Respuesta :
Answer:
The theoretical yield of aspirin is 3.95 grams
Explanation:
Step 1: Data given
Mass of salicylic acid = 3.03 grams
Volume of acetic anhydride = 3.61 mL
Density of acetic anhydride = 1.08 g/cm³
Step 2: The balanced equation
C4H6O3+C7H6O3→C9H8O4+C2H4O2
Step 3: Calculate moles salicylic acid
Moles salicylic acid = mass salicylic acid / molar mass salicylic acid
Moles salicylic acid = 3.03 grams /138.121 g/mol
Moles salicylic acid = 0.0219 moles
Step 4: Calculate mass acetic anhydride
Mass acetic anhydride = volume * density
Mass acetic anhydride = 3.61 mL * 1.08 g/mL
Mass acetic anhydride = 3.90 grams
Step 5: Calculate moles acetic anhydride
Moles acetic anhydride = 3.90 grams / 102.09 g/mol
Moles acetic anhydride = 0.0382 moles
Step 6: Calculate limiting reactant
For 1 mol salicylic acid we need 1 mol acetic anhydride to produce 1 mol aspirin
Salicylic acid is the limiting reactant. It will completely be consumed. (0.0219 moles). Acetic anhydride is in excess. There will react 0.0219 moles. There remain 0.0382 - 0.0219 =0.0163 moles
Step 7: Calculate moles aspirin
For 1 mol salicylic acid we need 1 mol acetic anhydride to produce 1 mol aspirin
For 0.0219 moles salicylic acid we'll have 0.0219 moles aspirin
Step 8: Calculate theoretical yield of aspirin
Mass of aspirin = moles aspirin *molar mass aspirin
Mass of aspirin = 0.0219 moles *180.15 g/mol
Mass of aspirin = 3.95 grams
The theoretical yield of aspirin is 3.95 grams
The theoretical yield of the aspirin obtained is 3.96 g.
What is theoretical yield?
The theoretical yield refers to the yield of the aspirin from the stoichiometry of the reaction. We have to note that the reaction is 1:1.
Number of moles of the salicylic acid = 3.03 g /138 g/mol = 0.022 moles
Number of moles of aspirin produced = 0.022 moles
Mas of aspirin produced = 0.022 moles * 180.15 g/mol = 3.96 g
Hence, the theoretical yield of the aspirin obtained is 3.96 g.
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