Aspirin is produced by the reaction of salicylic acid (M = 138.1 g/mol) and acetic anhydride (M = 102.1 g/mol) .
C₇H₆O₃(s) + C₄H₆O₃( $\ell$ ) ? C₉H₈O₄(s) + C₂H₄O₂( $\ell$ )
If 2.04 g of C₉H₈O₄ (M = 180.2 g/mol) is produced from the reaction of 3.03 g C₇H₆O₃ and 4.01 g C₄H₆O₃, what is the percent yield?

Question

Aspirin is produced by the reaction of salicylic acid (M = 138.1 g/mol) and acetic anhydride (M = 102.1 g/mol) .
C₇H₆O₃(s) + C₄H₆O₃(

\ell

) ? C₉H₈O₄(s) + C₂H₄O₂(

\ell

)
If 2.04 g of C₉H₈O₄ (M = 180.2 g/mol) is produced from the reaction of 3.03 g C₇H₆O₃ and 4.01 g C₄H₆O₃, what is the percent yield?

Quizplus · Accepted Answer

The theoretical yield of aspirin is calculated based on the limiting reactant, salicylic acid. The moles of salicylic acid are 3.03 g / 138.1 g/mol = 0.0219 mol. The theoretical yield of aspirin is 0.0219 mol * 180.2 g/mol = 3.95 g. The percent yield is (2.04 g / 3.95 g) * 100% = 51.6%.

Aspirin Is Produced by the Reaction of Salicylic Acid (M ℓ\ellℓ

Aspirin Is Produced by the Reaction of Salicylic Acid (M $\ell$