Liquid hexane CH3CH24CH3 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. Suppose 4.3 g of hexane is mixed with 25.8 g of oxygen. Calculate the maximum mass of carbon dioxide that could be produced by the chemical reaction. Round your answer to 2 significant digits.

13g of CO₂ is the maximum amount that could be produced

Explanation:

The reaction of hexane with oxygen is:  

C₆H₁₄ + 19/2O₂ → 6CO₂ + 7H₂O  

Where 19/2 moles of oxygen react per mole of C₆H₁₄

To solve this question we need to find theoretical yield finding limiting reactant :

Moles C₆H₁₄:  

4.3g C₆H₁₄ * (1mol / 86.18g) = 0.0499 moles  

Moles O₂:  

25.8g * (1mol / 32g) = 0.806 moles  

For a complete reaction of 0.0499 moles of C₆H₁₄ are needed:

0.0499 moles of C₆H₁₄ * (19/2 mol O₂ / 1mol C₆H₁₄) = 0.474 moles of O₂.

As there are 0.806 moles, O₂ is in excess and C₆H₁₄ is limiting reactant

In theoretical yield, the moles of hexane added = 6Moles of CO₂ produced. Moles of CO₂ are:

0.0499 moles C₆H₁₄ * (6mol CO₂ / 1mol C₆H₁₄) = 0.299 moles CO₂

In grams:

0.299 moles CO₂ * (44.01g / mol) = 13g CO₂

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.