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Solved: Calculating Theoretical Yield and Percent
Chapter , Problem 1PE(choose chapter or problem)
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?
Questions & Answers
QUESTION:
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?
ANSWER:Step 1 of 2
(a) The theoretical yield is:
\(=(125.0\ g\ C_6H_{12})\times(1\ mol\ C_6H_{12})\times(2\ mol\ H_2C_6H_8O_4)(2\ mol\ C_6H_{12})\times(146.0\ g\ H_2C_6H_8O_4)(1\ mol\ H_2C_6H_8O_4)\)
\(=43.4\ g\ H_2C_6H_8O_4\)