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 0.981-g sample of L-ascorbic acid (CgHgO6) in a bomb calorimeter containing 1060. g of water. The temperature increases from 24.80 °C to 27.30 °C. The heat capacity of water is 4.184 Jgl-c•!. The molar heat of combustion is -2340. kJ per mole of L-ascorbic acid. C,H2O6(s) + 5 O,(g) -6 CO,(g) + 4 H,O(1) + Energy Calculate the heat capacity of the calorimeter. heat capacity of calorimeter - | J/°C
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 0.981-g sample of L-ascorbic acid (CgHgO6) in a bomb calorimeter containing 1060. g of water. The temperature increases from 24.80 °C to 27.30 °C. The heat capacity of water is 4.184 Jgl-c•!. The molar heat of combustion is -2340. kJ per mole of L-ascorbic acid. C,H2O6(s) + 5 O,(g) -6 CO,(g) + 4 H,O(1) + Energy Calculate the heat capacity of the calorimeter. heat capacity of calorimeter - | J/°C
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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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 0.981-g sample of L-ascorbic acid (CH3O6) in a bomb calorimeter
containing 1060. g of water. The temperature increases from 24.80 °C to 27.30 °C. The heat capacity of water
is 4.184 Jglc!.
The molar heat of combustion is –2340. kJ per mole of L-ascorbic acid.
C,HgO6(s) + 5 O2(g)6 CO,(9) + 4 H,0(1) + Energy
Calculate the heat capacity of the calorimeter.
heat capacity of calorimeter =
J/°C](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fca28178a-3d47-4681-8e63-a516498b8666%2F5985578e-8b3c-430c-9649-644ede1eca7a%2Fx1yzabb_processed.png&w=3840&q=75)
Transcribed Image Text: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 0.981-g sample of L-ascorbic acid (CH3O6) in a bomb calorimeter
containing 1060. g of water. The temperature increases from 24.80 °C to 27.30 °C. The heat capacity of water
is 4.184 Jglc!.
The molar heat of combustion is –2340. kJ per mole of L-ascorbic acid.
C,HgO6(s) + 5 O2(g)6 CO,(9) + 4 H,0(1) + Energy
Calculate the heat capacity of the calorimeter.
heat capacity of calorimeter =
J/°C
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