Please explain step by step (in legible print) how you got the answer. Enter you

Question

Please explain step by step (in legible print) how you got the answer.

Enter your answer in the provided box. The enthalpy of combustion of benzoic acid (C6HCOOH) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be -3226.7 kJ/mol. When 2.7245 g of benzoic acid are burned in a calorimeter, the temperature rises from 21.84°C to 26.67°C. What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly 2250 g.) kJ/OC

Explanation / Answer

Hcomb = -3226.7 kJ/mol

m = 2.7245 g of acid

mol = mass/MW = 2.7245/122 = 0.0223 mol

Q = n*HRXN = 0.0223*3226.7 = 71.95541 kJ

then

Cbomb = Qbomb/dT = 71.95541/(26.67-21.84) = 14.897 kJ/°C

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