Conclusions drawn from preliminary experiments
We discovered that…
- Timing the experiment for 60 seconds was far too long in the sense that some reactions finished faster than expected, especially the higher concentrations, i.e. 80 and 100M where reactions occur at faster rates.
- In some experiments, particularly of those of 80 and 100M concentrations, the reactions finished far too soon, and released oxygen at a very fast rate into the measuring cylinder, thus making the recording of how much oxygen was collected very difficult as all the water had been displaced. To solve this problem, a larger measuring cylinder would be required.
- 15ml of hydrogen peroxide is far too much considering you are only using 1g of processed liver; this is one of the many reasons why the reaction finished too soon as there are a greater amount of substrate molecules and fewer enzyme molecules; this ensures that each individual enzymes’ active site is always working, reacting with the substrate molecules.
Planning This is an experiment to examine how the concentration of the substrate Hydrogen Peroxide (H2O2) affects the rate of reaction of the enzyme Catalase.
Hypothesis: an increase in the substrate concentration will result in an increase in reaction rate. After a certain point, the rate of reaction will decrease due to an excess of substrate and therefore a queue for reaction will occur. Catalase is able to speed up the decomposition of Hydrogen peroxide because the shape of its active site matches the shape of the Hydrogen peroxide molecule. This type of reaction where a molecule is broken down into smaller pieces is called an Anabolic Reaction.
In order for a reaction to occur:
Reacting Molecules must collide with one another
The reacting molecules must collide with sufficient energy
The reacting molecules must collide in an orientation that can lead to rearrangement of the atoms
The rate steadily increases when more substrate is added because more of the active sites of the enzyme are being used which results in more reactions so the amount of Oxygen released in a given time is higher. Once the amount of substrate molecules added exceeds the number of active sites available then the rate of reaction will no longer go up. This is due to the maximum number of reactions being done at once, so any extra substrate molecules have to wait until some of the active sites become available.
Variables: Factors that affect reaction rates.
There are five main factors affecting rates of reaction. They are:
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Enzyme concentration: if there are more substrate molecules then there are enzyme molecules, the available number of active sites becomes a limiting factor. The concentration factor reaches its optimum rate of reaction when all active sites are being used.
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Temperature: when heat energy is added to the enzyme and substrate, random movement is increased. This means that when a lot of energy is transferred, there is an increase in molecule collision. When there are more collisions, there is more chance of the substrates finding their allocated active sites. This only works up to a certain temperature, at which point the enzymes are denatured, this temperature is normally after 30 and 40*C which is where most enzymes are at their optimum.
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Substrate concentration: when an excess amount of substrate is added to a constant amount of enzyme, the enzyme is soon working as hard as it can and each molecules active site is being used, this is known as Vmax. From this point, it is almost as if the substrate molecules are literally queuing up and waiting to fit into their allocated active site.
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Levels of pH: The pH of the reaction does affect the secondary and tertiary structures of the enzymes. If this happens and the active site changes shape, it’s action will be affected. The majority of enzymes have optimum pH levels around neutral or are mildly alkali. Changes in pH, especially if acidic conditions occur, mean that the enzyme will not bind with the substrate, but neutralisation of the acid will generally make the active site normal again.
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Surface area of substance containing enzyme: An increase in surface area means that there is a larger area and therefore larger number of exposed enzyme molecules to act. This increase in collisions causes an increase in rate of reaction and is therefore a factor that can limit rate of reaction and can also optimise reaction rates.
In this particular experiment, the variable that has been selected to vary is “substrate concentration” i.e. the concentration of hydrogen peroxide: every other factor would be controlled to ensure fairness of conductivity.
Safety Precautions –
- Hydrogen peroxide is an irritant and harmful. Safety precautions like safety goggles and lab coats must be worn so to prevent burning.
- If hydrogen peroxide is spilt in the lab make sure the proper safety coat, gloves and protective specks are adorned. Cover with a mineral absorbent; there may be different regulations in different places/areas about disposal, these must be followed.
- All beakers and test tubes containing H2O2 have to be labelled.
- Hydrogen peroxide is dangerous with many other chemicals. Avoid mixing it with any substances where the out come is unknown or may be a potential health risk.
Specifications
To improve reliability, three tests would need to be conducted for each of the concentrations used, in order to produce sufficient averages of results. A suitable range i.e. 5, for the concentrations of the substrate, hydrogen peroxide: 20, 40, 60, 80 and 100M would be required to do so. The amount of the substrate (hydrogen peroxide) is also important; if you have more of the substrate, then reactions could occur a lot quicker due to the enzymes’ active site constantly reacting with the large numbers of the substrate; the same applies if you have less of the substrate molecules than enzyme molecules, resulting in the reaction finishing a lot quicker than the time expected. A reasonable volume of the substrate would be 10ml as it is roughly proportional to the amount of the enzyme catalase contained within the liver. Again, keeping the tests fair, 10ml of the hydrogen peroxide would be used each time.
1g of homogenised/processed liver would be used for each experiment, keeping the test fair; the processed liver contains the enzyme catalase, which helps to catalyse the substrate, in this case, the hydrogen peroxide would be catalysed. The reaction would also need to be timed; a reasonable time would be approximately 30 seconds; this allows sufficient time for the reaction to take place. Also, by timing each experiment for 30 seconds, you are ensuring fairness of conductivity.
Method of conductivity:
- Set up the apparatus as shown in the diagram; ensure that you fill the 250ml measuring cylinder before hand and place it in the container which should also be filled with water. Make sure that the tube on the Buchner flask is inserted directly in the container to the measuring cylinder. To help keep the cylinder in place, use a clamp stand to secure its position.
- Using a spatula, extract exactly 1g of homogenised liver. To ensure that you extract 1g of the liver, weigh the spatula using the weighing scales. Then weigh the spatula together with the liver, if the weight has risen by a difference of 1g compared to the weight of the spatula alone, this ensures that you have extracted 1g of the liver.
- Carefully place the liver extract inside the buchner flask.
- Put the bung in place to ensure the flask is sealed. To seal the hole even further, you could use blue-tak for example, preventing oxygen from escaping during the reaction; this may have a negative effect on the results if the flask was not properly sealed. Because the reaction involves the enzyme catalase breaking down hydrogen peroxide into two products, water and oxygen, the oxygen will be collected at the measuring cylinder. However, if the flask was not properly sealed, some or even most of the oxygen produced from the reaction will escape and very little will be collected at the measuring cylinder.
- Using a syringe, extract 10ml of hydrogen peroxide of 20% concentrate.
- Through the hole in the bung of the sealed flask, inject the hydrogen peroxide onto the liver extract.
- As soon as the hydrogen peroxide is injected, time the reaction for 30 seconds with the aid of a stopwatch.
- As soon as the 30 seconds are over, read the measurement from the measuring cylinder from which the oxygen has displaced some of the water. The reading that you obtain refers to the amount of oxygen that has been produced and released from the reaction between catalase and hydrogen peroxide.
- Record results in a suitable table.
- Clean all equipment out and set the apparatus the same way in which you previously did.
- Repeat the same experiment, following the same method, for each of the concentrations 3 times. So, concentrates of 20, 40, 60, 80 and 100% of hydrogen peroxide would need to be tested 3 times each; you will end up having conducted a total of 15 experiments.
Equipment required:
- Syringe
- Spatula
- 20, 40, 60, 80 and 100% concentrate of hydrogen peroxide
- Homogenised liver
- Buchner flask
- 250ml measuring cylinder
- Clamp stand
- Container
- Stopwatch
Justification of equipment used:
The Buchner flask was used instead of the standard test tube because it provides a larger surface area for the reaction to take place, leaving more of the catalase for exposure. So, a healthy amount of oxygen will be collected.
A syringe is used instead of the standard pipette because an even more accurate amount of substrate can be drawn, thus improving accuracy and increasing the reliability of results obtained.
Analysis
Calculating the rate of reaction:
By interpreting the following formula…
Rate = 1 ÷ Time… the initial rate of reaction can be calculated.
To simplify the formula so that it is relevant to this particular experiment, the “1” is replaced by the average volume of gas collected. You then divide this value by 30 seconds…
Rate = average volume of gas collected (cm3) ÷ 30secs
For example; to calculate the rate for 20% concentration, you divide 19cm3 (which is the average amount of oxygen collected), by the time taken, 30 seconds.
Rate = 19 ÷ 30
= 0.6 cm3/s
The effect of substrate concentration:
As substrate concentration increases, the initial rate of reaction also increases. This is only what you would expect: the more substrate molecules there are around, the more often an enzyme’s active site can bind with one. However, if you continue increasing substrate concentration, keeping the enzyme concentration constant, there comes a stage where every enzyme’s active site is working continuously. If more substrate is added, the enzyme simply cannot work faster; substrate molecules are literally “queuing up” for an active site to become vacant. The enzyme is working at its maximum possible rate, known as “V-max”, as indicated on the graph above.
Interpretation of the graph:
Referring to the graph showing the initial rate of reaction, theoretically speaking, the rate of reaction should be directly proportional to the substrate concentration. This suggests that if the substrate concentration were increased, the rate would also increase. Respectively, if you double one thing, the other would also double. It is due to the fact that as there are more hydrogen peroxide molecules around, the more often the enzyme’s active site (catalase) can bind with one, thus releasing products of water and oxygen gas. (Note: the process of a substrate combining with an enzyme’s active site can be explained in the “background”; “lock and key” theory of enzymes).
Again referring to the graph of initial rates, it shows a steady increase in the rate, almost proportional to that of the increase of substrate concentration (hydrogen peroxide). The rate of reaction starts off very low at the first stages, i.e. it is very low at 20% concentration of hydrogen peroxide. This is because there are fewer particles within a certain area of the solution and so less of the particles, when given the necessary amount of kinetic energy, move close together. So, fewer collisions occur between particles, in this case, the enzyme catalase and the substrate hydrogen peroxide; therefore fewer reactions occur at this particular point.
By increasing the substrate concentration, the amount of particles within a certain area in solution also increases; therefore, more of the particles would collide with one another due to the fact that they are closer to one another, thus more reactions between catalase and hydrogen peroxide occurs, resulting in an increase of the rate. In conclusion, it is safe to state that by increasing the substrate concentration would result in an increase in the rate of reaction; the rate at which the enzyme breaks down hydrogen peroxide to water and oxygen gas.
Explanation of why the line on the graph does not fit the theoretical line
- The 100% concentration of hydrogen peroxide use was actually 20%, and so the point where all the active sites of catalase are supposed to be occupied by hydrogen peroxide molecules, did not occur. Thus this explains why there is no “plateau” on the shape of the graph because the “v-max” does not occur.
- The reason why 20% concentration of hydrogen peroxide was used as 100% in this experiment was because actual 100% concentrate is very corrosive and dangerous. So, to avoid any accidents thus improving safety of conductivity, 20% concentration was used and referred to as 100%.
Evaluation
Due to adequate results obtained from the various experiments, we were able to prove the initial hypothesis: as the concentration doubles, so does the rate of reaction. A point is reached however, where all sites are being used and by raising the substrate concentration the rate won’t increase, as the limiting factor is the amount of enzymes.
The experimental procedures were very acceptable in the sense that accurate results were obtained, reflecting the theoretical ideas of the initial hypothesis. The procedures were simple to follow, enforcing safety of conductivity and in some cases, allowing you to achieve accurate data.
Although results obtained were substantial enough to draw a conclusion, there were some that were anomalous. For example: the rate of reaction for 40% concentration of hydrogen peroxide was anomalous; the point on the graph which indicates this, does not fit to the line of best fit.
To enable this experiment to be completed as accurately as possible, we repeated it three times and then used an average of all the results to best plot a graph with a line of best fit. To keep the experiment fair, all variables were controlled apart from one, the one that was tested; the concentration of hydrogen peroxide. However and unfortunately in practice, it is impossible with the basic apparatus we had to keep all the measurements precisely the same. For example…
- There is a slight delay between inserting the hydrogen peroxide into the flask with the liver extract. This will slightly affect all the results for each individual experiment but as we carried out all the steps in the same way, it should not make any negotiable difference to the overall result.
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It is also impossible to precisely measure out the amounts of hydrogen peroxide and the liver extract each time. As the scale on the measuring cylinder shows the measurement to the nearest mm3, the solutions that we used should be correct to the nearest mm3.
- The theoretical maximum rate of reaction is when all the sites are being used but in reality, this theoretical maximum is never reached due to the fact that not all active sites are being used at the same time. The substrate molecules need time to attach to the enzyme and to leave it so the maximum rate achieved is always slightly below the theoretical maximum. The time taken to fit into and leave the active site is the limiting factor in the rate of reaction.
- Another reason of how anomalous results were obtained may be due to the presence of enzyme inhibitors. The active site of an enzyme fits one particular substrate perfectly. It is also possible for some other molecule to bind to an enzyme’s active site if it is very similar to the enzyme’s substrate; this could inhibit the enzyme’s function, slowing down the rate of reaction.
- There could have been non-competitive inhibitors, which attach themselves to a part other than the active site and altering the shape of the enzyme and slowing down the rate of reaction.
- It may have been due to the lack of monovalent cations, e.g. chlorine, as it needs this activator to fill a gap in the active site, so that the substrate fits perfectly.
Improvements and further investigating
To improve the investigation, you could try more accurate ways of conducting the experiment so the oxygen released is not lost and the reading is therefore more accurate. Ways of improving the investigation are as follows…
- You could use a gas syringe for extra accuracy.
- You could place the flask with the reactants in it (sealed with a bung) on a balance, and measure the weight loss. This would be very accurate as you could measure the loss on a balance very accurately and you need not worry about losing oxygen.
- An oxygen probe could be used to detect oxygen levels and very precisely send the data to a computer. This would eliminate the chance of reading off the amount of oxygen on the measuring cylinder incorrectly.
- Another possibility would be to use a burette, which is far more accurate than a measuring cylinder and hence it would give more precise readings and therefore the experiment would be more accurate.
- You could investigate on the other variables, temperature and pH.
- One final thing that you could do is to conduct the experiment all over again and to make an average of the two averages. This will insure great accuracy, but results obtained from the initial investigation have sufficient evidence to support a firm conclusion regardless of the fact that an anomalous result was obtained.
- To extend this experiment even further, you could try the enzymes extracted from plants such as celery, as that contains catalase to break down hydrogen peroxide.
Bibliography
- Michael Roberts, “Nelson Science Biology”, Nelson, 1995 (p22-27)
- Mary Jones, Richard Fosbery, Dennis Taylor, “Biology 1”, Cambridge University Press, 2000 (p42-50)
- website: www.h2o2.com
- website: www.webref.org/chemistry/collisiontheory