In the laboratory a student burns a 1.13-g sample of dimethyl oxalate (C,H,04) in a bomb calorimeter containing 1070. g of water. The temperature increases from 24.00 °C to 27.00 °C. The Water heat capacity of water is 4.184 J glec!. The molar heat of combustion is -1675 kJ per mole of dimethyl oxalate. Insulated Sample dish outside chamber CH,O,(s) + 7/2 O,(3) →4 CO2(2) + 3 H,0(1) + Energy Combustion (boml Calculate the heat capacity of the calorimeter. heat capacity of calorimeter =
In the laboratory a student burns a 1.13-g sample of dimethyl oxalate (C,H,04) in a bomb calorimeter containing 1070. g of water. The temperature increases from 24.00 °C to 27.00 °C. The Water heat capacity of water is 4.184 J glec!. The molar heat of combustion is -1675 kJ per mole of dimethyl oxalate. Insulated Sample dish outside chamber CH,O,(s) + 7/2 O,(3) →4 CO2(2) + 3 H,0(1) + Energy Combustion (boml Calculate the heat capacity of the calorimeter. heat capacity of calorimeter =
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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
Ignition
wires
heat
sample
Thermometer
absorb energy, a separate
experiment is needed to
determine the heat capacity of the
calorimeter. This is known as
Stirrer
calibrating the calorimeter.
In the laboratory a student burns a
1.13-g sample of dimethyl
oxalate (C,H,04) in a bomb
calorimeter containing 1070. g of
water. The temperature increases
from 24.00 °C to 27.00 °C. The
Water
heat capacity of water is 4.184 J
gl•c-!.
The molar heat of combustion is
-1675 kJ per mole of dimethyl
oxalate.
Insulated
Sample
dish
Burning
sample
Steel
bomb
outside
chamber
C̟H,O4(s) + 7/2 O(g)
→4 CO2(g) + 3 H2O(1)
+ Energy
Combustion (bomb) calorimeter.
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%2F5cf9748b-73ad-454f-b8c8-eb416a7a6a68%2F31dc6831-8db6-4f35-ab35-200ac48f8661%2Fipsby9t_processed.jpeg&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
Ignition
wires
heat
sample
Thermometer
absorb energy, a separate
experiment is needed to
determine the heat capacity of the
calorimeter. This is known as
Stirrer
calibrating the calorimeter.
In the laboratory a student burns a
1.13-g sample of dimethyl
oxalate (C,H,04) in a bomb
calorimeter containing 1070. g of
water. The temperature increases
from 24.00 °C to 27.00 °C. The
Water
heat capacity of water is 4.184 J
gl•c-!.
The molar heat of combustion is
-1675 kJ per mole of dimethyl
oxalate.
Insulated
Sample
dish
Burning
sample
Steel
bomb
outside
chamber
C̟H,O4(s) + 7/2 O(g)
→4 CO2(g) + 3 H2O(1)
+ Energy
Combustion (bomb) calorimeter.
Calculate the heat capacity of the
calorimeter.
heat capacity of calorimeter =
J/°C
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