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

An investigation into energy released during heating with a range of alcoholic fuels

Extracts from this document...

Introduction

An investigation into energy released during heating with a range of alcoholic fuels By Michael Finley, 11LY PLANNING This experiment is designed to determine which fuel out of the eight tested releases the most energy, to determine which is best. We will be using Ethanol, Propan-1-ol, Butan-1-ol, Pentan-1-ol, Hexan-1-ol and Octan-1-ol. METHOD In order to collect the results, I will need to heat up some water with a micro burner powered by each alcoholic fuel. I will need to weigh the fuel before and after the experiments to see how much of the fuel has been used up. I will also need to take the temperature of the water before and after the experiment to see how much the temperature changed. The two changes should allow me to see which fuel releases the most energy. I will do the experiment three times and collect the results, and take the average. ...read more.

Middle

= 756 KJ/Mol 2062 + 746 = 2808 KJ/Mol, which is the energy needed to break the bonds. Then I calculated the energy released when new bonds are made: 2 x C=O (2 x 740) = 1480 KJ/Mol 4 x O-H (4 x 463) = 1852 KJ/Mol 1480 + 1852 = 3332 KJ/Mol To calculate the energy balance, I did: 3332 - 2808 = 523 KJ/Mol Therefore the molar mass of Methanol was 523 KJ/Mol To find the molar mass of Ethanol, I had to do: Ethanol = 524 KJ/Mol + Balance I worked the balance out to be: 2406 - 1918 = 488 I then calculated the molar mass of all the fuels. Methanol = 524 KJ/Mol Ethanol = 524 + 488 = 1012 KJ/Mol Propan-1-ol = 1012 + 488 = 1500 KJ/Mol Butan-1-ol = 1500 + 488 = 1988 KJ/Mol Pentan-1-ol = 1988 + 488 = 2476 KJ/Mol Hexan-1-ol = 2476 + 488 = 2964 KJ/Mol ...read more.

Conclusion

REVISED DIAGRAM OF APPARATUS SECONDARY TESTS Fuel Starting temp/weight Finishing temp/weight Temp/weight change Ethanol 14�C/73.25g 37�C/71.91g 23�C/1.34g Octan-1-ol 18�C/73.49g 44�C/73.39g 26�C/0.1g We used a beer can with air holes in to insulate the Micro burner - we also moved the micro burner to 2cm away from the boiling tube rather than 6cm. RESULTS For this test (And the two before hand) I used 10cm3 of water. Test One Temperature Start Temp End Temp Change in Temp 19�C 32�C 13�C 20�C 31�C 11�C 22�C 32�C 10�C 18�C 29�C 11�C 18�C 30�C 12�C 19�C 30�C 11�C 18�C 28�C 10 Test Two Temperature Start Temp. Finishing Temp. Temp. change 16�C 39�C 23�C 15�C 42�C 27�C 14�C 50�C 36�C 18�C 44�C 26�C 15�C 50�C 35�C 19�C 60�C 41�C 13�C 46�C 33�C Test three Temperature Start Temp. Finishing Temp. Temp. change 11�C 34�C 23�C 11�C 33�C 22�C 11�C 37�C 26�C 11�C 34�C 23�C 16�C 41�C 25�C 14�C 28�C 14�C 14�C 36�C 22�C ...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. An investigation into the heat energy released upon burning different fuels

    Weigh the mass of the alcohol burner (with lid) on the scales and record its' mass before being lit. ? Place the burner underneath the beaker and light. Wait for the temperature to rise by 30ºc and then put the lid over the burner to stop it burning. ?

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

    The nuclear reaction occurs in the nuclei (centres) of atoms. This can happen in two ways: when the nucleus of a heavy atom splits, in a process called fission, and when two light weight nuclei joined together, in a process called fusion. In nuclear weapons, fission, or fusion occurs in a split second.

  1. The Energy Content Of Different Fuels

    This means that the formula had something to do with 492. I found that if you times the number of carbons by 492 and then add 37 you get the expected enthalpy of combustion. This can therefore be written as: 492n + 37 = enthalpy of combustion.

  2. Hydrocarbons As Fuels.

    and cracking ( to produce more gasoline and alkanes ). There is insufficient gasoline and naphtha fractions from the primary distillation to satisfy the demand for petrol. So higher boiling fractions are cracked to produce more gasoline and naphtha. Modern petrol engines require higher proportions of branched-chain alkanes, cycloalkanes and arenes to promote efficient combustion.

  1. Energy Transfer in Fuels

    Weighing The Fuel - When weighing each fuel, in the initial and final weights, the cap of the Paraffin Burner needs to be off as they may weigh different masses. This is essential for a correct answer to our formula of energy transfer.

  2. Burning Fuels Investigation.

    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 when they are burnt because they split. This tells us the more bonds the more energy in the alcohol, and more energy to be released.

  1. Investigation into burning fuels.

    To make sure my final experiment is correct and I cannot do it any better I have done a test run. I followed my method for 1 fuel. I chose ethanol. I ran this experiment 1 minute and only did one run of the experiment.

  2. GCSE Chemistry Revision Notes - everything!

    This takes advantage of the different in boiling points in ethanol and water. Water boils at 100 °C whereas ethanol boils at 78 °C. The source of the sugar determines the type of alcoholic drink produced, for example, grapes produce wine and barley for beer.

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