(a) If a sample contains 1.97 mL of nitroglycerine (density = 1.592 g/mL) is det

Question

(a) If a sample contains 1.97 mL of nitroglycerine (density = 1.592 g/mL) is detonated, how much total moles of gas are produced?

(b) If each mole of gas occupies 58 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?
Detonation of nitroglycerin proceeds as shown in the following equation. 4 C3H5O9N3(l) rightarrow 12 CO2(g) + 6 N2(g) + O2(g) + 10 H2O(g) If a sample contains 1.97 mL of nitroglycerine (density = 1.592 g/mL) is detonated, how much total moles of gas are produced? If each mole of gas occupies 58 L under the conditions of the explosion, how many liters of gas are produced? How many grams of N2 are produced in the detonation?

Explanation / Answer

Mass nitroglycerine = 1.99 mL x 1.592 g/mL = 3.13624
Moles = 3.13624 g/ 227.09 g/mol= 0.01381056

Moles CO2 = 0.01381056 x 12 / 4 = 0.041431679

moles N2 = 0.01381056 x 6 / 4 = 0.020715839

moles O2 = 0.01381056 x 1 / 4 = 0.00345264

moles H2O = 0.01381056 x 10 / 4 = 0.0345264

(b)volume= 0.01381056*29/4*58=5.80734

(c)grams of N2 are produced=0.020715839*28=0.580043507 grams

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