The complete combustion of RDX is 2C3H6N6O6 + 302 --> 6H2O + 6CO2 + 6N2. How much heat is liberated from the complete combustion of 10g of RDX? delta H values: H20 = -286, CO2 = -394, RDX = +65 (all in kJ/mol) I thought it'll be (6*-286 + 6*-394) - (2*65) = -4210 kJ/mol Then divide that by the amount of moles in 100g. But I end up with this massive number which is wrong. I'm not sure whether to take into acount the 2 moles of RDX reacting when finding the amount of moles in 100g as well. Thanks.