Question

Calculate the number of pounds of CO2CO2 released into the atmosphere when a 22.0 gallon22.0 gallon tank of gasoline is burned in an automobile engine. Assume that gasoline is primarily octane, C8H18,C8H18, and that the density of gasoline is 0.692 g⋅mL−1.0.692 g⋅mL−1. This assumption ignores additives. Also, assume complete combustion. CO2CO2 released:

Answer 1

391.28771 pounds of carbon-dioxide was released into the atmosphere when 22.0 gallon tank of gasoline is burned in an automobile engine.

Step-by-step 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= (Mass)/(Volume)`

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`

Mass of octane burnt in the tank = M = 57,629.081 g

Moles of octane =
`(57,629.081 g)/(114.08g/mol)=505.1637 mol`

According to reaction, 2 moles of octane gives 16 moles of carbon-dioxide.

Then 505.1637 mol of octane will give:

`(16)/(2)* 505.1637 mol=4,041.3100 mol` 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.