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Bomb Calorimetry

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Submitted By swtbeybiivan
Words 2205
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Abstract:
The purpose of this experiment was to determine the energy of combustion for benzoic acid pellet and Di-Butyl Phthalate (DBP) in excess oxygen under constant volume. To perform this experiment we set up the apparatus for a bomb calorimeter, which would help to find the change in internal heat of the combustion of DBP. We also find the molar enthalpy of combustion by using the resulting equation. The experimental molar heat of combustion was precisely close to the literature value,-8628.85 kJ/mol, for trial 1 of DBP. But for trail 2, the percent error was higher than trail one making the accuracy and precision slightly off. The percent values of DBP trial 1 were 1.61% and 5.33% for trial 2, resulting that the data for trial 1 was more accurate and precise than trial 2.

Introduction:
The purpose of this experiment was to determine the heat of combustion under constant volume and excess oxygen. We identify ∆H°comb, heat of combustion, as the change in heat when the reaction between oxygen and two moles of DMP at a temperature of 298K and a pressure of 1 atm. The reaction for the combustion is expressed as….
2 (l) + 39 O2 (g) → 32 CO2 (g) + 22 H2O (l) (1)
A Parr bomb calorimeter was used in the experiment. As starting the experiment the volume was constant in the process. We can also say that changes in internal energy and molar enthalpy related with chemical changes are independent of pressure.
Having a good understanding of the principles of calorimetry and thermodynamics would be beneficial while performing the experiment. The First Law of Thermodynamics states that energy is neither created nor destroyed, but remains constant in the universe. The change in internal energy of a system, ΔU, at a constant volume is the main thermodynamic property and is expressed by the following equation:
ΔU = qv + w (2)
Where, qv and w represent the heat and

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