Answer to Question #95640 in Physical Chemistry for m

Question

Calculate the number of pounds of CO2 released into the atmosphere when a 16.0 gallon tank of gasoline is burned in an automobile engine. Assume that gasoline is primarily octane, C8H18, and that the density of gasoline is 0.692 g⋅mL−1. This assumption ignores additives. Also, assume complete combustion.
Useful conversion factors:
1 gallon=3.785 L
1 kg=2.204 lb

Answer 1

Combustion of octane is given by:

$2C_8H_{18}+25O_2\to 16CO_2+18H_2O$

Molar mass of octane = $114.23\ g\ mol^{-1}$

228.46 gm of octane will produce 704 gm of carbondioxide

Mass of octane taken = $692\times 16\times 3.785=41907.52\ g$

41907.52 gm octane will produce $\frac{704\times41907.52}{228.46}=129,138.12\ gm\ CO_2$

= $129.13812\ kg\ CO_2$

$129.13812\times 2.204\ lb$

$=284.6\ pounds\ CO_2$