A student measures out exactly 0.105 g of salicylic acid and runs the experiment as dictated in the lab manual. They obtain 0.111 g of aspirin. What is the percent yield for their reaction?

The percent yield of the reaction is 8.10 %.

Explanation:

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

     .....(1)

Given mass of salicylic acid = 0.105g

Molar mass of salicylic acid = 138.12 g/mol

Putting values in equation 1, we get:

The chemical equation for the formation of aspirin from salicylic acid follows:

By Stoichiometry of the reaction:

1 mole of salicylic acid produces 1 mole of aspirin

So, 0.0076 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 = 0.0076 moles

Putting values in equation 1, we get:

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

Experimental yield of aspirin = 0.111 g

Theoretical yield of aspirin = 1.37 g

Putting values in above equation, we get:

Hence, the percent yield of the reaction is 8.10 %.

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