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. Ignition Thermometer wires Stirrer heat sample Water Insulated outside Sample Burning Steel dish sample bomb chamber Combustion (bomb) calorimeter. In an experiment, a 0.3601 g sample of anthracene ( C4H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.041 x 103 g of water. During the combustion the temperature increases from 22.55 to 25.33 °C. The heat capacity of water is 4.1843-C The heat capacity of the calorimeter was determined in a previous experiment to be 996.1 J. "C"¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of anthracene based on these data. CH()+(33/2)0, (g) → 5H₂O(1)+14CO2(g) +Energy Molar Heat of Combustion = kJ/mol
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. Ignition Thermometer wires Stirrer heat sample Water Insulated outside Sample Burning Steel dish sample bomb chamber Combustion (bomb) calorimeter. In an experiment, a 0.3601 g sample of anthracene ( C4H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.041 x 103 g of water. During the combustion the temperature increases from 22.55 to 25.33 °C. The heat capacity of water is 4.1843-C The heat capacity of the calorimeter was determined in a previous experiment to be 996.1 J. "C"¹. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of anthracene based on these data. CH()+(33/2)0, (g) → 5H₂O(1)+14CO2(g) +Energy Molar Heat of Combustion = kJ/mol
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
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 112AE: In a bomb calorimeter, the reaction vessel is surrounded by water that must be added for each...
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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
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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.
Ignition
Thermometer
wires
Stirrer
heat
sample
Water
Insulated
outside
Sample
Burning
Steel
dish
sample
bomb
chamber
Combustion (bomb) calorimeter.
In an experiment, a 0.3601 g sample of anthracene (
C4H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by
1.041 x 103 g of water. During the combustion the temperature increases from 22.55 to 25.33 °C. The heat capacity of water is
4.1843-0
The heat capacity of the calorimeter was determined in a previous experiment to be 996.1 J. "C¹
Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of anthracene based on these data.
CH()+(33/2)0,(9) 5H₂O(I)+14CO2(g) +Energy
Molar Heat of Combustion =
kJ/mol
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