Liquid hexane CH3CH24CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2
and gaseous water H2O . If 21.1g of carbon dioxide is produced from the reaction of 27.57g
of hexane and 179.0g of oxygen gas, calculate the percent yield of carbon dioxide.
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1. Determine the limiting reactant:
First, calculate the number of moles of each reactant:
Moles of hexane = 27.57g / 86.18g/mol = 0.319 moles
Moles of oxygen gas = 179.0g / 32.00g/mol = 5.59 moles
Next, write the balanced chemical equation for the reaction:
2C6H14 + 19O2 -> 12CO2 + 14H2O
Using the stoichiometry of the balanced chemical equation, the mole ratio between hexane and carbon dioxide is 2:12. Therefore, the number of moles of carbon dioxide that can be produced from 0.319 moles of hexane is:
0.319 moles * (12 moles CO2 / 2 moles hexane) = 1.91 moles
Since the number of moles of carbon dioxide produced is limited by the amount of hexane, and the actual amount produced is 21.1g, convert this to moles:
21.1g / 44.01g/mol = 0.479 moles
2. Calculate the percent yield:
Theoretical yield (based on the limiting reactant) = 1.91 moles * 44.01g/mol = 83.97g
Percent yield = (actual yield / theoretical yield) * 100% = (21.1g / 83.97g) * 100% = 25.1%
Therefore, the percent yield of carbon dioxide is 25.1%.
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