Two experiments were conducted in a bomb calorimeter. The first one to determine the heat capacity...
Two experiments were conducted in a bomb calorimeter. The first one to determine the heat capacity of the calorimeter, the second to determine the heat of combustion of the carcinogenic substance benzene (C6H6). In the first experiment, the temperature rises from 22.37degrees C to 24.68degrees C when the calorimeter absorbs 5682 J of heat. the second experiment, the comustion of 0.258g of benzene increases the temperature from 22.37degreesC to 26.77degreesC. Determine the heat of combustion for 1 mol of benzene.
Homework Answers
Question 1
determine the heat capacity of the calorimeter
heat capacity of the calorimeter = 5682 Joules / (24.68 degreesC - 22.37 degreesC) = 2459.74 J/degreesC
heat capacity of the calorimeter = 2459.74 J/degreesC
Question 2
Temperature change when benzene in combusted = 26.77 DegreesC - 22.37 DegreesC = 4.4 DegreesC
The amount of heat released = 2459.74 J/degreesC x 4.4 DegreesC = 10822 Joules or 10.822 Kilo Joules
Moles of benzene combusted = 0.258 gm / 78 gm /mol = 0.00330 Moles
heat of combustion for 1 mol of benzene = 10.822 Kilo Joules / 0.00330 Moles = 3271.769 Kilo Joules / Moles
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Ignition wires heat sample Thermometer Stirrer A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter This is known as calibrating the calorimeter In the laboratory a student burns a 0.319-g sample of phenanthrene (C14H10 in a bomb calorimeter containing 1070. g of water....
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A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.425-g sample of diphenylacetylene (C14H10) in a bomb calorimeter containing 1170. g of water. The temperature increases from...
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1.
2.
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.425-g sample of diphenylacetylene (C14H10) in a bomb calorimeter containing 1170. g of water. The temperature increases from...
Thermometer Ignition wires heat sample Stirrer A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Water In an experiment, a 0.3916 g sample of phenanthrene (C14H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.266x10 g of water. During the combustion the temperature increases from 23.47 to 26.10 °C. The heat capacity of water is 4.184 J gloc-1....
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 1.14-g sample of L-ascorbic acid (C6H306) in a bomb calorimeter containing 1040. g of water. The temperature increases from 24.30...
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