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 0.815-g sample of isophthalic acid (C₈H₆O₄) in a bomb calorimeter containing 1110. g of water. The temperature increases from 25.80 °C to 28.70 °C. The heat capacity of water is 4.184J g⁻¹.°C⁻¹ The molar heat of combustion is -3203 kJ per mole of isophthalic acid.
C₈H₆O₄(s) + 15/2O₂(g) —> 8 CO₂(g) + 3 H₂O(l) + Energy
Calculate the heat capacity of the calorimeter.
heat capacity of calorimeter = _______ J°C
