Calculate the mass in grams of carbon dioxide produced from 11.2 g of octane (C8H18) in the reaction above. 18 + 25 O2 --> 16 CO2 + 18 H2O

89.6 g
17.3 g
34.5 g
46.2 g

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  =  

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

Number of moles of octane  =   = 0.098mole

    2 mole of octane produced 16 moles of carbon dioxide

    0.098 mole of octane will produce   = 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

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the atomic number of carbon is six, which means that a carbon atom has six protons. carbon has three naturally occurring isotopes: carbon-12, carbon-13, and carbon-14. which of these statements are true about carbon and its isotopes? select all that appl