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

Thank you for the opportunity to help you with your question!

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


Please let me know if you need any clarification. I'm always happy to answer your questions.
Jul 24th, 2015

Wrong answer I said 1.97 u are using 1.99 

Jul 24th, 2015

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