• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

To investigate the heat outputs of fuels

Extracts from this document...


To investigate the heat outputs of fuels Obtaining Method) Some preliminary work was carried out to confirm reliability of the test, where we burned ethanol-covered rocksil wool under a conical flask of increasing volumes of water. This test was carried out in much the same way. Equipment was set up as in diagram. The temperature of the water was recorded. We squeezed some droplets of Ethanol with a pipette onto the rocksil wool, and placed the wool into a crucible. The crucible was weighed before and after the ethanol had been added (this measurement included the rocksil wool), and placed under the conical flask (which contained 250cm3 of water). The wool was lit and the highest (or lowest) temperature reached was recorded. The experiment was then repeated using Methanol and Propanol on the rocksil wool. Each alcohol was done twice. Safety goggles were worn throughout. Apparatus We were using: Three pipette-fulls of Methanol, Ethanol and Propanol Retort stand Clamp, Boss Thermometer Conical Flask Tap Water Crucible Three pieces of rocksil wool Lit Splint Fuel Mass of water (g) ...read more.


This vast difference between the two was probably caused by the loss of heat to the air in the four-centimetre gap between the crucible and the conical flask. Although there would have been heat loss to the air in the second test as well, there may have been objects present around the equipment after we did test one, or during test one there may have been an increase of activity around the equipment that didn't occur during the other tests (for example, people walking past, objects on the work surface being moved, etc.). If I was to do the test again, this is one thing I would try to avoid. I would also decrease the gap between the crucible and the conical flask if I were to do the test again, to reduce loss of heat to the air. Loss of heat could also be minimised by performing the test in a more enclosed area such as a fume cupboard. ...read more.


Rise in temp (oC) Heat given out in reaction (kJ) Heat given out per mole (kJ) There were very close similarities in the final mass of the fuels, perhaps due to their (H properties, and to the initial mass properties. There were also similarities in the mass of fuel burned each time, and this went down by a small amount for each fuel (due, I suspect, to the difference in quantity of fuel used each time). However, this similarity in mass of fuel burned each time does not affect the heat output equations, as that is affected by the temperature change. Proving my prediction that propanol would have the greatest heat output, the results (when displayed in a bar chart) escalate in order of methanol (the lowest heat output) to propanol (the highest). I also made predictions on the actual heat outputs of each fuel, and the obtained results (for ethanol and propanol, at least) proved to be quite a lot less than my predictions. To conclude my analysis, despite the inaccurate results caused by loss of heat to the air, propanol still proved to have the greatest heat output of the three fuels tested. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Organic Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Organic Chemistry essays

  1. Peer reviewed

    Burning Fuels Coursework

    4 star(s)

    Methanol - 5% error margin Ethanol - 6% error margin Propan-1-ol - - 6 % error margin Butan-1-ol - 6% error margin Pentan-1-ol - 5% error margin We have found that Pentan-1-ol did not use less fuel than butan-1-ol. This may have been due to incomplete combustion between pentan-1-ol and the oxygen it reacted with.

  2. Hydrocarbons As Fuels.

    A large variety of compounds, including carcinogens, appear in the smoke from burning coal and wood. Alternatives to fossil fuels Biofuels Plants can be grown to be used directly as fuels, e.g. wood. Plants can also be grown for conversion into fuels, e.g. sugar cane is easily fermented into ethanol.

  1. To Investigate the Combustion of Fuels

    From this I can conclude that the more hydrogen and carbon atoms in an alcohol, the more energy will be released when it is burnt. This is because the difference between energy released by bonds being formed and energy used by bonds being broken is greater with more carbon and hydrogen atoms.

  2. Energy Transfer in Fuels

    flames, we shall adjust the Clamp to have the tip of the flame touching the base of the tin. Reading Thermometer - This is very important as the thermometer should be read at eye-level as reading it from different angles the temperature may look different, and if not read at eye-level is incorrect.

  1. In this report the effects of fire and explosion are examined based on quantitative ...

    The information is then displayed on screen as a temperature reading. 2.3 Description of Experimental Apparatus - The Pensky-Martins Closed Tester Diagram 2. Penskey-Martens Closed Tester The Pensky-Martins closed tester consists of a containment vessel, which is placed in an electrically heated metal vessel; the heating power of the metal vessel is 50V.

  2. This is a mini-project on fuel - topics include petrol and fossil fuels.

    On land too, mud covers dead plants and trees. Slowly the mud hardens into rock. More layers of rock from above and press down on the plants, burying them deeper and heating them up. 3. The pressure and heat slowly change the sea plants into oil and then into gas.

  1. Burning fuels.

    METHANOL CH3OH + 3O2 CO2 + 4 H2O H 2(H - C - O - H) + 3 (O=O) (C=O) + 4 (H - O - H) H Bonds Broken: C - H x 6 = 413 x 6= 2478 C - O x 2 = 335 x 2= 670

  2. GCSE Chemistry Revision Notes - everything!

    Alkenes burn in carbon dioxide to give carbon dioxide and water. But more importantly, they undergo addition reactions. Part of the double bond breaks and the electrons are used to join other atoms are the carbon atoms. After undergoing an addition reaction, the unsaturated alkene becomes a saturated alkane.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work