Problem: The explosive nitroglycerin (C3H5N3O9) decomposes rapidly upon ignition or sudden impact according to the following balanced equation:4 C3H5N3O9 (l) →12 CO2 (g) +10 H2O (g) + 6 N2 (g) + O2 (g)       ΔHorxn = −5678 kJCalculate the standard enthalpy of formation (ΔHof) for nitroglycerin.

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For the reaction:

$4\ C_3H_5N_3O_{9\ (l)} →12\ CO_{2\ (g)} +10\ H_2O_ {(g)} + 6\ N_{2\ (g)} + O_{2\ (g)} \qquad \qquad ΔH^o_{rxn} = −5678\ kJ$

In order to find $ΔH^o_{reactant}$ , use the equation:

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Problem Details

The explosive nitroglycerin (C3H5N3O9) decomposes rapidly upon ignition or sudden impact according to the following balanced equation:
4 C3H5N3O(l) →12 CO(g) +10 H2O (g) + 6 N(g) + O(g)       ΔHorxn = −5678 kJ

Calculate the standard enthalpy of formation (ΔHof) for nitroglycerin.

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