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A 2.56 g sample of anthracene, C 14 H 10 , was burned to heat an

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 20.5oC and a final temperature of 34.3oC. 

a) Calculate the molar heat of combustion of anthracene.

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

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

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