Question

If 2.00g of p-Aminophenol ( 109.1 g/mol) reacts with 5.00 mL of acetic anhydride (102.1 g/mol and density = 1.08 g/mL), what mass of acetaminophen (180.2 g/mol) would be made? Show all calculations.

Mass of acetaminophen: _________________

b. If you only isolated 2.41 g of acetaminophen, what would the percent yield of your reaction be? Show all calculations.

Percent Yield: _________________

Answer 1

p-Amino phenol + Acetic anhydride Acetaminophenol + Acetic acid.

From 1 mole of p-Amino phenol gives 1 mole of Acetaminophenol.

Acetic anhydride is a reagent no of moles = weight / M. Wt

Weight = density x Volume

= 5 x 1.08

= 5.4 g

Moles = 5.4/102.1 = 0.05288 moles

Weight of p-Amino phenol = 2.00 g

M. Weight = 109.1 g/mol

No of moles of p-Amino phenol = no of moles of Acetaminophenol

= weight /M. Wt

= 2/109.1

= 0.01833 moles

Weight of Acetaminophenol =?

M. Wt = 180.2 g/mol

No of moles = 0.01833 moles

Weight = moles x M. Wt

= 0.01833 x 180.2

= 3.303 g (theoretical yield)

We have got 2.41 g of product (practical yield).

=? %

= 2.41/3.303 x 100

= 72.96%.