lab3

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York University *

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Chemistry

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Feb 20, 2024

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Title: Lab 3 Report- Calorimeter (Using a Bomb Calorimeter)

Purpose: To ascertain whether octane is a viable chemical for energy storage, we will use a bomb calorimeter to detect the change in heat associated with octane combustion in this experiment. Introduction/Theory The theory underlying this experiment is based on several fundamental thermodynamic ideas, such as calorimetry, enthalpy, internal energy, and the First Law of Thermodynamics. The field of science known as calorimetry is concerned with measuring heat transfer in chemical or physical processes. A calorimeter, a tool made to precisely measure the heat exchanged between a system and its surroundings, is used in this process. “By knowing the change in heat, it can be determined whether or not a reaction is exothermic (releases heat) or endothermic (absorbs heat)” (1). The thermodynamic parameter known as enthalpy (H) is used to describe the heat energy transfer between a system and its surroundings under constant pressure. It accounts for both the system's internal energy (U) and the work performed on or by the system. The formula for enthalpy is ΔH = ΔU + PΔV , where P is the pressure and V is the volume change (2). The entire quantity of energy that makes up a system is referred to as internal energy (ΔU). It contains the potential energy derived from the locations of the particles as well as their kinetic energy. The heat transfer (q) into or out of the system less any work (w) performed by or on the system determines the change in internal energy or ΔU. In mathematics, ΔU = q - w. Energy cannot be generated or destroyed, according to the First Law of Thermodynamics; it can only be moved or changed from one form to another (3). This law is sometimes stated as ΔU = q + w, where ΔU denotes the change in internal energy, q denotes the transfer of heat, and w denotes the work performed by or on behalf of the system. The bomb calorimeter in this experiment runs at a set volume, therefore the heat being measured is qv, where v stands for the fixed volume. The simulation, however, makes the false assumption that the measured quantity is the change in enthalpy (ΔH), which is written as ΔH = cΔT, where c is the calorimeter's heat capacity and T is the change in temperature. It is important to note that, in this configuration, ΔH and ΔU are quite close to the same value, therefore the theoretical error has little impact on the calculations. Since the calorimeter runs at a fixed volume, the experiment actually measures the change in internal energy (ΔU), thus the equation should be ΔU = qv. Materials: Equipment  Protective eyewear  Lab coat  Gloves

 Pipette  Crucible  Analytical balance  Cotton string  Trash bin  Oxygen vessel (top & bottom)  Pipette tip  Calorimeter Chemicals  Oxygen gas  Octane (1.00 g)  Water (1.2 L) Procedure 1. Put on a pair of gloves. 2. Insert the crucible into the analytical balance, then push the tare button 3. Attach a pipette tip to the pipette 4. Use the pipette to pour 1.00 g of octane into the crucible. 5. Throw away the pipette tip in the trash bin 6. Insert the crucible into the holder in the oxygen vessel top 7. Attach the liquid sample and the ignition wire together by placing a brief length of cotton string on the ignition wire 8. Put the oxygen vessel's top portion into its bottom portion. 9. Insert the oxygen vessel into the calorimeter's oxygen vessel dock. 10. To place the oxygen vessel into the calorimeter, press the insert button on the control panel. 11. To pressurize the oxygen vessel with oxygen until the chamber reaches a pressure of 25 bars, press the O, FILL button. 12. Press the water in button to add 1.2 L of water to the water bath. 13. Press the ignite button to begin the combustion reaction after waiting until the temperature in the oxygen vessel and the temperature in the water vessel have stabilized. 14. Calculate the water bath's initial and end temperatures. 15. Dispose of your gloves Calculations The following equation will be used to get the molar enthalpy of combustion of octane because the volume of the bomb calorimeter is constant:

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Conclusion After conducting the experiment, we found that the ΔH = 5219.26 ± 13.38 kJ/mol. This suggests that octane combustion is an exothermic process, which means that when it combines with oxygen, heat energy is released. All in all, we can conclude that octane is a viable chemical for energy storage. Octane is a potential chemical for energy storage since it generates a significant quantity of heat energy. This is because regulated combustion processes can liberate energy from octane. References (1) Libretexts. (2023, January 30). Calorimetry . Chemistry LibreTexts. https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textboo k_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/ Thermodynamics/Calorimetry#:~:text=Calorimetry%20is%20the%20process%20of,or %20endothermic%20(absorbs%20heat). (2) Enthalpy . Enthalpy - an overview | ScienceDirect Topics. (n.d.). https://www.sciencedirect.com/topics/biochemistry-genetics-and-molecular-biology/ enthalpy#:~:text=Enthalpy%2C%20normally%20denoted%20H%2C%20is,H%20%3D %20%CE%94%20U%20%2B%20%CE%94%20pV (3) First Law of Thermodynamics . First Law of Thermodynamics - an overview | ScienceDirect Topics. (n.d.). https://www.sciencedirect.com/topics/chemistry/first-law- of-thermodynamics#:~:text=The%20first%20law%20of%20thermodynamics%20states %20that%20energy%20can%20neither,energy%20within%20the%20control%20volume.

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