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Combustion of Alcohol.

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Introduction

Combustion of Alcohol Introduction: This experiment is based on the combustion of alcohols. In alcohol there are different amounts of carbon. We will be burning the alcohols to see weather the amount of carbon affects the energy given out. Combustion is basically a reaction of a fuel with oxygen creating heat. I know that the reactions in this experiment will be exothermic because they will give out heat. Therefore energy is produced by the reaction. Aim: To find out weather the amount of carbon in alcohols affect the amount of energy given out when the alcohol is burnt. We will see how much it heats up water and then we will figure out the amount of energy produced then how much energy produced per mole. The alcohols that I will be using will be: propan-1-ol, butan-1-ol, ethan-1-ol, methan-1-ol and pentan-1-ol. Prediction: I predict that the more carbon in an alcohol then the more energy released. I believe this because the alcohol with more carbon means that more bonds have to be broken, this would require more energy to break the many bonds whereas, if there were less carbons then not as much energy is needed because there are less bonds to break. ...read more.

Middle

Setting up: Apparatus: * Alcohols * Clamp * Clamp stand * Stopwatch * Top-pan Balance * Water * Copper can * Measuring cylinder * Thermometer Diagram: Method: First of all get all the apparatus and set them up as shown in the diagram above. Take the alcohol and weigh it, take down the mass and then fill your measuring cylinder with water until the level that you want it (200ml) and put it into the copper can, then take the temperature of the water and record that. When both those are done check that the clamp is set at the right distance from the surface. When all these are done we an start the experiment. 1. Take the cap off the alcohol and light it under the copper tin. 2. Start the stop watch. 3. Wait till the set time has finished. 4. Recap the alcohol 5. Take temperature of water. 6. Weigh the alcohol 7. Figure out temperature rise and alcohol burnt 8. Use the equations to figure out the energy per mol. 9. Repeat with other alcohols You should test each alcohol twice so that you can figure out an accurate average. Plot your results on a graph and see if you get a positive or negative correlation. ...read more.

Conclusion

I predicted this because I knew the reaction would be bond making, therefore, it is exothermic which means energy is given out. Evaluation The procedure was complete. We obtained all the results that we wanted and they were fairly accurate which indicated that there were no problems in the procedure. There were no anomalous results. They were fairly accurate and you an clearly see the positive correlation in the graph. The quality of the evidence is fairly accurate. K There is not definite straight line in the positive correlation but it is fairly close with no results being too far away from the line of best fit. We could have done the experiment more times to get more accurate results, therefore, reducing the amount of time we burnt the alcohols would give us more time to re-test the alcohols. Also if I was to do the experiment again, I would use a great number of alcohols making it easier to make a line of best fit. The evidence is fairly reliable because we kept it a fair test by keeping certain factors consistent, therefore, we know that the results are reliable enough to be correct. It can support my conclusion. Other experiments we could do could be to see whether the amount of carbon in an alcohol would affect the rate of speed at which it burns. ...read more.

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