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

The Combustion rate of Alcohols and how much energy is required to break their bonds

Extracts from this document...

Introduction

Lordswood Boys School My Investigation H Name : Alex Byrd Set: 11Z The Combustion rate of Alcohols and how much energy is required to break their bonds Planning I am going to investigate what happens when I heat some water using sprit burners containing different alcohols and then find how much mass was lost. As I am going to be heating water up then some way or another I will be losing heat, plus if I'm in a room with a window open then the flame will be disturbed and the beaker will cool down from the cool air coming through. To help prevent this I shall put cardboard pieces around the flame to protect the flame and the beaker. I am going to use a copper container because it conducts heat better and so there will be better results. Diagram Sprit burners: Propanol Methanol Hexanol Ethanol Pentanol Copper beaker 50 ml water Clamp stand Clamp claw 4 cardboard tiles Heat proof mat Splint Lighter Measuring cylinder 1) Firstly set up the clamp stand and attach the clamp claw to it. ...read more.

Middle

I am going to use 5 different alcohols and repeat the experiment 3 times then I am going to take an average result. I predict that the alcohols with the bigger Carbon chain will need more energy to burn, because there are more bonds and so it is harder to break them all up. Science Theory I predict this because I have calculated the energy required to break the hydrocarbon bonds. I did this by working out the mass of the reactants and taking this away from the products. The results show that to break the methanol hydrocarbons would require less energy than to break the pentanol hydrocarbon and even more energy is required to break octanol hydrocarbons. This is because the structure of the carbon atom, each carbon atom is covalently linked to four hydrogen atoms this causes a structure of great hardness. This means that methanol will lose the most mass because less energy is needed to break the bonds. ...read more.

Conclusion

My prediction was correct because what I predicted in theory is true. Evaluating Problems There weren't many problems that faced me with the experiment. Accuracy. My results are as accurate as I could possibly get them, I tried to do an accurate fair test but without the exact equipment heat would always be lost and cause inaccuracies in my results. If I were to re-do my experiment I would investigate ways in which I could retain the heat maybe by surrounding the spirt burner in tin foil and around the metal container. If I were able to do this safely then I would be able to get more accurate results, which then may prove my theory correct. Odd Results. There weren't any odd results. Firm Conclusion Looking at my results and the results I was able to obtain I conclude that the smaller the hydrocarbon chain the less energy is needed to break the covalent bonds so more mass will be lost. The longer the hydrocarbons the more energy is required so less mass will be lost. ...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. Marked by a teacher

    Experiment to investigate the heat of combustion of alcohols.

    4 star(s)

    on a graph and another graph was plotted, from the calculated bond energies that were present in my planning before. However there are 2 other graphs that were plotted from the original data before it was averaged. Here is the calculated energy change, which is a little simplified to save time and space.

  2. Investigating the Combustion of Alcohols

    Nevertheless the results I obtained are sufficient enough to prove my hypothesis, in which I predicted that the enthalpy change between successive alcohols would increase as you go down the homologous series. This is because on burning, each alcohol molecule forms one more CO2 molecule and one more H2O molecule than the previous alcohol.

  1. Titration experiment - write up

    28.5 28.5 28.5 Initial burette reading 0.00 0.00 0.00 0.00 0.00 0.00 Titre cm3 27.8 28.2 27.4 28.5 28.5 28.5 Average table of results: Titration (cm3) 1 2 3 Final burette reading 28.5 28.5 28.5 Initial burette reading 0.00 0.00 0.00 Titre cm3 28.5 28.5 28.5 In the above table

  2. Comparing the enthalpy changes of combustion of different alcohols.

    The enthalpy change of combustion is measured in KJ mol-1. On the graph you can see that I have drawn an estimation of the enthalpy change of combustion value for ethanol. I can estimate that the value for ethanol is approximately -1350 KJ mol-1.

  1. The Combustion of Alcohols and the factors affecting these reactions

    = 6300 � 0.82 = 7682.92 J/g ?H2= 7.682 kJ/g n= 7.682 � 60 ?H3 = -460.91 kJ/mol of heat released Butanol Q= ?H = 100 � 4.2 � 15 ?H1= 6300 for 0.76g of butanol burned. = 6300 � 0.76 = 8289.47 J/g ?H2= 8.289 kJ/g n= 8.289 �

  2. Molar Heat of Combustion of Alcohols

    the burner so any transportation of these items would have to be done with caution to avoid being burnt or scolded by the water. We will always carry and store the burners and containers carefully to avoid any risk of breaking them and spilling the contents.

  1. An investigation into the heat of combustion of alcohol's

    I will also make sure that I have 100cm3 of water each time in the calorimeter. The temperature will always go up to 60? each time as well. I will also keep the height of the calorimeter at 5cm each time.

  2. GCSE Chemistry Revision Notes - everything!

    Bitumen ( a think black material) is melted and mixed with rock chips to make tar for roads. Cracking Although the fractions from crude oil distillation are useful, the amount of each fraction you get depends on the proportions of the various hydrocarbons available in the crude oil, not the amount in which they are need.

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