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 0.4596 g sample of 1,6-hexanediol (C6H14O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.337×103 g of water. During the combustion the temperature increases from 21.64 to 23.88 °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 769.4 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 1,6-hexanediol based on these data. C6H14O2(s) + (17/2) O2(g)  7 H2O(l) + 6 CO2(g) + Energy Molar Heat of Combustion =  ____  kJ/mol

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Chapter8: Thermochemistry
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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 0.4596 g sample of 1,6-hexanediol (C6H14O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.337×103 g of water. During the combustion the temperature increases from 21.64 to 23.88 °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 769.4 J/°C.

Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 1,6-hexanediol based on these data.

C6H14O2(s) + (17/2) O2(g)  7 H2O(l) + 6 CO2(g) + Energy

Molar Heat of Combustion =  ____  kJ/mol
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