##### Chemistry Stoichem Problems

 Chemistry Tutor: None Selected Time limit: 1 Day

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?

Jul 24th, 2015

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

Jul 24th, 2015

Wrong answer I said 1.97 u are using 1.99

Jul 24th, 2015

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Jul 24th, 2015
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Jul 24th, 2015
May 29th, 2017
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