In an experiment to determine the calorific value of octane (left(mathrm{C}_{8} mathrm{H}_{18} ight)) with a bomb calorimeter

In an experiment to determine the calorific value of octane \(\left(\mathrm{C}_{8} \mathrm{H}_{18}\right)\) with a bomb calorimeter the mass of octane was \(5.42195 \times 10^{-4} \mathrm{~kg}\), the water equivalent of the calorimeter including water \(2.677 \mathrm{~kg}\) and the corrected temperature rise in the water jacket \(2.333 \mathrm{~K}\). Calculate the lower heat of reaction of octane, in \(\mathrm{kJ} / \mathrm{kmol}\) at \(15{ }^{\circ} \mathrm{C}\).

If the initial pressure and temperature were 25 bar and \(15{ }^{\circ} \mathrm{C}\), respectively and there was \(400 \%\) excess oxygen, estimate the maximum pressure and temperature reached immediately after ignition assuming no heat losses to the water jacket during this time. No air was present in the calorimeter.

\([-5,099,000 \mathrm{~kJ} / \mathrm{kmol} ; 3135 \mathrm{~K}]\)