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Aspirin can be made in the laboratory by reacting acetic anhydride (C4HgO3) with

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 91P Chapter 8

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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1
Problem 91P

Aspirin can be made in the laboratory by reacting acetic anhydride (\(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3}\)) with salicylic acid (\(\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3}\)) to form aspirin (\(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\)) and acetic acid (\(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\)). The balanced equation is:

\(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3}+\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3} \rightarrow \mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}+\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\)

In 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.

Equation Transcription:

Text Transcription:

C_4 H_6 O_3

C_7 H_6 O_3

C_9 H_8 O_4

C_2 H_4 O_2

C_4 H_6 O_3 + C_7 H_6 O_3 right arrow C_9 H_8 O_4 + C_2 H_4 O_2

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 mL1.08 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 of 5

Chapter 8, Problem 91P is Solved
Step 3 of 5

Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

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Aspirin can be made in the laboratory by reacting acetic anhydride (C4HgO3) with