Aspirin or acetyl salicylic acid is synthesized by reacting salicylic acid with acetic anhydride: C7H6O3 (salicylic aci...

Since the given reaction is

C₇H₆O₃ + C₄H₆O₃ -----> C₉H₈O₄ + C₂H₄O₂ 

a) Hence from the above balanced reaction, we can say that 1 mole of salicylic acid is required to produce 1 mole of aspirin if 100 % of salicylic acid is converted

Since moles = mass / molar mass 

And molar mass of aspirin = 12 X 9 + 8 X 1 + 4 X 16 = 12 X Atomic mass of C + 8 X Atomic mass of H + 4 X Atomic mass of O = 180 g/mol 

And molar mass of salicylic acid = 7 X Atomic mass of C + 6 X Atomic mass of H + 3 X Atomic mass of O = 138 g/mol

Hence moles of aspirin produced = 4 / 180 = 0.02222 

Since moles of salicylic acid reacted = moles of aspirin produced = 0.02222

Hence mass of salicylic acid = moles X molar mass = 0.02222 X 138 = 3.067 g

b) Since when 100 % of salicylic acid was reacting, we needed 3.067 g of salicylic acid 

Hence if 74.9 % of salicylic acid is converted, the mass required = 3.067 X 100 / 74.9 = 4.095 g

c) Since moles of salicylic acid reacting = mass / molar mass = 9.26 / 138 = 0.0671

And since molar mass of acetic anhydride = 12 X Atomic mass of C +  6 X Atomic mass of H + 3 X Atomic mass of O = 102 g/mol

Hence moles of acetic anhydride reacting = 8.54 / 102 = 0.0837

Since 1 mole of salicylic acid needs 1 mole of acetic anhydride for complete reaction

And since moles of acetic acid is more than required 

Hence salicylic acid is limiting reagent 

Hence moles of aspirin produced theoretically = moles of salicylic acid = 0.0671 

Hence mass of aspirin produced theoretically = moles X molar mass = 0.0671 X 180 = 12.08 g = the theoretical yield of aspirin

Hence percent error = aspirin produced X 100 / the theoretical yield of aspirin = 10.9 X 100 / 12.08 = 90.24 % approx