Question

Calculate the number of pounds of CO2 released into the atmosphere when a 22.0 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. CO2 released:

Answer 1

Answer:

391.28771 pounds of carbon-dioxide released into the atmosphere.

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 gasolin be M

$d=\frac{M}{V}$

M = V × d = 83,279.02 mL × 0.692 g/mL=57,629.081 g

Assume that gasoline is primarily octane (given)

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

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

Moles of octane =$\frac{57,629.081 g}{114.08 g/mol}=505.1637 mol$

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

Then 505.1637 mol of octane will give:

$\frac{16}{2}\times 505.1637 mol=4,041.3100 mol$ 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 released into the atmosphe

Answer 2

The number of pounds of CO₂ released into the atmosphere when a 22.0 gallon tank of gasoline is burned in an automobile engine is 392.3 pounds.

We'll begin by converting 22 gallon to mL.

1 gallon = 3785.412 mL

Therefore,

22 gallon = 22 × 3785.412

22 gallon = 83279.064 mL

Next, we shall determine the mass of 83279.064 mL of gasoline (C₈H₁₈).

Density = 0.692 g/mL

Volume = 83279.064 mL

Mass of C₈H₁₈ =?

Mass = Density × Volume

Mass of C₈H₁₈ = 0.692 × 83279.064

Mass of C₈H₁₈ = 57629.11 g

Next, we shall determine the mass of C₈H₁₈ that reacted and the mass of CO₂ produced from the balanced equation.

2C₈H₁₈ + 25O₂ —> 16CO₂ + 18H₂O

Molar mass of C₈H₁₈ = (12×8) + (1×18)

= 96 + 18

= 114 g/mol

Mass of C₈H₁₈ from the balanced equation = 2 × 114 = 228 g

Molar mass of CO₂ = 12 + (16×2)

= 12 + 32

= 44 g/mol

Mass of CO₂ from the balanced equation = 16 × 44 = 704 g

Thus,

From the balanced equation above,

228 g of C₈H₁₈ reacted to produce 704 g of CO₂

Next, we shall determine the mass of CO₂ produced by the reaction of 57629.11 g of C₈H₁₈. This can be obtained as follow:

From the balanced equation above,

228 g of C₈H₁₈ reacted to produce 704 g of CO₂

Therefore,

57629.11 g of C₈H₁₈ will react to produce = $\frac{57629.11 * 704}{228}$ = 177942.515 g of CO₂

Finally, we shall convert 177942.515 g of CO₂ to pounds.

453.592 g = 1 pound

Therefore,

177942.515 g = $\frac{177942.515}{453.592}$

177942.515 g = 392.3 pounds

Therefore, the number of pounds of CO₂ released into the atmosphere is 392.3 pounds.

Learn more: https://brainly.com/question/13476603