Burning Fuels Investigation.

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Chemistry coursework: Burning Fuels Investigation

Aim: To find out how much energy is released by each alcohol per gram (g).

Research: Alcohols are organic, and each one has its own formula. In this experiment we have used Ethanol, Propanol, Butanol, Pentanol Hexanol, Heptenol, and Octanol. Alcohols react with oxygen in the air to form water and carbon dioxide. The reaction that is involved in burning alcohols is exothermic because heat is given out. Form this reason the reactant energy is higher than that of the product.

Ethanol, (C2H5OH)

Propanol, (C3H7OH)

Butanol, (C4H9OH)

Pentanol, (C5H11OH)

Hexanol, (C6H13OH)

Heptanol, (C7H15OH)

Octanol, (C8H17OH)

 When these alcohols are burnt they show a trend that the fewer the bonds the less energy is released, so the more bonds the more energy is released.

  Alcohols are good to use in this experiment because they burn easily and all have simular chemical formulas.

The equation to work out the energy released per gram is:

Mass of water X 4.2 X change in temperature of water

Change in mass of fuel (in grams)

4.2 is the specific heat capacity of water.

This are the predicted results for burning fuels, calculated using bond energies from a book of data.

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· Mass of the water 100ml

· Type of beaker

· Surrounding temperature of around 23ºC

· The height of the beaker from the wick

· Same set of scales

Pendiction: I predict that Octanol will release more energy because it has more bonds that the other alcohols, and than Ethanol will release the least due to its few bond properties. All of these bonds are called hydrocarbon bonds. As the list of alcohols go down it will have a steady increase in energy released. These bonds only ever realease there energy ...

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