A)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 0.392-g sample of bisphenol A (C15H16O2) in a bomb calorimeter containing 1140. g of water. The temperature increases from 25.00 °C to 27.40 °C. The heat capacity of water is 4.184 J g-1°C-1.
The molar heat of combustion is â7821 kJ per mole of bisphenol A.
C15H16O2(s) + 18 O2(g) ------>15 CO2(g) + 8 H2O(l) + Energy
Calculate the heat capacity of the calorimeter.
heat capacity of calorimeter =_________ J/°C
B)
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.
In an experiment, a 0.5574 g sample of benzil (C14H10O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.379Ã103 g of water. During the combustion the temperature increases from 26.36 to 28.99 °C. The heat capacity of water is 4.184 J g-1°C-1.
The heat capacity of the calorimeter was determined in a previous experiment to be 847.1 J/°C.
Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of benzil based on these data.
C14H10O2(s) + (31/2) O2(g) ------->5 H2O(l) + 14 CO2(g) + Energy
Molar Heat of Combustion = _________ kJ/mol
C) 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.
In an experiment, a 0.9900 g sample of β-D-fructose (C6H12O6) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.292Ã103 g of water. During the combustion the temperature increases from 21.82 to 24.12 °C. The heat capacity of water is 4.184 J g-1°C-1.
The heat capacity of the calorimeter was determined in a previous experiment to be 991.1 J/°C.
Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of β-D-fructose based on these data.
C6H12O6(s) + 6O2(g) -------> 6 H2O(l) + 6 CO2(g) + Energy
Molar Heat of Combustion = ____________ kJ/mol
All three problems are a set for one question on my homework, so please answer all three. Thank you so much!
A)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 0.392-g sample of bisphenol A (C15H16O2) in a bomb calorimeter containing 1140. g of water. The temperature increases from 25.00 °C to 27.40 °C. The heat capacity of water is 4.184 J g-1°C-1.
The molar heat of combustion is â7821 kJ per mole of bisphenol A.
C15H16O2(s) + 18 O2(g) ------>15 CO2(g) + 8 H2O(l) + Energy
Calculate the heat capacity of the calorimeter.
heat capacity of calorimeter =_________ J/°C
B)
| 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. In an experiment, a 0.5574 g sample of benzil (C14H10O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.379Ã103 g of water. During the combustion the temperature increases from 26.36 to 28.99 °C. The heat capacity of water is 4.184 J g-1°C-1.The heat capacity of the calorimeter was determined in a previous experiment to be 847.1 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of benzil based on these data. C14H10O2(s) + (31/2) O2(g) ------->5 H2O(l) + 14 CO2(g) + Energy Molar Heat of Combustion = _________ kJ/mol C) 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. In an experiment, a 0.9900 g sample of β-D-fructose (C6H12O6) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.292Ã103 g of water. During the combustion the temperature increases from 21.82 to 24.12 °C. The heat capacity of water is 4.184 J g-1°C-1.The heat capacity of the calorimeter was determined in a previous experiment to be 991.1 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of β-D-fructose based on these data. C6H12O6(s) + 6O2(g) -------> 6 H2O(l) + 6 CO2(g) + Energy Molar Heat of Combustion = ____________ kJ/mol All three problems are a set for one question on my homework, so please answer all three. Thank you so much! |
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