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
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
