Question

If a sample of nitroglycerin containing 2 mL (density = 1.592g/mL) is detonated, how many total moles of gas are produced? If each mole of gas occupies 55L under the conditions of the explosion, how many liters of gas are produced? How many grams of nitrogen gas are specifically produced?

Answer 1

Total moles of gas = 0.1225

Volume of gas produced : 6.7375 L

mass of Nitrogen : 0.588 g

Further explanation

Given

2 ml of Nitroglycerin(ρ=1.592 g/ml)

Required

Total moles of gas

Solution

Nitroglycerin detonated ⇒ decomposition reaction

4C₃H₅N₃O₉(s)⇒ 6N₂(g)+12CO(g)+10H₂O(g)+7O₂(g)

mass of Nitroglycerin :

$\tt mass=2~ml\times 1.592~g/ml=3.184~g$

moles of Nitroglycerin :

$\tt moles=\dfrac{3.184}{227,0865~g/mol}=0.014$

Total moles of gas:

$\tt \dfrac{6+12+10+7}{4}\times 0.014=0.1225$

Volume of gas produced :

$\tt 0.1225\times 55=6.7375~L$

moles of Nitrogen :

$\tt \dfrac{6}{4}\times 0.014=0.021$

mass of Nitrogen :

$\tt 0.021\times 28=0.588~g$