Synthesis of Aspirin 7-10 EXPERIMENTAL DATA: Fill in the tables below. Use the p

Question

Synthesis of Aspirin 7-10 EXPERIMENTAL DATA: Fill in the tables below. Use the proper number of significant figures for your data. (5 pts) 2. Synthesis Data Volume of acetic anhydride (mL) Mass of acetic anhydride (g) (density 1.080 g/mL) Moles of acetic anhydride (molecular weight = 102.09 g/mol) Mass of salicylic acid (g) 403 Moles of salicylic acid (molecular weight = 138.12 g/mol) Limiting reagent for this reaction Theoretical yield of Aspirin (g) (molecular weight-180.16 g/mol) Actual yield of Aspirin (g) Percent Yield of Aspirin

Explanation / Answer

density = mass /volume

1.08 = mass / 1

mass = 1.08 gms

Mass of acetic anhydride = 1.08 gms

MOles of acetic anhydride = mass /molar mass = 1.08 / 102.09 = 0.0105789

Moles of salicyclic acid = mass /molar mass = 0.403 / 138.12 = 0.0029177

Reaction :

acetic anhydride + salicylic acid aspirin + acetic acid

C7H6O3(salicylic acid) + C4H6O3 C9H8O4(aspirin) + HC2H3O2.

Here 1 mole of acetic anhydride reacts with 1 mole of salicylic acid and forms 1 mole of aspirin

Here there are less moles of salicylic acid that react completely with acetic anhydride

so the limiting reagent is salicylic acid

Moles of aspirin formed = moles of salicylic acid (limiting reagent) = 0.0029177

Mass = moles*molar mass = 0.0029177*180.16 = 0.52566 gms

Theoritical yield of Aspirin = 0.52566 gms

Actual yield must be given

Percent yield = Actual yield*100 /Theoritical yield

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