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# Solved: Aspirin can be made in the laboratory by reacting ## Problem 91P Chapter 8

Introductory Chemistry | 5th Edition

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Problem 91P

PROBLEM 91P

Aspirin can be made in the laboratory by reacting acetic anhydride (C4HgO3) with salicylic acid (C7H6O3) to form aspirin (C9HgO4) and acetic acid (C2H4O2). The balanced equation is:

C4H6O3 + C7H6O3 → C9H8O4 + C2H4O2

ln a laboratory synthesis, a student begins with 5.00 mL of acetic anhydride (density = 1.08 g/mL) and 2.08 g of salicylic acid. Once the reaction is complete, the student collects 2.01 g of aspirin. Determine the limiting reactant, theoretical yield of aspirin, and percent yield for the reaction.

Step-by-Step Solution:

Solution 91P

Step 1:

C4H6O3 + C7H6O3 → C9H8O4 + C2H4O2

Given that initial volume of acetic anhydride is  5.00 mL and density is 1.08 g/mL

Mass= density volume=5.00 mL 1.08 g/mL=5.4 g

Number of moles of C4H6O3 = Given mass/Molecular mass

Molecular mass of C4H6O3=102g/mol

Thus number of moles of C4H6O3= =0.052 moles

Step 2:

Given that mass of C7H6O3 is 2.08 g

Number of moles of C7H6O3 =Given mass/Molecular mass

Molecular mass of C7H6O3=138g/mol

Thus number of moles of C7H6O3= =0.015 moles

Step 3:

From the equation it is clear that 1 mole of C4H6O3 combines with 1 mole of  C7H6O3 to give 1 mole each of aspirin and acetic acid.Thus we can say that the ratio in which both the reactants should be present is 1:1.Since lesser amount (less than 0.052)of C7H6O3 is present ,it should be the limiting reagent.

Step 4 of 5

Step 5 of 5

##### ISBN: 9780321910295

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