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.

The complete reaction is as,

      4-Aminophenol + Acetic Anhydride → Acetaminophen + Acetic Acid

First of all convert the ml of Acetic anhydrite to grams,
As,
                                Density  =  mass / volume
Solving for mass,
                                mass  =  Density × Volume
Putting values,
                                mass  =  1.08 g/ml × 5ml

                                mass =  5.4 g of acetic anhydride

First Find amount of  acetic anhydride required to react completely with 2 g of p-Aminophenol,
As,
       109.1 g of p-aminophenol required  =  102.1 g of acetic anhydride
so,     2 g of p-aminophenol will require  =  X g of Acetic Anhydride

Solving for X,
                                X  =  (2 g × 102.1 g) ÷ 109.1 g
 
                                X  =  1.87 g of acetic anhydride is required to be reacted.

But, we are provided with 5.4 g of Acetic Anhydride, means p-aminophenol is the limiting reactant and it controls the formation of product. Now Let's calculate for product,
As,
       109.1 g of p-aminophenol produced  =  180.2 g of Acetaminophen
So    2.00 g of p-aminophenol will produce  =  X g of Acetaminophen

Solving for X,
                               X  =  (2.00 g × 180.2 g) ÷ 109.1 g
 
                               X  =  3.30 g of Acetaminophen

Result:
          If 2.00g of p-aminophenol reacts with 5.00 ml of acetic anhydride 3.30 g of acetaminophen is made.

It starts to rust i think