# To measure the energy released by 1g of fuel from a series of alcohols which represent hydrocarbons.

Burning Fuels Investigation

Aim: To measure the energy released by 1g of fuel from a series of alcohols which represent hydrocarbons.

Diagram:

Fair test: The independent variable is the type of fuel I will be using. I will be controlling the following variables:

• The same amount of water-150 cm
• The same length of wick- 0.5cm
• The same burn time- 3 minutes
• The same size can
• The Height of can above flame
• The room temperature
• The alcohol must be up to the wick on all the test otherwise it is unfair.

Method:

1. Set up the experiment as shown in the diagram.
2. Weigh the mass of the fuel before it is burnt using the mass balance.
3. Check the temperature of the water using a alcohol thermometer.
4. Light the fuel for 3 minuets.
5. Weigh the fuel again and calculate the mass burnt.
6. Measure the temperature and calculate the temperature rise.
7. Repeat again twice to get a fair test.

Use this equation to find out the energy released per g for all the fuels.

Risk assessment: The alcohols are flammable and vaporise easily. Only take the cap off when necessary and wear goggles. Take care when handing the fuels and wash your hands if the fuel is spilt yourself.

Results:

I have now found the average initial, final mass, initial temperature and the final temperature. I did this by adding up the three run and dividing it by three.

Conclusion: The results show that our experiments did not trap 100 percent of the energy released from each fuel. The graph below shows that the results we obtained do not the follow the pattern of the book of data as they go up and down there as the book of data shows the energy released per j/g increased as the chemical bonds did.

In a molecule there are bond energies that hold the atoms together. When the fuel combusts a chemical reaction takes place, this breaks the bonds, ...