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Butane, C4H10, is widely used as a fuel for disposable lighters. When one mole of butane is burned in oxygen, carbon dioxide and steam are formed and 2658 kJ of heat is evolved.
a) Write the thermochemical equation for the reaction.

First I wrote the chemical equation for the reaction:
2C4H10 + 13O2 --> 8CO2 + 10H2O

Since the problem gives the heat for one mole of butane, would the correct thermochemical equation be this:
C4H10 + 13/2O2 --> 4CO2 + 5H2O delta-H= -2658.3 kJ


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