Here are the results for this experiment using this method and various catalysts: The experiment will then be repeated but by using different concentrations of Hydrogen peroxide: O BTAINING Safety Throughout this experiment, we are using highly reactive substances; therefore it is useful for us to have some sort of safety knowledge about them so we know how to handle such chemicals.
At this point no more products are produced as no more Hydrogen peroxide is reacting, as no more Hydrogen peroxide is colliding with catalyst particles, because it has all decomposed. Method for the main experiment Apparatus list- Weighing scales- This is used to measure out the mass of catalyst required and the weight over time of the equipment and solution to determine weight loss.
This is designed to measure the mass of Oxygen gas produced and lost from the system. This is because when the concentration is increased there are more particles which means there is more of a chance of them colliding which therefore means the faster a chemical reaction takes place.
If the Hydrogen peroxide is at a higher concentration, the molecules are also more tightly packed together and are therefore denser, and if the volume is the same, there are more Hydrogen peroxide molecules present.
I will not go below 5 concentration simply because the reaction below this concentration will be too slow and insignificant to be worth measuring, and any small inaccuracies would amount to huge percentage errors.
Instead of changing the concentration, we could have done a weight loss.
Variables- There are various variables in this experiment affecting the catalytic decomposition of Hydrogen peroxide; these are: I will keep all my bags under my desk along with my stool; this is so no one is able to trip over them. This means that the experiment has to be easily reproducible; i.
This is a diagram of the equipment: I will be changing the mass of catalyst used to see what effect it has on the decomposition of Hydrogen peroxide. I predict that the higher the concentration of hydrogen peroxide, the faster hydrogen eroxide and manganese oxide decomposes.
During this time the hydrogen peroxide could have decomposed. This is because increasing the temperature of the medium gives the particles in that medium a higher average energy. Therefore there will be more collisions with an entity such as a catalyst. I will do two check readings, three readings in all, for each concentration.
More essays like this: I believe this rate of reaction will be proportional to the concentration as by increasing the concentration a certain amount you increase the number of molecules present by a proportional amount.
Aim Investigating the decomposition of hydrogen peroxide by using potato catalyse, which is a biological catalyst. Also, you can see that our prediction was correct by looking at the first graph, the steeper the gradient of the line; the faster it took to decompose.
If we could do this experiment again, I would have tried to be more accurate when weighing out the catalyst, timing the experiment and reading out the readings. The experiment is easy to carry out in the same fashion each time with the given equipment.
This is the total weight on the scale. This is because the increased chance of collisions with the catalyst, due to the increased number and density of the Hydrogen peroxide, means at the start of the reaction there are more collisions with the catalyst leading to a higher initial rate of reaction.
Factors Affecting Decomposition of Hydrogen Peroxide C) and pH () on the rate and extent of the decomposition of H2O2 were examined over a. Pd catalysts on ACC, oxidized with nitric acid, are considerably less active in catalytic decomposition (H 2 O 2 → H 2 O + (1/2)O 2) and hydrogenation (H 2 O 2 + H 2 → 2H 2 O) of hydrogen peroxide than the corresponding ones on non-oxidized ACC.
to detect which factors affect the rate of the decomposition of hydrogen peroxide with a fixed mass of catalyst. A catalyst is a substance, which alters the speed, or rate of a chemical reaction but is chemically unchanged at the end of the reaction.
In this study, the decomposition of free cyanide by hydrogen peroxide was studied. The results have shown that the rate and extent of cyanide removal ([CN]0: mg/l) improve with increasing the.
The Hydrogen Peroxide Breakdown Laying the Foundation in Biology 7 Enzymes work by lowering the energy of activation.
For example, hydrogen peroxide decomposes to form water, H2O, and oxygen gas, O2. While this is a catabolic reaction, the rate at which it occurs is slow. Our aim is to detect which factors affect the rate of the decomposition of hydrogen peroxide with a fixed mass of catalyst.
A catalyst is a substance, which alters the speed, or rate of a chemical reaction but is chemically unchanged at the end of the reaction.Factors affect rate decomposition hydrogen peroxide fixed