Investigation into transition metals as catalysts Essay

Hydrogen peroxide decomposes slow to form piddle and atomic number 8 gas pedal. Transition metal oxides pass on catalyze this reaction. A catalyst speeds up a reaction without organism use up. The outgo catalyst for a reaction increases the dictate of reaction the most. The rate of reaction can be measured by the amount of ware formed divided by the time of the reaction. If 40 ml of oxygen were produced in 30 siemensonds (0. 5min), then the rate of reaction would be 80 ml/min. Planning- the apparatus available will be20 script total heat peroxide solution (irritant), copper dioxide (harmful), cast-iron oxide, atomic number 25 dioxide (harmful), spatulas, ele4ctronic balance, amount cylinder, trough (water bath), stop watch, thistle funnel, delivery subway system, bungs to take funnel and tube, boiling tubes. preventive Precautions Wear goggles. Make sure that the hydrogen peroxide does not chance on contact with skin and/or hair. Wipe bench thoroughly after experim ent. Variables Each catalyst should be tested twice, however the catalyst should be altered after for each one experiment. Constants.Volume/concentration of hydrogen peroxide (10cm3 of 20 vol. hydrogen peroxide + 10cm3 of water). Amount of each catalyst (1g). succession left for/intervals at which gas is measured (every 5 seconds for 50 seconds). equivalent general apparatus. NB. Wash apparatus after each experiment. Measurements The volume of gas (oxygen) produced will be measured during each test at 5-second intervals- this will be done by measuring how much water is displaced in the measuring cylinder by the gas. Each catalyst will be tested twice, and the test will last for 50 seconds on each occasion. Results Manganese. succession (secs) Experiment 1 (vol. of type O cm3) Experiment 2 (vol. of type O cm3) reasonable (vol. Of Oxygen cm3) Copper Time (secs) Experiment 1 (vol. of Oxygen cm3) Experiment 2 (vol. of Oxygen cm3) Average (vol. Of Oxygen cm3) Iron Time (secs) Experim ent 1 (vol. of Oxygen cm3).Experiment 2 (vol. Of Oxygen cm3) Average (vol.Average rate of reaction Average rate= volume/time=.. cm3/sec Manganese dioxide= 96/40= 2. 4 cm3/sec. Copper oxide= 27/50= 0. 54 cm3/sec. Iron dioxide= 27/50= 0. 54 cm3/sec. 20 vol. of hydrogen peroxide means that each cm3 gives off 20 cm3 of oxygen gas. We thin it to 10 vol. Using water and so we would piddle expected hundred cm3 of oxygen. Hence manganese dioxide as well as being the best catalyst in like manner cause much hydrogen peroxide to break down. paygrade Although the results obtained were fairly good, there were quite a few problems during the experiment, which affected them. These were It was ticklish to fill the measuring cylinder with water, as well as break in it into the trough (water bath) without any escaping and creating difficulties in measuring the gas produced. The largest measuring cylinder was only coulomb cm3. This was very relevant as one of the tests for manganese dioxide ex ceeded snow cm3 in gas produced, therefore a larger cylinder was needed.The catalysts were very fine powders, which made it difficult to measure out barely 1g. When gas was being produced and coming off fast, it was difficult to read the measurements accurately as the shape up of the water wasnt steady. (It was also difficult when a gas bubble came up while the gas volume was being measured). In act to improve the experiment and thus make the results more accurate, the following could have been done A wider measuring cylinder used so that gas being produced rapidly would not disturb the water surface as much, making the volume of gas easier to measure.A larger measuring cylinder used so that gas volumes exceeding 100 cm3 could be measured and therefore the results not interrupted with. Repeat scrutiny (i. e. 3 tests for each catalyst) carried out so that there is less way of life for error whilst obtaining results. This would also make them more reliable. When the results were obtained, there were some noted abnormalities i. e. anomalous results. These were the measurement of gas after 5 seconds when testing iron dioxide, and the tests when using manganese dioxide.This was because when manganese dioxide was being tested, there were large disagreements in measurements at each time interval, therefore experimental errors must have occurred (after 40 seconds on the first test, the gas volume also exceeded 100 cm3, whilst in the second test this did not happen until after the 50 second limit). The other anomalous result was when testing iron dioxide, as after the first 5 seconds, there was a large difference in the volume of gas between the 2 tests carried out (30 cm3 20 cm3).The cause of these anomalous results is most likely related to the surface discipline of the catalyst in correlation with each test carried out i. e. the pulverised catalyst may have been slanted up the boiling tube during one test, but not on the other, resulting in different surf ace areas. Shaking the boiling tube before each test and/or using a wider testing tube, could have however prevented this. From the results obtained, you can also not definitely state the best catalyst for his reaction, as whole 31 transition metals were not tested.Therefore to extend this investigation to witness the best catalyst for producing oxygen gas from hydrogen peroxide solution, whole the transition metals could have been tested as well as assume tested for verification. This, in conclusion, would have found the best catalyst for this peculiar(prenominal) reaction. Daniel Powell. 10k. Show preview only The above preview is unformatted text This disciple written piece of work is one of many that can be found in our GCSE Patterns of Behaviour section.