Nitroglycerin detonates according to the balanced reaction:
4 C₃H₅N₃O₉( l ) → 12 CO₂( g ) + 6 N₂( g ) + O₂( g ) + 10 H₂O( g ) .
If 1.00 kg of nitroglycerin is detonated, how many L of products (assume all gases at standard temperature and pressure, so 1.00 mole = 22.4 L of volume) are released?

Question

Quizplus · Accepted Answer

The balanced equation shows that 4 moles of nitroglycerin produce 29 moles of gas (12 CO + 6 N2 + 10 H2O + 1 O2). The molar mass of nitroglycerin (C3H5N3O9) is approximately 227 g/mol, so 1.00 kg (1000 g) is about 4.41 moles. Multiplying the moles of nitroglycerin by the moles of gas produced per mole of nitroglycerin (4.41 moles * 29 moles/4 moles) gives approximately 32.07 moles of gas. At STP, 1 mole of gas occupies 22.4 L, so the total volume of gas produced is 32.07 moles * 22.4 L/mole = 718.37 L, which rounds to 715 L.

Nitroglycerin Detonates According to the Balanced Reaction