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 1.12g sample of -D-fructose ( C6H12O6 ) in a bomb calorimeter containing 1160g of water. The temperature increases from 24.50C to 27.60C. The heat capacity of water is 4.184J/(gC) The molar heat of combustion is 2810kJ per mole of -D-fructose. C6H12O6(s)+6O2(g)6CO2(g)+6H2O(l)+Energy Combustion (bomb) calorimeter. Calculate the heat capacity of the calorimeter. Heat capacity =J/C