Calculate Heat in Combustion of C4H10(g)

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The discussion focuses on calculating the heat evolved during the complete combustion of 1.325 g of butane (C4H10) at specified conditions. The combustion reaction releases -2877 kJ of heat per mole of butane. Participants express confusion about the calculation process and the concept of heat of enthalpy. Clarification is sought on how to determine the amount of butane needed for the calculation. Understanding the heat of enthalpy is essential for accurately determining the energy released in combustion reactions.
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How much heat, in kilojoules, is evolved in the complete combustion of 1.325 g C4H10(g) at 23.6 degrees Celsius and 738 mmHg? The complete combustion of butane is represented by this equation

C4H10(g) + \frac{13}{2} O2(g)\rightarrow 4CO2(g) + 5H2O(l)
\DeltaH degrees Celsius = -2877 kJ

I am not sure at all how to do this and this is something we went over very briefly in class without any examples, so any help would be greatly appreciated.
 
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You were given the heat of enthalpy of...?

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