A \(1.000 \mathrm{~mol}\) sample of propane, a gas used for cooking in many
rural areas, was placed in a bomb calorimeter with excess oxygen and ignited.
The initial temperature of the calorimeter was \(25.000^{\circ} \mathrm{C}\) and
its total heat capacity was \(97.13 \mathrm{~kJ}^{\circ} \mathrm{C}^{-1}\). The
reaction raised the temperature of the calorimeter to \(27.282^{\circ}
\mathrm{C}\).
(a) Write the balanced chemical equation for the reaction in the calorimeter.
(b) How many joules were liberated in this reaction?
(c) What is the heat of reaction of propane with oxygen expressed in
kilojoules per mole of \(\mathrm{C}_{3} \mathrm{H}_{8}\) burned?