A car burns octane in the following balanced reaction: 2C8H18 + 25O2 -> 16CO2 + 18H2O. If the car burns 500 grams of octane, how many grams of CO2 will be produced?

The answer to your question is 1544 g of CO₂

Explanation:

Data

mass of octane = 500 g

mass of CO₂ = ?

Balanced chemical reaction

               2C₈H₁₈  +  25O₂   ⇒    16CO₂   +   18H₂O

Process

1.- Calculate the molar mass of octane and of carbon dioxide

C₈H₁₈ = 2[(12 x 8) + (1 x 18)] = 2[(96 + 18] = 2[114] = 228 g

CO₂ = 16[(12 x 1) + (16 x 2)] = 16[12 + 32] = 16[44] = 704 g

2.- Calculate the mass of carbon dioxide produced

                    228 g of C₈H₁₈ 704 g of CO₂

                     500 g of C₈H₁₈  x CO₂

                              x = (500 x 704) / 228

                              x = 352000/228

                              x = 1544 g of CO₂