation funnel, and the drop speed should be uniform. When viewed, bubbles gush out of the bottle quickly. This is the image of hydrogen peroxide decomposing under the catalysis of manganese dioxide to produce oxygen. Collect oxygen by drainage method, first fill the gas collection bottle with water, and place it upside down in the water tank. When there are continuous and uniform bubbles emerging from the mouth of the catheter, the catheter is extended into the mouth of the gas collection bottle until the bottle is full of water and gas. Remove the catheter, cover the frosted glass sheet, and take out the gas collection bottle.
IV. Experimental Phenomenon and Analysis
During the experiment, a large number of bubbles gushed out, indicating that the reaction was carried out violently. After testing, the collected gas can reignite the wood strip with fire star, which proves to be oxygen. According to the chemical principle, the reaction formula for the decomposition of hydrogen peroxide is: $2H_ {2} O_ {2}\ stackrel {MnO_ {2 }}{=\!=\!=} 2H_ {2} O + O_ {2}\ uparrow $. The reason why manganese dioxide can speed up the reaction rate is that it reduces the activation energy of the reaction, so that more hydrogen peroxide molecules can exceed the energy barrier of the reaction, and the effective collision increases, so the reaction accelerates.
Fifth, Conclusion
Therefore, hydrogen peroxide can be successfully decomposed to produce water and oxygen under the catalysis of manganese dioxide. This experiment not only proves the important role of catalysts in chemical reactions, but also gives us a deeper understanding of the chemical properties of hydrogen peroxide. The method of experimentation requires careful observation of subtle changes in order to explore the true meaning of chemistry and lay the foundation for future research on the principles of material change and the use of chemical methods to benefit people's livelihood.
I. INTRODUCTION
Learning is more valuable than practice, and the experimenter is the path to understanding the truth. There is now an experiment on the decomposition of hydrogen peroxide, which is related to the mystery of chemistry and can reveal the wonders of material changes. It is necessary to study it in detail.
II. Experimental supplies
Hydrogen peroxide solution, which is oxidizing, colorless and transparent. Also prepared manganese dioxide, which is a black-brown powder, acts as a catalyst in the reaction, which can change the rate of chemical reaction, and its own quality and chemistry remain unchanged before and after the reaction. In addition, a conical bottle is required, which is the place for the reaction; a liquid separation funnel to control the dripping rate of the hydrogen peroxide solution; a gas collection bottle to collect the generated gas; a water tank, with a drainage method to collect gas; several pipes to pass gas.
Third, experimental steps
First, put manganese dioxide in a clean conical bottle, and the dosage is appropriate, not too much or too little. More reactions will be excessive, and at least the catalytic effect will be poor. Second, fix the liquid separation funnel on the conical bottle, and ensure that the connection is well airtight to prevent gas from escaping. Slowly add hydrogen peroxide solution to the separation funnel, and the drop speed should be uniform. When viewed, bubbles gush out of the bottle quickly. This is the image of hydrogen peroxide decomposing under the catalysis of manganese dioxide to produce oxygen. Collect oxygen by drainage method, first fill the gas collection bottle with water, and place it upside down in the water tank. When there are continuous and uniform bubbles emerging from the mouth of the catheter, the catheter is extended into the mouth of the gas collection bottle until the bottle is full of water and gas. Remove the catheter, cover the frosted glass sheet, and take out the gas collection bottle.
IV. Experimental Phenomenon and Analysis
During the experiment, a large number of bubbles gushed out, indicating that the reaction was carried out violently. After testing, the collected gas can reignite the wood strip with fire star, which proves to be oxygen. According to the chemical principle, the reaction formula for the decomposition of hydrogen peroxide is: $2H_ {2} O_ {2}\ stackrel {MnO_ {2 }}{=\!=\!=} 2H_ {2} O + O_ {2}\ uparrow $. The reason why manganese dioxide can speed up the reaction rate is that it reduces the activation energy of the reaction, so that more hydrogen peroxide molecules can exceed the energy barrier of the reaction, and the effective collision increases, so the reaction accelerates.
Fifth, Conclusion
Therefore, hydrogen peroxide can be successfully decomposed to produce water and oxygen under the catalysis of manganese dioxide. This experiment not only proves the important role of catalysts in chemical reactions, but also gives us a deeper understanding of the chemical properties of hydrogen peroxide. The method of experimentation requires careful observation of subtle changes in order to explore the true meaning of chemistry and lay the foundation for future research on the principles of material change and the use of chemical methods to benefit people's livelihood.
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