• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month
Page
  1. 1
    1
  2. 2
    2
  3. 3
    3
  4. 4
    4
  5. 5
    5
  6. 6
    6
  7. 7
    7
  8. 8
    8
  9. 9
    9
  10. 10
    10
  11. 11
    11

Investigation to compare the energy given out when alcohol's burn

Extracts from this document...

Introduction

Charlie Cowley Planning an investigation 30/09/02 Investigation to compare the energy given out when alcohol's burn I am investigating how different types of alcohol's effect the amount of energy given off. The types of alcohol used will be; Alcohol Formulae * Methanol CH3 OH * Ethanol C2 H5 OH * Propanol C3 H7 OH * Butanol C4 H9 OH I am going to investigate the amount of energy given out by the creating of bonds by subtracting the amount of energy needed to break the bonds to the amount given out from the creating of bonds. Methanol; C H3 OH + O2 ? CO2 + 2H2O H ? H - C - O -H ? H C - H O - H O = C = O O = O H - H ( 412 ) ( 463 ) ( 743 x 2 ) ( 496 x 1.5 ) ( 463 ) Input : ( 3 x 412 ) + ( 463 ) + ( 360 ) + ( 496 x 1.5 ) = 2803 Output : ( 743 x 2 ) + ( 643 x 4 ) = 3338 Energy out 3338 - 2803 = 535 = 535 kJ Ethanol C2 H5 OH + 2O2 ? ...read more.

Middle

being lost and this will help the distance between the burner and calorimeter stay the same, convection will remain the same and heat loss into the calorimeter How will I get my Results To get my results I am going to light the burner and heat water in a copper calorimeter. I will be heating the water 10?, making sure of this by using a thermometer. I will then measure the amount of alcohol burnt using a balance straight before and after to get the most accurate results I can. Obtaining the evidence I used the following apparatus: Chemicals: * Methanol, * Ethanol, * Propanol, * Butanol, Apparatus: * Copper calorimeter * Fuel burners * Fuel burner lids * Thermometer * Balance * Clamp stand * Measuring cylinder This is how I did the experiment: I measured the temperature change (which was from a certain temperature to another certain temperature), and the amount of alcohol burnt off (by measuring the weight of the burner before and after and measure the different.), and the amount of water. I measured the temperature with a thermometer, the mass change with a balance and the water with a measuring cylinder. To make shore my results are reliable repeated the experiment a three times, compared it to my predicted results and looked at other people's results and compared them. ...read more.

Conclusion

This method could have been improved but not using classroom methods. To make the results as accurate as possible it would have been necessary to use a thermometer that measures to a degree of accuracy within 0.5(, and I would have to stop heating the water exactly on 30( so the change in water temp would have been the same. The results I obtained did make sense but they weren't as accurate as I would have liked, they were accurate enough to obtain and support a firm conclusion apart from the predictions do not make much sense as to being so far off the actual results. In experiment 1 there were unexpected results that made the results slightly inaccurate ethanol burnt using more energy than methanol. This was resulting in an unfair test, as the flame sizes were different and there was no protection against convection and draught. The only limitations were that it was impossible to do the experiment in great detail. To support my conclusion I have the evidence of the bond energies and knowledge of the fact that there are more bonds to break in butanol. To further support my conclusion I could have experimented with different alcohols. ...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. Marked by a teacher

    What an ester is, how it is made, examples of esters, animal testing issues ...

    4 star(s)

    saying something about a product, then the product is thought to be good as they are recommending it and they can afford more expensive products. Also, linking to what I said about the previous question, cosmetic companies compete for new products that do new things, but they may exaggerate what the product does.

  2. Investigate the enthalpy change of different alcohol

    fuel, because they are more stable so they gives out more energy. Butan-1-ol has the OH group attached to C1, and butan-2-ol has the OH group attached to C2, in addition, butan-1-ol gives out 600J more energy per mole, the trend would be the further the carbon the functional group is attached to, the less energy it gives out.

  1. Esters. Esters are formed from an alcohol and carboxylic acid; this is an ...

    Yes/ No 4) Do you agree with animal testing? Yes/ Kind of/ No 5) Would you buy a product if you knew it had been tested on animals? Yes/ No/ Maybe 6) Do you think that it is ok to test on some animals but not others? (e.g. rats)

  2. The aim of this investigation is to compare the enthalpy of the following different ...

    = 6 x 346 = 2076 14(C - H) = 14 x 435 = 6090 2(C - O) = 2 x 336 = 672 2(O - H) = 2 x 464 = 928 18(O = O) = 18 x 497 = 8946 12(C = O)

  1. The Energy Content Of Different Fuels

    Energy produced per mole = energy produced to heat the water No. of moles of fuel used Energy produced per mole = 7402.5 / 0.038043478 = 194580.0/ 1000 = 194.58 kjmol-1 1st Ethanol: 1. Temperature rise= (91-20)= 71?C 2. Mass of fuel used = (246.4 -244.4)

  2. hydrogen peroxide experiment

    hydrogen peroxide break naturally, as hydrogen peroxide decomposes, and reform to create the new products. However they break very slowly as the activation energy for the bonds to break is very high. The catalyst provides a reaction path with lower activation energy.

  1. Alcohol investigation

    O=O = O=C=O + H-O-H H H H H O=O O=C=O H-O-H O=O O=C=O H-O-H O=O H-O-H O=O Reactants-bonds present products-bonds present 9XC-H=9X413=3717kJ 8XO=C=8X740=5920kJ 3XC-C=3X346=1038kJ 10XO-H=10X463=4630kJ 1XC-O=1X360=360kJ 1XO-H=1X463=463kJ 6XO-O=6X498=2988kJ TOTAL ENERGY IN=8566kJ TOTAL ENERGY OUT=10550kJ ?Hcombustion = 8566 - 10550 = -1984kJ per mole Prediction The theoretical values show the

  2. GCSE Chemistry Revision Notes - everything!

    AS you go down the Series, the reactions become less rigorous. Metals below hydrogen do not react with water or steam. This is why copper is used in rum stills and for bother hot and cold water pipes. Metal + cold water ? metal hydroxide + hydrogen Metal + steam

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