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

GCSE Chemistry Coursework-Burning Fuels Investigation

Extracts from this document...


GCSE CHEMISTRY COURSEWORK- BURNING FUELS INVESTIGATION CANDIDATE NO. 8218 - ANDR� SKEPPLE-GARRAWAY AIM: My aim is to measure the energy released by a series of alcohols. APPARATUS: Fuel, matches, stand, clamp, steel can, calibrated digital scales, thermometer (digital or alcohol), and stopwatch. METHOD: Fill can with 150cm� of water. Then get a stand and the clamp and connect the clamp to the stand if it not already connected. Place the can filled with water and tighten it with the clamp. Then place a thermometer, either a digital on or an analogue one which uses alcohol and record the waters room temperature before the experiment. Then get the chosen fuel in its spirit burner container and measure its mass before the experiment on the digital scales and record it down in the table. Then open the cap of the fuel and light the wick of the burner with matches and heat the water with the flame for 3 minutes using the stopwatch and move the can slightly above the flame so that the flame is barely touching the steel can. Repeat with same fuel three times and then extinguish the flame by snuffing the flame putting the lid back on the spirit burner. Afterwards, measure the fuels mass on the scales again and record the waters temperature after the experiment. ...read more.


Mass after (/g) Start temp. (�c) End temp. (�c) Methanol CH�OH n/a n/a n/a n/a Ethanol C�H5O4 191.31 190.38 22.1 41.1 Propanol C�H7OH 224.17 220.78 22.3 35.2 Butanol C4H9OH 221.32 215.94 23 54 Pentanol C6H13OH 184.55 183.43 22.3 37.4 Hexanol C6H13OH 213.28 210.99 26 39 Heptanol C7H15OH 233.84 239.14 23 85 Octanol C8H17OH 231.95 229.72 22 41 RESULT AVERAGES: Name of fuel Average temp. rise Energy released Methanol CH�OH n/a n/a Ethanol C�H5O4 17.8 6300 Propanol C�H7OH 32 4675.5 Butanol C4H9OH 26 4561.5 Pentanol C6H13OH 17.5 11250 Hexanol C6H13OH 21.1 7153.9 Heptanol C7H15OH 31 9231.3 Octanol C8H17OH 19.8 5829 MY RESULTS AGAINST THE BOOK OF DATA: Name of fuel Results from experiment (j/g) Book of data results (j/g) Methanol CH�OH 11960 Ethanol C�H5O4 6300 17450 Propanol C�H7OH 4675.5 20810 Butanol C4H9OH 4561.5 23070 Pentanol C6H13OH 11250 24700 Hexanol C6H13OH 7153.9 25470 Heptanol C7H15OH 9231.3 26890 Octanol C8H17OH 5829 27660 Graph is on next page... CONCLUSION: According to the results the outcome is that if a fuel has more carbons in its atomic structure, the more energy it releases during combustion. This information was received from looking at the Book of Data results and not the results from the experiment. This is because the experiment results have no correlation to the book of data's results and they are not in numerical order like the results in the Book of Data and they are not as high as the Book of Data's. ...read more.


In the case of the time limit, the investigators should use stopwatches that alarm or alert the users when the set time for the experiment counts down to the alert to make the time used to perform the experiments are equal. Therefore the new method is to place 3x150cm�of water in a refrigerator 30 minutes before the start of the experiment and make sure that the water has the same temperature. Then collect the chosen fuel and weigh it in three different calibrated scales and then find the average mass before combustion. Do the same for the average mass after combustion and the same with each fuel. Place the steel can 27cm above the surface the experiment is on. Collect one or two boxes of matches that are the same and are lit the same way. Light the fuel and place three digital thermometers in the can filled with water and correctly countdown 3 minutes on two stopwatches. After the end of the trial measure the temperatures from the three thermometers and then average them out and work out the average temperature rise and the energy released. To make sure that the room temperature is the same and to cut down on time consumption try to get as many people to perform the different experiments at the same time. ...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)

    A Kelvin is a unit increment of thermodynamic temperature and is equal to an increment of one degree Celsius. Energy is a difficult variable to measure, and it can never be taken as 100% accurate, as there will be some form of energy loss in any activity.

  2. Peer reviewed

    Alcohols Coursework

    3 star(s)

    heat capacity X temperature rise 1000 Where q is the quantity of heat. The specific heat capacity is the amount of energy required to heat the substance, and is calculated using the formula q = MC?, where q is the enthalpy, is the specific heat capacity and ?

  1. Energy Transfer in Fuels

    So this formula shows us (by using the initial and final masses) which fuel was most efficient (used up the least amount of fuel). This shows us that Octanol gave the largest energy transfer to the water. So, my prediction was correct as I predicted that the fuel with the most carbons would create the largest energy transfer.

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

    Internal Combustion Engine The engine that powers almost all the world's cars is the internal-combustion engine. It uses the power of gases created by exploding fuel to produce movement. A mixture of air and tiny droplets of petrol enters the engine's cylinders, each of which contains a piston.

  1. The Energy Content Of Different Fuels

    If you find the differences between the different enthalpy of combustions and relate them to the amount of Carbons I have been able to find a formula that relates the amount of Carbons to the enthalpy of combustion. To do this I found that there is exactly 492 kjmol-1 between each one as a carbon is added.

  2. hydrogen peroxide experiment

    The Presence Of a Catalyst Vary With Time If there is a lower activation energy, more collisions result in a reaction. If more collisions react the R of R is faster. This allows us to collect data in a short time period.

  1. Alcohol investigation

    = + H-O-H H Reactants- Bonds present Products- Bonds present 3XC-H=3X413=1239KJ 2XC-O=2X740=1480KJ 1XC-O=1X360=360KJ 4XO-H=4X463=1852KJ 1XO-H=1X463=463KJ 1.5XO=O=1.5X747=747KJ TOTAL ENERGY IN=2809KJ TOTAL ENERGY OUT=3332KJ Energy change for = total bond energy - total bond energy The reaction of reactants of products ?Hcombustion = 2809 - 3332 = -523kJ per mole Ethanol +

  2. GCSE Chemistry Revision Notes - everything!

    Cations are positive because they have lost one electron, so it has the same number of positively charged protons but one less electron to balance them. Anions are negatively charged because they have gained an extra negative electron. A lot of energy is needed to overcome the strong forces of attraction between oppositely charged ions.

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