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?
Thank you for the opportunity to help you with your question!
a) mass=vol x density
=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
Why did you divide by 536 for a
that is dividing actual mass by the molar mass to get moles
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