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Calculate the molar heat of combustion of

A 2.56 g sample of anthracene, C14H10, was burned to heat an aluminum calorimeter (mass = 948 g). The calorimeter contained 1.50 L of water with an initial temperature of 20.5 C and a final temperature 34.3C

a) Calculate the molar heat of combustion of anthracene.

b) Write the thermochemical equation, two ways, for the complete combustion of anthracene.

c) If the actual value for ΔH = -7150 kJ/mol, what is the percentage error?

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