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Answer: Nitroglycerin, an explosive compound, decomposes
Chapter 5, Problem 97P(choose chapter or problem)
Nitroglycerin, an explosive compound, decomposes according to the equation
\(4 \mathrm{C}_{3} \mathrm{H}_{5}\left(\mathrm{NO}_{3}\right)_{3}(\mathrm{s}) \rightarrow 12 \mathrm{CO}_{2}(\mathrm{g})+10 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+6 \mathrm{N}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})\)
Calculate the total volume of gases when collected at 1.2 atm and 25°C from \(2.6 \times 10^{2}\) g of nitroglycerin. What are the partial pressures of the gases under these conditions?
Questions & Answers
QUESTION:
Nitroglycerin, an explosive compound, decomposes according to the equation
\(4 \mathrm{C}_{3} \mathrm{H}_{5}\left(\mathrm{NO}_{3}\right)_{3}(\mathrm{s}) \rightarrow 12 \mathrm{CO}_{2}(\mathrm{g})+10 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+6 \mathrm{N}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})\)
Calculate the total volume of gases when collected at 1.2 atm and 25°C from \(2.6 \times 10^{2}\) g of nitroglycerin. What are the partial pressures of the gases under these conditions?
ANSWER:Step 1 of 6
Here, we are going to calculate the total volume of the product and partial pressure of gases under the condition.
We have to calculate the number of moles of the product formation.
Given that,
The molar mass of nitroglycerin = 227.09 g/mol
Mass of the nitroglycerin = 