Nitroglycerin $($C$3$H$5($NO$3)3)$ is produced by adding concentrated nitric acid $($HNO$3)$ to glycerin $($C$3$H$8$O$3).$

In the past, this was performed as a semi$-$batch operation in a large stirred pot containing ~ $1$ ton of material. The pot was initially filled with glycerin and the acid was then added slowly over a $2-$hour period. Nitroglycerin might explore if heat from the reaction is not removed. The story is told that operators used to sit on one$-$legged stools to make sure they didn't fall asleep while watching the pot. Now, a safer continuous$-$flow process has been developed that reduces the size of the reactor and the reaction time.

In this simple exercise, you just need to determine the heat of reactions for nitroglycerin production and explosive decomposition.

$**$ Please use $-371\mathrm{.}1$ kJ$/$mol for the enthalpy of formation for liquid nitroglycerin. One version of the table in the book has the value equal to $-279\mathrm{.}1,$ which is the value for gas phase.