A bomb calorimeter , or a constant volume calorimeter, is a device often used to

Question

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 0.462 g sample of 1,6-hexanediol (C6H14O2) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1104 g of water. During the combustion the temperature increases from 21.85 to 24.66 oC.  

The heat capacity of the calorimeter was determined in a previous experiment to be 908.9 J/oC.

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

Explanation / Answer

Heat generated by burning 0.462g of sample = C*dT = 908.9*(24.66-21.85) = 2554.0 J

Molar mass of 1,6-hexanediol = 118 g/mol

Therefore molar heat of combustion = 2554.0*118/0.462 = 652.3 kJ/mol

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