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Hydrogen peroxide decomposition using bovine catalase.
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Department of Chemical EngineeringUniversity of Wisconsin – Madison
CBE 424 – Operations and Process LaboratoryInformal 1
Hydrogen Peroxide Decomposition Using Bovine Catalase
Christian FabianLen Roche
Experiment Date:07/11/13
Instructor:Jiménez
Abstract
Hydrogen peroxide was allowed to decompose under the influence
of catalysts at various temperatures, pH values, and substrate
concentrations. Specifically, potassium iodine and bovine catalase were
used to increase the rate of decomposition to adequate levels.
Furthermore, the decomposition was used to characterize catalase under
various conditions. The effects of temperature, pH, and initial enzyme and
substrate concentration on decomposition rates were used to accomplish
this. Enzyme performance was then modeled by Michaelis-Menten
kinetics. The Km for the decomposition was determined to be 0.1208 M,
while the V max found was 0.0097 M/min. Lastly, as hypothesized, catalase
activity is a maximum at bovine body temperature (~40 ºC) and blood pH
of 7.
i
Table of Contents
Abstract i
Introduction and Theory 1
Procedure 2
Startup 2
Adjusting Temperature 3
Adjusting pH 4
Adjusting Enzyme Concentration 4
Results and Discussion 5
Conclusions 10
References 11
Nomenclature 12
Appendices 13
Supplementary Graphs and Figures 13
Original Data 13
Sample Calculations 16
ii
Introduction and Theory
Hydrogen peroxide undergoes decomposition to form oxygen and
water according to (1).
2H 2O2→2H 2O+O2 (1)
this decomposition, however, is slow with typical concentrations (3-30 wt
%) found in household antiseptics and laboratory stock solutions. One way
of speeding the decomposition is to use a catalyst or enzyme. Both
potassium iodide and the enzyme catalase increase the rate of
decomposition; hence these were suitable for investigating the reaction
order of (1).
A simple way of measuring the decomposition progress is to
monitor the pressure change △ p over time t in a closed vessel containing
the solution of hydrogen peroxide and a catalyst, or enzyme. This
pressure change is then used to determine the moles of oxygen nO 2
produced according to the Ideal Gas Law (2). Pressure changes are
expected to be small – deviations not far from atmospheric pressure – so
the ideal gas assumption should be valid. Finally, using stoichiometry (3)
and the volume of the solution V s one can find the concentration of
hydrogen peroxide CH 2O2.
pV=nRT (2)
1
CH 2O2=12
nO2V s
(3)
The effects of concentration, temperature, and pH on the rate of
decomposition of H 2O2 were further investigated using bovine catalase.
Michaelis-Menten kinetics (4) and Lineweaver-Burk plots (5) can be
implemented to characterize the enzyme and decomposition reaction
V=V max [S ]Km+ [S ]
(4)
1V
=K m
V max
1[S ]
+ 1V max
(5)
where V is the rate of decomposition, Km is the Michaelis-Menten
constant, and [S ] is H 2O2 concentration in the solution.
Procedure
Startup
Determining the reaction order of hydrogen peroxide decomposition
was the primary goal of the investigation. Monitoring the decomposition
using pressure change requires that the volume of the vessel housing the
hydrogen peroxide solution be constant. Accomplishing this required a
125 ml filter flask was connected to a monometer and closed off by a
rubber stopper to contain the oxygen gas produced. A stir bar was added
2
to the flask to mix the reagents and maintain a homogeneous mixture.
Furthermore, a water bath was utilized to keep the temperature of the
flask constant – this is especially useful in the trials using potassium
iodide as the catalyst since the reaction releases heat. Figure 1 shows
how the filter flask is connected to the monometer and covered by the
rubber stopper, as well as how the water bath is employed to keep a
steady temperature.
Figure 1. Apparatus for measuring the pressure changes resulting from hydrogen peroxide decomposition.
Adequate amounts of both catalyst/enzyme and hydrogen peroxide
had to be determined to allow pressure changes within the range of the
monometer used in the experiments. Ultimately, a 1 ml aliquot of 3 wt%
H 2O2 mixed with 2 ml H 2O and approximately 0.1 g KI gave pressure
changes of about 0.15-0.18 psi (a suitable range for the monometer
utilized). For the trials involving catalase, a standard solution was
3
prepared by dissolving 0.1 g bovine liver catalase in 50 ml H 2O. In those
runs 0.2 ml of the catalase solution was added to a 10 ml solution, which
contained H 2O and H 2O2 at varying concentrations. Only in the trials
studying the effects of enzyme concentration did the added volume of
catalase vary.
Adjusting Temperature
Temperature effects were studied using the same apparatus as
shown in Figure 1, with the exception of an added temperature regulator
that circulated water in the bath. A temperature regulator was necessary
because the changes in temperature affect water vapor pressure, and it
was essential that the flask and solution were at the same temperature.
Once in equilibrium, the monometer was relieved of any pressure built up
from the water vapor – this should be done to avoid reading an excess
pressure change not created by the oxygen.
Adjusting pH
Like many other enzymes, catalase functions are affected by pH.
Testing was done by measuring 0.2 ml of the catalase solution and
addeding it to a 10 ml solution, which contained 5 ml of 3 wt% H 2O2 and 5
ml of a standard buffer solution. The pH of the buffer solutions used were
1.0, 4.0, 7.0, and 10.0. Again, the pressure changes caused by H 2O2
decomposition and catalase were measures by the apparatus described in
the Startup section.
4
Adjusting Enzyme Concentration
Lastly, catalase concentration was varied to study its effect on H 2O2
decomposition. The standard solution of catalase outlined in the Startup
section was used again, but this time the added volume was varied.
Aliquots of 50 μl, 100 μl, 200 μl, 350 μl, and 400 μl from the catalase
solution were added to a 10 ml solution, which contained 5 ml of 3 wt%
H 2O2 and 5 ml of H 2O. Pressure readings were taken again from flask-
monometer apparatus.
Results and Discussion
Characterizing the decomposition required that the reaction order
be determined. For this, H 2O2 was allowed to decompose under the
catalytic influence of potassium iodide. A plot of pressure change versus
time revealed that the pressure increased at a constant rate – this hinted
that the decomposition might be first order. To validate this hypothesis
the pressure changes first had to be correlated to H 2O2 concentration
changes over time. Finally, integral analysis (assuming first order) on that
data confirmed the hypothesis. Figure 2 shows that the log of
concentration of H 2O2 is linear with time.
5
0 20 40 60 80 100 120 140 160
-1.26
-1.25
-1.24
-1.23
-1.22
-1.21
-1.2
f(x) = − 0.000214928741872406 x − 1.22287272100055
1% H2O2 with KI catalystIntegral analysis assuming 1st order
Time (s)
ln(C
H2
O2
)
Figure 2. Assuming a first order decomposition, the log of the concentration (M) of hydrogen peroxide in the solution should be linear with time.
The same decomposition was allowed to run under the influence of
a bovine enzyme, catalase. This enzyme is common in numerous
organisms, and serves the purpose of protecting the cell from oxidative
damage. 1 Just like other enzymes, catalase activity is affected by its
initial concentration, temperature, pH, and substrate concentration. To
study these effects, each one had to be varied while the remaining factors
were held constant.
As mentioned in Adjusting Enzyme Concentration, the volume of
catalase solution used was varied so as to span concentrations from 0.01
g/L to 0.08 g/L. This was done to ensure observing a trend in the data, as
well as to prevent pressure changes outside the range of the monometer
used. Figure 3 shows that by increasing the initial concentration of
6
catalase the rate of decomposition rises exponentially. This trend can be
attributed to the remarkable efficiency of catalase – a single molecule of
the enzyme can decompose millions of H 2O2 every second. 2
0 0.01 0.02 0.03 0.04 0.05 0.06 0.07 0.08 0.090
0.002
0.004
0.006
0.008
0.01
0.012
0.014
0.016
f(x) = 0.000924126737539129 exp( 34.8454252398597 x )
Enzyme conc. (g/L)
Init
ial rate o
f decom
posit
ion
(M/m
in)
Figure 3. Effect of catalase initial concentration on hydrogen peroxide decomposition. A
Temperature is a factor that greatly influences the activity level of
catalase. From the experiments conducted, catalase activity improved by
an order of magnitude from 3.323×10−3 M/min at 5.25 ºC to 1.173×10−2
M/min at 41.3 ºC – this is a 253% increase in activity. The opposite is true
for temperatures above the denaturation temperature, somewhere above
41.3 ºC. For instance, at 50 ºC the rate of H 2O2 decomposition drops to
9.615×10−3 M/min. Figure 4 presents this relationship between
temperature and catalase activity. One thing to note about the trend is
that the maximum catalase activity occurs around 40 ºC, which is in the
7
range of cattle body temperature. 3 This is expected because enzymes are
most efficient when they are placed in environments resembling their
natural conditions.
0 10 20 30 40 50 60 700
0.002
0.004
0.006
0.008
0.01
0.012
0.014
Temperature (ºC)
Init
ial ra
te o
f decom
posit
ion
(M/m
in)
Figure 4. The rate of hydrogen peroxide decomposition increases with temperature.
The pH effect was expected to have similar trends as those of
temperature. As with high and low temperatures, enzymes tend to be less
efficient at high and low pH. Again, this is due to denaturization of
catalase at extremely low pH. Based on what was learned from
temperature effects, a prediction was made that catalase should be the
most efficient at a pH around 7. This hypothesis was made because the
pH of bovine blood is around 7. 3 Figure 5, which shows a maximum
decomposition rate at around pH of 7, confirmed the hypothesis. At pH of
8
1, catalase denatures and so it fails to catalyze the decomposition of H 2O2
.
0 2 4 6 8 10 120
0.001
0.002
0.003
0.004
0.005
0.006
pH
Rate
of
decom
posit
ion
(M/m
in)
Figure 5. Effects of pH on the rate of decomposition of hydrogen peroxide. The rate is at its maximum around pH of 7.
Lastly, initial substrate concentration effects were analyzed using
Michaelis-Menten kinetics. In order to successfully fit the data to that
model, substrate concentrations had to be varied without making them
too concentrated, i.e. carefully choosing concentrations that fell within the
Michaelis-Menten kinetics regime. For that reason, a range from 0.0265 M
to 0.3528 M H 2O2 was chosen. Figure 6 shows initial rates of
decomposition resulting from the variation of substrate concentration, as
well as the fitted Michaelis-Menten model. The data was also used to
obtain values for Km and V max from a Lineweaver-Burk plot (Figure 7). The
Km for the decomposition is 0.1208 M, while the V max is 0.0097 M/min.
9
0 0.05 0.1 0.15 0.2 0.25 0.3 0.35 0.4 0.450
0.0010.0020.0030.0040.0050.0060.0070.0080.009
Substrate Conc. (M)
Rate
of
deco
mpo-
sit
ion (
M/m
in)
Figure 6. Effects of initial substrate concentration on the rate of decomposition. The line represents the fitted Michaelis-Menten model.
Conclusions
At low concentration, the rate of decomposition of hydrogen
peroxide is slow. Using potassium iodide as a catalyst, H 2O2 decompostion
was determined to be first order with respect to its concentration.
Furthermore, the results of varying temperautre, pH, and initial enzyme
and substrate concentrations showed that H 2O2 decomposition rates
reach a maximum and deteriorate at extremes, with the exception of
initial enzyme concentration. Catalase function was shown to be sensitive
to temperatures and pH changes. It was also confirmed that catalase
activity was at its maximum when it was placed in conditions that
mimicked its natural environment, i.e. bovine body temperature (~40 ºC)
and blood pH of 7. 2
10
Further studies could improve on the methods of regulating the
temperature of the solution decomposing. This would also allow more
data to be collected, to the extent of being able to pin-point the
denaturation temperature. A similar approach can be taken for pH, where
more data collection could reveal exactly at what pH catalase activity
ceases.
References
1. Chelikani P, Fita I, Loewen PC. (2004). Diversity of structures and
properties among catalases. Cell. Mol. Life Sci. 61 (2): 192–208.
2. Goodsell, David. (2004). Catalase. Molecule of the Month. RCSB Protein
Data Bank. Retrieved 7/15/13.
3. MacDonald, David. (1984). Mammals. Oxford: Equinox, 1984: 545.
11
Nomenclature
△ p pressure change (cm H2O, kPa)
t time (s)
nO 2 moles of oxygen produced
V s volume of the solution (L)
CH 2O2 concentration of hydrogen peroxide (M)
V rate of decomposition (M/min)
V max maximum rate of decomposition (M/min)
Km Michaelis-Menten constant (M)
[S ] H 2O2 concentration in the solution (M)
R gas constant (L-kPa/K-mol)
T temperature (ºC)
12
Appendices
Supplementary Graphs and Figures
0 5 10 15 20 25 30 35 400
100
200
300
400
500
600
700
f(x) = 12.478296405284 x + 103.328281873752
1/S (M-1)
1/V
(m
in/M
)
Figure 7. Lineweaver-Burk plot used to find Vmax and Km.
Original Data
1% H2O2 with KI catalystRun 1 Run 2
Time (s) cm H2O Time (s) cm H2O0 0 0 0
10 0.3 10 0.320 0.7 15 0.630 1.3 20 135 1.6 25 1.340 1.9 30 1.645 2.3 35 2.0550 2.6 40 2.455 3 45 2.760 3.4 50 3.365 3.7 55 3.770 4.1 60 475 4.5 65 4.35
13
80 4.85 70 4.785 5.3 75 5.190 5.6 80 5.4595 5.95 85 5.7
100 6.3 90 6.2105 6.7 95 6.5110 7 100 6.9115 7.4 105 7.3120 7.8 110 7.6125 8.2 115 8.1130 8.5 120 8.4135 8.9 125 8.7140 9.2 130 9.1145 9.7 135 9.5150 10.1 140 9.7
145 10.3150 10.6
Adjusting pHH2O2 (ml) 5 H2O2 (ml) 5 H2O2 (ml) 5 H2O2 (ml) 5H2O2 (ml) 5 H2O2 (ml) 5 H2O2 (ml) 5 H2O2 (ml) 5Cat. (μl) 50 Cat. (μl) 50 Cat. (μl) 50 Cat. (μl) 50Temp (ºC) 21
Temp (ºC) 21
Temp (ºC) 21
Temp (ºC) 21
pH 1 pH 4 pH 7 pH 10
Time (s)cm H2O Time (s)
cm H2O Time (s)
cm H2O Time (s)
cm H2O
0 0 0 0 0 0 0 010 0 10 1 10 2.9 5 0.620 0 20 2.5 20 7.4 10 1.5
30 4 30 10.8 15 2.640 5.7 40 14.1 20 4.350 6.9 50 17.4 30 6.960 8.1 40 9.2
50 11.760 13.1
14