what was the percent yield of the reaction?

Question

The balanced equation below shows the reaction by which aspirin, C9H8O4C9H8O4, can be synthesized from salicylic acid, C7H6O3C7H6O3, and acetic anhydride, C4H6O3C4H6O3. If the reaction of 80.680.6 g C7H6O3C7H6O3 with excess C4H6O3C4H6O3 produced 60.660.6 g of aspirin, what was the percent yield of the reaction?

The molar mass of C7H6O3C7H6O3 is 138.1 g/mol and that of C9H8O4C9H8O4 is 180.2 g/mol.

C7H6O3(s)+C4H6O3(l)⟶C9H8O4(s)+CH3CO2H(l)

Answer 1

1. 0.584 mol C7H6O3 x 1 mol C9H8O4/1 mol C7H6O3 x 180.2 g C9H8O4/mol = 105.2 g C9H8O4 The percent yield of the reaction is calculated as follows:
2. percent yield = actual yield / theoretical yield x 100%
3. percent yield = 60.6 g / 105.2 g x 100% = 57.6% Therefore, the percent yield of the reaction is 57.6%.