a 2.56 g sample of anthracene, C14H10, was burned to heat an aluminum calorimeter (mass=948 g). The calorimeter contained 1.50 L

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 degrees Celsius and a final temperature of 34.3 degrees Celsius.
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 of delta H = -7150 kJ/mol, what is the percentage error?

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