Aspirin can be prepared from salicylic acid ( c 7 h 6 o 3 ), which has a molar mass of 138.12 g/mol, and acetic anhydride ( c 4 h 6 o 3 ), which has a molar mass of 102.04 g/mol. the density of acetic anhydride is 1.082 g/ml. c 7 h 6 o 3 + c 4 h 6 o 3 ⟶ c 9 h 8 o 4 + c 2 h 3 o 2 what is the yield of aspirin ( c 9 h 8 o 4 ), which has a molar mass of 180.15 g/mol, possible when reacting 2.18 g of salicylic acid with 1.01 ml of acetic anhydride?

The yield of aspirin obtained from the reaction is 1.93 g

Given that;

The reaction equation is

Amount of salicylic acid = 2.18 g/138.12 g/mol = 0.0158 moles

Density of acetic anhydride = 1.082 g/mL

Mass of acetic anhydride =  1.082 g/mL × 1.01 mL = 1.093 g

Amount of acetic anhydride = 1.093 g/102.04 g/mol = 0.0107 moles

We have to find the limiting reactant. It is the reactant that gives the lowest yield of products

Since the mole ratio of the reaction is 1:1:1:1, the limiting reactant is acetic anhydride.

Mass of aspirin produced = 0.0107 moles of asprin × 180.15 g/mol = 1.93 g

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