Shanxian Chemical
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Hydrogen Peroxide Decomposition Kinetics Lab Report
Experimental Report on Kinetics of Hydrogen Peroxide Decomposition
1. Experimental Purpose
To explore the kinetic law of hydrogen peroxide decomposition reaction, and to determine the kinetic parameters such as reaction rate constant and reaction order.
Second, the experimental principle
The equation of hydrogen peroxide decomposition reaction is:\ (2H_ {2} O_ {2}\ stackrel {k} {\ longrightarrow} 2H_ {2} O + O_ {2}\ uparrow\).
The relationship between the reaction rate and the concentration of hydrogen peroxide can usually be expressed as\ (r = k [H_ {2} O_ {2}] ^ {n}\), where\ (r\) is the reaction rate,\ (k\) is the reaction rate constant, and\ (n\) is the reaction order. By experimentally measuring the concentration of hydrogen peroxide at different times, the relationship between the reaction rate and the concentration is analyzed, and the values of\ (k\) and\ (n\) are determined.
The commonly used method for determining the concentration of hydrogen peroxide is the dosage gas method, which calculates the decomposition amount of hydrogen peroxide according to the volume of oxygen produced by decomposition, so as to obtain the concentration of hydrogen peroxide at different times.
III. Experimental Instruments and Reagents
1. ** Instruments **: supported conical flask, liquid separation funnel, measuring cylinder, water tank, electronic balance, stopwatch, etc.
2. ** Reagents **: hydrogen peroxide solution, manganese dioxide (catalyst), water, etc.
IV. Experimental Steps
1. ** Device Construction **: Connect the supported conical flask with the liquid separation funnel to ensure that the device is airtight. Place the supported conical flask in the water tank and connect the measuring cylinder through a catheter for collecting the generated oxygen.
2. ** Sample preparation **: Accurately weigh a certain mass of manganese dioxide into a conical flask with branches, measure a certain volume of hydrogen peroxide solution of known concentration with a measuring cylinder and add it to the separation funnel.
3. ** Reaction start and data recording **: Open the separation funnel piston, so that the hydrogen peroxide solution is slowly dripped into the conical flask with branches, and start the stopwatch at the same time. Record the volume of oxygen in the measuring cylinder at regular intervals.
4. ** Repeat the experiment **: Change the initial concentration of the hydrogen peroxide solution, repeat the above steps, and perform the experiment multiple times.
5. Data recording and processing
1. ** Data recording **: Record the volume of oxygen corresponding to different time points in each experiment.
| Number of experiments | Time\ (t\)/s | Volume of oxygen\ (V\)/mL |
|---|---|---|
| 1 |\ (t_ {1 }\) | \( V_ {1}\) |
| 1 |\ (t_ {2 }\) | \( V_ {2}\) |
|... |... |
| 2 |\ (t_ {1 }'\) | \( V_ {1 }'\) |
| 2 |\ (t_ {2 }'\) | \( V_ {2 }'\) |
|... |... |
2. ** Data Processing **:
- According to the ideal gas state equation and reaction equation, the volume of oxygen is converted into the amount of hydrogen peroxide decomposed substance, and then the concentration of hydrogen peroxide at different times\ ([H_ {2} O_ {2}]\).
- Graph with\ (\ ln [H_ {2} O_ {2}]\) vs. time\ (t\), if a straight line is obtained, the reaction is a first-order reaction, and the slope of the straight line is\ (-k\), from which the reaction rate constant\ (k\) can be obtained.
- Perform multiple experiments by changing the initial concentration of hydrogen peroxide, analyze the relationship between reaction rate and concentration, and determine the reaction order\ (n\).
6. Experimental results and discussion
1. ** Experimental results **: Through experimental data processing, the rate constant\ (k\) and reaction order\ (n\) of hydrogen peroxide decomposition reaction under different conditions are obtained.
2. ** RESULTS DISCUSSION **: Analyze the difference between the experimental results and the theoretical values, and discuss the factors that may affect the experimental results, such as the airtightness of the experimental device, the amount and activity of the catalyst, and the influence of reading errors on the determination of the reaction rate constant and reaction order.
VII. CONCLUSION
Through this experiment, the kinetic parameters of the hydrogen peroxide decomposition reaction were successfully determined, and the factors affecting the reaction rate were understood. It provides an experimental basis and method reference for further research on the kinetics of similar decomposition reactions.
1. Experimental Purpose
To explore the kinetic law of hydrogen peroxide decomposition reaction, and to determine the kinetic parameters such as reaction rate constant and reaction order.
Second, the experimental principle
The equation of hydrogen peroxide decomposition reaction is:\ (2H_ {2} O_ {2}\ stackrel {k} {\ longrightarrow} 2H_ {2} O + O_ {2}\ uparrow\).
The relationship between the reaction rate and the concentration of hydrogen peroxide can usually be expressed as\ (r = k [H_ {2} O_ {2}] ^ {n}\), where\ (r\) is the reaction rate,\ (k\) is the reaction rate constant, and\ (n\) is the reaction order. By experimentally measuring the concentration of hydrogen peroxide at different times, the relationship between the reaction rate and the concentration is analyzed, and the values of\ (k\) and\ (n\) are determined.
The commonly used method for determining the concentration of hydrogen peroxide is the dosage gas method, which calculates the decomposition amount of hydrogen peroxide according to the volume of oxygen produced by decomposition, so as to obtain the concentration of hydrogen peroxide at different times.
III. Experimental Instruments and Reagents
1. ** Instruments **: supported conical flask, liquid separation funnel, measuring cylinder, water tank, electronic balance, stopwatch, etc.
2. ** Reagents **: hydrogen peroxide solution, manganese dioxide (catalyst), water, etc.
IV. Experimental Steps
1. ** Device Construction **: Connect the supported conical flask with the liquid separation funnel to ensure that the device is airtight. Place the supported conical flask in the water tank and connect the measuring cylinder through a catheter for collecting the generated oxygen.
2. ** Sample preparation **: Accurately weigh a certain mass of manganese dioxide into a conical flask with branches, measure a certain volume of hydrogen peroxide solution of known concentration with a measuring cylinder and add it to the separation funnel.
3. ** Reaction start and data recording **: Open the separation funnel piston, so that the hydrogen peroxide solution is slowly dripped into the conical flask with branches, and start the stopwatch at the same time. Record the volume of oxygen in the measuring cylinder at regular intervals.
4. ** Repeat the experiment **: Change the initial concentration of the hydrogen peroxide solution, repeat the above steps, and perform the experiment multiple times.
5. Data recording and processing
1. ** Data recording **: Record the volume of oxygen corresponding to different time points in each experiment.
| Number of experiments | Time\ (t\)/s | Volume of oxygen\ (V\)/mL |
|---|---|---|
| 1 |\ (t_ {1 }\) | \( V_ {1}\) |
| 1 |\ (t_ {2 }\) | \( V_ {2}\) |
|... |... |
| 2 |\ (t_ {1 }'\) | \( V_ {1 }'\) |
| 2 |\ (t_ {2 }'\) | \( V_ {2 }'\) |
|... |... |
2. ** Data Processing **:
- According to the ideal gas state equation and reaction equation, the volume of oxygen is converted into the amount of hydrogen peroxide decomposed substance, and then the concentration of hydrogen peroxide at different times\ ([H_ {2} O_ {2}]\).
- Graph with\ (\ ln [H_ {2} O_ {2}]\) vs. time\ (t\), if a straight line is obtained, the reaction is a first-order reaction, and the slope of the straight line is\ (-k\), from which the reaction rate constant\ (k\) can be obtained.
- Perform multiple experiments by changing the initial concentration of hydrogen peroxide, analyze the relationship between reaction rate and concentration, and determine the reaction order\ (n\).
6. Experimental results and discussion
1. ** Experimental results **: Through experimental data processing, the rate constant\ (k\) and reaction order\ (n\) of hydrogen peroxide decomposition reaction under different conditions are obtained.
2. ** RESULTS DISCUSSION **: Analyze the difference between the experimental results and the theoretical values, and discuss the factors that may affect the experimental results, such as the airtightness of the experimental device, the amount and activity of the catalyst, and the influence of reading errors on the determination of the reaction rate constant and reaction order.
VII. CONCLUSION
Through this experiment, the kinetic parameters of the hydrogen peroxide decomposition reaction were successfully determined, and the factors affecting the reaction rate were understood. It provides an experimental basis and method reference for further research on the kinetics of similar decomposition reactions.
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