A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.6336 g sample of nonanedioic acid (C9H16O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.236×103 g of water. During the combustion the temperature increases from 26.86 to 29.59 °C. The heat capacity of water is 4.184 J g-1°C-1.

The heat capacity of the calorimeter was determined in a previous experiment to be 980.4 J/°C.

Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of nonanedioic acid based on these data.

C9H16O4(s) + 11O2(g) 8 H2O(l) + 9 CO2(g) + Energy