(Solved): Combustion (bomb) calorimeter. In an experiment, a \( 0.3615 \mathrm{~g} \) sample of anthracene \( ...

Combustion (bomb) calorimeter. In an experiment, a \( 0.3615 \mathrm{~g} \) sample of anthracene \( \left(\mathrm{C}_{14} \mathrm{H}_{10}\right) \) is bumed completely in a bomb calorimeter. The calorimeter is surrouinded by \( 1.110 \times 10^{3} \mathrm{~g} \) of water. During the combustion the temperature increases from \( 23.97 \) to \( 26.61^{\circ} \mathrm{C} \). The heat capacity of water is \( 4.184 \mathrm{~J} \cdot \mathrm{g}^{-1} \cdot{ }^{-} \mathrm{C}^{-1} \) The heat capacity of the calorimeter was determined in a previous experiment to be \( 976.2 \mathrm{~J}^{\circ} \mathrm{C}^{-1} \) Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of anthracene based on these data. \[ \mathrm{C}_{14} \mathrm{H}_{10}(s)+(33 / 2) \mathrm{O}_{2}(g) \rightarrow 5 \mathrm{H}_{2} \mathrm{O}(l)+14 \mathrm{CO}_{2}(g)+\text { Energy } \]