In the reaction, 72.2 g C7H6O3 , reacts with excess C4H6O3 , producing 41.2 g of aspirin, C9H8O4 . C7H6O3(s)+C4H6O3(l)⟶C9H8O4(s)+CH3CO2H(l) Calculate the percent yield of this reaction.

Answer 1

Since the equation is balanced, one mole of C₇H₆O₃ produces one mole of aspirin.

Since C₇H₆O₃ is the limiting reagent the yield is = Moles of aspirin/moles of C₇H₆O₃