Nitroglycerin, an explosive compound, decomposes according to the equation below. 4 c3h5(no3)3(s) 12 co2(g) + 10 h2o(g) + 6 n2(g) + o2(g) calculate the total volume of gases when collected at 1.2 atm and 25°c from 2.5 ✕ 102 g of nitroglycerin.

162.6 liter

Explanation:

1) Balanced chemical equation:

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

2) Convert 2.5 × 10² g of C₃H₅(NO₃)₃ into number of moles

molar mass of C₃H₅(NO₃)₃ = 227.0865 g/mol

number of moles = mass in grams / molar mass = 250 g / 227.0865 g/mol = 1.10 moles

3) Using proportion find the number of moles of each product:

1.10 moles C₃H₅(NO₃)₃ / 4 moles C₃H₅(NO₃)₃ × equation coefficient

i) CO₂:

12 ⇒ 1.10 / 4 × 12 = 3.3 moles

ii) H₂O:

10 ⇒ 1.10 / 4 × 10 = 2.75 mol

iii) N₂:

6 ⇒ 1.10 / 4 × 6 = 1.65 mol

iv) O₂:

1 ⇒ 1.10 / 4 × 1 = 0.275 mol

4) Total number of moles

3.3 mol + 2.75 mol + 1.65 mol + 0.275 mol = 7.975 mol of gas

5) Use ideal gases equation to find the volume

pV = nRT ⇒ V = nRT / p

V = 7.975 mol × 0.0821 atm×liter / K×mol × 298K / 1.2 atm = 162.6 liter