A 2.461-g sample of glutamic acid, C5H9NO4 (147.13 g/mol) was burned in a bomb calorimeter with

Question

excess oxygen. The temperature of the calorimeter and the water before combustion was 23.76 °C; after
combustion the calorimeter and the water had a temperature of 29.46 °C. The calorimeter had a heat capacity of
660 J/K, and contained 1.405 kg of water. Use these data to calculate the molar heat of combustion (in kJ) of
glutamic acid

Answer 1

dH(comb) = [dH(cal)*(Tfinal-Tinitial)] + [dH(H2O)*(Tf-Ti)
dH(comb) = [660 J/K*(29.46-23.76)] + [1,405 g*4,184*(29.46-23.78)]
dH(comb) will be in J for a 2.461 g sample of glutamic acid. Convert to kJ/mol. Check my thinking.