In this experiment, the data that was collected was not close to being satisfactory as the final calculation yielded enthalpies of combustion of -7966.1±5.70% for Trial 1, -8303.5±8.44 for Trial 2 and -7190.9kJ±8.78for Trial 3. These results are a far cry from the theoretical or accepted value of -13316.4kJ/mole for the enthalpy change of combustion. Using the percentage error formula, the percentage errors calculated for this experiment was 44% for Trial 1, 38% for Trial 2 and 46% for Trial 3. These huge percentages of error indicate a low yield of enthalpy change of combustion of eicosane. Therefore, it is determined that this particular calorimetric procedure to determine and calculate enthalpy change of combustion of eicosane is a flawed one. Since the total thermal energy values (q total) of the trials rises with an increase in time, there is a proportional relationship between time and total thermal energy of the system. This makes sense as the total thermal energy values depend on the temperature change which will rise as more time is giving for the water molecules to absorb thermal energy. However, the molar enthalpies of combustion remains fairly constant which is because the mass of wax melted increases as time increases too. When the total thermal energy of the system is divided by the total moles of wax melted, a constant molar enthalpy of combustion should be obtained. However, an increased duration improved the range of uncertainties of measurements calculated. This is because majority of the uncertainty is from the uncertainty of measurement of temperature using the thermometer. With a bigger temperature change, the uncertainty will have a smaller impact percentage wise and will give a smaller number in terms of uncertainty in the final results. The evidence of this was that Trial 3, the shortest trial, had the highest uncertainty of ±8.78%, Trial 2 had an uncertainty of ±8.44 and Trial 1, the longest trial, had the lowest uncertainty of ±5.4%. An increase in time will increase the temperature which will decrease the uncertainty of the molar enthalpy change of combustion which will hopefully give a more accurate result. This seems to be the case in the trials conducted as the set of data (Trial 3) with the highest uncertainty values had the biggest % error of 46%. However, the molar enthalpy of combustion calculated In the fields of science, there is no such thing as a perfect experiment and this experiment is far from perfect with percentage errors all above 80%. There were many experimental errors that occurred throughout the duration of this experiment and many of them were beyond the control of the experimenters. Firstly, metals such as iron that make up the can are excellent thermal conductors. They are capable of conducting heat from the burning paraffin candle towards the water but they are also capable of conducting heat away from the water into the atmosphere. This would make the temperature change of water lower than it should theoretically be, resulting in a much lower total heat value. This would result in a lower enthalpy change of combustion value, partly explaining the sources of error. On the note of thermal conductivity, ideal calorimeters are supposed to be perfect thermal insulators and are not supposed to conduct heat at all. The calorimeter used in this experiment was the opposite of perfect as it was made out of iron which is an extremely good conductor of thermal energy. The iron calorimeter would have conducted thermal energy away from the candle into the atmosphere, decreasing the temperature change recorded in the water bath. This would, in the end, result in a lower change of enthalpy of combustion value as the total heat energy values will be lower. The material of the calorimeter might one of many reasons why such a high percentage error was calculated. Ideally, the height at which the iron can was located above the lab surface should be kept at a constant level as it was one of the controlled variables. However, all three trials had to be completed in a time period of sev