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 0.749-g sample of acetylsalicylic acid (C9H8O4) in a bomb calorimeter containing 1030. g of water. The temperature increases from 24.10 °C to 27.20 °C. The heat capacity of water is 4.184 J g-1°C-1. The molar heat of combustion is −3869 kJ per mole of acetylsalicylic acid. C9H8O4(s) + 9 O2(g) 9 CO2(g) + 4 H2O(l) + Energy Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = J/°C