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

Burning Fuels Investigation.

Extracts from this document...


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. ...read more.


* Leave to heat up until the alcohol evaporates. * Take the temperature when the alcohol has evaporated. * Record the temperature of the water now. * Weigh alcohol * Record all results Results: Alcohol Mass of spirit buner (g) Fianl mass of spiit burner (g) Mass of alcohol burnt Temp. of water (�C) Final temp of water (�C) Temp rise in water (�C) Ethanol 229.05 228.35 0.7 24 31 7 229.75 226.75 3 23 29 6 228.75 224.90 3.85 26 33 7 Propanol 225.18 224.90 0.28 26 33 7 224.90 223.31 1.59 23 31 8 223.31 221.50 1.81 22 28 6 Butanol 227.75 227.40 0.35 23 29 6 227.32 226.75 0.57 23 30 7 225.45 225.35 0.1 21 27 6 Pentanol 227.68 226.45 1.23 24 31 7 225.20 225.32 25 29 4 225.35 Hexanol 230.18 229.39 0.79 23 29 6 229.39 228.23 1.16 23 31 8 227.33 226.52 0.81 23 28 5 Heptanol 220.54 211.06 9.48 24 31 7 220.49 210.59 9.9 24 30 6 210.09 209.90 0.19 22 25 3 Octanol 226.38 225.40 0.98 25 29 4 225.40 224.17 1.23 24 29 5 224.17 222.67 1.5 24 30 6 Alcohol Ave.mass of alcohol burnt (g) ...read more.


As these errors were only small, they could not have made the massive differences between the predicted results, so there must have been other factors that caused the heat from the burner not to reach the water. These could have been energy wasted on heat and light. Each of the alcohols were burnt by different groups, and each group could have done their experiment slightly different making the results different, which could have caused the results not to have come out as they were meant to. The results for heptanol came out a surprise, as the mass of alcohol burnt was far greater for two of the experiments than any of the other results. Octanol did not burn as well as expected either. The temperature variation in the water was simular for all of the results also this could be due to human error as the reading on the thermometer could have not been read in a straight line making mistakes in degrees centigrade. Even the electronic equipment could have made a difference like the time on the stopwatch, or the measuring cylinder for water, and even the temperature of the beaker. The mass balance results could have been different as the scales are very sensitive so almost anything could have changed the wieghts. ...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)

    as a more conductive material will raise the temperature of the water to a higher degree than a less conductive object. Other control variables are: The height of the fuel wick, the length between the wick and the beaker, whether the container will have a lid on and any insulation (if required.)

  2. Investigating the energy released from burning different alcohols.

    The heats of combustion of each alcohol also follow this pattern with the lowest heat of combustion at the top for methanol and the highest heat of combustion at the bottom for octanol. This pattern can also be seen in the graph drawn as well.

  1. The Energy Content Of Different Fuels

    This will be in ?C. * Calculate the mass of fuel used. By weighing the fuel at the beginning and at the end of the experiment and subtracting the beginning one from the end to find the difference. I will measure this in grams. I will weigh the fuel while it is in the burner

  2. Combustion of Alcohols Investigation.

    AVERAGES alcohol average mass change (g) Methanol 2.27 Ethanol 1.8 Propanol 1.4 Pentanol 0.97 mass of mole 32 46 60 88 ANALYSIS: Heat energy = mass of water x temperature change x specific heat capacity ?H = 100 x 40 x 4.18 = 16720J METHANOL: Heat per gram of methanol

  1. Hydrocarbons As Fuels.

    Solid fuels (coal) are sometimes powered for use in large industrial furnaces. - A fuel should be readily available, in large quantities and at a reasonable price. The availability and price of oil, for example, affect national economies so much that governments can fall and countries go to war when these change.

  2. Energy Transfer in Fuels

    Also by recording the results in a table, it would be easier to read off the results and produce a graph in the analysing part of the coursework. I think my plan will be a safe one as we are using the necessary equipment to make it safe, for instance we are using a burn proof mat and safety goggles.

  1. In this investigation I will be burning alcohol's to heat up a can of ...

    � Put the chosen alcohol under the beaker allowing the flame to just touch the beaker. � Leave to heat up until the alcohol evaporates. � Take the temperature when the alcohol has evaporated. � Record the temperature of the water now.

  2. GCSE Chemistry Revision Notes - everything!

    Example equation: Calcium carbonate ? calcium oxide + carbon dioxide CaCO3 (s) ? CaO (s) + CO2 (g) Most carbonates of metals lower in the Reactivity Series than calcium behave the same way. Metal hydroxides at the top of the Reactivity Series have hydroxides that are unchanged by heat, such as potassium and sodium.

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