4 C_{3}H_{5}O_{9}N_{3}(l) → 12 CO_{2}(g) + 6 N_{2}(g) + O_{2}(g) + 10 H_{2}O(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 N_{2} are produced in the detonation?

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

Why did you divide by 536 for a

that is dividing actual mass by the molar mass to get moles

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