Shanxian Chemical
SUPPLEMENTS
Hydrogen Peroxide Decomposition Catalase Activation Energy
INTRODUCTION
I. INTRODUCTION
The occurrence of chemical reactions requires overcoming a certain energy barrier, which is the activation energy. The catalyst can reduce the activation energy of the reaction and speed up the reaction rate. Catalase can efficiently catalyze the decomposition of hydrogen peroxide. Exploring the activation energy of its catalytic reaction is of great significance for understanding the mechanism of enzymatic reactions.
II. EXPERIMENTAL PRINCIPLE
Hydrogen peroxide is decomposed into water and oxygen under the catalysis of catalase. According to the Arrhenius formula $k = A e ^ {-\ frac {Ea} {RT}} $ (where $k $is the reaction rate constant, $A $is the pre-index factor, $Ea $is the activation energy, $R $is the gas constant, $T $is the absolute temperature), by measuring the reaction rate constants at different temperatures, plot $\ ln k $to $\ frac {1} {T} $, and the activation energy $Ea $can be obtained from the slope of the straight line.
III. Experimental Materials and Methods
(1) Experimental Materials
1. ** Hydrogen peroxide solution **: a certain concentration, as the reaction substrate.
2. ** Catalase **: Extraction or purchase of finished products from biological materials such as fresh liver.
3. ** Other reagents **: Buffers, etc. used to maintain the pH and other conditions of the reaction system.
4. ** Experimental instruments **: constant temperature water bath pot, stopwatch, measuring cylinder, conical bottle, rubber stopper, catheter, sink, tray balance, thermometer, etc.
(2) Experimental methods
1. ** Extraction and preparation of catalase **: Take fresh liver as an example, wash, shred, add an appropriate amount of quartz sand and buffer to grind, centrifuge the supernatant, obtain the crude extract of catalase, measure the protein content or enzyme activity, and dilute it appropriately for later use.
2. ** Determination of the decomposition reaction rate of hydrogen peroxide at different temperatures **
- Take multiple clean conical bottles, add the same amount of hydrogen peroxide solution respectively, and place them in a constant temperature water bath at different temperatures to preheat.
- Add the same amount of catalase solution to the preheated hydrogen peroxide solution, quickly plug the rubber plug, and the other end of the catheter is passed into the water tank to collect oxygen.
- Record the time taken to collect a certain volume of oxygen in the cylinder, repeat it many times, take the average value, and calculate the reaction rate at different temperatures $v $.
- Calculate the reaction rate constant at different temperatures $k $according to the relationship between the reaction rate and the rate constant.
IV. Experimental Results and Analysis
(1) Experimental Data Records
Record different temperatures $T $and corresponding reaction rate constants $k $, as follows:
| Temperature $T (K) $| Reaction rate constant $k (s ^ {-1}) $|
|---|---|
| $T_1 $| $k_1 $|
| $T_2 $| $k_2 $|
|... |
(2) Data Processing and Analysis
1. The graph is plotted with $\ ln k $as the ordinate and $\ frac {1} {T} $as the abscissa.
2. From the slope of the obtained line $m = -\ frac {Ea} {R} $, it is known that $R = 8.314 J\ cdot mol ^ {-1}\ cdot K ^ {-1} $, the activation energy of catalase-catalyzed decomposition of hydrogen peroxide can be calculated $Ea = -mR $.
Fifth, Conclusion
The activation energy value of catalase-catalyzed decomposition of hydrogen peroxide is obtained by experimental measurement and calculation. This value reflects the degree to which catalase reduces the activation energy of the reaction, providing an experimental basis for in-depth understanding of the enzyme catalysis mechanism, and has important reference value for the research of related metabolic processes in organisms and industrial enzyme catalysis applications.
I. INTRODUCTION
The occurrence of chemical reactions requires overcoming a certain energy barrier, which is the activation energy. The catalyst can reduce the activation energy of the reaction and speed up the reaction rate. Catalase can efficiently catalyze the decomposition of hydrogen peroxide. Exploring the activation energy of its catalytic reaction is of great significance for understanding the mechanism of enzymatic reactions.
II. EXPERIMENTAL PRINCIPLE
Hydrogen peroxide is decomposed into water and oxygen under the catalysis of catalase. According to the Arrhenius formula $k = A e ^ {-\ frac {Ea} {RT}} $ (where $k $is the reaction rate constant, $A $is the pre-index factor, $Ea $is the activation energy, $R $is the gas constant, $T $is the absolute temperature), by measuring the reaction rate constants at different temperatures, plot $\ ln k $to $\ frac {1} {T} $, and the activation energy $Ea $can be obtained from the slope of the straight line.
III. Experimental Materials and Methods
(1) Experimental Materials
1. ** Hydrogen peroxide solution **: a certain concentration, as the reaction substrate.
2. ** Catalase **: Extraction or purchase of finished products from biological materials such as fresh liver.
3. ** Other reagents **: Buffers, etc. used to maintain the pH and other conditions of the reaction system.
4. ** Experimental instruments **: constant temperature water bath pot, stopwatch, measuring cylinder, conical bottle, rubber stopper, catheter, sink, tray balance, thermometer, etc.
(2) Experimental methods
1. ** Extraction and preparation of catalase **: Take fresh liver as an example, wash, shred, add an appropriate amount of quartz sand and buffer to grind, centrifuge the supernatant, obtain the crude extract of catalase, measure the protein content or enzyme activity, and dilute it appropriately for later use.
2. ** Determination of the decomposition reaction rate of hydrogen peroxide at different temperatures **
- Take multiple clean conical bottles, add the same amount of hydrogen peroxide solution respectively, and place them in a constant temperature water bath at different temperatures to preheat.
- Add the same amount of catalase solution to the preheated hydrogen peroxide solution, quickly plug the rubber plug, and the other end of the catheter is passed into the water tank to collect oxygen.
- Record the time taken to collect a certain volume of oxygen in the cylinder, repeat it many times, take the average value, and calculate the reaction rate at different temperatures $v $.
- Calculate the reaction rate constant at different temperatures $k $according to the relationship between the reaction rate and the rate constant.
IV. Experimental Results and Analysis
(1) Experimental Data Records
Record different temperatures $T $and corresponding reaction rate constants $k $, as follows:
| Temperature $T (K) $| Reaction rate constant $k (s ^ {-1}) $|
|---|---|
| $T_1 $| $k_1 $|
| $T_2 $| $k_2 $|
|... |
(2) Data Processing and Analysis
1. The graph is plotted with $\ ln k $as the ordinate and $\ frac {1} {T} $as the abscissa.
2. From the slope of the obtained line $m = -\ frac {Ea} {R} $, it is known that $R = 8.314 J\ cdot mol ^ {-1}\ cdot K ^ {-1} $, the activation energy of catalase-catalyzed decomposition of hydrogen peroxide can be calculated $Ea = -mR $.
Fifth, Conclusion
The activation energy value of catalase-catalyzed decomposition of hydrogen peroxide is obtained by experimental measurement and calculation. This value reflects the degree to which catalase reduces the activation energy of the reaction, providing an experimental basis for in-depth understanding of the enzyme catalysis mechanism, and has important reference value for the research of related metabolic processes in organisms and industrial enzyme catalysis applications.
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