In the reaction of 1.15 g of salicylic acid, molar mass 138.12 g/mol, with 2.83 g of acetic anhydride, molar mass 102.10 g/mol, a student obtained 1.21 g of acetylsalicylic acid, molar mass 180.17 g/mol. What is the percent yield?

Question

Patsy

Chemistry

14 March, 15:04

In the reaction of 1.15 g of salicylic acid, molar mass 138.12 g/mol, with 2.83 g of acetic anhydride, molar mass 102.10 g/mol, a student obtained 1.21 g of acetylsalicylic acid, molar mass 180.17 g/mol. What is the percent yield?

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Alyson · Answer 1

The balanced reaction would be written as:

C7H6O3 + C4H6O3--->C9H8O4 + HC2H3O2

To determine the percent yield, we need to first determine the theoretical yield if the reaction were to proceed completely. Then, we divide the actual yield that is given to the theoretical yield times 100 percent. The limiting reactant from the reaction would be salicylic acid. We do as follows:

Theoretical yield: 1.15 g C7H6O3 (1 mol / 138.12 g) (1 mol C9H8O4 / 1 mol C7H6O3) (180.17 g / mol) = 1.50 g C9H8O4 should be produced

Percent yield = 1.21 / 1.50 x 100 = 80.66 %

Thus, only 80.66% of the theoretical C9H8O4 is being produced.