The maximum theoretical yield of aspirin can be calculated using stoichiometry. The balanced chemical equation for the synthesis of aspirin is:C7H6O3 salicylic acid + C4H6O3 acetic anhydride C9H8O4 aspirin + C2H4O2 acetic acid From the balanced equation, we can see that 1 mole of salicylic acid reacts with 1 mole of acetic anhydride to produce 1 mole of aspirin. To calculate the maximum theoretical yield, we need to know the amount in moles of each reactant.Let's assume we have 1 mole of salicylic acid 138.12 g and 1 mole of acetic anhydride 102.09 g . Since the reaction is a 1:1 ratio, the limiting reactant is the one with the least amount of moles. In this case, both reactants have the same amount of moles, so neither is limiting.Now, we can calculate the maximum theoretical yield of aspirin:1 mole of salicylic acid 1 mole of aspirin / 1 mole of salicylic acid 180.16 g of aspirin / 1 mole of aspirin = 180.16 g of aspirinSo, the maximum theoretical yield of aspirin is 180.16 g.However, the actual yield of aspirin is often less than the theoretical yield due to several factors, including the presence of impurities. Impurities can affect the actual yield in several ways:1. Impurities can react with the reactants, reducing their concentration and thus decreasing the amount of aspirin produced.2. Impurities can cause side reactions, leading to the formation of unwanted byproducts that reduce the yield of aspirin.3. Impurities can lower the efficiency of the reaction by affecting the reaction rate or equilibrium.In practice, chemists often use purification techniques to minimize the impact of impurities on the actual yield. However, it is rare to achieve a 100% yield in a chemical reaction due to various factors, including the presence of impurities.