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Burning a variety of fuels to see which one gives off the most energy.

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Introduction

Plan Introduction In this investigation we are going to burn a variety of fuels to see which one gives off the most energy Preliminary work For the first experiment we burnt the fuels but most of the heat was lost so for the real experiment we will put heat mats around the flame to reduce heat loss. Prediction I predict that the more carbon atoms in the molecule, the more energy will be transferred and I think this because the more carbon atoms in the molecule will make more energy, as there are more carbon atoms to burn. I can show this by the term 'Break in Make out' and this means that the higher the carbon atoms in the molecule are, we will need more energy to break up the molecule. So if we need more energy to break it up then we will have more energy left over at the end. This is extra energy and usually this is heat. Extra energy (Heat) Break in Make out I also predict that my results will be very near to the textbook answers results, but I think that the percentage of heat that will be captured will be quite low. ...read more.

Middle

Safety There are a few safety rules that we must abide by * Wear safety goggles all the time during the experiment. * Tie back long hair and remove dangling jewellery or ties. * Mop up any Alcohol spills immediately. * Refrain from handling hot objects and allow them to cool before touching them. Precise and reliable data The textbook answers are the answers that we are supposed to have but the graph next to it are the answers that I actually got. We can see differences between the two graphs; the textbook answers graph is in a perfectly straight line where as my graph is not, it is reasonably straight but not quite. Analysis Statement In my results as the molecules got bigger the more energy was transferred but not as much energy as the textbook answers. Trends As the molecule in the atom gets bigger the more energy is transferred. Percentage Table Name of Alcohol Formula % Energy Capture kJ/mole Methanol CH3OH 4.62549 Ethanol C2H5OH 2.559085 Propanol C3H7OH 4.063819 Butanol C4H9OH 4.068119 Pentanol C5H11OH 3.764237 The end column is the percentage of how much energy was captured by the boiling tube to change the temperature. ...read more.

Conclusion

Also the percentage of the heat captured is correct because the percentages are really low. The highest percentage was 4.62549%. My results are quite good but could be better as the percentage of heat captured was low. I got less than 5% of the textbook answers for kilojoules per mole of fuel for each fuel, I don't think this was good enough Kilojoules per mole of fuel kJ/Mole "Textbook answers" kJ/mole %energy capture kJ/mole 33.07225 715 4.62549 35.05946 1370 2.559085 81.68276 2010 4.063819 107.8052 2650 4.068121 124.9727 3320 3.764238 This is a table produced from my results. Comparing the repeated results On the main graph named Kilojoules in fuel there is two sets of results, one set of results is the original results and the other set are the repeated results. The repeated results are quite close to the original ones. The results vary, as the repeated Methanol and Propanol results are just a bit less than the original results whereas the repeated Ethanol result is just a bit higher. I would probably have to do the Methanol, Ethanol and Propanol results again to certify the exact marks. Further work A 'Bomb calorimeter' is used for measuring heats of combustion. It consists of a strong container where the sample is sealed with excess oxygen and is electrically ignited. ...read more.

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