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Bomb Lab - Dennis Zollo Thermodynamics laboratory...

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Dennis Zollo Thermodynamics laboratory: Measurement of the Heat of Combustion Using a Bomb Calorimeter Abstract: Combustion of hydrocarbons and organic molecules is a vital chemical process in modern society and technology. This reaction runs our transportation, generates our electricity, and warms our homes. As such, the exact heat evolved from the combustion of various substances is a very relevant quantity. This laboratory exercise explores the use of a bomb calorimeter to measure the heat produced by combustion reactions of solid and liquid fuels. It will then compare these empirical heats of combustion with accepted values, and the specific effect of incomplete combustion on these empirical results. It lastly will explain any qualitative differences between the type of fuel (liquid, solid, etc) and its heat of combustion. Results: Combustion of Benzoic Acid 22.5 23 23.5 24 24.5 25 25.5 26 0 100 200 300 Time Temperature (C) "1g benzoic acid delta T = 2.64K Amount of Oxygen- Equivalence Ratio: We first need to make sure that there is enough oxygen inside the bomb such that we can assume all fuel was consumed by the reaction. The bomb has a volume of .343 L, and in the charcoal trial, had a pressure of 19.1 atmospheres.
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oal molscharch g g MM M n molO atm L RT pv n nRT pv fuel fuel fuel 0782 . 12 946 . 2675 . 273)K (23 * mol atm/K L 0.08205784 19 * ) 343 (. 2 = = = = + = = = We can stop this analysis right here: the molar ration of fuel to oxygen is more than sufficient to allow the combustion to move completely to products; it is a very rich mixture. The stochiometric ratio of charcoal to oxygen is 1 : 1, and our actual ratio is . 0782/.2675 = .3. This gives us an equivalence ration of 1/.3, or 3.42, which is clearly rich enough for full combustion. Since this analysis occurred with our lowest molar mass sample, charcoal, charcoal had the most number of moles put in the combustion chamber.
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