0.1 mole of nitroglycerin is exploded in a confined volume of 10 ml. The reaction equation is approximately: 2 C3H5N3O9(l) = 6 CO2(g) + 5 H2O(g) + 3 N2(g) + 1/2 O2(g) The enthalpy of the reaction is -337.4 kcal/mole of nitroglycerin at 20C. At what do you estimate the maximum temperature and pressure reached during detonation? Use the following heat capacity values (cal/K-mole) at constant volume (Cv): H2O(g) CO2(g) O2(g) N2(g) 7.0 7.0 5.0 5.0 Assume that these CVs remain constant. Neglect the air originally present in the container. Ans.: Tmax = 7523 K Pmax = 44757 atm