Benzoic Acid (C7H6O2) burns in oxygen to form carbon dioxide and water. The dHcombustion of the reaction is measured to be -3225 kJ/m of Benzoic Acid burned. In an experiment, a Bomb Calorimeter is charged with 0.2568g of Benzoic Acid and excess oxygen. The calorimeter is placed in an insulated jacket containing 500.0g of water [Cp(water)= 4.18 J/g°C]. The reaction is run, and the temperature of the calorimeter and its surroundings is found to increase from 22.08°C to 24.34°C.
What mass of oxygen should be placed in the calorimeter? Assume that a 10-fold excess of Oxygen is used to ensure complete reaction.
How much energy is released by the experiment?
Assuming that all of the energy released by the experiment is used to heat the calorimeter and the water, determine the Calorimeter Constant of the calorimeter in J/g°C.