Answer to Question #173712 in Chemistry for anonymous

Question

The explosion of nitroglycerin, CHS (NO3)3 , is chemically speaking an instantaneous decomposition of a fairly complex compound into several gases, including nitrogen and water vapor. How many grams of nitrogen will result from the explosion of 2900 grams of nitroglycerine ? this equation is already balanced for you! The molar mass of nitro is 227 grams/1 mol

4C3H5(NO3)----12CO2+6N2+O2+10H2O

Answer 1

Solution:

The balanced chemical equation:

4C₃H₅(NO₃)₃ → 12CO₂ + 6N₂ + O₂ + 10H₂O

According to the equation above:

Moles of C₃H₅(NO₃)₃ / 4 = Moles of N₂ / 6

Moles of C₃H₅(NO₃)₃ / 2 = Moles of N₂ / 3

Moles of C₃H₅(NO₃)₃ = Mass of C₃H₅(NO₃)₃ / Molar mass of C₃H₅(NO₃)₃

The molar mass of C₃H₅(NO₃)₃ is 227 g mol^-1.

Hence,

Moles of C₃H₅(NO₃)₃ = 2900 g / 227 g mol^-1 = 12.775 mol

Moles of N₂ = 3 × Moles of C₃H₅(NO₃)₃ / 2 = (3 × 12.775 mol) / 2 = 19.163 mol

Mass of N₂ = Moles of N₂ × Molar mass of N₂

The molar mass of N₂ is 28 g mol^-1.

Hence,

Mass of N₂ = 19.163 mol × 28 g mol^-1 = 536.564 g = 536.56 g

Mass of N₂ = 536.56 g

OR (short form solution):

(2900 g C₃H₅N₃O₉) × (1 mol C₃H₅N₃O₉ / 227 g C₃H₅N₃O₉) × (6 mol N₂ /4 mol C₃H₅N₃O₉) × (28 g N₂ / 1 mol N₂) = 536.56 g

Answer: 536.56 grams of nitrogen (N₂) will result from the explosion of 2900 grams of nitroglycerine.