Calculating the Mass of Carbon Dioxide Produced from Hexane Combustion
What mass of carbon dioxide (CO2) can be produced from 15.6 g of C6H14 and excess oxygen?
Answer: The mass of carbon dioxide produced is 46.7 grams.
Explanation:
To calculate the number of moles, we use the equation:
Number of moles = Given mass / Molar mass
Given mass of hexane = 15.6 g
Molar mass of hexane = 88.2 g/mol
Putting values in the equation, we get:
Moles of hexane = 15.6 g / 88.2 g/mol = 0.177 mol
The chemical equation for the combustion of hexane is:
2 C6H14 + 19 O2 → 12 CO2 + 14 H2O
As oxygen gas is present in excess, it is considered an excess reagent. Hexane is considered a limiting reagent because it limits the formation of the product.
By stoichiometry of the reaction:
2 moles of hexane produce 12 moles of carbon dioxide
So, 0.177 moles of hexane will produce = (12/2) x 0.177 = 1.062 mol of carbon dioxide
Now, calculating the mass of carbon dioxide by using the equation:
Molar mass of carbon dioxide = 44 g/mol
Moles of carbon dioxide = 1.062 mol
Putting values in the equation, we get:
1.062 mol = Mass of carbon dioxide / 44 g/mol
Mass of carbon dioxide = (1.062 mol x 44 g/mol) = 46.7 g
Hence, the mass of carbon dioxide produced is 46.7 grams.
What is the chemical equation for the combustion of hexane? The chemical equation for the combustion of hexane is 2 C6H14 + 19 O2 → 12 CO2 + 14 H2O.