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

The differences between the Enthalpy Changes of Combustion of the alcohols

Extracts from this document...

Introduction

The differences between the Enthalpy Changes of Combustion of the alcohols

Hypothesis

The differences between the Enthalpy Changes of Combustion of the alcohols when calculated using bond enthalpy values are as follows:

Methanol → Ethanol : 587kJ

Ethanol → Propan-1-ol : 617kJ

Propan-1-ol → Butan-1-ol : 617kJ

I shall check to see the differences

...read more.

Middle

Ethanol → Propan-1-ol : 606kJ

Propan-1-ol → Butan-1-ol : 233kJ

I would say that the first two were fairly normal, and it is because the measured value for Butan-1-ol was so low, that the difference between that and Propan-1-ol was so low. This means that this hypothesis

...read more.

Conclusion

class="c2">Energy Produced Using Bond Energies:         1274 kJ

Measured Energy Value:        822 kJ

Propan-1ol:

Energy Produced Using Bond Energies:         1891 kJ

Measured Energy Value:        1431 kJ

Butan-1-ol:

Energy Produced Using Bond Energies:         2508 kJ

Measured Energy Value:        1702 kJ

Bibliography

The other sources that I have used for information on this investigation are:

Salter’s Chemical Ideas Book

...read more.

This student written piece of work is one of many that can be found in our GCSE Electricity and Magnetism 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 Electricity and Magnetism essays

  1. Marked by a teacher

    Investigation into Energy Released From Burning Various Alcohols.

    4 star(s)

    If I substitute some numbers into the formula I get the following results: Methanol 1 80 x 4.2 x 27 = 9.07 Kj Ethanol 2 80 x 4.2 x 40 = 13.44 Kj I used the Excel spreadsheet to work out the rest of the data.

  2. Investigating the heat of combustion of a series of Alcohols

    To find out the total amount of energy transferred to the water I used the following equation. Energy Transferred = Rise in Mass of Specific heat temperature X water (kg) X capacity of of water (oC) water (kJ/kg/oC) This equation only gives the energy given off by 0.5g of the alcohol.

  1. Investigating The Heat Of Combustion Of Alcohols.

    When this is done we see that the total energy released is 5996kJ. When the energy used to break the bonds is taken away from the energy produced when bonds are made we get a total of 1161kJ. We must also notice that 2 moles of carbon dioxide and 3 moles of water is produced.

  2. Combustion of Alcohols

    many moles were burnt, and as a result how many KJ per mole is released. Time: This should to be constant because you should not vary more than one thing in an experiment, but it really does not matter, as the result in the end will be the same, because

  1. In my investigation I will measure the heat given out by different types of ...

    the first law of thermodynamics states that energy can neither be created nor destroyed but is simply transferred from one form or system another, the decrease in the energy level of the electrons must mean that energy is transferred to the surroundings.

  2. To investigate the relationship between the structure and heat provided by combustion of a ...

    during a reaction, by allowing the substance reacting to heat a measured mass of liquid. The temperature change of this liquid is measured and recorded, and the following equation may be used to calculate the heat energy transferred to the liquid: Heat change = MC?T (where M = mass of liquid, C = critical temperature, and T = temperature change).

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