Answered Essay: Topic: Synthesis of aspirin Use stoichiometry calculations on the starting mass of the limiting reactant

Topic: Synthesis of aspirin

Use stoichiometry calculations on the starting mass of the limiting reactant to determine what amount of acetic anhydride to add.

1. Assume 2.0 g of salicylic acid will be used. Calculate the moles of salicylic acid using its molar mass. 2. Use the mole ratio from the chemical equation to determine the ideal moles of acetic anhydride. Then multiply the answer by three to obtain an excess of the acetic anhydride. Convert the moles of acetic anhydride to mass in grams using its molar mass. 3. 4. Convert the mass to volume in mL using the density of acetic anhydride, which is 1.082 g/mL. Finally round the volume to the nearest 0.1 mL so it can be measured in the lab.

1. Assume 2.0 g of salicylic acid will be used. Calculate the moles of salicylic acid using its molar mass. 2. Use the mole ratio from the chemical equation to determine the ideal moles of acetic anhydride. Then multiply the answer by three to obtain an excess of the acetic anhydride. Convert the moles of acetic anhydride to mass in grams using its molar mass. 3. 4. Convert the mass to volume in mL using the density of acetic anhydride, which is 1.082 g/mL. Finally round the volume to the nearest 0.1 mL so it can be measured in the lab.

Expert Answer

Answer

no of moles of salicyclic acid=weight/molecular weight=2/138=0.01449 moles

C7H6O3 + C4H6O3 → C9H8O4 + HC2H3O2

from the equation one mole of salicyclic acid reacts with one mole of acetic anhydride

molar mass of acetic anhydride=102 g/mol

0.01449 moles of salicyclic acid reacts with 0.01449 moles of acetic anhydride

therefore excess of acetic anhydride=0.01449*3=0.04347 moles

weight of acetic anhydride=moles*molecular weight=0.04347*102=4.43394 g

density=mass/volume

volume=mass/density=4.43394/1.082=4.097 ml~4.1ml

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