Answer:
52.206 kg
Explanation:
From the given information:
Mass of hexane C6H14 = [tex]19.3*10^3 \ g \times \dfrac{38.3}{100}[/tex]
= 7391.9 g
Mass of octane C8H18 = [tex]19.3*10^3 \ g \times \dfrac{13.9}{100}[/tex]
= 2682.7 g
Mass of decane C10H22 = [tex]19.3*10^3 \ g \times \dfrac{47.8}{100}[/tex]
= 9225.4 g
However, recall that:
number of moles of an atom = mass/molar mass
∴
For hexane, no of moles = 7391.9 g/86.18 g/mol
= 85.77 moles
For octane, no of moles = 2682.7 g/114.23 g/mol
= 23.49 moles
For decane, no of moles = 9225.4 g/142.29 g/mol
= 64.84 moles
Therefore:
number of moles of CO2 produced = (6 × 85.77)+(23.49)+(10×64.84) moles
= 1186.51 moles
Finally, the mass of CO2 produced is:
= 1186.51 mol × 44 g/mol
= 52206.44 g
= 52.206 kg
