How much CO2 in m3 is formed from burning 10.000 kg octane?

Answer 1

Reaction of octane combustion-

2C8H18+25O2= 16CO2+ 18H2O

That mean from 228g octane (16*22.4dm3) = 358.4dm3 of CO2 is produced. {because volume of each mole is 22.4dm3}

Now, from 10 kg of octane produced volume of CO2 is = (358.4*10000)/228

=(15719.298 dm3/1000)m3

=15.719 m3.

Answer 2

The balanced chemical equation for the combustion of octane (C8H18) is 2C8H18 + 25O2 → 16CO2 + 18H2O. From this equation, 1 mole of octane produces 16 moles of CO2. Knowing that the molar mass of octane is approximately 114 g/mol, 10,000 kg (or 10,000,000 g) of octane would produce around 139,000 kg (or 139,000 m3 since the density of CO2 is about 1 kg/m3) of CO2.