Aspirin sun thesis green chemistry and assime the aspirin is prepared by the following reaction and that 10.09. of salicylic acid and an excess of acetic anhydride are used. if you get 5.og of aspirin: cy hco3 +cu the oz - cats o4 + c a hu oz what is the percent yield of aspirin? show calculations formula : experimental performance theoretical performance x 100

The percentage yield of aspirin is 38.02 %.

Explanation:

To calculate the number of moles, we use the equation:

     .....(1)

Given mass of salicylic acid = 10.09 g

Molar mass of salicylic acid = 138.12 g/mol

Putting values in equation 1, we get:

The chemical equation for the formation of aspirin follows:

As, acetic anhydride is present in excess. So, it is considered as an excess reagent.

Thus, salicylic acid is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of salicylic acid produces 1 mole of aspirin.

So, 0.0730 moles of salicylic acid will produce = of aspirin

Now, calculating the mass of aspirin from equation 1, we get:

Molar mass of aspirin = 180.16 g/mol

Moles of aspirin = 0.073 moles

Putting values in equation 1, we get:

To calculate the percentage yield of aspirin, we use the equation:

Experimental yield of aspirin = 5.0 g

Theoretical yield of aspirin = 13.15 g

Putting values in above equation, we get:

Hence, the percent yield of aspirin is 38.01 %.

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