Description
Detonation of nitroglycerin proceeds as shown in the following equation.
4 C3H5O9N3(l) → 12 CO2(g) + 6 N2(g) + O2(g) + 10 H2O(g)
(a) If a sample containing 1.97 mL of nitroglycerine (density = 1.592 g/mL) is detonated, how many total moles of gas are produced?
(b) If each mole of gas occupies 43 L under the conditions of the explosion, how many liters of gas are produced?
(c) How many grams of N2 are produced in the detonation?
Explanation & Answer
Thank you for the opportunity to help you with your question!
a) mass=vol x density
=1.97x1.592
=3.13624g
moles=3.13624/536
=5.85 x 10^-3
b) 5.85 x 10^-3 x 43= 0.2516 L
c) 5.85 x 10^-3 x6/29
=1.21 x 10^-3 g
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