Final answer:
The total pressure produced by the explosion of nitroglycerin is calculated using Dalton's law of partial pressures, considering the total gases produced, which makes the specific pressure increase difficult to predict without precise data.
Step-by-step explanation:
The total pressure produced in the explosion of nitroglycerin can be significant owing to the liberation of various gaseous products. The chemical equation representing the explosion is:
4C3H5(ONO2)3 → 12CO2 + 10H2O + 6N2 + O2
Using Dalton's law of partial pressures, we know that the total pressure of a gaseous mixture is equal to the sum of the partial pressures of each component gas. Therefore, in calculating the pressure increase during the explosion, we must consider the volumes, temperatures, and moles of each gas produced.
Given that reactions such as nitroglycerin explosion are spontaneous reactions, they tend to be exothermic and result in an increase in entropy. These properties affect the pressure increase, making it difficult to predict without specific measurements and calculations of the system before and after the reaction.