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 0.491-g sample of 1,6-hexanediol (C6H14O2) in a bomb calorimeter containing 1180. g of water. The temperature increases from 24.60 °C to 27.30 °C. The heat capacity of water is 4.184 J g-1°C-1.

The molar heat of combustion is −3792 kJ per mole of 1,6-hexanediol.
C6H14O2(s) + 17/2 O2(g) 6 CO2(g) + 7 H2O(l) + Energy
Calculate the heat capacity of the calorimeter.