chemistry
1. In the recent tutorial we calculated that the enthalpy change for the decomposition of nitroglycerine:
4C3H5N3O9(l) → 6N2(g) + 12CO2(g) + 10H2O(l) + O2(g)
was H = -1541.4kJ mol-1. Calculate the amount of energy, ∆U, released by the reaction.
Explain, as specifically as you can why the energy released is larger than the enthalpy change. Does this explain why nitroglycerine decomposes explosively?
4C3H5N3O9(l) → 6N2(g) + 12CO2(g) + 10H2O(l) + O2(g)
was H = -1541.4kJ mol-1. Calculate the amount of energy, ∆U, released by the reaction.
Explain, as specifically as you can why the energy released is larger than the enthalpy change. Does this explain why nitroglycerine decomposes explosively?
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