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**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:__

$\overline{){\mathbf{+}}{\mathbf{q}}{\mathbf{}}\mathbf{(}\mathbf{from}\mathbf{}\mathbf{anthracene}\mathbf{)}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{-}}{\mathbf{q}}{\mathbf{}}\mathbf{(}\mathbf{to}\mathbf{}\mathbf{water}\mathbf{)}}$

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

$\overline{){\mathbf{q}}{\mathbf{=}}{\mathbf{mc}}{\mathbf{\u2206}}{\mathbf{T}}}$

q = heat, J

###### Problem Details

When 0.455 g of anthracene, C_{14}H_{10} (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

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