Question

Calculate the mass in grams of carbon dioxide produced from 11.2 g of octane (C8H18) in the reaction above.

Answer 1

Answer:

34.6g

Explanation:

Given parameters:

Mass of Octane  = 11.2g

  Reaction expression;

      2C₈H₁₈  + 25O₂  →  16CO₂  + 18H₂O

Mass of octane = 11.2g

Unknown:

Mass of carbon dioxide produced  = ?

Solution:

From the balanced reaction equation;

         2 mole of octane produced 16 moles of carbon dioxide

From the given specie, let us find the number of moles;

    Number of moles  = $\frac{mass}{molar mass}$  

 Molar mass of C₈H₁₈   = 8(12) + 18(1) = 114g/mole

Number of moles of octane  = $\frac{11.2}{114}$   = 0.098mole

   

    2 mole of octane produced 16 moles of carbon dioxide

    0.098 mole of octane will produce $\frac{0.098 x 16}{2}$   = 0.79mole of CO₂

Mass of CO₂ = number of moles x molar mass

           Molar mass of CO₂ = 12 + 2(16)  = 44g/mol

Mass of CO₂  = 0.79 x 44  = 34.6g