Question

Determine the volume of carbon dioxide gas produced at STP when 2.5 g of nitroglycerin decomposes by this balanced equation. 4C3H5N3O9(l) → 12CO2(g) + 10H2O(g) + 6N2(g) + O2(g)

Answer 1

0.67 L

Step-by-step explanation:

Given data:

Volume of carbon dioxide = ?

Mass of nitroglycerine = 2.5 g

Temperature = standard = 273.15 K

Pressure = standard = 1 atm

Solution:

Chemical equation:

4C₃H₅N₃O₉ → 12CO₂ + 10 H₂O + 6N₂ + O₂

Number of moles of nitroglycerine:

Number of moles = mass/ molar mass

Number of moles = 2.4 g/ 227.1 g/mol

Number of moles = 0.01 mol

Now we will compare the moles of nitroglycerine and carbon dioxide from balance chemical equation.

C₃H₅N₃O₉ : CO₂

4 : 12

0.01 : 12/4×0.01 = 0.03 mol

Volume of CO₂:

PV = nRT

V = nRT/P

V = 0.03 mol× 0.0821 atm.L/mol.K× 273.15 K / 1 atm

V = 0.67 L