Investigation on in to the combustion of Alcohols
Hypothesis
As the number for carbon atoms in alcohol increases the more energy is released.
I am going to conduct an experiment, which will allow me to compare the heat energy given off by three alcohols, those being ethanol, propanol and butanol. These alcohols have a difference of one carbon atom within there atomic structure. I am going to investigate the amount of energy given out per mole once we burn the alcohol, which is the enthalpy of combustion (?H c).
This can be supported with the calculations of the bond energies
We know that chemical bonds are broken in reagents for this to happen energy must be put in and also chemical bonds are made in the products when this happens and energy is given out.
How much energy has to be put into break a given bond or how much is given out when this bond is made depends on the strength of the bond
The net energy change ?H depends on the relative strength of the bonds being made and broken.
Exothermic reactions
Exothermic reactions stored chemical energy is converted into heat energy because the bonds being broken are weaker than the bonds being formed.
This energy diagram is for an exothermic reaction. It shows the energy content of the reactants and the products.
The energy change for a reaction delta H can be calculated using bond energies
?H = (sum of bonds being broken) - (sum of the bond being made)
Bond energy is defined as the energy required to break one mole of bonds in a substance in the gaseous state.
Bond
Bond energy in KJ/Mol
C-C
348
C-H
412
C-O
360
O-H
463
O=O
496
C=O
743
H-H
436
Apparatus
Thermometer
Measuring cylinder (100cm2)
Stopwatch
Distilled water
Clamp
Stand
Scales
Spirit burner
Heatproof mat
Beaker (250cm2)
Ruler
Towelling, cloths (for cleaning beakers)
Top pan balance (nearest 2 at degrees)
Graph paper
Method
Set up the following experiment as shown in the diagram above. Make sure that the beaker is set exactly 10cm above the wick bearing in mind that the wick is 1cm high. Fill the beaker with 100 grams of distilled water (H2O), to do this accurately use a measuring cylinder so that you measure to the nearest millimetre. Weigh the mass of the selected alcohol, so that you can work out the initial mass loss of the alcohol after the experiment. Use the electronic weighing scales which has a minimum of degree of accuracy to at least two decimal points. Then quickly take off the cover and light the wick while also starting the timer. I will time the experiment for 100 seconds. While I am heating the water will also be stirring the water with a thermometer so that the temperature of all of the water and not just the water at the bottom. Then when the timer has reached 100 seconds (one minute forty seconds) quickly cover the flame so that no more mass is burnt off and leave the lid on so that there isn't any evaporation. Then read the temperature of water and note down the highest temperature the thermometer records. Then weigh the end mass of the alcohol and note it down, as you will need this data to work out the mass burnt.
Hypothesis
As the number for carbon atoms in alcohol increases the more energy is released.
I am going to conduct an experiment, which will allow me to compare the heat energy given off by three alcohols, those being ethanol, propanol and butanol. These alcohols have a difference of one carbon atom within there atomic structure. I am going to investigate the amount of energy given out per mole once we burn the alcohol, which is the enthalpy of combustion (?H c).
This can be supported with the calculations of the bond energies
We know that chemical bonds are broken in reagents for this to happen energy must be put in and also chemical bonds are made in the products when this happens and energy is given out.
How much energy has to be put into break a given bond or how much is given out when this bond is made depends on the strength of the bond
The net energy change ?H depends on the relative strength of the bonds being made and broken.
Exothermic reactions
Exothermic reactions stored chemical energy is converted into heat energy because the bonds being broken are weaker than the bonds being formed.
This energy diagram is for an exothermic reaction. It shows the energy content of the reactants and the products.
The energy change for a reaction delta H can be calculated using bond energies
?H = (sum of bonds being broken) - (sum of the bond being made)
Bond energy is defined as the energy required to break one mole of bonds in a substance in the gaseous state.
Bond
Bond energy in KJ/Mol
C-C
348
C-H
412
C-O
360
O-H
463
O=O
496
C=O
743
H-H
436
Apparatus
Thermometer
Measuring cylinder (100cm2)
Stopwatch
Distilled water
Clamp
Stand
Scales
Spirit burner
Heatproof mat
Beaker (250cm2)
Ruler
Towelling, cloths (for cleaning beakers)
Top pan balance (nearest 2 at degrees)
Graph paper
Method
Set up the following experiment as shown in the diagram above. Make sure that the beaker is set exactly 10cm above the wick bearing in mind that the wick is 1cm high. Fill the beaker with 100 grams of distilled water (H2O), to do this accurately use a measuring cylinder so that you measure to the nearest millimetre. Weigh the mass of the selected alcohol, so that you can work out the initial mass loss of the alcohol after the experiment. Use the electronic weighing scales which has a minimum of degree of accuracy to at least two decimal points. Then quickly take off the cover and light the wick while also starting the timer. I will time the experiment for 100 seconds. While I am heating the water will also be stirring the water with a thermometer so that the temperature of all of the water and not just the water at the bottom. Then when the timer has reached 100 seconds (one minute forty seconds) quickly cover the flame so that no more mass is burnt off and leave the lid on so that there isn't any evaporation. Then read the temperature of water and note down the highest temperature the thermometer records. Then weigh the end mass of the alcohol and note it down, as you will need this data to work out the mass burnt.