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)

0.67 L

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

i just calculated it all out, and not including weekends, and all the different days off. as of this school year (2018-2019) students are spending 2198 hours in school this year