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Homework answers / question archive / Calculate the standard enthalpy of formation (ΔH?f) for nitroglycerin
Calculate the standard enthalpy of formation (ΔH?f) for nitroglycerin.
The explosive nitroglycerin (C3H5N3O9) decomposes rapidly upon ignition or sudden impact according to the following balanced equation:
4C3H5N3O9(l)→12CO2(g)+10H2O(g)+6N2(g)+O2(g)ΔH?rxn=−5678kJ
4C3H5N3O9(l)→12CO2(g)+10H2O(g)+6N2(g)+O2(g)
Hprocucts = 12*CO2 + 10*H2O + 6*N2 + O2 = 12*CO2 + 10*H2O +0 +0
Hreactants = 4*Hnitro
Hrxn = Hproducts - Hreactants
-5678 = 12*CO2 + 10*H2O -(4*Hnitro)
4H Nitro = 12*CO2 + 10*H2O + 5678
4H Nitro = 12*-393.509 + 10*-241.818 + 5678
Hnitro= (-1462.288)/4 = -365.572 kJ/mol
