Question

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?

Answer 1

The answer to your question is 1544 g of CO₂

Step-by-step 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