Textbook Problem

Aspirin (C₉H₈O₄) is synthesized by reacting salicylic acid (C₇H₆O₃) with acetic anhydride (C₄H₆O₃). The balanced equation is

${\text{C}}_{\text{7}}{\text{H}}_{\text{6}}{\text{O}}_{\text{3}}\text{+}{\text{C}}_{\text{4}}{\text{H}}_{\text{6}}{\text{O}}_{\text{3}}\to {\text{C}}_{\text{9}}{\text{H}}_{\text{8}}{\text{O}}_{\text{4}}\text{+}{\text{HC}}_{\text{2}}{\text{H}}_{\text{3}}{\text{O}}_{\text{2}}$

a. What mass of acetic anhydride is needed to completely consume 1.00 × 10² g salicylic acid?

b. What is the maximum mass of aspirin (the theoretical yield) that could be produced in this reaction?