Calculating the Theoretical Yield and the Percent Yield for a Reaction
Adipic acid, \(\mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{4}\), is used to produce nylon, The acid is made commercially by a controlled reaction between cyclohexane \(\left(\mathrm{C}_{6} \mathrm{H}_{12}\right)\) and \(\mathrm{O}_{2}\):
\(2\mathrm{\ C}_6\mathrm{H}_{12}(l)+5\mathrm{\ O}_2(g)\rightarrow2\ \mathrm{H}_2\mathrm{C}_6\mathrm{H}_8\mathrm{O}_4(l)+2\mathrm{\ H}_2\mathrm{O}(g)\)
(a) Assume that you carry out this reaction with 25.0 g of cyclohexane and that cyclohexane is the limiting reactant. What is the theoretical yield of adipic acid?
(b) If you obtain 33.5 g of adipic acid from your reaction, what is the percent yield of adipic acid?
Step 1 of 2
We are given a chemical equation and the quantity of the limiting reactant, 25.0 g of \(C_6H_{12}\). We are asked to calculate the theoretical yield of a product \(H_2C_6H_8O_4\) and the percent yield if only 33.5 g of product is obtained.
(a) The theoretical yield, which is the calculated quantity of adipic acid formed, can be calculated using the sequence of conversions.
(b) The percent yield is calculated by using the given actual yield (33.5 g) with the theoretical yield.
