Give the percent yield when 28.16 g of CO2 are formed from the reaction of 5.000 moles of C8H18 with 10.00 moles of O2.
2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
First, calculate the theoretical yield of CO2 that can be formed from the given amounts of reactants.
From the balanced chemical equation, it is clear that 2 moles of C8H18 react with 25 moles of O2 to produce 16 moles of CO2.
So, for every 2 moles of C8H18, 16 moles of CO2 are produced.
Given that there are 5.000 moles of C8H18 and 10.00 moles of O2, the limiting reactant is C8H18.
Calculate the moles of CO2 produced:
(5.000 moles C8H18) x (16 moles CO2 / 2 moles C8H18) = 40.00 moles CO2
Now, calculate the mass of the theoretical yield of CO2:
(40.00 moles CO2) x (44.01 g/mol) = 1760.4 g CO2
Now, calculate the percent yield:
Percent Yield = (Actual Yield / Theoretical Yield) x 100
Percent Yield = (28.16 g / 1760.4 g) x 100 ≈ 1.60%
Therefore, the percent yield is approximately 1.60%.