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 0.972 g sample of glutaric acid (C5H8O4) in a bomb calorimeter containing 1130 g of water. The temperature increases from 26.00°C to 28.80°C. The heat capacity of water is 4.184 J/(g · °C). The molar heat of combustion is -2151 kJ per mole of glutaric acid. C5H8O4(s) + 5O2(g) ? 5CO2(g) + 4H2O(l) + Energy
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Given mass of glutaric acid = 0.972 g Molar mass of glutaric acid = 132.12 g/mol Number of moles = 0.972 g / 132.12 g/mol = 7.35 x 10^-3 moles ** Show more…
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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 0.976-g sample of dimethyl oxalate (C4H6O4) in a bomb calorimeter containing 1100. g of water. The temperature increases from 25.80 °C to 28.30 °C. The heat capacity of water is 4.184 J/g°C. The molar heat of combustion is -1675 kJ per mole of dimethyl oxalate. C4H6O4(s) + 7/2 O2(g) -> 4 CO2(g) + 3 H2O(l) + Energy Calculate the heat capacity of the calorimeter. Heat capacity of calorimeter = J/°C
Lane F.
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. Ignition wires heat sample Thermometer Stirrer In the laboratory a student burns a 0.655-g sample of phthalic acid (C8H6O4) in a bomb calorimeter containing 1180. g of water. The temperature increases from 24.10 °C to 26.30 °C. The heat capacity of water is 4.184 J g-1°C-1. Water The molar heat of combustion is -3224 kJ per mole of phthalic acid. Insulated outside chamber Sample dish Burning sample Steel bomb C8H6O4(s) + 15/2 O2(g) -> 8 CO2(g) + 3 H2O(l) + Energy Combustion (bomb) calorimeter. Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = J/°C
Adi S.
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 0.601-g sample of 1,2-benzenediol (C6H6O2) in a bomb calorimeter containing 1030. g of water. The temperature increases from 25.20 °C to 28.20 °C. The heat capacity of water is 4.184 J g-1°C-1. The molar heat of combustion is -2864 kJ per mole of 1,2-benzenediol. C6H6O2(s) + 13/2 O2(g) -> 6 CO2(g) + 3 H2O(l) + Energy Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = J/°C
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