# Problem: When 0.455 g of anthracene, C14H10 (molar mass = 178.23 g/mol) is combusted in a bomb calorimeter that has a water jacket containing 500.0 g of water, the temperature of the water increases by 8.63°C. Assuming that the specific heat of water is 4.18 J/(g • °C), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion per mole of anthracene. A) -39.7 kJ/mol B) -8120 kJ/mol C) -7060 kJ/mol D) +39.7 kJ/mol

###### FREE Expert Solution

Determine the heat involved during the combustion of anthracene using the calorimetry equation and the provided values

In bomb calorimetry, we can determine the heat of combustion by analyzing the temperature rise in water. In mathematical terms, the heat released by anthracene is equal to the heat absorbed by water:

We will use the heat released by the reaction to calculate its initial temperature. Recall that heat can be calculated using the following equation:

$\overline{){\mathbf{q}}{\mathbf{=}}{\mathbf{mc}}{\mathbf{∆}}{\mathbf{T}}}$

q = heat, J

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###### Problem Details

When 0.455 g of anthracene, C14H10 (molar mass = 178.23 g/mol) is combusted in a bomb calorimeter that has a water jacket containing 500.0 g of water, the temperature of the water increases by 8.63°C. Assuming that the specific heat of water is 4.18 J/(g • °C), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion per mole of anthracene.

A) -39.7 kJ/mol

B) -8120 kJ/mol

C) -7060 kJ/mol

D) +39.7 kJ/mol