If you used 0.155 mL of acetic anhydride, and 0.165 g of p-aminophenol what was your theoretical yield of acetaminophen?
___________g
If you recovered 0.173 g of acetaminophen, what was your percent yield?
________%
To determine the theoretical yield of acetaminophen, you need to calculate the stoichiometric ratio between acetic anhydride and p-aminophenol in the reaction, and then calculate the amount of acetaminophen that would be produced based on the limiting reactant.
Step 1: Write the balanced chemical equation for the reaction:
C6H7NO + (CH3CO)2O → C8H9NO2 + CH3COOH
Step 2: Calculate the molar mass of acetic anhydride (MW(CH3CO)2O) and p-aminophenol (MWC6H7NO).
MW(CH3CO)2O = (2*MW(C)) + (4*MW(H)) + (2*MW(O)) = 102.09 g/mol
MW(C6H7NO) = (6*MW(C)) + (7*MW(H)) + MW(N) + MW(O) = 109.13 g/mol
MW(C8H9NO2) = (8*MW(C)) + (9*MW(H)) + MW(N) + (2*MW(O)) = 151.17 g/mol
Step 3: Calculate the number of moles for acetic anhydride and p-aminophenol used.
Number of moles of acetic anhydride = 0.155 mL * (1 g/mL) / MW(CH3CO)2O
Number of moles of p-aminophenol = 0.165 g / MWC6H7NO
Step 4: Determine the limiting reactant.
The reactant with the smaller number of moles is the limiting reactant. Let's assume acetic anhydride is the limiting reactant.
Step 5: Calculate the theoretical yield of acetaminophen.
Using the stoichiometric ratio from the balanced equation:
1 mole of acetic anhydride produces 1 mole of acetaminophen (C8H9NO2).
Therefore, the theoretical yield of acetaminophen is equal to the number of moles of acetic anhydride used.
Theoretical yield of acetaminophen = number of moles of acetic anhydride * MW(C8H9NO2)
Finally, to calculate the percent yield:
Percent yield = (actual yield / theoretical yield) * 100
Given: actual yield = 0.173 g, theoretical yield = calculated in the previous step.
Therefore, you can now substitute the values into the formulas to get the answers:
The theoretical yield of acetaminophen is ________ g.
The percent yield is ________ %.