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

GCSE Science Coursework

Extracts from this document...

Introduction

GCSE Science Coursework Title: Burning Fuels. What are you trying to find out? I will be carrying out an investigation, which allows me to calculate and compare how much energy/fuel is used to raise 100cmcubed of water to 20 degrees centigrade. I will be using 5 different fuels; Butanol, Pentanol, Propanol, Methanol and Ethanol. The aim is to find out how much energy is produced when burning these alcohols. Alcohol's react with oxygen in the air to form water and carbon dioxide. This is an exothermic reaction, meaning that when energy is put in, more energy is given off. The formulae of the alcohols that I will be using are. Methanol CH OH Ethanol C H OH Propanol C H OH Butanol C H OH Pentanol C H OH Prediction: I predict that the more bonds there are holding the carbon, oxygen and hydrogen atoms together; more energy will be required to break them apart. For example Ethanol has the formula C H OH. ...read more.

Middle

There will be 15 altogether. Controlled variables. To make sure the experiment will be a fair and reliable test, I will keep the following exactly the same every time the experiment is done; same distance between the burner and the can containing the water. Same temperature change in degrees centigrade. I will always use a foil shield placed around the burner to stop the wind blowing out the flame. Mass of water, 100cm. Type of container, tin. The same set of scales and always weigh the alcohol with the lid on. Safety aspects: Tie long hair back, work standing up, never leave a flame unattended, turn flame off roaring after heating, tidy all other objects and work away. Method: The method I used to conduct my experiment went as followed: Measure 100cm of water in to a tin container. Place the container into the grasp of the clamp stand. Record the starting temperature of the water Weigh the alcohol burner with the lid on. ...read more.

Conclusion

This is because there are more bonds in the alcohols with more carbons per molecule than in the alcohols with fewer carbons per molecule. When energy is put in, the bonds are broken. For the bonds to form again, energy is given out, and the amount of energy given out in the reaction is greater than that put in, meaning the reaction is exothermic. This means that to start the reaction, you need energy. Once the reaction is started, you get more energy back than you put in. This means that if you put more energy in, you get more energy out. You need more energy to break the bonds of Pentanol than Methanol, so you will get more energy out of burning Pentanol per mole, that you will with burning Methanol per mole. Overall the experiment went well for me, even though the results could have been more accurate had I used foil to protect my flame and heat loss. I'm glad that I didn't use foil however, as it gives me something to change next time and improve on in further experiments. By Tom Spence 11H. ...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)

    Put out the wick and weigh the alcohol. Record the mass loss of each alcohol. 8. Repeat the experiment 3 times per fuel. 9. Change the alcohol, and repeat the previous methods. Preliminary Results My first sets of preliminary results were tested using a Bunsen burner, a 2cm wick,

  2. Peer reviewed

    Alcohols Coursework

    3 star(s)

    These can be of two types: covalent, in which the atoms share electrons. Examples of this are water and carbon dioxide, which has a double covalent bond because it shares two pairs of electrons are shared. The other type of bonds are ionic, where a metal is involved.

  1. The Energy Content Of Different Fuels

    not come out anyway near the results that I predicted but this is due to experimental error. Although my experiment did not show exactly these results, it still followed the trend of increasing apart from Pentanol, where one of the results was a long way out and that could have been for any reason.

  2. Calculate and compare how much energy/fuel is used to raise 100cmcubed of water to ...

    All of the other alcohols can be broken up in this way. Below is a table showing the energy required to break up the bonds in each alcohol. Type of alcohol Energy required to break the bonds in the alcohol (j)

  1. Investigate the different amounts of energy given off when different alcohols are combusted. I ...

    I can also work this prediction out using bond energies. I expect these bond energy results to show negative results, which means that the experiment is exothermic and is giving out heat. Although I know I must appreciate that my results will not be entirely accurate as heat will not completely be transferred to heating the water.

  2. Which Alcohol is the best fuel?

    I will experiment with: Methanol CH OH Ethanol C H OH Propanol C H OH Butanol C H OH Pentanol C H OH These five alcohols will allow me to produce a good set of results that I can make accurate conclusions from.

  1. The aim of this experiment is to compare the amount of energy released when ...

    They then make new bonds. 2 of the hydrogen atoms join to an oxygen atom, and the other 2 hydrogen atoms join to the other oxygen atom. This forms two water molecules. The reaction is exothermic as the energy released in making new bonds is greater than the energy taken in to break the original bonds.

  2. GCSE Chemistry Revision Notes - everything!

    When the zinc chloride melts, the ions are free to move. The positive zinc ions are attracted to the cathode, as the electrons are transferred from the cathode to the ion and the ion is changed into a zinc atom.

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