Answer:
391.28771 pounds of carbon-dioxide was released into the atmosphere when 22.0 gallon tank of gasoline is burned in an automobile engine.
Explanation:
Density of the gasoline ,d= 0.692 g/mL
Volume of gasoline in an tanks,V = 22.0 gallons = 83,279.02 mL
Let mass of the gasoline be M
![Density= \frac{Mass}{Volume}](https://tex.z-dn.net/?f=Density%3D%20%5Cfrac%7BMass%7D%7BVolume%7D)
M = V × d = 83,279.02 mL × 0.692 g/mL=57,629.081 g
Given that gasoline is primarily octane.
![2C_8H_{18}+25O_2\rightarrow 16CO_2+18H_2O](https://tex.z-dn.net/?f=2C_8H_%7B18%7D%2B25O_2%5Crightarrow%2016CO_2%2B18H_2O)
Mass of octane burnt in the tank = M = 57,629.081 g
Moles of octane =![\frac{57,629.081 g}{114.08g/mol}=505.1637 mol](https://tex.z-dn.net/?f=%5Cfrac%7B57%2C629.081%20g%7D%7B114.08g%2Fmol%7D%3D505.1637%20mol)
According to reaction, 2 moles of octane gives 16 moles of carbon-dioxide.
Then 505.1637 mol of octane will give:
of carbon-dioxide
Mass of 4,041.3100 mol of carbon-dioxide:
4,041.3100 mol × 44.01 g/mol = 177,858.05 g
Mass of carbon-dioxide produced in pounds = 391.28771 pounds
391.28771 pounds of carbon-dioxide was released into the atmosphere when 22.0 gallon tank of gasoline is burned in an automobile engine.