Hypothesis: The energy released by an alcohol increases as the number of carbon atoms increases.
Variables:
- Mass of water used: The mass of water used throughout the reaction was kept constant so that there would be consistency during the process of calculating the energy released.
- Time of combustion of alcohol: The time of combustion was kept fairly constant throughout the reaction for about 30s. This is because alcohols burn very fast and it was more convenient for consistency throughout the reaction.
- Temperature of water: The temperature of the water used was not constant throughout the reaction. This is because different alcohols release different amounts of energy that would lead to temperature rise at different rate. This is because some alcohols would require more energy than others to break their bond while others less, so this lead to different rise of temperature of alcohol.
- The distance between the burner and the calorimeter: The distance between the copper calorimeter and the burner was kept fairly constant throughout the experiment. This is because if the distance is increased, it would take more time to heat up the water, thus recording a low temperature rise and if increased high temperature rise would be recorded. Thus for a matter of consistency it was kept constant throughout the reaction.
- Copper calorimeter: Copper calorimeter was use because it conducts heat quickly and thus avoids the escape of heat.
Apparatus:
- Copper calorimeter
- Water (50ml)
- Insulator (glass shield)
- Alcohols: Methanol, Propanol, Butanol, Pentanol and Hexane.
- Matches
- Digital balance
- Thermometer.
- Heat proof mat.
- Clamp
Safety precautions.
- The alcohol flame was switch off immediately and gently after burning to prevent it from burning the lab.
- The chairs where kept in position to prevent anyone from tripping over them and falling.
- The room was well ventilated so that the incompletely burnt alcohol was removed from the lab without being inhaled in much quantity by the students.
- Goggles were worn to prevent alcohol from entering eyes in cases of accident.
- The alcohol was handled safely so that they will not spill over the lab and catch fire.
- Long hair was tied back and kept away from the flame at all times.
Method:
This investigation involves burning alcohol in air. Key Science – Chemistry by Eilleen Ramsden says that ‘an alcohol is a series of organic, homologous compounds’. The alcohol reacts with the oxygen in the air to form the product water and carbon dioxide (Combustion):
Alcohol (aq) + Oxygen (g) -> Carbon Dioxide (g) + Water (g)
CnH2n+1 (aq) + O2 (g) -> CO2 (g) + H2O (g)
This reaction is exothermic, as heat is given out. This is because the amount of reactant energy is more than the product energy the difference between this is energy is given off, therefore some energy has been given in the form of heat. The energy is given out in forming the bonds between the new water and carbon dioxide molecules. To measure the energy given off from the combustion, I must use this heat energy to heat something and this will water. This is assuming that all the heat produced by the combustion of the alcohol will be equal to the amount of heat absorbed by the water. So I will measure the amount of energy required to do so. There is no instrument which measures heat directly. So therefore I will have to arrange for the heat I wish to measure to be transferred into water and then I must measure the temperature rise. The heat is then given by the expression:
Heat = Mass of water × Heat capacity of water × Temperature rise
Heat =
- Using a 100ml measuring cylinder I measured 50ml of tap water and then transferred the contents of the measuring cylinder to a copper calorimeter. A thermometer was placed in the calorimeter to adjust to the correct temperature.
- The initial mass of alcohol was weighed and recorded on a digital balance.
- The initial temperature of water was recorded (this has given the thermometer time to adjust)
- The copper calorimeter was shielded to prevent heat loss to the environment and then clamped to a stand to keep it in the same position in the room and the same distance from the flame if possible.
- The alcohol was burnt until the temperature reached 80°C under the copper calorimeter attached to the clamp stand.
- After the temperature reached this point I removed the alcohol from beneath the calorimeter and placed the glass lid back on it.
- The final temperature of water was measured using the thermometer, although I removed the alcohol at 80°C there may still be some heat transfer so I waited till the temperature on the thermometer reached its peak.
- Then the alcohol was re-weighed and the mass loss was recorded.
- The process was repeated four different times with different alcohols ranging from methanol to Hexane. Then the energy change is calculated.
DATA COLLECTION.
DATA PROCESSION
Enthalpy of combustion = (-Q * molar mass)
Mass of alcohol used
Where Q = m * c* ∆t
Where Q = energy released, c = specific heat capacity of water, ∆t = temperature change = t2 – t1
Methanol
Q = mc∆t
= 50 * 4.18*24 = 5016J
but 0.74g = 5016J
32g = 32 * 5016
0.74 = 216908.1 J = -216KJmol-1
Ethanol
Q = mc∆t
= 50 *4.18* 19 = 3971J
but 0.41g = 3971J
46g = 46 * 3971
-
= 445526.8J = -445Kjmol-1
Propanol
Q = mc∆t
= 50 * 4.18* 20.4 = 4263.6J
0.33g = 4264J
60g = 60 * 4264
0.33
= 775272.73J = - 775Kjmol-1
Butanol
Q = mc∆t
= 50 * 4.18 * 22.4 = 4681.6J
0.35g = 4681.6J
74g = 74 * 4681.6
0.35
= 989824 J = 989.824
= - 990Kjmol-1
Pentanol
Q =mc∆t
= 50 * 4.18 * 20.2 = 4221.8J
but 0.28g = 4221.8J
88g = 88 * 4221.8
0.28
= 1326851.4J = - 1327Kjmol-1
CONCLUSION
From the results gotten from the above experiment, it is clearly seen that energy released by alcohols increases as we increase the number of carbon atoms. This is because with the increase in the number of carbon atoms, more energy would be required to burn more carbon atoms that would in turn increase the amount of energy released.
EVALUATION
The experiment has thus been very useful in showing that energy increases with increase in the number of carbon atoms in the compound. But the experiment was not entirely accurate because some errors where associated with the method used during the experiment. Some precaution was taken during the process of experimentation to make sure the hypothesis is proved true. Such precaution includes
- The flame was put off immediately and covered to prevent the alcohol from vaporising after burning.
- The water was constantly stirred when heated to allow for even heat distribution throughout the water.
- The calorimeter was insulated to prevent heat loss during the process.
- The spirit burner was insulated when the experiment was being carried out to prevent heat from being lost into the environment.
Some errors were encountered in the experiment. This includes
- The digital balance was not set accurately which resulted in errors in the data obtained from it.
- The insulator used in covering the calorimeter was not changed which resulted in it absorbing heat during combustion but the was released back to the calorimeter, which resulted in temperature rise above expected value.
- The spirit burner was not well insulated when burning so some of the heat escaped into the surrounding thus reducing the amount of heat absorbed by the water.
- Parallax error involve in reading the thermometer.
Despite the precautions that were taken during the experiment, some errors were also encountered in the experiment. Although the experiment in itself cannot be 100% accurate, but the result s that would be gotten can be improved by improving the methods used for carrying out the reaction. Such precautions includes:
- Changing the insulator each time the experiment was carried out to reduce heat from warming up the calorimeter.
- Cooling the calorimeter after every reaction.
- Making sure the digital balance is set accurately to ensure accurate results.
- Making sure the experiment was fully and well insulated with a good material that absorb heat readily.
REFERENCE:
A- LEVEL CHEMISTRY BY E.N RAMSDEN AND NEW SCHOOL CHEMISTRY BY ABABIO.