At STP, what volume of N2 is produced by the complete decomposition of 1 mole of nitroglycerin?

At STP, what volume of N2 is produced by the complete decomposition of 1 mole of nitroglycerin?

• A. 5 L
• B. 10 L
• C. 20 L
• D. 30 L

Answer: (D)

To determine the volume of nitrogen gas (N2) produced from the decomposition of nitroglycerin, we first need to analyze the decomposition reaction of nitroglycerin. The balanced chemical equation for the decomposition of nitroglycerin is: 4 C3H5N3O9 (l) → 6 N2 (g) + 10 H2O (g) + 6 CO2 (g) From this equation, we can see that four moles of nitroglycerin produce six moles of nitrogen gas. To find out how much nitrogen gas is produced from one mole of nitroglycerin, we can set up a conversion: \[ \text{Moles of N2 from 1 mole of nitroglycerin} = \frac{6 \text{ moles N2}}{4 \text{ moles nitroglycerin}} = 1.5 \text{ moles N2} \] Since we know that one mole of any ideal gas at standard temperature and pressure (STP) occupies a volume of 22.4 liters, we can calculate the volume of nitrogen gas produced: \[ \text{Volume of N2} = 1.5 \

To determine the volume of nitrogen gas (N2) produced from the decomposition of nitroglycerin, we first need to analyze the decomposition reaction of nitroglycerin. The balanced chemical equation for the decomposition of nitroglycerin is:

4 C3H5N3O9 (l) → 6 N2 (g) + 10 H2O (g) + 6 CO2 (g)

From this equation, we can see that four moles of nitroglycerin produce six moles of nitrogen gas. To find out how much nitrogen gas is produced from one mole of nitroglycerin, we can set up a conversion:

[

\text{Moles of N2 from 1 mole of nitroglycerin} = \frac{6 \text{ moles N2}}{4 \text{ moles nitroglycerin}} = 1.5 \text{ moles N2}

]

Since we know that one mole of any ideal gas at standard temperature and pressure (STP) occupies a volume of 22.4 liters, we can calculate the volume of nitrogen gas produced:

[

\text{Volume of N2} = 1.5 \